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WorksheetsAP Chem Quiz (Red)
Total questions: 20
Worksheet time: 12mins
Name
Class
Date
1.
Which of the following liquids experiences dipole-dipole intermolecular forces?
a)
H2 (l)
b)
CF4 (l)
c)
SO2 (l)
d)
CCl4 (l)
2.
Which of the following best explains why temperature increases cause reaction rates to increase.
a)
As temperature increases, activation energy increases
b)
As temperature increases, activation energy decreases
c)
As temperature increases, collisions between reactant particles increases
d)
As temperature increases, more collisions between particles have a required amount of energy.
3.
A sample of a solid substance does not conduct electricity in either the solid or liquid phase. The solid is soluble in water. Which of the following types of interactions is most likely found between particles in the pure substance?
a)
ionic bonds
b)
metallic bonds
c)
network covalent bonds
d)
dipole-dipole forces
4.
Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. Which of the following changes would cause more ammonia to be present in the mixture when equilibrium is reestablished?
a)
decrease the temperature
b)
increase the container’s volume
c)
add a chemical that reacts with hydrogen gas
d)
remove nitrogen gas from the container
5.
Which of the following shows the molecules F2, Cl2, and Br2 in order of their bond enthalpies from least to greatest?
a)
F2 < Cl2 < Br2
b)
Cl2 < Br2 < F2
c)
Br2 < Cl2 < F2
d)
Br2 < F2 < Cl2
6.
Based on Coulomb’s Law and the data in the table above, which of the following would have the weakest interactions with an adjacent water molecule in an aqueous solution?
a)
Hg2+
b)
Ba2+
c)
Mg2+
d)
Al3+
7.
A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?
a)
a strong acid was titrated with a strong base
b)
a weak acid was titrated with a weak base
c)
a weak acid was titrated with a strong base
d)
a strong acid was titrated with a weak base
8.
A sample of a compound contains 18.0 g C, 2.0 g H, and 8.0 g O. Which of the following is the empirical formula of the compound?
a)
C2H2O
b)
C6H8O2
c)
C3H4O
d)
C3H4O2
9.
The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the highest Br- concentration?
a)
PbBr2
b)
CuBr
c)
AgBr
d)
HgBr2
10.
What is the standard reduction potential for the lead (II) half reaction?
a)
-3.13 V
b)
-0.13 V
c)
+0.13 V
d)
+3.13 V
11.
Which of the following is true for the balanced reaction under standard conditions?
3Pb+2Au3+→3Pb2++2Au Eo=1.63V
3Pb+2Au3+→3Pb2++2Au Eo=1.63V
a)
K>1, ΔGo<0
b)
K>1, ΔGo>0
c)
K<1, ΔGo>0
d)
K<1, ΔGo<0
12.
C2H2 (g)+H2 (g) → C2H4 (g)
For the reaction above, which of the following will most likely increase the rate of reaction?
For the reaction above, which of the following will most likely increase the rate of reaction?
a)
decrease the temperature of the reaction container
b)
decrease the volume of the reaction container
c)
pressurize the system with an inert gas, keeping temperature constant
d)
remove acetylene (C2H2) from the reaction container
13.
Which of the following molecules is least soluble in water?
a)
CH2F2
b)
CH3OH
c)
CH2O
d)
CH3CH3
14.
At room temperature, chlorine, Cl2, is a gas. Which of the following provides a characteristic of chlorine with a correct explanation?
a)
chlorine has a lower boiling point than bromine (which is a liquid at room temperature) because chlorine has fewer electrons than bromine
b)
chlorine has a lower first ionization energy than argon (an atomic element that is also a gas at room temperature) because elemental chlorine forms molecules whereas elemental argon does not.
c)
chlorine is a not a good conductor of electricity because it has lone pairs of electrons.
d)
chlorine is soluble in water because chlorine is polar.
15.
Based on the information in the table, which liquid has a higher vapor pressure at 25oC and why?
a)
CBr4 (l), because it has weaker intermolecular forces
b)
CBr4 (l), because it has stronger intermolecular forces
c)
CHBr3 (l), because it has weaker intermolecular forces
d)
CHBr3 (l), because it has stronger intermolecular forces
16.
Based on the information which is the strongest acid?
a)
HX (aq)
b)
Y- (aq)
c)
HY (aq)
d)
X- (aq)
17.
The pH of a 0.01 M HCN solution (Ka=6x 10-10) would be approximately
a)
between 1–2
b)
between 3–4
c)
between 5–6
d)
between 6–7
18.
The photoelectron spectra for chlorine and argon are shown. Which of the following answers provides the correct set of peaks for chlorine, and correct justification?
a)
The solid line peaks represent chlorine. This is true because the solid peaks are slightly to the left of the dashed peaks and chlorine is to the left of argon in the periodic table
b)
The solid line peaks represent chlorine. This is true because chlorine has fewer protons than argon.
c)
The dashed line peaks represent chlorine. This is true because argon’s 2p sublevel has 6 electrons, whereas chlorine’s 2p sublevel has only 5 electrons, as shown on the peaks at approximately 2 MJ/mol
d)
The dashed line peaks represent chlorine. This is true because argon has more protons than chlorine.
19.
A 10.0 L container has a [CuNO3] = 0.0002 M and a [Pb(NO3)2] = 0.01 M. When 0.009 moles NaBr is added to the container, according to the data in the table above, what will happen?
a)
only PbBr2 will precipitate
b)
only CuBr will precipitate
c)
both PbBr2 and CuBr will precipitate
d)
neither PbBr2 or CuBr will precipitate
20.
What can you conclude about the sign of ΔSo?
a)
ΔSo must be greater than zero because Δngas= -2
b)
ΔSo must be greater than zero because K > 1
c)
ΔSo must be less than zero because Δngas = -2
d)
ΔSo must be less than zero because K > 1
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