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2nd Semester: Chemistry Weekly Quiz #1 (1/9-1/12) - Chapter 14 and 7
1. As the atmospheric pressure around a liquid decreases, the boiling temperature of the liquid (1 point)
increases
decreases
stays the same
may increase or decrease depending on the liquid.
none of these
2. Which of the following is true for ionic solids dissolved in water? (1 point)
The solution will conduct electricity.
The solid will dissolve into neutral molecules.
The solution will not conduct electricity.
The ions in solution will form a large crystal.
none of these
3. The process of evaporation happens when which of the following occurs? (1 point)
A solid becomes a liquid.
A liquid becomes a solid.
A liquid becomes a gas.
A gas becomes a liquid.
A solid becomes a gas.
4. Identify the major attractive force in the following molecule. N2 (1 point)
dipole-dipole
London dispersion
ionic
hydrogen bonding
none of these
5. The freezing point of helium is approximately -270°C. The freezing point of xenon is -112°C. Both of these are in
the noble gas family. Which of the following statements is supported by these data? (1 point)
Helium and xenon form highly polar molecules.
As the molar mass of the noble gas increases, the freezing point decreases.
The London forces between the helium molecules are greater than the London forces between the xenon
molecules.
The London forces between the helium molecules are less than the London forces between the xenon
molecules.
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none of these.
6. The intermolecular forces called hydrogen bonding will not exist between molecules of (1 point)
H 2O
H2
NH3
HF
any of these
7. Identify the major attractive force in the following molecule. Na 2 S (1 point)
dipole-dipole
London dispersion
ionic
hydrogen bonding
none of these
8. Identify the major attractive force in the following molecule. NH3 (1 point)
dipole-dipole
London dispersion
ionic
hydrogen bonding
none of these
9. Which of the following has the highest melting temperature? (1 point)
H 2O
CO2
S8
MgF 2
P4
10. When the following equation is balanced using the smallest possible integers, what is the number in front of the
bolded substance? C 4 H 10 (g) + O 2 (g) → CO2 (g) + H 2 O (g) (1 point)
2
4
6
8
10
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11. Name the type of crystalline solid formed by potassium bromide. (1 point)
molecular solid
atomic solid
ionic solid
amorphous solid
none of these
12. When the following equation is balanced using the smallest possible integers, what is the number in front of the
bolded substance? CH 3 OH (l) + O 2 (g) → CO2 (g) + H 2 O (g) (1 point)
1
2
4
6
12
13. How many of the following statements are true concerning chemical equations? I. Coefficients can be fractions. II.
Subscripts can be fractions. III. Coefficients represent the relative masses of the reactants and/or products. IV.
Changing the subscripts to balance an equation can only be done once. V. Atoms are conserved when balancing
chemical equations. (1 point)
1
2
3
4
5
14. Which of the following processes must exist in equilibrium with the evaporation process when a measurement of
vapor pressure is made? (1 point)
fusion
vaporization
sublimation
boiling
condensation
15. Water sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the water
__________ as the water evaporates. (1 point)
increases
decreases
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stays the same
16. Name the type of crystalline solid formed by copper. (1 point)
molecular solid
atomic solid
ionic solid
amorphous solid
none of these
17. The normal boiling point of liquid X is less than that of Y, which is less than that of Z. Which of the following is the
correct order of increasing vapor pressure of the three liquids at STP (standard temperature and pressure)?
(1 point)
X, Y, Z
Z, Y, X
Y, X, Z
X, Z, Y
Y, Z, X
18. Identify the major attractive force in the following molecule. H 2 O (1 point)
dipole-dipole
London dispersion
ionic
hydrogen bonding
none of these
19. Identify the major attractive force in the following molecule. HF (1 point)
dipole-dipole
London dispersion
ionic
hydrogen bonding
none of these
20. Name the type of crystalline solid formed by SiO2 (1 point)
molecular solid
atomic solid
ionic solid
amorphous solid
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none of these
21. When the following equation is balanced using the smallest possible integers, what is the number in front of the
bolded substance? N2 (g) + O 2 (g) → N 2 O 3 (g) (1 point)
1
2
4
6
12
22. When the equation Si (s) + HF (aq) → SiF 4 (g) + H 2 (g) is balanced, what is the coefficient for HF? (1 point)
0
1
2
3
4
23. Of the following substances, choose the one with the greatest vapor pressure. (1 point)
He (l)
Ne (l)
Ar (l)
Xe (l)
Rn (l)
24. As the temperature of a liquid increases, the vapor pressure of the liquid generally (1 point)
increases
decreases
stays the same
depends on the type of intermolecular forces
25. When the following equation is balanced using the smallest possible integers, what is the number in front of the
bolded substance? NH3 (g) + O 2 (g) → NO 2 (g)+ H 2 O (g) (1 point)
3
6
7
12
14
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26. All the following are clues that a chemical reaction has taken place except (1 point)
a color change
a solid forms
the reactant is smaller
bubbles form
a flame occurs
27. When the following equation is balanced using the smallest possible integers, what is the number in front of the
bolded substance? Sb (s) + O 2 (g) → Sb2 O 5 (s) (1 point)
1
2
4
6
12
28. Which of the following should have the lowest boiling point? (1 point)
Na 2 S
HF
NH3
N2
H 2O
29. An alloy has a metallic properties. (1 point)
True
False
30. Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen bonding) from weakest to
strongest. (1 point)
dipole-dipole, London dispersion, ionic, hydrogen bonding
London dispersion, dipole-dipole, hydrogen bonding, ionic
hydrogen bonding, dipole-dipole, London dispersion, ionic
dipole-dipole, ionic, London dispersion, hydrogen bonding
London dispersion, ionic, dipole-dipole, hydrogen bonding
31. When the equation Cr 2 S 3 + HCl → CrCl 3 + H 2 S is balanced in standard form, one of the terms in the balanced
equation is (1 point)
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3 HCl
CrCl 3
3 H 2S
2 Cr 2 S 3
Preview Results
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