Chemistry Multiple Questions Assignment
Chem 101: Introduction to General Chemistry Quiz #9 100 points possible Due before noon on
Wednesday, Nov. 5, 2014 Each question is worth five points. 1. Which of these molecules cannot
form hydrogen bonds with another molecule of itself? A. CH3CH2—OH B. CH3—O—CH3 C.
CH3—NH2 D. HF 2. Generally, the solubility of a gas in a liquid A. increases with increasing
temperature B. increases with decreasing pressure C. is unaffected by pressure D. decreases with
increasing temperature 3. The energy associated with hydrogen bonding is __ the
energy associated with a covalent bond. A. the same as B. greater than C. less than 4. Which of
these compounds has the highest boiling point? A. CH4 B. NH3 C. CO D. H2 5. What accounts
for the structural differences between diamond and graphite since both have the same atomic
composition? A. In the composition of diamond, the carbons are all covalently bonded whereas in
graphite there are sheets of carbon covalently bonded and the sheets are held together through
London dispersion forces. B. In the composition of graphite, the carbons are all covalently bonded
whereas in diamond there are sheets of carbon covalently bonded and the sheets are held together
through London dispersion forces. C. The statement is false. Diamond and graphite do not have
any structural differences. D. The statement is false. Diamond and graphite do not have the same
atomic composition. 6. The substance found in the greatest amount in a solution is called the: A.
solute B. colloid C. solvent D. liquid 7. If the temperature of water is increased, what effect will it
have on the solubility of sugar in the water? A. the solubility of sugar will increase B. the
solubility of sugar will decrease C. the solubility of sugar will remain the same 8. Which type of
intermolecular force exists for all molecules? A. covalent bonding B. dipole-dipole forces C.
London dispersion forces D. hydrogen bonding 9. Which of the following would you expect to
have the lowest boiling point? A. C2H6 B. CH3—OH C. NaBr D. H2O 10. Which of these
compounds has the highest boiling point? A. CH4 B. CH3—CH2—CH2—CH2—CH3 C. C CH3
H3C CH3 CH3 D. CH3—CH2—CH3 11. Which of the following cannot serve as a solvent in a
solution? A. a gas B. a liquid C. a solid D. none, all can serve as solvents 12. True or False. For
most pure substances, the solid phase is more dense than the liquid phase. A. True B. False 13.
Which of these compounds has the highest boiling point? A. CH4 B. NH3 C. CO D. H2 14.
Which of the following describes what is meant by the phrase “like dissolves like” A. The more
similar two molecules are with respect to their intermolecular forces the more likely they will be
soluble with one another. B. The more similar two molecules are with respect to their
intramolecular forces the more likely they will be soluble with one another. C. The more similar
two molecules are with respect to their mass the more likely they will be soluble with one another.
D. The more similar two molecules are with respect to their charge the more likely they will be
soluble with one another. 15. The strongest intermolecular force operating between two OF2
molecules is A. London dispersion force B. hydrogen bond C. covalent bond D. dipole-dipole
attraction 16. Which of the following is mostly likely to be soluble in water? A. CH3—OH B.
CH4 C. CCl4 D. C2H4 17. What property of water is responsible for the fact that solid water is
less dense than liquid water. A. hydrogen bonding between water molecules B. intramolecular
forces present in water C. the allotropes of water D. none of the above 18. Which of the following
would you expect to have the highest boiling point? A. C2H6 B. Fe C. CH3—NH2 D. HCl 19.
What is the name of the phase shift for changing a solid into a liquid? A. sublimation B.
vaporization C. fusion D. condensation 20. If the strongest intermolecular force in a molecular
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sample is London Dispersion forces, this means the molecule must be: A. CH4, because this is the
only molecule with just London Dispersion forces B. A polar molecule that has lone pairs of
electrons on the central atom C. A very polar molecule with hydrogen directly bonded to oxygen
D. A nonpolar molecule
Question one
D
Question two
D
Question three
C
Question four
B
Question five
A
Questions six
C
Question seven
A
Question eight
C
Question nine
A
Question ten
C
Question eleven
C
Question twelve
A
1
Question thirteen
B
Question fourteen
B
Question fifteen
D
Question sixteen
A
Question seventeen
A
Qusestion eighteen
B
Question nineteen
B
Question twenty
C
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Reference
Hettleman, H. (2000). Quantity Chemistry: Classic and Physical Scientific Papers. Singapore:
World Scientific.
