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Unit 3 AP Chemistry Quiz

Total questions: 50

Worksheet time: 13hrs 30mins

Name
Class
Date
1.

Polar molecules have

a)

no charges.

b)

positive and negative charges on opposite ends of the molecules.

c)

only positive charges.

d)

either positive or negative charges, but not both.

2.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
3.

This is an example of a(n) __________.

a)

Hydrogen Bonding

b)

Dipole

c)

Nonpolar Molecule

d)

Intermolecular Force

4.

If fluorine has a higher electronegativity value than carbon, what charge will the fluorine receive?

a)

negative

b)

partial negative

c)

positive

d)

partial positive

5.

Intramolecular forces are the forces

a)

within molecules

b)

between molecules

6.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
7.

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

8.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

9.
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
10.

A Lewis structure for acetone is shown above. What type of intermolecular forces will be present between the molecules of acetone in a pure sample of acetone? Select all that apply.

a)

ion-dipole attractions

b)

dipole-dipole attractions

c)

hydrogen bonding

d)

London forces

11.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
12.

Which of the following intermolecular forces can all types of matter participate in?

a)

London dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

13.

Propane is a gas at room temperature, while bromine is a liquid at room temperature. Which statement correctly explains these observations?

a)

Bromine has weaker intermolecular forces than propane does

b)

Bromine has greater molecular polarity than propane does

c)

Bromine has weaker molecular polarity than propane does

d)

Bromine has stronger intermolecular forces than propane does

14.

Which intermolecular force increases with increasing molar mass?

a)

London forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

15.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
The same
16.

Which force is only found between polar covalent molecules?

a)

Ionic bond

b)

Dipole Dipole

c)

London Dispersion Force

d)

Covalent bond

17.

In this force type, electron movement causes a slight charge at a single instant (known as a wobble). This charge is temporary.

a)

Hydrogen bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

18.

All polar covalent molecules contain:

(Check all that apply)

a)

Hydrogen bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

19.

Which state of matter has a high density (tightly packed particles) and an indefinite shape?

a)

solids

b)

liquids

c)

gases

d)

both solids and liquids

20.
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.
21.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
22.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
23.
If the temperature of a gas increase, the pressure...
a)
Decreases
b)
Increases
c)
Does not change
24.
Consider a sample of oxygen gas at 27° C with a volume of 9.55L at a pressure if 2.97 atm.  The pressure is changed to 8.25 atm and the gas is heated to 125° C.  What’s the new volume? 
a)
4.56 L
b)
4.6 L
c)
15.9 L
d)
16 L
25.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
26.
A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be if it is lowered to a pressure of 0.658 atm and the temperature remains constant?
a)
72 mL
b)
144 mL
c)
216 mL
d)
288 mL
27.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
28.

A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory is known as

a)

real gas

b)

ideal gas

c)

imaginary gas

d)

perfect gas

29.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

30.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

31.

Electrolytes

a)

don't conduct electricity

b)

conduct electricity

32.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

33.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
34.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
35.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
36.

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.

a)

0.08 M

b)

12.5 M

c)

1.37 M

d)

0.74 M

37.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

38.
How many grams of calcium hydroxide are needed to produce 500. ml of 1.66 M calcium hydroxide solution?
 (M = mol solute/ L solution)
a)
38.7 g
b)
61.5 g
c)
94.0 g
d)
19.7 g
39.

How many liters 0.110 M nitric acid can be prepared by diluting 5.00 mL of 15.3 M stock solution?

a)

1530 mL

b)

1.53 L

c)

0.0654L

d)

0.153 L

40.

Under which conditions is a gas most likely to behave ideally?

a)

low pressure and high temperature

b)

low temperature and high pressure

c)

just high pressure

d)

just low temperature

41.

What happens to a real gas at low temperatures that makes it behave less ideally?

a)

particles have less energy and so exert less pressure on the container

b)

particles have more energy and so exert more pressure on the container

c)

volume of container decreases so particles occupy significant volume

d)

volume of container increases so particles occupy significant volume

42.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
43.
Which electromagnetic waves have the highest frequencies and the shortest wavelengths?
a)
microwaves
b)
visible light
c)
gamma rays
44.

Which color has the longest wavelength?

a)

Red

b)

Orange

c)

Yellow

d)

Blue

45.

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

46.

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

47.
What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?
a)
0.488 M
b)
7.66 M
c)
7.67 M
d)
0.00767 M
48.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
49.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

50.

Which intermolecular force is most notable in noble gases, and non-polar molecules?

a)

London dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

gravitational forces

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