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AP Chemistry Full Unit 3 Review

Total questions: 181

Worksheet time: 5hrs 32mins

Name
Class
Date
1.

Which of the following substances contains both ionic and

covalent bonds?

a)

NH3

b)

CH4

c)

NaOH

d)

C2H5OH

2.

What type of bonding is found within a water molecule?

a)

ionic bonding

b)

polar covalent bonding

c)

nonpolar covalent bonding

d)

hydrogen bonding

3.

How many of the following molecules have a measurable dipole moment?

S03 CCl4 PF3 BH3

a)

1

b)

2

c)

3

d)

4

4.

Which best describes the bonding in the cyanide ion (CN-)?

a)

3 (sigma) bonds

b)

2 (sigma) bonds and I (pi) bond

c)

1 (sigma) bond and 2 (pi) bonds

d)

3 (pi) bonds

5.

Which bond is the most polar?

a)

F-O

b)

H-O

c)

Na -O

d)

Sn-O

6.

Which of the following compounds would have the highest lattice energy?

a)

LiF

b)

MgCl2

c)

CaBr2

d)

C2H6

7.

List ALL the Intermolecular forces that exist in PCl3

a)

hydrogen bonding, london dispersion

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole

d)

london dispersion

8.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

9.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

10.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

11.

P and V are ___________________ related?

a)

inversely

b)

directly

12.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

13.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

14.

Real gases behave most like an ideal gas at what conditions of temperature and pressure?

a)

High T, Low P

b)

High P, Low T

c)

High V, Low T

15.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

16.

When a molecular solid melts or boils, which bonds break?

a)

Intermolecular

b)

Intramolecular

17.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

18.

What type of alloy is made when the radii of one element are similar in size with the other element making up the alloy?

a)

interstitial

b)

substitutional

19.

The dashed line is a representation of a hydrogen bond.

a)

True

b)

False

20.

The dotted line is a representation of a hydrogen bond.

a)

True

b)

False

21.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

22.

Chromatography separates mixtures based on what property?

a)

particle size

b)

intermolecular forces

c)

boiling points

d)

state of matter

23.

In paper chromatography, if water is the mobile phase, what kind of substance will move up the farthest?

a)

polar substance

b)

non polar substance

24.

List the 4 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, ion-dipole, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, ion-dipole, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding, ion-dipole

d)

dipole dipole, hydrogen bonding, ion-dipole, london dispersion

25.

What type of solid will not conduct electricity until it is liquid or aqueous?

a)

Ionic Solid

b)

Covalent Network Solid

c)

Molecular Solid

d)

Metallic Solid

26.

What type of solid always conducts electricity?

a)

Ionic Solid

b)

Metallic Solid

c)

Covalent Network Solid

d)

Molecular Solid

27.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container

28.
Which of the following assumption of kinetic molecular theory describes why gases are extremely fluid?
a)
particles do  not attract or repel one another
b)
particles have elastic collisions
c)
gases are made of tiny particles that are far apart
d)
particles travel in straight line, continuous rapid, random motion
29.
Consider the lab station with the syringe probe. When the volume of air decreased what happened to pressure?
a)
pressure increased due to increased kinetic energy of each gas particle
b)
pressure increased due to the smaller volume and more collisions with the sides of the syringe
c)
molecules collided less due to the pressure decreased due to smaller volume  of molecules
d)
pressure increased because molecules were moving faster due to the increase number of molecules
30.
If container A is 10L and is under 5 atm of pressure and container B is 10L, but under 7 atm of pressure, what is true about the number of particles inside the containers?
a)
can not tell from the information
b)
they contain the same number of particles
c)
container A has less particles
d)
container B has less particles
31.
Which of the following is equivalent to 1,068kPa?
a)
7,516.45 mmHg
b)
7,814.2 torr
c)
155.0 psi
d)
11.3 atm
32.

Gases generally have

a)

low density

b)

high density

c)

closely packed particles

d)

no increase in volume when temperature is increased

e)

no decrease in volume when pressure is increased

33.

Pressure is

a)

defined as the mass that an object exerts when at rest

b)

measured in Newtons

c)

defined as the number of moles of substance divided by the mass of the substance

d)

defined as the force per unit area

e)

measured in grams

34.

A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.42 L.

a)

312K

b)

278K

c)

20.4K

d)

295K

e)

552K

35.

A balloon has a volume of 2.32 liters at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon.

a)

2.32L

b)

2.51L

c)

2.15L

d)

4.64L

e)

1.16L

36.

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?

a)

H2

b)

He

c)

Ne

d)

O2

e)

All have the same volume.

37.

According to kinetic molecular theory, in which of the following gases will the root mean square speed of the molecules be the highest at 200ºC?

a)

SF6

b)

H2O

c)

HCl

d)

Cl2

e)

None, the molecules of all gases have the same root mean square speed at any given temperature.

38.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

39.

A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ___L at 423 K and 1.00 atm.

a)

0.709 L

b)

57.9 L

c)

41.1 L

d)

81.6 L

e)

1.41 L

40.

The density of N2O at 1.52 atm and 45.2ºC is ____ g/L.

a)

0.388 g/L

b)

2.58 g/L

c)

9.99 g/L

d)

1.76 g/L

e)

18.2 g/L

41.

The volume of a sample of gas (2.49 g) is 752 mL at 1.98 atm and 62ºC. What is the gas?

a)

NO2

b)

SO3

c)

SO2

d)

Ne

e)

NH3

42.

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide and 3.33 g of argon; all at 42ºC is ____ mmHg.

a)

116 mmHg

b)

395 mmHg

c)

134 mmHg

d)

263 mmHg

e)

0.347 mmHg

43.

According to kinetic molecular theory, in which of the following gases will the root mean square speed of the molecules be the highest at 200ºC?

a)

SF6

b)

H2O

c)

HCl

d)

Cl2

e)

None, the molecules of all gases have the same root mean square speed at any given temperature.

44.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
45.
Which of the following assumption of kinetic molecular theory describes why gases are extremely fluid?
a)
particles do  not attract or repel one another
b)
particles have elastic collisions
c)
gases are made of tiny particles that are far apart
d)
particles travel in straight line, continuous rapid, random motion
46.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
47.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
48.
You have a 0.5 M MgSO4 stock solution available.  Calculate the volume of the stock solution needed to make 2.0 L of 0.20 M MgSO4.
a)
0.8 L
b)
5 L 
c)
0.1 L
d)
0.5 L
49.
What are the values for STP?
a)
0 K and 1 atm
b)
0oC and 1 atm
c)
760 K and 1 atm
d)
273oC and 1 atm
50.
A student extracts the colour from some green smarties and uses paper chromatography to separate components colours. She finds blue has a Rf =0.38 and yellow Rf =0.75 this suggests 
a)
the yellow is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
b)
the yellow is more strongly adsorbed onto the stationary phase and is more soluble in the mobile phase.
c)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
d)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
51.
A high Rf value indicates strong
a)
strong affinity to the stationary phase
b)
strong affinity to the mobile phase
c)
no affinity to the stationary phase
d)
 no affinity to the stationary phase
52.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
53.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
54.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
55.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
56.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
57.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
58.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

59.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

60.

Which type of spectrum is this?

a)

Emission Spectrum

b)

Absorption Spectrum

c)

Continuous Spectrum

61.

Gases generally have

a)

low density

b)

high density

c)

closely packed particles

d)

no increase in volume when temperature is increased

e)

no decrease in volume when pressure is increased

62.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
63.

According to kinetic molecular theory, in which of the following gases will the root mean square speed of the molecules be the highest at 200ºC?

a)

SF6

b)

H2O

c)

HCl

d)

Cl2

e)

None, the molecules of all gases have the same root mean square speed at any given temperature.

64.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

65.

A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ___L at 423 K and 1.00 atm.

a)

0.709 L

b)

57.9 L

c)

41.1 L

d)

81.6 L

e)

1.41 L

66.

The volume of a sample of gas (2.49 g) is 752 mL at 1.98 atm and 62ºC. What is the gas?

a)

NO2

b)

SO3

c)

SO2

d)

Ne

e)

NH3

67.

How are pressure and temperature related?

a)

Directly

b)

Indirectly

c)

They aren't related

68.

A dissolved solute that does not form ions is

a)

a nonelectroyte

b)

a weak electrolyte

c)

a strong electrolyte

d)

insoluble

69.

Which does not affect the rate at which a solid solute dissolves?

a)

the vapor pressure of the solvent

b)

the temperature of the solvent

c)

the surface area of the solid

d)

the speed at which the solution is stirred

70.

Which of the following occurs as temperature increases?

a)

solubility decreases

b)

solubility increases

c)

solubility remains the same

d)

molarity doubles

71.

At 333 K, which of the pairs of gases below would have the most nearly identical rates of effusion?

a)

CO and CO2

b)

CO and N2

c)

NO2 and N2O4

d)

N2O and NO2

e)

N2 and O2

72.

What is the pressure in a container that has 3 atm H2, 2 atm of N2 and 5 atm of F2?

a)

2 atm

b)

3 atm

c)

5 atm

d)

10 atm

73.
The conditions under which real gases most resemble ideal gases are 
a)
low pressure & high temperature
b)
low pressure & low temperature
c)
high pressure & high temperature
d)
high pressure & low temperature
74.

The shape of a liquid's meniscus is determined by ____.

a)

the viscosity of the liquid

b)

the type of material the container is made of

c)

the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container

d)

the amount of hydrogen bonding in the liquid

75.

Which type of solid typically has the lowest melting point of the four types of crystals?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

76.
Which of these typically increases when IMF's increase?
a)
boiling point
b)
melting point
c)
viscosity
d)
all of these 
77.

Chromatography separates solutions on the basis of _____ while distillation separates solutions on the basis of ______.

a)

IMFs; solubility

b)

solubility; conductivity

c)

IMFs; boiling point

d)

boiling point; solubility

78.

Which of the following will be the least soluble in water?

a)

CH3CH2CH2OH

b)

CH3OH

c)

CH3CH2OH

d)

None of them are soluble in water.

e)

They are all equally soluble in water.

79.

How can you increase the solubility of a gas in a liquid?

a)

Decrease the IMFs between the gas the and the liquid.

b)

Increase the temperature of the solution.

c)

Increase the pressure of the solution.

d)

All of these would work.

80.

In general, how could you increase the solubility of a solid in a liquid?

a)

Increase the pressure.

b)

Decrease the pressure.

c)

Increase the temperature.

d)

Decrease the temperature.

81.

A photon is a (a)   of light

82.

If the frequency of electromagnetic radiation is high, then the wavelength will be (a)  

83.
Which of the following assumption of kinetic molecular theory describes why gases are extremely fluid?
a)
particles do  not attract or repel one another
b)
particles have elastic collisions
c)
gases are made of tiny particles that are far apart
d)
particles travel in straight line, continuous rapid, random motion
84.
A student extracts the colour from some green smarties and uses paper chromatography to separate components colours. She finds blue has a Rf =0.38 and yellow Rf =0.75 this suggests 
a)
the yellow is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
b)
the yellow is more strongly adsorbed onto the stationary phase and is more soluble in the mobile phase.
c)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
d)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
85.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
86.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
87.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
88.
What is the Energy of a blue light with the frequency of 6.91x1014Hz? (E=hv)
a)
4.56x1049J
b)
9.55x10-49J
c)
4.56x10-19J
d)
5.82x1019J
89.
What best explains the difference in melting points between Cl2 (-101.5) and F2 (-219)?
a)
Increased mass (polarizability) of chlorine
b)
Increased electronegativity of fluorine
c)
Increased number of electrons in chlorine
d)
Decrease metallic character of fluorine
90.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
91.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
92.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
93.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

94.

A balloon has a volume of 2.32 liters at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon.

a)

2.32L

b)

2.51L

c)

2.15L

d)

4.64L

e)

1.16L

95.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

96.

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide and 3.33 g of argon; all at 42ºC is ____ mmHg.

a)

116 mmHg

b)

395 mmHg

c)

134 mmHg

d)

263 mmHg

e)

0.347 mmHg

97.

Carbon dioxide, CO2, has the following bonding:

a)

lattice of positive and negative ions held together by electrostatic forces

b)

closely packed lattice with delocalized electrons throughout

c)

strong single covalent bonds with weak intermolecular forces

d)

strong multiple covalent bonds with weak intermolecular forces

98.

Of the following molecules, which is the most polar?

a)

CO

b)

CO2

c)

O2

d)

HF

e)

F2

99.

Which of the following has the lowest melting point?

a)

Zn

b)

SiO2

c)

CaCl2

d)

C2H6

100.

Which of the following probably has the highest solubility in hexane, C6H14?

a)

Metals

b)

Polar covalent molecules

c)

Ionic compounds

d)

Nonpolar covalent molecules

101.

Copper (II) nitride, Cu3N2, has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

102.

Ethane, C2H6, has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

103.

Which of the following is most likely to be soluble in water?

a)

NaF

b)

C12H22O

c)

Mn

d)

Cl2

104.

A dissolved solute that does not form ions is

a)

a nonelectroyte

b)

a weak electrolyte

c)

a strong electrolyte

d)

insoluble

105.

List ALL the Intermolecular forces that exist in PCl3

a)

hydrogen bonding, london dispersion

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole

d)

london dispersion

106.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

107.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

108.

P and V are ___________________ related?

a)

inversely

b)

directly

109.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

110.

Real gases behave most like an ideal gas at what conditions of temperature and pressure?

a)

High T, Low P

b)

High P, Low T

c)

High V, Low T

111.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

112.

The dashed line is a representation of a hydrogen bond.

a)

True

b)

False

113.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

114.

Chromatography separates mixtures based on what property?

a)

particle size

b)

intermolecular forces

c)

boiling points

d)

state of matter

115.

In paper chromatography, if water is the mobile phase, what kind of substance will move up the farthest?

a)

polar substance

b)

non polar substance

116.

List the 4 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, ion-dipole, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, ion-dipole, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding, ion-dipole

d)

dipole dipole, hydrogen bonding, ion-dipole, london dispersion

117.

What type of solid will not conduct electricity until it is liquid or aqueous?

a)

Ionic Solid

b)

Covalent Network Solid

c)

Molecular Solid

d)

Metallic Solid

118.

Copper (II) nitride, Cu3N2, has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

119.

Ethane, C2H6, has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

120.

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

a)

0.13 atm

b)

0.27 atm

c)

0.63 atm

d)

0.90 atm

121.

Which of the following typically has the lowest melting point?

a)

Metals

b)

Covalent network solids

c)

Ionic compounds

d)

Molecular solids

122.

Sodium chloride (NaCl) can dissolve in polar solvents such as H2O due to what intermolecular forces?

a)

Ionic

b)

Ion-Dipole

c)

Hydrogen Bonding

d)

Dipole-dipole

123.

What types of intermolecular force present in hydrogen chloride (HCl)?

a)

dipole dipole

b)

london dispersion

c)

hydrogen bonding

d)

ion-dipole

124.

What type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

hydrogen bonding

c)

london dispersion

d)

dipole induced dipole

125.

Which of these typically increases when intermolecular forces increase?

a)

Surface Tension

b)

Melting Point

c)

Viscosity

d)

All of these

126.

Which of the following has the highest melting point?

a)

H2

b)

NH3

c)

CO2

d)

MgCl2

127.

Under which conditions does a real gas behave very much like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and high pressure

d)

low temperature and low pressure

128.

According to kinetic molecular theory, in which of the following gases will the speed of the molecules be the highest at 200ºC?

a)

SF6

b)

H2O

c)

HCl

d)

Cl2

e)

None, the molecules of all gases have the speed at any given temperature.

129.

What best explains the difference in melting points between Cl2 (-101.5) and F2 (-219)?

a)

Increased # of electrons and polarizability of chlorine

b)

Increased electronegativity of fluorine

c)

Increased molar mass in chlorine

d)

Decrease metallic character of fluorine

130.

Which of the following has the highest solubility in hexane, C6H14?

a)

Metals

b)

Polar covalent molecules

c)

Ionic compounds

d)

Nonpolar covalent molecules

131.

A chromatography experiment uses water as a mobile phase. Which of the following would have the greatest affinity for the mobile phase?

a)

C2H5OH

b)

C2H6

132.

A mixture of butane (C4H12) and octane (C8H18) is separated using distillation. Which will be collected first?

a)

butane (C4H12)

b)

octane (C8H18)

133.

Which ionic compound (NaCl or MgS) will have a lower melting point and why?

a)

MgS will have lower melting point because the strength of the attraction between its 2+ ions and 2− ions are stronger than those between the ions in NaCl.

b)

NaCl will have a lower melting point because NaCl is a polar covalent compound whereas MgS is an ionic compound which has stronger attractive forces.

c)

NaCl will a lower melting point because the strength of the attraction between its +1 ion and -1 ion are weaker than those between the +2/-2 ions in MgS.

134.

Which statement best helps to explain the observation that NH3 boils at −28°C, whereas PH3 boils at −126°C?

a)

The dispersion forces in NH3 are weaker than the dispersion forces in PH3.

b)

The dispersion forces in NH3 are stronger than the dipole-dipole forces in PH3.

c)

NH3 has hydrogen bonding which is stronger than the dipole-dipole forces in PH3.

135.

A real gas has observable IMF at low temperatures. What will happen to the observed pressure compared to the ideal/predicted pressure?

a)

The real pressure will be less than the ideal pressure

b)

The real pressure will be more than the ideal pressure

c)

The real pressure will be the same as the ideal pressure

136.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The average kinetic energy of the gas particles depends on the kelvin temperature of the gas.

137.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

138.

Which of the following explains how the dispersion-force model of intermolecular attraction does not account for the unusually high boiling point of HF?

a)

F2 is soluble in water, whereas HF is insoluble in water.

b)

The F2 molecule has a greater mass than the HF

HF molecule has.

c)

Liquid F2 has weak dispersion force attractions between its molecules, whereas liquid has strong ionic interactions between H+ and F ions.

d)

Liquid F2 has weak dispersion force attractions between its molecules, whereas liquid HF has both weak dispersion force attractions and hydrogen bonding interactions between its molecules.

139.

Intermolecular forces between the gas molecules will cause them to condense into the liquid phase if the temperature is lowered. Which of the following best describes how the model is limited in its depiction of the phenomenon?

a)

It does not show how hydrogen bonds are constantly forming, breaking, and reforming, which results in a net force of attraction between the molecules.

b)

It does not show how the interactions between ions and the induced molecular dipoles result in a net force of attraction between the molecules.

c)

It does not show how the interacting permanent dipoles of the molecules result in a net force of attraction between the molecules.

d)

It does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force of attraction between the molecules.

140.

This form of boron nitride is one of the hardest substances known. Which of the following best helps explain why boron nitride is so hard?

a)

Boron ions and nitrogen ions are held together by ionic bonds.

b)

Boron nitride is a network solid of atoms connected by covalent bonds with fixed bond angles.

c)

Boron nitride is an alloy, and alloys are typically harder than the elements used to make them.

d)

Boron nitride is a polymer made of long chains of boron atoms and nitrogen atoms held together by dispersion forces.

141.

Compounds NaCl MgS, which statement correctly identifies diagram 1 and identifies the compound with the lower melting point.

a)

Diagram 1 represents MgS; it has a lower melting point than NaCl because the coulombic attractions between its doubly charged Mg 2+ ions and the S 2− ions are stronger than those between the ions in NaCl.

b)

Diagram 1 represents NaCl ; it has a lower melting point than MgS has because the coulombic attractions between the singly charged Na+ ions and the Cl− ions in NaCl

NaCl are stronger than those between the ions in MgS.

c)

Diagram 1 represents NaCl; it has a lower melting point than MgS because the coulombic attractions between its singly charged Na+ ions and the Cl− ions are weaker than those between the ions in MgS.

142.

Which statement best helps to explain the observation that NH3(l) boils at −28°C, whereas PH3(l) boils at −126°C?

a)

The dispersion forces in NH3 are weaker than the dispersion forces in PH3.

b)

The dispersion forces in NH3 are stronger than the dipole-dipole forces in PH3.

c)

NH3 has hydrogen bonding that is stronger than the dipole-dipole forces in PH3.

143.

Of the following, the best explanation for the fact that most gases are easily compressed is that the molecules in a gas

a)

are in constant motion

b)

are relatively far apart

c)

have relatively small masses

d)

have a real, nonzero volume

144.

A gas mixture at 0°C and 1.0atm contains 0.010mol

0.010mol of H2, 0.015mol of O2, and 0.025mol

0.025mol of N2. Assuming ideal behavior, what is the partial pressure of hydrogen gas (H2) in the mixture?

a)

About 0.20atm 0.20atm, because H2 comprises 20%

20% of the total number of moles of gas.

b)

About 0.050atm, because there is 0.050mol of gases at 0°C and 1.0atm.

c)

About 0.010atm, because there is 0.010mol

0.010mol of H2 in the sample.

145.

A 2 L container will hold about 4 g of which of the following gases at 0°C and 1 atm?

a)

SO2

b)

N2

c)

CO2

d)

C4H8

146.

A sample of an ideal gas is cooled from 50.0oC to 25.0oC in a sealed container of constant volume. Which of the following values for the gas will decrease?

I. The average molecular mass of the gas

II. The average distance between the molecules

III. The average speed of the molecules

a)

only I

b)

only II

c)

only III

d)

I and III

147.

A student uses visible spectrophotometry to determine the concentration of CoCl2(aq) in a sample solution. First the student prepares a set of CoCl2(aq) solutions of known concentration. Then the student uses a spectrophotometer to determine the absorbance of each of the standard solutions at a wavelength of 510nm and constructs a standard curve. Finally, the student determines the absorbance of the sample of unknown concentration.

The original solution used to make the solutions for the standard curve was prepared by dissolving 2.60g of

CoCl2 (molar mass 130.g/mol) in enough water to make 100.mL of solution. What is the molar concentration of the solution?

a)

.200 M

b)

.500 M

c)

1.00 M

d)

5.00 M

148.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
149.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
150.
You have a 0.5 M MgSO4 stock solution available.  Calculate the volume of the stock solution needed to make 2.0 L of 0.20 M MgSO4.
a)
0.8 L
b)
5 L 
c)
0.1 L
d)
0.5 L
151.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
152.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
153.
What is the Energy of a blue light with the frequency of 6.91x1014Hz? (E=hv)
a)
4.56x1049J
b)
9.55x10-49J
c)
4.56x10-19J
d)
5.82x1019J
154.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms only
d)
There is an attraction between the hydrogen and nitrogen atoms only
155.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
156.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
157.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
158.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

159.

1. Under which conditions does a real gas behave very much like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and high pressure

d)

low temperature and low pressure

160.

According to kinetic molecular theory, in which of the following gases will the root mean square speed of the molecules be the highest at 200ºC?

a)

SF6

b)

H2O

c)

HCl

d)

Cl2

e)

None, the molecules of all gases have the same root mean square speed at any given temperature.

161.

Which of the following has the lowest melting point?

a)

Zn

b)

SiO2

c)

CaCl2

d)

C2H6

162.

Which of the following probably has the highest solubility in water?

a)

Metals

b)

Covalent network solids

c)

Ionic compounds

d)

Covalent molecules

163.

Which of the following probably has the highest solubility in hexane, C6H14?

a)

Metals

b)

Polar covalent molecules

c)

Ionic compounds

d)

Nonpolar covalent molecules

164.

The density of an unknown gas is 2.00 grams per Liter at 3.00 atmosphere pressure and 127oC. What is the molar mass of this gas?

a)

(254/3) R

b)

188 R

c)

(800/3) R

d)

600 R

165.

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

a)

0.13 atm

b)

0.27 atm

c)

0.63 atm

d)

0.90 atm

166.

Chromatography separates solutions on the basis of _____ while distillation separates solutions on the basis of ______.

a)

IMFs; solubility

b)

solubility; conductivity

c)

IMFs; boiling point

d)

boiling point; solubility

167.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
168.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
169.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
170.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
171.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
172.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

173.

1. Under which conditions does a real gas behave very much like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and high pressure

d)

low temperature and low pressure

174.

Which of the following has the lowest melting point?

a)

Zn

b)

SiO2

c)

CaCl2

d)

C2H6

175.

Which of the following typically has the lowest melting point?

a)

Metals

b)

Covalent network solids

c)

Ionic compounds

d)

Covalent molecules

176.

Which of the following probably has the highest solubility in water?

a)

Metals

b)

Covalent network solids

c)

Ionic compounds

d)

Covalent molecules

177.

Ethane, C2H6, has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

178.

Which of the following is most likely to be soluble in water?

a)

NaF

b)

C12H22O

c)

Mn

d)

Cl2

179.

The density of an unknown gas is 2.00 grams per Liter at 3.00 atmosphere pressure and 127oC. What is the molar mass of this gas?

a)

(254/3) R

b)

188 R

c)

(800/3) R

d)

600 R

180.

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

a)

0.13 atm

b)

0.27 atm

c)

0.63 atm

d)

0.90 atm

181.

Chromatography separates solutions on the basis of _____ while distillation separates solutions on the basis of ______.

a)

IMFs; solubility

b)

solubility; conductivity

c)

IMFs; boiling point

d)

boiling point; solubility

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