General Chemistry MCQ
1. Hydrophobic molecules tend to be ________ by water.
Repelled
Absorbed
Mixed
Attracted
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2. The bright lines of an emission spectrum are the result of _____.
Electrons transitioning from a higher energy level to a lower energy level
The frequency decreases and the energy per photon decreases
An exothermic process, and the change in enthalpy, ΔH, will be a negative number
The system lost heat and did work on the surroundings.
Answer
Correct Answer:
Electrons transitioning from a higher energy level to a lower energy level
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3. The quantity 1.0 mg/cm2 is the same as 1.0 ________ kg/m2.
10-4.
102.
106.
10-2.
104.
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4. Based on the octet rule, phosphorus most likely forms a __________ ion.
P3+
P3-
P5+
P5-
P+.
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5. The hybridization scheme for bef2 is ________.
Sp
Sp2
Sp3
Sp3d
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6. Which ion will correctly complete the formula _________2hpo4?
2HPO4
Chlorite.
K+
HPO₄⁻²
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7. The formal charge on carbon in the molecule below is ________.
0.
+1.
+2.
+3.
-1.
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8. The hybridization of the oxygen atom labeled x in the structure below is ________.
Sp^8 hybrid orbitals
Sp^10 hybrid orbitals
Sp^2 hybrid orbitals
Sp^12 hybrid orbitals
Answer
Correct Answer:
Sp^2 hybrid orbitals
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9. An sp-hybridized atom has ______ remaining p orbitals.
Molecular
One, three
A group of sp2 hybrid orbitals assumes a trigonal planar geometry.
The formation of sp2 hybrid orbitals leaves one unhybridized valence p orbital.
Answer
Correct Answer:
A group of sp2 hybrid orbitals assumes a trigonal planar geometry.
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10. Given the following reactions is __________ kj.
Fe2O3 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g) ΔH = -28.0 kJ
3Fe (s) + 4CO2 (s) → 4CO (g) + Fe3O4 (s) ΔH = +12.5 kJ
the enthalpy of the reaction of Fe2O3 with CO
3Fe2O3 (s) + CO (g) → CO2 (g) + 2 Fe3O4 (s)
-59.0
-15.5
-109
+109
40.5
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11. Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2).
CaC2 (s) + 2H2O (g)= Ca(OH)2 (s) + C2H2 (g)
production of 13 g of c2h2 requires consumption of ________ g of h2o.
13
12
18
11
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12. The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:
C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)
when 7.3 g of c3h8 burns in the presence of excess o2, __________ g of co2 is produced.
21
12
22
4
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13. The atmospheric layer in which gases do not maintain a uniform composition is the ________.
Heteropshere
Ionosphere
Homosphere
Troposphere
Answer
Correct Answer:
Homosphere
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14. Amines can form ________ bonds with water molecules.
Hydrogen
Oxygen
Carbon
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15. All of the orbitals in a given electron shell have the same value as the ________ quantum number.
Principal
Angular momentum
Magnetic
Spin
Psi.
Answer
Correct Answer:
Principal
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16. A phase diagram assumes ______ is kept constant.
Temperature
Volume
Pressure
Density
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17. A basic amino acid has a side chain that contains ________.
An alcohol group
A methyl group
An ammonium group
A carboxyl ate group
A thiol group Moving to another question will save this response.
Answer
Correct Answer:
An ammonium group
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18. _________________ is the movement of an object or a change in its physical structure.
Work
Force
Action
None of the above
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19. Which additional product balances the reaction h2so4 + 2naoh na2so4 + ________?
2H2O
2OH
H2O2
H3O
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20. When two monosaccharides link to form a disaccharide, the by-product is __________.
Water
Fire
Mud
None of the above
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21. Water, h2o, is an example of a(n) ________.
Wave
Solid
Electric charge
Element
Chemical
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22. Van der waals interactions may result when _____.
A hydrogen atom loses an electron
Electrons are not symmetrically distributed in a molecule
Two polar covalent bonds react
Molecules held by ionic bonds react with water
Answer
Correct Answer:
Electrons are not symmetrically distributed in a molecule
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23. Typically, amides will hydrolyze under ________ conditions than esters.
Less vigorous
More dilute
More saline
Stronger
Milder
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24. The type of compound that is most likely to contain a covalent bond is ________.
One that has metals from far left and nonmetals from far right of periodic table
A solid metal
One that is composed of only nonmetals
Held together by electrostatic forces bw oppositely charged atoms
No general rule
Answer
Correct Answer:
One that is composed of only nonmetals
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25. The substance ________ is always produced when an active metal reacts with water.
NaOH
H2O
CO2
H2
O2
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26. The production of smog from no gas requires ________.
CFCs
Chlorine
Oxygen
Water
Nitrogen
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27. The production of carbon-14 ____.
Takes place in the upper atmosphere
Is mostly due to fallout from nuclear explosions
Occurs to a large extent in nuclear reactors
Is caused by photosynthesis in plants
Answer
Correct Answer:
Takes place in the upper atmosphere
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28. The process of ___ occurs when a hydrate loses its water of hydration.
Effloresce
Hydration
Deliquescent
Solvation
Answer
Correct Answer:
Effloresce
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29. The presence of reducing sugars _______.
Means that amylase has been denatured
Is detected using Benedict's reagent
Is detected using IKI
Means that the substrate is present
Answer
Correct Answer:
Is detected using Benedict's reagent
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30. The oxidation number of hydrogen when it is in a compound other than a hydride is _____.
+2
+1
+7
+3
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31. The number of protons in a cation must always be ________ the number of electrons.
Less than
Greater than
Equal to
Answer
Correct Answer:
Greater than
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32. The n = 1 shell contains ________ p orbitals. all the other shells contain ________ p orbitals.
3,6
6,2
3,3
0,6
0,3
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33. The innermost electron shell of an atom can hold up to _____ electrons
8
32
2
18
1
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34. The hybridizations of nitrogen in nf3 and nh3 are __________ and __________, respectively.
Sp2, sp2 1
Sp, sp3
Sp3, sp
Sp3, sp3
Sp2, sp3
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35. The hybridization of the oxygen atom labeled x in the structure below is ________. н н н 10:-х н-с-с-с-с-8-н H-CH Н
Sp
Sp2
Sp3
Sp3d
Sp3d2
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36. The ground-state electron configuration of the element ________ is [kr]5s14d5.
Nb
Mo
Cr
Mn
Tc
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37. The functional groups shown are the _______ group, the _______ group, and the _______ group.
Proteins, nucleic acid, carbohydrates
Proteins, lipids, carbohydrates
Lipids, carbohydrates, and nucleic acids
Proteins, carbohydrates, and nucleic acids
Answer
Correct Answer:
Proteins, lipids, carbohydrates
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38. The following molecule is best described as a ______. ch3-ch2-ch2-ch2
Hydrocarbon
Carbohydrates
Proteins
None of the above
Answer
Correct Answer:
Hydrocarbon
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39. The correct name for [fe(nh3)5br]so4 is _____.
Pentaaminebromoiron(III) sulfate
Sulfate
Hydrogen
None of the above
Answer
Correct Answer:
Pentaaminebromoiron(III) sulfate
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40. The compound koh is ________.
Soluble, because all compounds containing K+ are soluble
Soluble, because all compounds containing OH- are soluble
Insoluble, because all compounds containing OH- are in soluble
Insoluble, because KOH is insoluble
Insoluble, because all compounds containing K+ are insolu
Answer
Correct Answer:
Soluble, because all compounds containing K+ are soluble
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41. The central atom in ________ does not violate the octet rule.
SF4
KrF2
CF4
XeF4
ICl4-
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42. The bohr shift on the oxygen-hemoglobin dissociation curve is produced by changes in _____.
The partial pressure of CO
Hemoglobin Concentration
Partial pressure of oxygen
Temperature
PH
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43. The bases (nucelotides) in each of the chains of dna are linked by _________ bonds.
Hydrogen bonds
Carbon dioxide bonds
Both a and b
None of the above
Answer
Correct Answer:
Hydrogen bonds
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44. The attractive forces that are important in the secondary structure of a protein are ________.
Hydrogen bond
Disulfide
Hydrophobic
Salt bridge
Answer
Correct Answer:
Hydrogen bond
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45. The 2+ in cu2+ tells us that this atom ________.
Has two more neutrons than electrons
Has two more protons than electrons
Has two more electrons than protons
None of the above
Answer
Correct Answer:
Has two more protons than electrons
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46. The ______ determines the chemical and physical properties of an atom.
Number of protons
Number of electrons
Number of neutrons
None of the above
Answer
Correct Answer:
Number of protons
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47. Solubility in water is ___ for smaller alcohols.
Low
High
Moderate
None of the above
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48. Pure substances that have properties entirely different from the atoms that make it up are _____.
Diatomic molecules
Compounds
Neurons
Photons
Answer
Correct Answer:
Compounds
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49. Pure chlorine is an example of a(n) _____.
Element
Compound
Mixture
Solution
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50. Protons, neutrons, and electrons are all ____.
Subatomic particles
Atomic particles
Both a and b
None of the above
Answer
Correct Answer:
Subatomic particles
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51. Most organic compounds contain carbon and _____.
Oxygen
Sulfur
Phosphate
Hydrogen
Nitrogen
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52. Most of the elements in the periodic table are __________.
Metals
Plastics
Chemicals
Liquids
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53. Matter is more likely to exist in the ________ state as the temperature is lowered.
Solid
Liquid
Gaseous
Elemental
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54. Materials of low mass are combined to form a substance of higher mass during ____.
Fission
Fusion.
Both A and B.
Neither A nor B
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55. J. j. thomson used ____________ to measure the ____________ of a cathode ray particle.
Magnetic and electric fields, mass-to-charge ratio
Mass-to-charge ratio, magnetic and electric fields
Both a and b
None of the abvoe
Answer
Correct Answer:
Magnetic and electric fields, mass-to-charge ratio
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56. Iron corrodes because _____ turns iron into ions through the process of _____.
Water, oxidation
Iron(III) oxide, oxidation
Iron(III) oxide, reduction
None of the above
Answer
Correct Answer:
Water, oxidation
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57. In the nitrite ion (no2-), __________.
Both bonds are single bonds
Both bonds are double bonds
One bond is a double bond and the other is a single bond
Both bonds are the same
There are 20 valence electrons
Answer
Correct Answer:
Both bonds are the same
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58. In the lewis symbol for a nitrogen atom, there are ________ paired and ________ unpaired electrons.
Two, three
One, three
Three, two
Zero, five
Two, two
Answer
Correct Answer:
Two, three
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59. In order to have a positive charge, an atom must have ________.
More electrons than protons
More protons than neutrons
More neutrons than protons
More protons than electrons
Answer
Correct Answer:
More protons than electrons
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60. In an ethane (c2h6) molecule, each carbon atom is bonded to ________ hydrogen atoms.
One
Two
Three
None
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61. In an equilibrium reaction with a keq of 1 108, the _____.
The reaction is nonspontaneous.
The reaction is endothermic.
Products are favored.
Reactants are favored.
Answer
Correct Answer:
Products are favored.
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62. In an ________ solution, red blood cells ________.
Isosmotic, swell and may burst
Hyposmatic, lose water and shrivel
Isomotic, have a normal shape
Isosmotic, lose water and shrivel
Hyperosmotic, have a normal shape
Answer
Correct Answer:
Isomotic, have a normal shape
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63. If the ph of a solution is decreased from 9 to 8, it means that the concentration of _____.
Concentration of H+ has increased tenfold (10X)
The concentration of OH- has decreased to one-tenth (1/10) what they were at pH 9
Both a and b
None of the above
Answer
Correct Answer:
Both a and b
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64. If a hydrogen atom gains an electron, then __________.
It becomes an isotope
Its mass number changes
Its atomic number changes
It acquires a negative charge
Answer
Correct Answer:
It acquires a negative charge
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65. Hydrogen bonding is most important in stabilizing the ________ structure of many proteins.
Quaternary
Primary
Tertiary
Secondary
All of the above
Answer
Correct Answer:
Secondary
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66. Hso4 is the conjugate _____ of h2so4 and the conjugate _____ of so42.
Acid / acid
Acid / base
Base / acid
Base / base
Answer
Correct Answer:
Base / acid
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67. Hemoglobin has a total of ________ protein chains in its quaternary structure.
One
Two
Three
Four
Five
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68. H2 is a molecule, but h2o is a _____.
Diatomic molecule
Compound
Neuron
Photon
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69. Galactose is a ________.
Monosaccharide
Disaccharide
Trisaccharide
Polysaccharide
Phosphosaccharide
Answer
Correct Answer:
Monosaccharide
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70. For a molecule with the formula ab3, the molecular shape is ________.
Linear, octahedral, or bent
Linear, bent, or trigonal planar
Linear, bent, or T-shaped
Tetrahedral
Trigonal planar, trigonal pyramidal, or T-shaped
Answer
Correct Answer:
Trigonal planar, trigonal pyramidal, or T-shaped
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71. Ethene is classified as an unsaturated hydrocarbon because it has _____.
Single-bonded carbon atoms
Double-bonded carbon atoms
Double-bonded carbon-hydrogen bonds
Single-bonded carbon-hydrogen bonds
Answer
Correct Answer:
Double-bonded carbon atoms
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72. Elements differ from each other in their ________.
Physical properties
Atomic mass
The type of subatomic particles they have
Both their physical properties and atomic mass
Answer
Correct Answer:
Both their physical properties and atomic mass
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73. Chemical reactions ____
Occur only in living organisms
Only occur outside living organisms
Create and destroy atoms
Produce new substances
Answer
Correct Answer:
Produce new substances
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74. Chain-branching __________ the contact surface area between molecules.
Increases
Decreases
Maintains
Answer
Correct Answer:
Decreases
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75. Carbohydrates and proteins are built up from their basic building blocks by the ________.
Removal of a nitrogen atom between each two units
Addition of a water molecule between each two units
Removal of a water molecule between each two units
Addition of a carbon atom between each two units
Answer
Correct Answer:
Removal of a water molecule between each two units
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76. Any substance that yields a hydrogen ion when placed in a water solution is called a(n) _____.
Acid
Base
Hydronium ion
Hydroxide ion
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77. Amino acids are linked together by peptide bonds in a ____
Protein
Amines
Alkalis
None of the above
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78. Amides are derivatives of ________ and ________.
Alcohols, carboxylic acids
Alkanes, amines
Amines, carboxylic acids
Carboxylic acids, alcohols
Amines, esters
Answer
Correct Answer:
Amines, carboxylic acids
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79. Adenosine triphosphate, or atp, is primarily used as _______ in living organisms.
A muscle relaxing hormone
A source of energy
A blood coagulant
A reproductive enzyme
Answer
Correct Answer:
A source of energy
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80. Acidity in grape juice is a result of ___ acid
Malic
Lactic acid
Both a and b
None of the above
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81. Acid rain results when humans put excess amounts of ________ into the atmosphere.
Nitrate
Sulfur
Oxygen
Carbon dioxide
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82. Achiral compounds are those which ________.
Have no "handedness"
Have different mirror images
Are a pair of enantiomers
Have D and L isomers
Answer
Correct Answer:
Have no "handedness"
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83. About _____ molecules in a glass of water are dissociated
1 in 500,000,000
1 in 1,000,000,000
1 in 1,000,000
1 in 5,000,000
1 in 2
Answer
Correct Answer:
1 in 500,000,000
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84. A substance that yields an anion plus a hydrogen ion is a(n) _____.
Salt
Acid
Base
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85. A substance that yields a cation plus the hydroxyl ion in water is a(n)_____.
Salt
Acid
Base
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86. A strong oxidizing agent _____.
Donate electrons
Gives electrons
Accepts electrons
Does not need electrons
Answer
Correct Answer:
Accepts electrons
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87. A strong acid like hcl _____.
Reacts with strong bases to create a buffered solution
Is a strong buffer at low pH
Dissociates completely in an aqueous solution
Increases the pH when added to an aqueous solution
Answer
Correct Answer:
Dissociates completely in an aqueous solution
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88. A strong acid is one that _____ and an example is _____.
Ionizes more completely; HC1.
Metabolic alkalosis may be caused by.
All of the above.
None of the above.
Answer
Correct Answer:
Ionizes more completely; HC1.
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89. A solution with [ oh-] of 5 10-3 has a ph of ________.
2.3
11.7
7.0
5.0
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90. A redox reaction has occurred ________.
When a substance reacts with elemental oxygen
When an alkali metal reacts with an alkaline earth metal
When one substance transfers electrons or protons to another
When one substance forms a solid
When all of the above occur
Answer
Correct Answer:
When a substance reacts with elemental oxygen
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91. A catalytic effect or acceleration of a reaction can occur in the ________ of an enzyme.
DNA
RNA
Substrates
Active site
Answer
Correct Answer:
Active site
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92. A carbon-hydrogen bond in ethane (ch3ch3) is best described a ________.
Multiple bond
Ionic
Resonance stabilized
Highly polar
Essentially nonpolar
Answer
Correct Answer:
Essentially nonpolar
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93. A ball-and-stick model of a molecule provides much the same information as a _____.
Space-filling model
Chemical-filling model
Molecule-filling model
None of the above
Answer
Correct Answer:
Space-filling model
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94. ___c2h6(g)+____o2(g)____co2(g)+____h2o(g)
2,7,4,6
2,2,4,7
2,7,3,6
7,1,4,6
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95. There are ________ σ bonds and ________ π bonds in h3c-ch2-ch=ch-ch2-cch.
12, 2
16, 3
14, 2
10, 3
13, 2
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96. Scientists prepared the ____ of solution for their next experiment.
Vial
Vile
Viol
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97. When using the ideal gas equation, if the numerical value of r is 0.08206, then ________.
The volume of the gas is expressed in milliliters.
The amount of the gas is expressed in grams.
The temperature is expressed on the Celsius scale.
The pressure of the gas is expressed in atmospheres.
Answer
Correct Answer:
The pressure of the gas is expressed in atmospheres.
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98. When electrons are shared, the type of bonding is called _____.
Atoms share their electrons for getting more stable.
Atoms share their electrons for getting more disrupted.
Atoms share their electrons for getting more mass.
None of the above.
Answer
Correct Answer:
Atoms share their electrons for getting more stable.
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99. Complete the equation: monosaccharide + monosaccharide ? ______ + water
Polypeptide
Polysaccharide
Nucleic acid
Disaccharide
Answer
Correct Answer:
Disaccharide
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100. A metal such with a face-centered cubic lattice will have ________________ atom(s) per unit cell.
2
3
4
10
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101. All of the ________ have a valence shell electron configuration ns1.
Halogens
Alkaline earth metals
Noble gases
Alkali metals
Chalcogens
Answer
Correct Answer:
Alkali metals
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102. The molecular geometry of the left-most carbon atom in the molecule below is ________.
Trigonal planar
Trigonal bipyramidal
Tetrahedral
Octahedral
Answer
Correct Answer:
Tetrahedral
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103. Urban sprawl is a result of people moving away from ________.
City centers
Rural communities
Current residences
Suburbs
Natural resources
Answer
Correct Answer:
City centers
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104. Genes that are not often transcribed generally have _____ sequences that bind to _____ proteins.
Inhibitor; mediator
Interrupter; regulatory
Obstruction; restraint
Silencer; repressor
Negative control; arrestor
Answer
Correct Answer:
Silencer; repressor
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105. Salts are always ________.
Hydrogen bonded
Single covalent compounds
Double covalent compounds
Ionic compounds
Answer
Correct Answer:
Ionic compounds
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106. In the reaction energy diagrams shown, reaction a is ________, and it occurs ________ reaction b.
Exergonic; faster than
Exergonic; at the same rate as
Exergonic; slower than
Endergonic; slower than
Answer
Correct Answer:
Exergonic; slower than
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107. The energy of 3600 cal is equal to ________ kj.
0.86
15
15 000
3.6
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108. An aqueous solution of glucose behaves as an aldehyde because ________.
It is hydrolyzed by water to the free aldehyde
It is a ketone, but is in equilibrium with the aldehyde form
Glucose is actually a cyclic aldehyde
Its cyclic hemiacetal, the predominant form, is in equilibrium with the free aldehyde form
Answer
Correct Answer:
Its cyclic hemiacetal, the predominant form, is in equilibrium with the free aldehyde form
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109. A molecule with the formula ax2 uses _________ to form its bonds.
Sp hybrid orbitals
Sp2 hybrid orbitals
Sp3 hybrid orbitals
Sp3d hybrid orbitals;
Answer
Correct Answer:
Sp hybrid orbitals
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110. [ar]4s23d104p3 is the electron configuration of a(n) __________ atom.
As
V
P
Sb
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111. Sodium is much more apt to exist as a cation than is chlorine. this is because ________.
Chlorine is a gas and sodium is a solid
Chlorine is bigger than sodium
Chlorine has a greater electronegativity than sodium does
Chlorine is more metallic than sodium
Answer
Correct Answer:
Chlorine has a greater electronegativity than sodium does
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112. The term anaerobic means ______.
Without O2
Without CO2
Without N2
Without NO2
Answer
Correct Answer:
Without O2
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113. The positions of the constellations appear to change throughout the year because ____.
Earth revolves around the Sun
Earth revolves around the Sun
The constellations revolve around Earth
The Sun revolves around Earth
Answer
Correct Answer:
Earth revolves around the Sun
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114. The main energy products currently being obtained from the ocean floor are oil and _____.
Natural gas
Coal
Salt
Manganese nodules
Answer
Correct Answer:
Natural gas
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115. The electron cloud model describes the _____ of electrons in an atom.
Charge
Precise locations
Likely locations
Number
Answer
Correct Answer:
Likely locations
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116. The electric field induces the flow of electrons, known as _____.
Voltage
Electric current
Resistance
Interference
Answer
Correct Answer:
Electric current
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117. The difference between mechanical and chemical weathering is ____.
The length of time each takes to break
That only chemical weathering involves water
The way they affect the makeup of a rock
All of the above
Answer
Correct Answer:
The way they affect the makeup of a rock
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118. The depolarization phase of an action potential requires _____.
Opening of Na+ channels in the membrane
Membrane potential would become less negative
Slow decrease of resting potential
Degradation on the postsynaptic membrane
Answer
Correct Answer:
Opening of Na+ channels in the membrane
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119. The density of ammonia gas in a 4.32 l container at 837 torr and 45°C is ________ g/l.
3.86
0.719
0.432
0.194
4.22 × 10-2
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120. The average kinetic energy of water molecules is greatest in _____.
Steam at 100 degrees C
Steam at 200 degrees C
Steam at 150 degrees C
Steam at 120 degrees C
Answer
Correct Answer:
Steam at 100 degrees C
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121. The ________ orbital is degenerate with 5py in a many-electron atom.
5px
4px
3px
None of these
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122. Systemic gas exchange is the unloading of ____________ and loading of carbon dioxide.
Oxygen
Nitrogen
Clorine
Carban
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123. In ionic interactions, __________.
Valence electrons in the outermost electron shell
The transfer of valence electrons results in a completed valence shell for each ion
One of the atoms sharing electrons is much more electronegative
Answer
Correct Answer:
The transfer of valence electrons results in a completed valence shell for each ion
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124. In the electron transport chain, electrons are passed from redox center to redox center ____.
With the assistance of a carrier protein
In an ATP dependent fashion
Spontaneously due to the redox potential gradient
As a result of the addition of free energy
As a result of the proton gradient
Answer
Correct Answer:
Spontaneously due to the redox potential gradient
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125. In an equilibrium reaction with a keq of 1 x 108, the _____.
The reaction is nonspontaneous
The reaction is endothermic
Products are favored
Reactants are favored
Answer
Correct Answer:
Products are favored
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126. For resonance forms of a molecule or ion, __________.
All the resonance structures are observed in various proportions
The same atoms need not be bonded to each other in all resonance forms
There cannot be more than two resonance structures for a given species
One always corresponds to the observed structure
The observed structure is an average of the resonance forms
Answer
Correct Answer:
The observed structure is an average of the resonance forms
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127. Foliated rocks are distinguished by ____.
Layers
Lack of layers
Large mineral grains
Air holes
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128. Examine the lewis symbol given below. based on this representation, ______.
There are three lone pairs and two bonding pairs of electrons
Nitrogen forms three single covalent bonds
Nitrogen atoms form a strong bond and a stable molecule
Only one nitrogen atom attains an octet of electrons
Answer
Correct Answer:
Nitrogen atoms form a strong bond and a stable molecule
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129. When a substance freezes, it changes from the liquid phase to the solid phase because of its _____.
Molecular bonding
Intermolecular bonding
Compactness
Ability to fit the shape of its container
Answer
Correct Answer:
Intermolecular bonding
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130. The cycle of increasing trade restrictions among nations is known as a _________.t
Ariff war
Quota war
Trade war
Customs war
Answer
Correct Answer:
Trade war
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131. President reagan supported _______ economics tax proposals.
Demand-side
Supply-side
Keynesian
Federal
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132. Employers hope that after employee reviews, workers will ______
.improve their production
Improve their pronunciation
Improve their prestidigitation
Improve their pension
Answer
Correct Answer:
.improve their production
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133. O2(g) effuses at a rate that is ______ times that of br2(g) under the same conditions.
2.236
1.2
3.421
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134. From the atomic mass, one can deduce the number of ________ in each atom of an element.
Protons plus neutrons
Neutrons
Protons
Electrons
Protons plus electrons
Answer
Correct Answer:
Protons plus neutrons
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135. Many of the macroscopic properties of a compound depend on ________.
The number of nucleons present in the sample.
How the atoms of the molecules are held together.
The mass of the constituent atoms.
The size of the sample.
How the atoms absorb light and the shape of the orbitals
Answer
Correct Answer:
How the atoms of the molecules are held together.
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136. The gold foil experiment performed in rutherford's lab ________.
Proved the law of multiple proportions
Confirmed the plum-pudding model of the atom
Was the basis for Thompson's model of the atom
Utilized the deflection of beta particles by gold foil
Led to the discovery of the atomic nucleus
Answer
Correct Answer:
Led to the discovery of the atomic nucleus
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137. There are ________ atoms of hydrogen in 300 molecules of ch3co2h.
300
500
600
1200
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138. The presence of ________ chemical groups makes carbohydrates ________.
Hydroxyl : polar
Fission; hydroxyl
Polar; fusion
Fission; fusion
Answer
Correct Answer:
Hydroxyl : polar
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139. The ductility of copper allows it to be pulled into a _________.
Wire
Gas
Solid
Liquids.
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140. The combining of the nuclei of atoms is known as nuclear _____.
Fission
Fusion
Bombardment
Fallout
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141. Of the following, Delta H°f is not zero for ________.
F2 (s)
O2 (g)
C (graphite)
Fuel value
Enthalpy
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142. Cubic closest packing is another name for _____________.
Simple cubic packing
Body-centered cubic packing
Face-centered cubic packing
Hexagonal closest packing
More than one of these
Answer
Correct Answer:
Face-centered cubic packing
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143. Addition of _____________ to pure water causes the greatest increase in conductivity.
Weak bases
Acetic acid
Ionic compounds
Organic molecules
Answer
Correct Answer:
Ionic compounds
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144. When nad+ is ________ it becomes nadh. when nadh is ________ it becomes nad+.
Oxidized; oxidized
Oxidized; reduced
Reduced; oxidized
Reduced; reduced
Answer
Correct Answer:
Reduced; oxidized
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145. Valence bond theory does not address the issue of ________.
Excited states of molecules
Simple cubic packing
Body-centered cubic packing
Face-centered cubic packing
Answer
Correct Answer:
Excited states of molecules
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146. Using the table of average bond energies below, the Δh for the reaction is ________ kj.
C≡O (g) + 2H2 (g) → H3CO2H (g)
Bond: C-O C=O C≡O C-H H-H O-H
KJ/Mol: 358 799 1072 413 436 463
+ 160 kJ
-63 kJ
- 160 kJ
-217 kJ
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147. The __________ of the organic molecule controls the chemistry of life.
NOT electrical charge
Electrical charge
Answer
Correct Answer:
NOT electrical charge
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148. Nitrogen has 7 electrons and can form a maximum of ________ bonds with other elements.
2
3
4
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149. In comparing gases with liquids, gases have ________ compressibility and ________ density.
Greater; smaller
Smaller; greater
Greater; greater
Smaller; smaller
None of the above
Answer
Correct Answer:
Greater; smaller
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150. In a px orbital, the subscript x denotes the __________ of the electron.
Axis along which the orbital is aligned
Spin of the electron
Size of the orbital
Energy of the electron
Answer
Correct Answer:
Axis along which the orbital is aligned
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151. If you precisely measure the position of a particle, you __________.
Destroy its wave nature.
Cause it to diffract.
Destroy information about its speed.
Cause the particle to be annihilated
Answer
Correct Answer:
Destroy information about its speed.
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152. Complete the relationship. __________ nm = __________ cm.
1 × 10^9; 100
1 × 10^9; 10
1 × 10^6; 100
Answer
Correct Answer:
1 × 10^9; 100
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153. Chains of enzyme reactions that break down or build molecules are called ____ pathways.
ATP
Energy
Metabolic
Sensory
Answer
Correct Answer:
Metabolic
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154. Carbon uses ______ hybrid orbitals in clcn.
Sp
Sp2
Sp3
Sp3d
Sp3d2
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155. A good buffer ________.
Diverts attention from the problem
Establishes common ground with the reader
Indicates that the message contains good news
Is a statement unrelated to the point of the message
Promises a positive answer
Answer
Correct Answer:
Establishes common ground with the reader
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156. A ________ covalent bond between the same two atoms is the longest.
Single
Double
Triple
They are all the same length
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157. _______ tend/s to speed up the absorption of alcohol.
Fruit Juice
Water
Carbonated Beverages
Answer
Correct Answer:
Carbonated Beverages
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158. The relationship between molecular velocities and temperature is a _____ relationship.
Indirect
Direct
Inversely proportional
Secondary
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159. The chemical reaction illustrated ________.
Links two polymers to form a monomer
Joins two fatty acids together
Is a hydrolysis reaction
Results in a peptide bond
Answer
Correct Answer:
Results in a peptide bond
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160. Water is an important molecule because it __________.
Can form hydrogen bonds
Have different substrate binding affinities
Have different product binding affinities
At any one time are present in different conformations
Answer
Correct Answer:
Can form hydrogen bonds
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161. The three catalytic sites of atp synthase ___________.
Have different substrate binding affinities
Have different product binding affinities
At any one time are present in different conformations
Pass sequentially through their three different conformations
All of the above
Answer
Correct Answer:
All of the above
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162. The molecular formula of a compound is always ________ the empirical formula.
An integral multiple of
Ore complex than
Different from
Simpler than
The same as
Answer
Correct Answer:
An integral multiple of
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163. Stable molecules usually contain atoms that have filled __________ orbitals.
Valence
Always take place at a rapid rate
Are always exothermic
Always release free energy
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164. The most important component when reporting a numerical scientific result is the ______.
Unit
± symbol
Number of digits
Decimal point
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165. Typically if oxygen has a formal negative charge, it is participating in ____ covalent bond(s).
1
2
3
4
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166. Antimicrobial drugs are selectively toxic. this means _____.
The drugs are more toxic to the pathogens than to the patient
The drug will kill or inhibit the growth of all of the sensitive bacterial cells
Prevents the formation of peptide bonds
Smallest amount of drug that will inhibit growth and reproduction
Answer
Correct Answer:
The drugs are more toxic to the pathogens than to the patient
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167. Carbon monoxide, a substance found in tobacco smoke, is also found in __________.
Household cleaning products
Vehicle exhaust
Nail polish remover
Paint thinner
Answer
Correct Answer:
Vehicle exhaust
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168. Distillation is used to separate _____.
Colloids
Suspensions
Solutions
Heterogeneous mixtures
Answer
Correct Answer:
Solutions
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169. Different ions of a given element will have differing numbers of __________.
Protons
Neutrons
Electrons
Molecular formulas
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170. Crystals can have _____ bonds between their atoms. ionic covalent metallic all types of
Metallic
Covalent
Ionic
All of the above
Answer
Correct Answer:
All of the above
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171. Chemoautotrophs use ___ as an energy source and ___ as a carbon source.
Inorganic compounds: CO2
Thermoacidophile
Ribosomes
Cell wall structure
Answer
Correct Answer:
Inorganic compounds: CO2
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172. Chemistry is the science that tries to understand ______.
Living organisms
The interactions between matter and energy
How atoms and molecules behave
The relationship between the mind and behavior
Answer
Correct Answer:
How atoms and molecules behave
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173. Chemical weathering ____.
Is caused by freezing and thawing
Breaks apart rocks by physical processes
Occurs when chemical reactions dissolve or change the minerals in rocks
None of above
Answer
Correct Answer:
Occurs when chemical reactions dissolve or change the minerals in rocks
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174. Both mechanical and electromagnetic waves _____.
Have compressions and rarefactions
Oscillate in the same direction as the wave motion
Transmit energy
Require a medium for transfer
Answer
Correct Answer:
Transmit energy
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175. Bohr stated that electrons in an atom can undergo _________.
Interference
The wave function
The atomic nucleus3
All of the above
Answer
Correct Answer:
Interference
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176. Atoms that satisfy the octet rule are said to be __________.
Inert
Matter
Isotopes
Acidic
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177. Atoms that are sp2 hybridized form ____ pi bond(s).
1
2
3
4
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178. At equilibrium, ________.
All chemical reactions have ceased
The rates of the forward and reverse reactions are equal
The rate constants of the forward and reverse reactions are equal
The value of the equilibrium constant is 1
The limiting reagent has been consumed
Answer
Correct Answer:
The rates of the forward and reverse reactions are equal
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179. As shown below, hydrogen bonds occur when _____.
Chemicals are fundamental to the structure and function of all living things.
Partial opposite charges on molecules come close enough to attract each other
An attraction between atoms that have opposite charges
The opposite ends of the molecule have opposite charges
Answer
Correct Answer:
Partial opposite charges on molecules come close enough to attract each other
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180. Any sugar that has a free aldehyde group is called a(n) _____.
Reducing sugar
Non-reducing sugar
Ketose
Aldohexose
Alditol
Answer
Correct Answer:
Reducing sugar
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181. An amorphous solid is the result of ______.
Atoms or molecules that are well-ordered and geometrically arranged
Atoms or molecules that are separated by large distances and do not interact significantly with one another
Atoms or molecules that are closely spaced but are free to move around and past each other
Atoms or molecules that do not have long range, well-ordered, geometric arrangement
Answer
Correct Answer:
Atoms or molecules that do not have long range, well-ordered, geometric arrangement
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182. All organic compounds contain ______, hydrogen, and usually oxygen.
Catabolic
Anabolic
Release
Carbon
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183. All amino acids (such as the four represented in the figure) contain ______.
An amine group and a fatty acid
A nitrogen-containing base and a pentose sugar
Phosphorus and nitrogen
An amine group and a carboxylic acid group
Answer
Correct Answer:
An amine group and a fatty acid
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184. Alchemists were able to _____.
Study the properties of common elements
Study the properties of compounds
Develop laboratory techniques used by later scientists
All of the above
Answer
Correct Answer:
All of the above
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185. Activation energy is ____. (1 point)the heat released in a reaction
The heat released in a reaction
The energy barrier between reactants and products
The energy given off when reactants collide
Generally very high for a reaction that takes place rapidly
Answer
Correct Answer:
The energy barrier between reactants and products
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186. A ph of 2 indicates a(n) _____.
Strong acid
Strong base
Carbonyls
Aminos
Answer
Correct Answer:
Strong acid
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187. A molecule with a single covalent bond is _____.
CO2
Cl2
CO
N2
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188. A biome is a large group of plants and animals living together in a specific _____.
Habitat
Population
Community
Climate
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189. A ________ will pass through a filter but not a semipermeable membrane.
Solid
Precipitate
Solution
Suspension
Colloid
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190. 3.00 moles of no2 have a mass of ________.
45.0 g
138 g
30.0 g
90.0 g
46.0 g
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191. There are ________ atoms of carbon in 300 molecules of ch3co2h.
300
600
150
3.6 x 10^36
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192. The present value of an expected future payment ________ as the interest rate increases.
Falls
Rises
Is constant
Is unaffected
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193. Carbonic acid dissolved in water is a ____________ (chemical/biological) weathering agent.
Chemical
Biological
Micro chemical
Micro biological
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194. The hybridization of the central atom in the xef4 molecule is ________.
Sp
Sp2
Sp3
Sp3 d3
Sp3 d2
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195. There are ________ σ and ________ π bond(s) in the h2c=ch2 molecule.
3 and 4
5 and 1
2 and 3
3 and 2
4 and 3
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196. Complete the relationship. 3.5 milliliters = __________ centiliters.
0.34 centiliter
0.35 centiliter
0.40 centiliter
None of these
Answer
Correct Answer:
0.35 centiliter
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197. To convert from one resonance structure to another, __________.
Only atoms can be moved
Electrons and atoms can be moved
Neither atoms or electrons can be moved
Electrons must be added
Only electrons can be moved
Answer
Correct Answer:
Only electrons can be moved
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198. _______ is formed whenever long molecules of starch break down.
Fructose
Lactose
Maltose
Glucose
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199. Valence bond theory predicts that tin will use _____ hybrid orbitals in sncl3–.
Sp
Sp2
Sp3
Sp3d
Sp3d2
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200. Ice floats in water because it _____
Is less dense than water.
Contains more oxygen than water.
Has a higher pH than water.
Has more surface tension than water
Answer
Correct Answer:
Is less dense than water.
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201. An inhibitory postsynaptic potential (ipsp) is associated with ________.
Lowering the threshold for an action potential to occur
Hyperpolarization
A change in sodium ion permeability
Opening of voltage-regulated channels
Answer
Correct Answer:
Hyperpolarization
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202. Acetylcholine binds to its receptor in the sarcolemma and triggers __________.
The opening of calcium-release channels
The opening of ligand-gated cation channels
The opening of ligand-gated anion channels
The opening of voltage-gated calcium channels
Answer
Correct Answer:
The opening of ligand-gated cation channels
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203. The free energy of a gas depends on __________.
Evaporating (turning into gas) and condensing (turning into liquid).
Temperature, the IMF, and the concentration in the gas phase.
The condensation rate will initially be zero since there are no molecules in the gas phase.
Partial pressure of the gas The free energy of a gas is a function of the pressure [G(P) = G° + RTln(P/P°)].
Answer
Correct Answer:
Partial pressure of the gas The free energy of a gas is a function of the pressure [G(P) = G° + RTln(P/P°)].
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204. Small particles of organic material are called _______
Discharge
Peat
Detritus
Brackish
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205. One mole of ________ contains the smallest number of atoms.
Na3PO4
C10H8
NaCl
Al2(SO4)3
S8
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206. Of the following metals, ________ exhibits multiple oxidation states.
Mg
Ni
Cs
Al
Rb
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207. Nitrifying bacteria convert _____ to _____
Nitrogen gas ... ammonium
Nitrogen gas ... nitrates
Ammonium ... nitrites
Nitrates ... nitrogen gas
Ammonium ... nitrogen gas
Answer
Correct Answer:
Ammonium ... nitrites
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208. Nitrogen and carbon are important to life because _____.
They're needed to breathe
They are needed for cellular growth
They produce water
They have strong bonds
Answer
Correct Answer:
They are needed for cellular growth
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209. Elements in group ________ have a np6 electron configuration in the outer shell.
4A.
6A.
7A.
8A.
5A'
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210. Brittle deformation is generally seen in _____.
Rocks with strong internal molecular bonds.
Gypsum and shale.
Rocks far below earths surface.
Limestone and schist
Answer
Correct Answer:
Rocks far below earths surface.
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211. The iupac name of this compound is ________.
5-methyl-1-hexene
2-methyl-1-hexene
2-methyl-5-hexene
5-methyl-2-hexene
1-hexene
Answer
Correct Answer:
5-methyl-1-hexene
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212. The energy of a photon that has a wavelength of 12.3 nm is __________ j.
1.99 × 10-25 J
1.51 × 10-17 J
4.42 × 10-23 J
1.6 x 10-17 J
Answer
Correct Answer:
1.6 x 10-17 J
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213. Plastics are ________.
Naturally occurring macromolecules
Unstable and break down easily
Moldable, petroleum-based hydrocarbons
Assembled by enzymes in cells
Synthetic proteins
Answer
Correct Answer:
Moldable, petroleum-based hydrocarbons
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214. When dissolved in water, acids release _____ and bases release _____.
Hydrogen ions; hydroxyl ions
Hydroxyl ions; hydrogen ions
Answer
Correct Answer:
Hydrogen ions; hydroxyl ions
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215. The mass percent of hydrogen in hydrogen peroxide, h2o2, is _____.
11%.
3.0%.
5.9%.
50%
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216. The formula weight of a substance is ________.
Identical to the molar mass
The same as the percent by mass weight
Determined by combustion analysis
The sum of the atomic weights of each atom in its chemical formula
The weight of a sample of the substance
Answer
Correct Answer:
The sum of the atomic weights of each atom in its chemical formula
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217. Of the following, a 0.1 m aqueous solution of ________ will have the highest freezing point.
Al(NO₃)₃
NaCl
Na₂SO₄
K₂CrO₄
Sucrose
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218. Cl2 (g) + h2o (l) → ________
HCl (aq) + HOCl (aq)
2Cl- (aq) + H2O (l)
2HCl (aq) + O2 (g)
2HCl (aq) + O2- (g)
Cl2 (aq) + H2O (l
Answer
Correct Answer:
HCl (aq) + HOCl (aq)
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219. Bond enthalpy is ________.
Always positive
Always negative
Sometimes positive, sometimes negative
Always zero
Unpredictable
Answer
Correct Answer:
Always positive
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220. 96 k = _____
-286.87 F
-177.15 C
Both
None of these
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221. Spontaneous reactions _____.
Always take place at a rapid rate
Are always exothermic
Always release free energy
Always result in increased disorder of the system
Answer
Correct Answer:
Always result in increased disorder of the system
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222. Chemical weathering is most active in a _____.
Warm, dry climate
Warm, humid climate
Cold, dry climate
None
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223. The water at the top of a waterfall has _____ energy.
Potential,
Kinetic,
Heat,
Metabolic
Answer
Correct Answer:
Potential,
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224. Temperature is a measure of _____
Work
Molecular movement
Chemical energy
Potential energy
Answer
Correct Answer:
Molecular movement
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225. Liquids that evaporate quickly are known as _____ liquids.
Viscous
Volatile
Evaporative
Transient
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226. In the following list, only ________ is not an example of a chemical reaction.
The condensation of water vapor
The rusting of iron
The formation of polyethylene form ethylene
A burning candle
Dissolution of a penny in nitric acid
Answer
Correct Answer:
The condensation of water vapor
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227. In a reaction, a gas being produced is ______.
A physical change
A chemical change
A phase change
No change
Answer
Correct Answer:
A phase change
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228. Gases, fluids, and other solids in contact with a moving object will produce ____ due to friction.
Heat flow
Current
Electrical energy
Radiation
Answer
Correct Answer:
Heat flow
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229. A static charge is developed in a substance _____.
As the substance acquires loose electrons due to friction
As the substance acquires loose protons due to friction
As the substance lose electrons due friction
As the substance loses protons due to friction
Answer
Correct Answer:
As the substance acquires loose electrons due to friction
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230. The list that correctly indicates the order of metallic character is ________.
B > N > C
F > Cl > S
Si > P > S
P > S > Se
Na > K > Rb
Answer
Correct Answer:
Si > P > S
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231. The salt water ______________ when poured into the glass containing cold tap water.
More dense; more dense
Cold, high
Remained at the top
Collected at the bottom
Answer
Correct Answer:
Collected at the bottom
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232. The hot water ______________ when poured into the glass containing cold tap water.
Remained at the top
More dense; more dense
Remains fairly constant
Collected at the bottom
Answer
Correct Answer:
Remained at the top
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233. With solutions of strong acids and strong bases, the word strong refers to _____.
Degree of ionization
Normality
Molarity
Solubility
Answer
Correct Answer:
Degree of ionization
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234. The organic products of a saponification reaction include soap molecules and _____.
Glycerol
Cell membrane
Water
Hydrophobic tails
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235. The following reaction is an example of a ________ reaction.
Single replacement
Decomposition
Double replacement
Combustion
Displacement
Answer
Correct Answer:
Combustion
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236. The electrons are unequally shared in _______, and transferred in __________.
CH4, Na+Cl-
O2, CH4
Na+Cl-, H2O
H2O, N2
Answer
Correct Answer:
CH4, Na+Cl-
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237. The addition of sodium chloride to pure water, causes the conductivity to _________.
Concentrated
Humid air
Water and sugar
Increase
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238. In a practical machine, the power output is _______ the power input
Smaller than.
Multiplied by.
Equal to.
Larger than
Answer
Correct Answer:
Smaller than.
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239. Distillation is used to separate _____. heterogeneous mixtures suspensions colloids solutions
Heterogeneous mixtures
Suspensions
Colloids
Solutions
Answer
Correct Answer:
Heterogeneous mixtures
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240. Complete the following sentence: the cathode in a voltaic cell is the electrode _____________.
To which anions from the salt bridge migrate
In which oxidation takes place
To which cations from the salt bridge migrate
In which electrons become available
Answer
Correct Answer:
To which cations from the salt bridge migrate
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241. An antibonding π orbital contains a maximum of ________ electrons.
1
2
4
6
8
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242. A straight chain hydrocarbon with the formula c6h12 _____.
Single Displacement
Has a double C-C bond
Supply energy to cells
It is polar
Answer
Correct Answer:
Has a double C-C bond
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243. A bureaucracy is organized like a pyramid with the head of the bureaucracy _____.
Between each level
In the middle
At the top
On the bottom None
Answer
Correct Answer:
At the top
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244. To complete its outermost shell, oxygen will likely __________.
Donate electrons
Accept electrons
Covalent
Electronegativity
Answer
Correct Answer:
Accept electrons
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245. A 30.5 gram sample of glucose (c6h12o6) contains ________ atoms of carbon.
1.22 X 1024
1.02 X 1023
6.12 X 1023
6.02 X 1023
Answer
Correct Answer:
6.12 X 1023
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246. A ________ δh corresponds to an ________ process.
Negative, endothermic.
Negative, exothermic.
Positive, exothermic.
Zero, exothermic
Answer
Correct Answer:
Negative, exothermic.
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247. A pressure of 0.500 atm is the same as a pressure of ________ of mm hg.
29.9
33.0
760.
193
380
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248. When the nonelectrolyte glucose is dissolved in water, the solution contains ________.
All glucose molecules.
All glucose ions.
Nothing
Answer
Correct Answer:
All glucose molecules.
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249. When the electron cloud of a molecule is easily distorted, the molecule has a high _____________.
Polarity
Polarizability
Dipole moment
Van der Waals radius
Compressibility
Answer
Correct Answer:
Dipole moment
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250. When h2so4 is neutralized by naoh in aqueous solution, the net ionic equation is ________.
SO42- (aq) + 2Na+ (aq) Na2SO4 (aq)
SO42- (aq) + 2Na+ (aq) Na2SO4 (s)
H+ (aq) + OH- (aq) H2O (l)
H2SO4 (aq) + 2OH- (aq) 2H2O (l) + SO42- (aq)
2H+ (aq) + 2NaOH (aq) 2H2O (l) + 2Na+ (aq
Answer
Correct Answer:
H+ (aq) + OH- (aq) H2O (l)
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251. The symbol for the hydroxide ion is _____
H+
H3O-
H(OH)
OH-
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252. The rate law of a reaction is rate = k[d][x]. the units of the rate constant are ________.
Mol L⁻¹ s⁻¹
L mol⁻¹ s⁻¹
Mol2 L⁻² s⁻¹
Mol L⁻¹ s⁻²
L² mol⁻² s⁻¹
Answer
Correct Answer:
L mol⁻¹ s⁻¹
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253. The overall enthalpy change for a reaction _____.
Can only be determined by making calorimetric measurements.
Depends only on the amount of matter that undergoes the change and on the initial state of the reactants and the final state of the products.
Can only be determined if it is carried out in one step.
Depends directly on the path by which the reaction is carried out
Answer
Correct Answer:
Depends only on the amount of matter that undergoes the change and on the initial state of the reactants and the final state of the products.
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254. The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is __________.
Zn(s) + 2H+ (aq) -- Zn2+(aq) + H2(g)
Zn(s) + 2HBr-(aq) -- ZnBr2(aq) +2H+(aq)
2Zn(s) + H+(aq) -- 2Zn2+(aq) + H2(aq)
Zn(s) + 2HBr(aq) -- ZnBr2(s) + 2H+(aq)
Zn(s) + 2Br-(aq) -- ZnBr2(aq
Answer
Correct Answer:
Zn(s) + 2HBr(aq) -- ZnBr2(s) + 2H+(aq)
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255. The molecular weight of a gas is ________ g/mol if 3.5 g of the gas occupies 2.1 l at stp.
41
5.5 x 103
37
4.6 x 102
2.7 x 10-2
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256. The metals in groups 1a, 2a, and 3a ____.
All have ions with a 1+ charge
Gain electrons when they form ions
All form ions with a negative charge
Lose electrons when they form ions
Answer
Correct Answer:
Lose electrons when they form ions
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257. The ion no- has ________ valence electrons.
15
14
16
10
12
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258. The intermolecular forces responsible for ch3ch2oh being at liquid at 20°c are ________ bonds.
Phases
Germanium
Hydrogen
NO2
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259. The half-life of the reaction when the initial [ch3nc] is 0.030 m is ________ s.
1.06 × 104.
5.29 × 103.
3.53 × 105.
7.33 × 103
Answer
Correct Answer:
7.33 × 103
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260. The following is a chemical reaction for _______ with ozone.
Chlorofluorocarbons
Halons
UV radiation
None of the above
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261. The energy levels of an atom are occupied by ____
Electrons
Protons
Neutrons
Ions
Answer
Correct Answer:
Electrons
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262. The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is __________.
Hno3(aq) + sr(oh)2(aq) → sr(no3)2 (aq) + h2 (g)
Hno3(aq) + sr(oh)2 (aq) → h2o (l) + sr(no3)2 (aq)
Hno3 (aq) + sroh (aq) → h2o (l) + srno3(aq)
2hno3 (aq) + sr(oh)2 (aq) → 2h2o (l) + sr(no3)2(aq
Answer
Correct Answer:
2hno3 (aq) + sr(oh)2 (aq) → 2h2o (l) + sr(no3)2(aq
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263. The activation energy of an endothermic reaction _____.
Must be greater than the required ΔH
Must be less than the required ΔH
Must be equal to the required ΔH
Is not needed for the required ΔH
Answer
Correct Answer:
Must be greater than the required ΔH
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264. Pressure has a large effect only on the solubility of ________ in liquids.
Gas.
Solid.
Liquids.
All of the above
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265. Oxides of the active metals combine with acid to form ________.
Hydrogen gas
Metal hydrides
Water and a salt
Oxygen gas
Answer
Correct Answer:
Water and a salt
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266. Of the ions below, only __________ has a noble gas electron configuration.
Li 2+.
Be2+
B2+
C2-
N2
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267. Of the following, δh°f is not zero for ________.
F2 (s)
O2 (g)
C (graphite)
Fuel value.
Enthalpy
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268. Of the following gases, __________ will have the greatest rate of effusion at a given temperature.
NH3.
CH4.
Ar.
HBr.
HCl
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269. Na+ is a(n) _____, and cl- is a(n) _____ .
cation; anion
anion; cation
Na(+) - cation
Cl(-) - anion
Answer
Correct Answer:
Na(+) - cation
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270. In the reaction shown, ________ is the oxidizing agent because it ________.
Ni(s) + CuCl2(aq)
Cu(s) + NiCl2(aq)
CuCl2; gets reduced
Answer
Correct Answer:
CuCl2; gets reduced
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271. In the periodic table we use today, the ordering of the elements is based on _____.
Atomic number
Phosphorous, P
Group number
Dmitri Mendeleev
Answer
Correct Answer:
Atomic number
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272. In an open system, the vapor pressure is equal to the _____.
Higher
Lower
Equal
Outside air pressure
Answer
Correct Answer:
Outside air pressure
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273. Hydrogen chloride gas, hcl, is an example of an arrhenius acid because _________.
It feels slippery.
When dissolved in water, it increases the concentration of H+ ions.
It has a bitter taste.
When dissolved in water, it increases the concentration of OH− ions
Answer
Correct Answer:
When dissolved in water, it increases the concentration of H+ ions.
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274. Heat applied to reactants causes a faster chemical reaction. heat is considered _____.
Chemical equilibrium
The law of mass action
Activation energy
Answer
Correct Answer:
Activation energy
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275. E) ____ is/represents a positively charged species.
Base Peak,
Molecular Ion,
Radical Cation,
Parent Ion
All of these
Answer
Correct Answer:
All of these
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276. Based on the octet rule, aluminum most likely forms an ________ ion.
Al3+
Al4+
Al4-
Al+
Al
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277. A chemical reaction in which bonds are broken is usually associated with ________.
A synthesis
Forming a larger molecule
The release of energy
The consumption of energy
Answer
Correct Answer:
The consumption of energy
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278. These molecules are _____.
Geometric isomers
Cis-trans isomers
Structural isomers
All of these
Answer
Correct Answer:
Geometric isomers
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279. Screening of the nuclear charge by core electrons in atoms is __________.
Responsible for a general decrease in atomic radius going down a group
Less efficient than that by valence electrons
More efficient than that by valence electrons
Essentially identical to that by valence electrons
Both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group
Answer
Correct Answer:
More efficient than that by valence electrons
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280. Osmotic pressure is measured in units of _______.
mm Hg
ml/min
mm/sec
mm/min
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281. Germ cells have __________ unpaired chromosomes and are thus called __________ cells.
23; somatic
23; haploid (n)
23; diploid (2n)
46; somatic
Answer
Correct Answer:
23; haploid (n)
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282. Enzymes are described as catalysts, which means that they _____.
Increase the free energy of the reactants to make the reaction go faster
Provide activation energy for the reactions they facilitate
Can alter the free energy change (ΔG) for a chemical reaction
Increase the rate of a reaction without being consumed by the reaction
Are proteins
Answer
Correct Answer:
Increase the rate of a reaction without being consumed by the reaction
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283. An ionic bond is shown below. it forms as a result of _____.
All are properties related to hydrogen bonding.
One of the atoms sharing electrons is much more electronegative
An attraction between atoms that have opposite charges
Chemicals are fundamental to the structure and function of all living things
Answer
Correct Answer:
An attraction between atoms that have opposite charges
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284. _____ are chemical mechanisms that start a reaction.
Inhibitors
Activators
Centrioles
Vacuoles
Answer
Correct Answer:
Activators
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285. All of the following are typical characteristics of neurotransmitters except __________.
The synaptic vesicles release acetylcholine
G protein dissociates from the NE Receptor
They are released into the bloodstream before reaching the postsynaptic cell
Synaptic vesicles secrete neurotransmitter by exocytosis
Answer
Correct Answer:
They are released into the bloodstream before reaching the postsynaptic cell
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286. The skeletal structure below is that of a ________.
Wax
Fat
Fatty acicd
Glycerophospholipid
Steroid
Answer
Correct Answer:
Fatty acicd
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287. The cross bridge cycle starts when _________.
Ca2+ from the sarcoplasmic reticulum binds to tropomyosin
ATP binds to troponin and is hydrolyzed to ADP and Pi
Ca2+ from the sarcoplasmic reticulum binds to troponin
Acetylcholine diffuses away from the synaptic cleft
Ca2+ is actively transported into the sarcoplasmic reticulum
Answer
Correct Answer:
Ca2+ from the sarcoplasmic reticulum binds to troponin
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288. There are ________ σ bonds and ________ π bonds in h3c-ch2-ch=ch-ch2-c≡ch.
12, 2
16, 3
14, 2
10, 3
13, 2
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289. The entropy of the universe is ________.
Continually increasing
Continually decreasing
Zero
The same as the energy, E
Constant
Answer
Correct Answer:
Continually increasing
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290. The energy of a photon that has a wavelength of 13.2 nm is ________ j.
9.55 x 10-25
1.51 x 10-17
1.99 x 10-25
4.42 x 10-23
Answer
Correct Answer:
1.51 x 10-17
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291. Of the molecules below, only ________ is nonpolar.
BF3
NF3
IF3
PBr3.
BrCl3
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292. Maltose has a (1→4) α linkage between glucose and ________.
Plants.
Asparagine.
Glucose
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293. ______ is a hydroxyl group
—NH2
—COOH
—H.
—OH
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294. This atom can form up to _____ single covalent bond(s).
Three
Four
Five
Six
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295. The atoms of different phosphorus isotopes _____.
Have different numbers of protons
React differently with other atoms
Have different atomic numbers
Have different numbers of neutrons
Answer
Correct Answer:
Have different numbers of neutrons
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296. A mineral that has _______ can be split fairly easily along planes with weak atomic attraction
Cleavage
Streak
Hardness
Luster
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297. A _______ is a mound of ocean water that's driven toward coastal areas by hurricane-force winds
Storm surge
Tsunami
Rogue wave
Cyclone
Answer
Correct Answer:
Storm surge
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298. The lewis structure of the co32- ion is ________.
[:O:=C-::O:-::O:]2-
H-C---C-H
Both
None of these
Answer
Correct Answer:
[:O:=C-::O:-::O:]2-
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299. ________ have the lowest first ionization energies of the groups listed.
Alkali metals
Halogens
Alkaline earth metals
Transition metals
Answer
Correct Answer:
Alkali metals
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300. A molecule with square planar geometry but with six electron regions has ______ lone pairs.
2
4
3
6
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301. When the equation, ___o2 + ___c5h12 → ___co2 + ___h2o is balanced, the coefficient of o2 is:
8
4
3
5
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302. When the equation, ___n2 + ___h2 → ___nh3 is balanced, the coefficient of hydrogen is:
3
4
5
1
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303. A 0.200 m k2so4 solution is produced by __________.
Dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L
Dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL
Diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL
Dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL
Answer
Correct Answer:
Diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL
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304. 9.73 g of lead(iv) chloride contains enough cl- ions to make ____ g of magnesium chloride.
5.31 g
0.188 g
17.8 g
1.32 g
0.0557 g
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305. 200. ml of a 12.0% (m/v) nacl solution is diluted to 600. ml. the new concentration is ________ %.
4.00 %
3.90%
5.00%
3.20
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306. 2.28 x 10–4 mm is equal to 2.28 x 10–13 ______?
Nm
Gm
Km
Mm
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307. When the following equation is balanced, the coefficients are ________.
NH3 (g) + O2 (g) → NO2 (g) + H2O (g)
1, 1, 1, 1
4, 7, 4, 6
2, 3, 2, 3
1, 3, 1, 2
Answer
Correct Answer:
4, 7, 4, 6
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308. Using the table of average bond energies below, the δh for the reaction is ________ kj. Bond: C equivalence c C-C H-I C-I C-H D (kJ/mole): 839 348 299 240 413 +63 +160 -63 -217 -160
-217
+63
-63
130
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309. Under constant conditions, the half-life of a first-order reaction ________.
Is the time necessary for the reactant concentration to drop to half its original value
Does not depend on the initial reactant concentration
Can be calculated from the reaction rate constant
Is constant
All of the above are correct
Answer
Correct Answer:
All of the above are correct
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310. The volume of a sample of gas (2.49 g) was 752 ml at 1.98 atm and 62 °c. the gas is ________.
SO2b
SO3c
NH3d
NO2
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311. When molecules fluoresce, the emitted photon has ________ energy compared to the absorbed photon.
Low
High
Equal
Moderate
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312. When aqueous solutions of __________ are mixed, a precipitate forms.
KOH and Ba(NO3)2
NaI and KBr
Li2CO3 and CsI
NiBr2 and AgNO3
Answer
Correct Answer:
NiBr2 and AgNO3
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313. What is the predicted ecell, using the nernst equation? ____ v
0.0446
0.0344
0.0445
0.0039
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314. Ti has __________ in its d orbitals.
1 electron
2 electrons
3 electrons
4 electrons
Answer
Correct Answer:
2 electrons
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315. The equilibrium expression for kp for the reaction below is ________. n2 (g) + o2 (g) 2no (g)
(2PO2)(2PN2)/2PNO
(PO2)(PN2)/2PNO
(PO2)(PN2)/PNO
(2PNO)/(2PN2)(2PO2)
None of these
Answer
Correct Answer:
None of these
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316. The electron affinity (ea) of an atom _____.
Is the energy associated with adding an additional electron in the gas phase to form an anion
Is always a negative number because it is the energy associated with an exothermic process
Increases as you go from left to right across a period
Is the energy change associated with removing an electron from an atom in the gas phase to form a cation
Answer
Correct Answer:
Is the energy associated with adding an additional electron in the gas phase to form an anion
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317. Reverse transcriptase produces __________ from an rna template.
CDNA
DNA
RNA
MRNA
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318. Most acids ionize in solution, and most bases _____ in solution.
Ionize
Disperse
Dissociate
Vaporize
Answer
Correct Answer:
Dissociate
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319. Low-density lipoproteins (ldl) are the principal transport vehicle for _______ in the blood.
Cholesterol
Protein
Steroid hormones
None of the above
Answer
Correct Answer:
Cholesterol
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320. The ________ have the most negative electron affinities.
Alkaline earth metals
Alkali metals
Halogens
Transition metals
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321. Of the following, a 0.2 m aqueous solution of ________ will have the highest freezing point.
Na₃PO₄
Mg(NO₃)₂
NaCl
(NH₄)₃PO₄
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322. Of the reactions below, only ________ is not spontaneous.
Mg (s) + 2HCl (aq) → MgCl2(aq) + H2(g)
2Ag (s) + 2HNO3(aq) → 2AgNO3(aq) + H2(g)
2Ni (s) + H2SO4(aq) → Ni2SO4(aq) + H2(g)
2Al (s) + 6HBr (aq) → 2AlBr3 (aq) + 3 H2(g
Answer
Correct Answer:
2Ag (s) + 2HNO3(aq) → 2AgNO3(aq) + H2(g)
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323. The total concentration of ions in a 0.625 m solution of hcl is ________.
0 M
0.500 M
0.625 M
1.25 M
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324. The principal quantum number of the first d subshell is ________.
3
2
4
1
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325. The normal boiling point of the substance with the phase diagram shown above is ________ °c.
10
20
30
40
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326. The molecular geometry of the right-most carbon in the molecule below is __________.
Trigonal planar
Trigonal bipyramidal
Tetrahedral
Octahedral
Answer
Correct Answer:
Trigonal planar
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327. The molecular geometry of the pf3 molecule is ________, and this molecule is ________.
Trigonal pyramidal, polar
Trigonal bipyramidal, nonpolar
Trigonal pyramidal, nonpolar
Trigonal bipyramidal, polar
Answer
Correct Answer:
Trigonal pyramidal, polar
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328. The molarity of a solution of 5.0 g of kcl in 100. ml of solution is __________.
.67m
.57m
.77m
.47m
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329. The lewin change model includes __________.
Unfreezing
Moving
Refreezing
All of the above.
Answer
Correct Answer:
All of the above.
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330. The h3o+ ion is called the ________ ion.
Hydroxide
Hydronium
Hydrogen
Protium
Answer
Correct Answer:
Hydronium
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331. The following reaction is an example of a ________ reaction. C5H8 + 7O2 → 5CO2 + 4H2O
Combustion
Single replacement
An exothermic reaction
An endothermic reaction
Answer
Correct Answer:
Combustion
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332. The density of no2 in a 4.50 l tank at 760.0 torr and 25.0 °c is ________ g/l.
3.27
1.68
9.30
1.88
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333. The density of nitric oxide (no) gas at 1.21 atm and 54.1 °c is ________ g/l.
0.0451
0.740
1.35
0.273
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334. The correct formula for the compound formed from mg and s is ________.
SMg
MgS
Both A & B
None of the above
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335. The central atom in ________ violates the octet rule.
Cl2CO
BF3
NCl3
BrCN
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336. The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is __________.
KOH (aq) + HC2H3O2 (aq) → OH- (l) + HC2H3O2+ (aq) + K (s)
KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 (aq)
KOH (aq) + HC2H3O2 (aq) → H2C2H3O3 (aq) + K (s)
KOH (aq) + HC2H3O2 (aq) → KC2H3O3 (aq) + H2 (g
Answer
Correct Answer:
KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 (aq)
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337. The angular momentum quantum number is 3 in __________ orbitals.
D
F
S
P
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338. The angular momentum quantum number (l) value of 2 indicates the ________ subshell.
D
F
S
P
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339. The [h3o+] of a solution with ph = 9.7 is ________.
2 × 10-10 M
2 × 10-9 M
1 × 10-2 M
1 × 10-9M
Answer
Correct Answer:
2 × 10-10 M
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340. Pcl5 has __________ electron domains and a __________ molecular arrangement.
6, trigonal bipyramidal
6, tetrahedral
5, trigonal bipyramidal
6, seesaw
Answer
Correct Answer:
5, trigonal bipyramidal
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341. One mole of copper(ii) sulfate, cuso4, contains ________ moles of o.
4
5
3
2
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342. Of the species below, only __________ is not an electrolyte.
HCl
Rb2SO4
Ar
KOH
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343. Of the molecules below, the bond in ________ is the most polar.
HCl
H2
HBr
HF
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344. Of the following, only ________ has sp2 hybridization of the central atom.
CO32-
ICl3
I3-
PF5
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345. Of the following, ________ is the most volatile.
CBr4
CCl4
CF4
CH4
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346. Of the following substances, an aqueous solution of ________ will form basic solutions.
NH4Cl, Cu(NO3)2
K2CO3, NH4Cl
NaF only
NaF, K2CO3
Answer
Correct Answer:
NaF, K2CO3
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347. Of the following species, __________ will have bond angles of 120?.
PH3
NCl3
ClF3
BCl3
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348. Of the following species, ________ has the largest radius.
Ar
Sr2+
Kr
Br-
Rb+
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349. Of the following molecules, only ________ is polar.
BCl3
NCl3
BeCl2
Cl2
CCl4
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350. Of the bonds below, ________ is the least polar.
C-Br
C-I
C-Cl
C-F
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351. O2(g) effuses at a rate that is ______ times that of xe(g) under the same conditions.
2.02
1.02
3.02
1.52
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352. Most gases show variations from ideality at ________ pressure and ________ temperature.
High; low
High;high
Low;high
Low;low
Answer
Correct Answer:
High; low
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353. ________ is reduced in the following reaction: cr2o7 2- + 6s2o3 2- + 14h+ → 2cr3+ + 3s4o6 2- + 7h2o
S2O3 2-
Cr3+
H+
Cr2O72-
S4O62
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354. Ne(g) effuses at a rate that is ______ times that of xe(g) under the same conditions.
2
3
2.17
3.17
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355. Bile salts are among the lipid class known as __________.
Steorides
Cholesterol.
Liver
Glycerophospholipids
Answer
Correct Answer:
Steorides
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356. Of the molecules below, only ________ is polar.
CCl4
CH4
CH3Cl
SiCl4
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357. The addition of hydrofluoric acid and __________ to water produces a buffer solution.
HCl
NaNO
NaF
NaCl
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358. The density of a 167.4 g sample of magnesium having a volume of 96.32 ml is ________ g/cm3.
3.625
25.26
1.738
16120
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359. There are __________ valence electrons in the lewis structure of ch3ch2cl.
20
220
30
40
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360. The wavelength of a photon that has an energy of 5.25 ? 10-19 j is ________ m.
3.79 x 10-7
2.64 x 106
2.38 x 1023
4.21 x 10-24
Answer
Correct Answer:
3.79 x 10-7
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361. The starch in oatmeal and wheat is composed of _____ molecules.
Lactose
Glucose
Fructose
Mannose
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362. The pressure of a sample of ch4 gas (6.022 g) in a 30.0 l vessel at 402 k is ________ atm.
2.42.
6.62.
0.413.
12.4
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363. The nutritional calorie (cal) is the same as __________ cal.
10000
1000
100
10
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364. The magnitude of kw indicates that ________.
Water autoionizes very slowly
Water autoionizes very quickly
Water autoionizes only to a very small extent
The autoionization of water is exothermic
Answer
Correct Answer:
Water autoionizes only to a very small extent
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365. Of the following substances, __________ has the highest boiling point.
H2O
CO2
CH4
Kr
NH3
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366. Of the acids in the table below, __________ is the strongest acid.
HOAc
HCHO2
HClO
HF
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367. If a stimulus opens ligand-gated sodium ion channels, the neuron will __________.
Depolarize
Polarize
Both of these
Non of these
Answer
Correct Answer:
Depolarize
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368. Choline is a quaternary ammonium compound with a __________ charge on the nitrogen.
Positive
Negative
Zero
Neutral
Double
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369. As an acidic compound dissolves in water, the ph of the water _______.
Increase
Decreases
Both of these
None of these
Answer
Correct Answer:
Decreases
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370. An electrical conductor is an element with ________ electrons in its outer orbit.
Less than 1
Less than 2
Less than 3
Less than 4
Answer
Correct Answer:
Less than 4
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371. An aqueous solution of ________ will produce an acidic solution.
KNO3
NH4NO3
Na2SO3
RbBr
Mg(ClO4)2
Answer
Correct Answer:
NH4NO3 Mg(ClO4)2
Note: This question has more than 1 correct answers
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372. _____ have the most calories per serving of all the food items.
Complete Proteins
Incomplete Proteins
Complex Carbohydrates
Fats
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373. In a mixture of 5 ml water, 10 ml alcohol, and 50 ml acetone the solvent(s) is(are) ________.
Acetone
Alcohol
Water
Acetone and alcohol
Alcohol and water
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374. In the following reaction, galactose is a ______. galactose + glucose → lactose + water
Polysaccharide
Monomer
Polymer
Protein
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375. There are ________ molecules of methane in 0.123 mol of methane (ch4).
2.46×10−2
2.04×10−25
7.40×1022
0.615
Answer
Correct Answer:
7.40×1022
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376. There are ________ ? and ________ ? bonds in the h - c?c - h molecule.
8 sigma bonds and 2 pi bonds
2 sigma bonds and 2 pi bonds
6 sigma bonds and 2 pi bonds
4 sigma bonds and 2 pi bonds
Answer
Correct Answer:
8 sigma bonds and 2 pi bonds
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377. When 2610 + 11.7 + 0.22 are added, the answer to the correct number of decimal places is ________.
2621.92
2621.9
2621
2620
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378. Valence bond theory predicts that tin will use _____ hybrid orbitals in snf5?.
Sp2
Sp3
Sp3d
Sp3d2
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379. Three monosulfur fluorides are observed: sf2, sf4, and sf6. of these, ________ is/are polar.
SF2 and SF4 only
SF6 only
SF4 only
SF2 only
Answer
Correct Answer:
SF2 and SF4 only
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380. There are ________ mol of carbon atoms in 4 mol of c4h8o2.
4
8
16
20
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381. There are ________ mol of bromide ions in 0.300 l of a 0.150 m solution of albr3.
0.450
0.150
0.0500
0.167
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382. The total concentration of ions in a 0.75 m solution of hcl is ________.
1.75 M
1.5 M
0.75 M
0.625 M
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383. The thermodynamic quantity that expresses the extent of randomness in a system is ________.
Enthalpy
Internal energy
Bond energy
Entropy
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384. There are __________ valence electrons in the lewis structure of ch3och2ch3.
18
20
26
32
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385. Of the following, ________ should have the highest critical temperature.
CF4
CCl4
CBr4
CH4
All are the same
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386. Of the following, ________ is the least volatile.
CI4
CF4
CBr4
CCl4
CH4
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387. The structural formulas of amino acids are the same except for the ________.
Carboxyl group.
Alpha carbon.
Amino group.
Side (R) group.
Hydrogen bonding
Answer
Correct Answer:
Side (R) group.
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388. The solubility of carbon dioxide in soda water decreases with _________ temperature.
Increases
Decreases
Decreases and then increases
Both b and c
Answer
Correct Answer:
Increases
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389. The solubility (in grams per liter) of caf2 in water at 25 0C is ____.(k sp = 1.5 × 10−10)
1.5 × 10+10
1.5 × 10−10
1.5 × 10+20
1.5 × 10−20
Answer
Correct Answer:
1.5 × 10−10
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390. The side chain for histidine is classified as a ________ side chain.
BASIC
Lysine
Alanine
Serine
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391. The root mean square speed of co at 113 c is ______ m/s
1.84
58.3
586
993
18.5
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392. The reduction in the freezing point of a solution is _____ to molal concentration.
Inversely proportional
Directly proportional
Not related
Unimportant
Answer
Correct Answer:
Inversely proportional
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393. The reaction between strontium hydroxide and chloric acid produces ________.
A molecular compound and a strong electrolyte
Loss of electrons
Gain of electrons
None of these
Answer
Correct Answer:
A molecular compound and a strong electrolyte
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394. The rate constant of a first-order process that has a half-life of 3.50 min is ________ s-1.
0.693
1.65
1.55
0.593
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395. The products in a decomposition reaction _____
Elements
Compound
Decomposition
Replacement
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396. The principal reason for the extremely low solubility of nacl in benzene (c6h6) is the ________.
Strong solvent-solvent interactions
Hydrogen bonding in C6H6
Strength of the covalent bond in NaCl
Weak solvation of Na+ and Cl- by C6H6
Increased disorder due to mixing of solute and solvent
Answer
Correct Answer:
Weak solvation of Na+ and Cl- by C6H6
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397. The ph of a solution is defined as the ____________ of the hydrogen ion concentration.
Negative logarithm
Positive logrithum
Zero
None of these
Answer
Correct Answer:
Negative logarithm
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398. The molecule shown in the accompanying figure is _____.
A hexose
A pentase
A octase
None of these
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399. The length of the side of a cube having a density of 12.6 g/ml and a mass of 7.65 g is ________ cm.
0.857
0.947
0.847
0.647
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400. The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.
Four-electron
Six-electron
Two-electron
One-electron
Three-electron
Answer
Correct Answer:
Two-electron
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401. The amount of gas that occupies 60.82 l at 31.0 ?c and 367 mm hg is ________ mol.
3.17mole
2.17mole
1.17mole
4.17mole
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402. The ________ is what needs to be overcome in a reaction so that it can proceed to the products.
Bond energy
Thermodynamics
Entropy
Catalyst
Activation energy
Answer
Correct Answer:
Activation energy
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403. Sucrose is a _____.
Monosaccharide
Polysaccharide
Disaccharide
All of these
Answer
Correct Answer:
Disaccharide
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404. Small objects denser than water can float on its surface because water has high _____.
Cohesion
Adhesion
Surface tension
Answer
Correct Answer:
Surface tension
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405. Slides are placed upside down in a slide projector to correct for the _______ image produced.
Inverted
Magnified
Virtual
Small size of the
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406. Production of 13 g of c2h2 requires consumption of ________ g of h2o.
20
18
22
16
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407. Pesticides are best described as _______.
Polluting chemicals toxic to all living things
Chemicals that destroy 33% of the world's potential food supply
Toxic chemicals used to control weed populations
Toxic chemicals used to control pest populations
Answer
Correct Answer:
Polluting chemicals toxic to all living things
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408. Oxygen, nitrogen, and carbon are all _____.
Metalloids
Nonmetals
Metals
Halogens
Answer
Correct Answer:
Nonmetals
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409. Oxidation and ________ mean essentially the same thing.
Sulfuric acid
Corrosion
Rusting of iron
None of these
Answer
Correct Answer:
Corrosion
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410. One million argon atoms is ________ mol (rounded to two significant figures) of argon atoms.
1.4 × 10-18
1.6 × 10-18
1.5 × 10-18
1.7 × 10-18
Answer
Correct Answer:
1.7 × 10-18
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411. One angstrom, symbolized å, is 10-10 m. 1 cm3 = ________ å3.
10^24
10^-24
10^30
10^-30
10^-9
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412. Of the acids, ________ is the strongest acid.
HCHO2
HClO
HF
HOAc
HOAc and HCHO2
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413. Ne(g) effuses at a rate that is ______ times that of kr(g) under the same conditions.
2
1.98
2.03
2.98
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414. Ne(g) effuses at a rate that is ______ times that of br2(g) under the same conditions.
2
1.98
2.02
2.98
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415. N2(g) effuses at a rate that is ______ times that of xe(g) under the same conditions.
1.73
2.16
1.59
1.43
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416. N2(g) effuses at a rate that is ______ times that of kr(g) under the same conditions.
1.59
1.43
1.73
2.16
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417. N2(g) effuses at a rate that is ______ times that of cl2(g) under the same conditions.
1.59
1.73
1.43
2.16
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418. Molecule a is a __________.
Triglyceride
Nucleotide
Steroid
Phospholipid
Answer
Correct Answer:
Phospholipid
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419. Mixtures can be separated by filtration and distillation. both methods take advantage of _____.
Differences in the chemical properties of the mixtures's components.
Differences in the physical properties of the mixture's components.
Similarities in the chemical properties of the mixture's components
Similarities in the physical properties of the mixture's components
Answer
Correct Answer:
Differences in the physical properties of the mixture's components.
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420. Large intermolecular forces in a substance are manifested by ________.
Low vapor pressure
High boiling point
High heats of fusion and vaporization
High critical temperatures and pressures
All of these
Answer
Correct Answer:
All of these
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421. In the reaction below, δh°f is zero for ________. ni (s) + 2co (g) + 2pf3 (g) → ni(co)2(pf3)2 (l)
Ni(s)
F2 (s)
Co (g)
None of these
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422. In the ionic compound xy3, if x has a charge of __________ then y has a charge of __________.
3+; 1-
2+; 1-
3+; 3-
3+; 2-
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423. In nature, rings with _____ carbon atoms are the most abundant.
3 or 4
4 or 7
5 or 6
2 or 3
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424. In liquids, the attractive intermolecular forces are ________.
Very weak compared with kinetic energies of the molecules
Strong enough to hold molecules relatively close together
Strong enough to keep the molecules confined to vibrating about their fixed lattice points
Not strong enough to keep molecules from moving past each other
Strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other
Answer
Correct Answer:
Strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other
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425. In experimentation, dependent variables are also known as _____________ variables.
Positive proof
Manipulative
Response
None of these
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426. In an equilibrium reaction with a keq of 1 × 10^8, the _____.
Products are favored
The reaction is nonspontaneous
The reaction is endothermic
Reactants are favored.
Answer
Correct Answer:
Products are favored
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427. In a saturated solution of a salt in water, ________.
The rate of crystallization > the rate of dissolution
The rate of dissolution > the rate of crystallization
Seed crystal addition may cause massive crystallization
The rate of crystallization = the rate of dissolution
Addition of more water causes massive crystallization
Answer
Correct Answer:
The rate of crystallization = the rate of dissolution
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428. In a neutral solution, the [h+] is _____.
10 ^– 13
10 ^– 17
10 ^– 14
10 ^– 12
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429. In a gas, the distance between the particles is ________.
Very close relative to the size of the molecules
Close relative to the size of the molecules
Fixed relative to the size of the molecules
Small relative to the size of the molecules
Very large relative to the size of the molecules
Answer
Correct Answer:
Very large relative to the size of the molecules
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430. If 50.75 g of a gas occupies 10.0 l at stp, 129.3 g of the gas will occupy ________ l at stp.
26.5
28.5
27.5
25.5
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431. How many moles of water are produced from the combustion of 0.100 mol pentane, c5h12?____ mol
0.100 mol
0.500 mol
0.600 mol
0.800 mol
None of the above
Answer
Correct Answer:
None of the above
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432. How many moles of [mn+] are dissolved in that compartment of the microwell plate? _____ mol
10.035 M
9.035 M
8.035 M
7.035 M
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433. H2po4- is the conjugate _____ of h3po4 and the conjugate _____ of hpo42−.
Base; acid
Acid; acid
Acid; base
Base; base
Answer
Correct Answer:
Base; acid
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434. Glycine is the only naturally occurring amino acid that is ________.
Negatively charged
Achiral
Ammonium group
Hydrophobic
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435. Glucose and galactose are _____ of each other.
Epimers
Enantiomers
Diastereomers
Anomers
None of the above
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436. For a molecule with the formula ab2, the molecular shape is ________.
Linear
Bent
Both
None of these
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437. Fluids used for an intravenous transfusion must be ________ with bodily fluids.
Isosmotic
Hyperosmotic
Hyposmotic
Neosmotic
Answer
Correct Answer:
Isosmotic
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438. Fibrinogen is a protein produced in platelets that _____.
Fights infections
Prevents hemophilia
Carries oxygen
Creates blood clots
Answer
Correct Answer:
Creates blood clots
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439. During hybridization, _____.
Identification of individuals based on their DNA profile
Cloning creates genetically identical offspring
Two organisms with desired traits are bred together
A process of breeding organisms because of their specific traits
Answer
Correct Answer:
Two organisms with desired traits are bred together
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440. Dna methylation of cytosine residues __________.
Occurs in the promoter region and enhances binding of RNA polymerase
May be related to the transformation of proto-oncogenes to oncogenes
May be a mechanism of epigenetic inheritance when methylation patterns are repeated in daughter cells
Is a signal for protein degradation
Initiates the acetylation of histones
Answer
Correct Answer:
May be a mechanism of epigenetic inheritance when methylation patterns are repeated in daughter cells
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441. Dacron is a ___________ compound and is produced by a __________ reaction.
Polyester; condensation
Polyester; a diamine with a diacid
Beta decay; condensation
Polyester; increases
Answer
Correct Answer:
Polyester; condensation
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442. ____ could be/represent a smaller, charged fragment of the original molecule.
Lower end of the chemical shift range
Middle of the chem shift range
M⁺ would not be observed.
Base peak and radical cations
Answer
Correct Answer:
Base peak and radical cations
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443. Collagen, a protein found in tendons and cartilage, would be classified as a ________ protein.
Glutamic acid
Catalytic
Structural
Salt bridges
Tyrosine
Answer
Correct Answer:
Structural
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444. Chirality occurs when stereoisomers have mirror images that are ________.
Alpha-1,2
Ketopentose
Fructose and glucose
Not superimposable
Monosaccharide
Answer
Correct Answer:
Not superimposable
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445. Carbon-14 in the atmosphere is transformed from _________.
Geiger counter
Electromagnetic
Never
Nitrogen
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446. Carbohydrates typically include ________.
An NH2 group
C, H, and O atoms
A hydrocarbon chain
A PO4 group
Answer
Correct Answer:
C, H, and O atoms
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447. Buffers are __________.
The opposite ends of the molecule have opposite electrical charges
Substances that minimize changes in the concentration of H+ and OH- in a solution
A compound that donates hydrogen ions to a solution
Are charged molecules that are attracted to the partial charge of the water molecule
Answer
Correct Answer:
Substances that minimize changes in the concentration of H+ and OH- in a solution
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448. Bombarding uranium-235 with _____ creates energy through fission.
High energy neutron
Low energy neutron
High energy protron
Low energy protron
Answer
Correct Answer:
High energy neutron
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449. Based on the octet rule, iodine most likely forms an ________ ion.
I4-
I2+
I+
I4+
I-
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450. Atomic radius generally increases as we move ________.
A group of atoms/ions that have the same number of electrons.
Down a group and from right to left across a period
Down a group and from left to right across a period
A group of atoms/ions that have the different number of electrons.
Answer
Correct Answer:
Down a group and from right to left across a period
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451. At a temperature of ________ °c, 0.444 mol of co gas occupies 11.8 l at 839 torr.
73 °C
379 °C
32 °C
14 °C
106 °C
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452. Arachidonic acid is associated with ________.
Glucose metabolism
Omega-3 fatty acid metabolism
Omega-6 fatty acid metabolism
Cholesterol metabolism
Answer
Correct Answer:
Omega-6 fatty acid metabolism
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453. Approximately____% of all alcohol consumed is metabolized by the liver.
90
80
70
60
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454. Any reaction that absorbs 150 kcal of energy can be classified as ________.
Activated
Exothermic
Oxidation
Endothermic
Answer
Correct Answer:
Endothermic
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455. An ion with six protons, seven neutrons, and a charge of 2+ has an atomic number of ________.
Six
Seven
Two
Nine
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456. An implication of hund's rule is that _____.
Electrons fill degenerate orbitals singly first, with parallel spins, before the electrons will pair up
The second ionization energy is always greater than the first ionization energy
The rows in the periodic table grow progressively longer because you are adding sublevels as the n level increases.
If two electrons occupy the same orbital, they must have opposite spin numbers
Answer
Correct Answer:
If two electrons occupy the same orbital, they must have opposite spin numbers
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457. An electron is most delocalized in a(n) ______________ orbital.
Atomic
Bonding molecular
Antibonding molecular
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458. an electron cannot have the quantum numbers n = __________, l = __________, ml = __________.
2, 0, 0
2, 1, -1
3, 1, -1
1, 1, 1
3, 2, 1
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459. An aqueous solution of ________ will produce a neutral solution.
NaF
NH4Br
Rb2CO3
KNO2
NaClO4
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460. An aqueous solution of ________ will produce a basic solution.
NaHSO4
NH4ClO4
NaCl
KBr
Na2SO3
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461. Ammonia is a ________.
Weak acid
Strong acid
Weak base
Strong acid
Salt
Answer
Correct Answer:
Weak base
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462. Amino acids and glucose enter cells by ________.
Active transport
Passive diffusion
Facilitated diffusion
Endocytosis
Answer
Correct Answer:
Facilitated diffusion
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463. All of the following are forms of radiation except _______ rays
Stabilizing
Beta
Alpha
Gamma
Answer
Correct Answer:
Stabilizing
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464. Aldosterone will ________.
Increases when environmental temperature rises
Intrinsic autoregulatory mechanisms
Increases as blood viscosity increases
Veins are called capacitance vessels or blood reservoirs.
Promote an increase in blood pressure
Answer
Correct Answer:
Promote an increase in blood pressure
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465. According to the arrhenius concept, if hno3 were dissolved in water, it would act as ________.
A base
An acid
A source of hydroxide ions
A source of H- ions
A proton acceptor
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466. According to the arrhenius concept, an acid is a substance that __________.
Is capable of donating one or more H+
Causes an increase in the concentration of H+ in aqueous solutions
Can accept a pair of electrons to form a coordinate covalent bond
Reacts with the solvent to form the cation formed by autoionization of that solvent
Tastes bitter
Answer
Correct Answer:
Causes an increase in the concentration of H+ in aqueous solutions
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467. A(n) ________ has charge but negligible mass, whereas a(n) ________ has mass but no charge.
Neutrons; proton
Electron; neutron
Ion ; neutron
Electron; proton
Answer
Correct Answer:
Electron; neutron
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468. A transmission electron microscope would be the best microscope choice to study _______.
Structures smaller than cells
Single celled organisms
Plant leaves
Amphibian organs
Answer
Correct Answer:
Structures smaller than cells
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469. A solution with ph 4 has __________ the h+ concentration of a solution with ph 8.
1/2
2 times
4 times
10,000 times
1/10,000
Answer
Correct Answer:
10,000 times
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470. A solution of ph 5 has _____ times more hydrogen ions than that of pure water.
10
100
5
50
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471. A solution at ph 10 contains __________ than the same amount of solution at ph 8.
100 times less H+
Hydrogen bonds
A higher boiling point
0.032G
Polar
Answer
Correct Answer:
100 times less H+
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472. A single gram of alcohol contains _____ calories.
7
8
6
5
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473. A sample of ch4o with a mass of 32.0 g contains __________ molecules of ch4o.
5.32 × 10^23
1.00
1.88 × 10^22
6.02 × 10^23
32.0
Answer
Correct Answer:
6.02 × 10^23
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474. A sample of ch2f2 with a mass of 19 g contains ________ atoms of f.
2.2 × 10^23
38
3.3 × 10^24
4.4 × 10^23
9.5
Answer
Correct Answer:
4.4 × 10^23
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475. A salt dissolved in water forms _____.
Anions and cations
Only anions
Only cations
Neutral atoms
Answer
Correct Answer:
Anions and cations
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476. A reaction between an acid and a base is called a(n) ________________ reaction.
Hydro
Ionization
Neutralization
Redox
Answer
Correct Answer:
Neutralization
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477. A phospholipid is a _____
Nonpolar lipid molecule that is made amphipathic by the addition of a phosphate
Polar lipid molecule that fully interacts with water
Nonpolar lipid molecule that is made polar by the addition of a phosphate
Polar lipid molecule that fully repels water
Answer
Correct Answer:
Nonpolar lipid molecule that is made amphipathic by the addition of a phosphate
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478. A molecule containing a central atom with sp3d2 hybridization has a(n) ________ electron geometry.
Trigonal bipyramidal
Octahedral
Trigonal planar
Linear
Answer
Correct Answer:
Octahedral
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479. A molecule containing a central atom with sp3d hybridization has a(n) ________ electron geometry.
Trigonal bipyramidal
Octahedral
Trigonal planar
Linear
Answer
Correct Answer:
Trigonal bipyramidal
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480. A molecule containing a central atom with sp hybridization has a(n) ________ electron geometry.
Trigonal bipyramidal
Octahedral
Trigonal planar
Linear
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481. A mole of red photons of wavelength 725 nm has ________ kj of energy.
1.65
165
227
0.00605
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482. A megamole of titanium contains __________ moles of titanium.
1.0 × 106
1 × 106
Nano-, 1 × 10-9
None of these
Answer
Correct Answer:
1.0 × 106
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483. A long chain of hydrocarbon bonded to cooh is a ________ acid.
Formic
Carbonic
Amino
Fatty
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484. A bond that is not symmetrical along the axis between two atomic nuclei is a _____.
Pi bond
Polar bond
Covalent bond
Ionic bond
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485. A 17.6-g sample of ammonium carbonate contains ________ mol of ammonium ions.
0.266
0.186
0.366
0.226
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486. A 0.100 m solution of ________ will contain the highest concentration of potassium ions.
Potassium phosphate
Potassium hydrogen carbonate
Potassium hypochlorite
Potassium iodide
Potassium oxide
Answer
Correct Answer:
Potassium phosphate
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487. A ______ property describes how a substance acts when it reacts with other substances.
Reactivity
Chemical
Both
None of these
Answer
Correct Answer:
Reactivity
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488. 1-methylcyclopentanol is classified as ________.
A primary alcohol
A secondary alcohol
A tertiary alcohol
A phenol
An enol
Answer
Correct Answer:
A tertiary alcohol
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489. 0.50 mole of nacl is added to 1.0 kg of water. the freezing point of the solution will be ________.
0.00 °C
0.93 °C
-1.86 °C
-0.93 °C
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490. _____, which is released from _____, acts on the ovaries and testes.
Anterior pituitary gland: Antidiuretic hormone
Follicle-stimulating hormone; the anterior pituitary gland
High levels of circulating juvenile hormone inhibiting molting.
Responsive cells express a receptor specific for the hormone.
Answer
Correct Answer:
Follicle-stimulating hormone; the anterior pituitary gland
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491. ________ are particularly polarizable.
Small nonpolar molecules
Small polar molecules
Large nonpolar molecules
Large polar molecules
Large molecules, regardless of their polarity
Answer
Correct Answer:
Large molecules, regardless of their polarity
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492. _____ make up the nucleus of an atom, whereas _____ surround the nucleus.
Carbohydrates and nucleic acids
Protons & neutrons; electrons
2, hydrophobic, and hydrophilic
Rovers have captured images of bacterial cells within rocks.
Answer
Correct Answer:
Protons & neutrons; electrons
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493. _____ is a process that helps fuel your metabolism.
Oxidation
Potential; kinetic
Thermodynamics
Light
Calvin cycle
Answer
Correct Answer:
Oxidation
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Chemistry MCQs | Topic-wise
