wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

AP Chemistry Unit 3

Total questions: 65

Worksheet time: 2hrs 58mins

Name
Class
Date
1.

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.

2.

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

3.

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

4.

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

5.

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

6.
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
7.
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
8.

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

9.
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
10.

How are pressure and temperature related?

a)

Directly

b)

Indirectly

c)

They aren't related

11.
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
12.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

13.
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.
14.

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

15.
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
16.
Which of these typically increases when IMF's increase?
a)
boiling point
b)
melting point
c)
viscosity
d)
all of these 
17.

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

18.
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
19.

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

20.

Which of the following occurs as temperature increases?

a)

solubility decreases

b)

solubility increases

c)

solubility remains the same

d)

molarity doubles

21.
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.
22.
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
23.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
24.
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
25.
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
26.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
27.

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.

28.

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.

29.

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.

30.
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.
31.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
32.

A photon is a (a)   of light

33.

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

34.

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

35.

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

36.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

37.

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

38.

The dashed line is a representation of a hydrogen bond.

a)

True

b)

False

39.

The dotted line is a representation of a hydrogen bond.

a)

True

b)

False

40.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

41.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

42.

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

43.

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

a)

Intermolecular

b)

Intramolecular

44.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container

45.

P and V are ___________________ related?

a)

inversely

b)

directly

46.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

47.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

48.

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

49.

Of the following molecules, which is the most polar?

a)

CO

b)

CO2

c)

O2

d)

HF

e)

F2

50.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
51.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
52.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
53.
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 
54.
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.
55.
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
56.
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
57.

Consider a sample of helium gas in a container fitted with a piston, as pictured below. The piston is frictionless, but has a mass of 10.0 kg. How many of the following processes will cause the piston to move away from the base and decrease the pressure of the gas? Assume ideal behavior.

I. heating the helium

II. removing some of the helium from the container

III. turning the container on its side

IV. decreasing the pressure outside the container

a)

0

b)

1

c)

2

d)

3

e)

4

58.
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
59.

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

60.

NH4NO3(s) → N2O(g) + 2 H2O(g)


A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? ( The value of the gas constant, R, is 0.082 L atm mol–1 K–1)

a)

3 atm

b)

1 atm

c)

0.5 atm

d)

0.1 atm

61.

1. Liquids are more ordered than gases because liquids have ?

a)

Weaker Intermolecular Forces And Lower Mobility Of The Particles

b)

stronger intermolecular forces and lower mobility of the particles.

c)

weaker intermolecular forces and greater mobility of the particles

d)

stronger intermolecular forces and greater mobility of the particles

62.
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
63.

Absorbing microwave radiation is associated with changes in

a)

molecular rotation (molecules changing spin)

b)

molecular vibration (temporary changes in bond length or angles)

c)

electronic energy levels (electrons changing orbitals)

d)

No changes

64.

Absorbing infrared radiation is associated with changes in

a)

molecular rotation (molecules changing spin)

b)

molecular vibration (temporary changes in bond length or angles)

c)

electronic energy levels (electrons changing orbitals)

d)

No changes

65.

Absorbing UV radiation or visible light is associated with changes in

a)

molecular rotation (molecules changing spin)

b)

molecular vibration (temporary changes in bond length or angles)

c)

electronic energy levels (electrons changing orbitals)

d)

No changes

Similar Resources on Wayground

ALKANE - ĐỒNG ĐẲNG, Đ PHÂN, DANH PHÁP

60 questions

ALKANE - ĐỒNG ĐẲNG, Đ PHÂN, DANH PHÁP

quiz

Worksheet

•

11th Grade

Measurement and The Atom Quiz Review

70 questions

Measurement and The Atom Quiz Review

quiz

Worksheet

•

9th - 12th Grade

Sig Fig and Measurement Practice

61 questions

Sig Fig and Measurement Practice

quiz

Worksheet

•

9th - 12th Grade

8.1 ALOI

63 questions

8.1 ALOI

quiz

Worksheet

•

11th - 12th Grade

Atom Models and Quarks

67 questions

Atom Models and Quarks

quiz

Worksheet

•

11th Grade

Chemistry Chapter 3 Practice Test

63 questions

Chemistry Chapter 3 Practice Test

quiz

Worksheet

•

11th Grade

Interim Assessment Review

62 questions

Interim Assessment Review

quiz

Worksheet

•

12th Grade