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SBVC Chem 101 Ch 12 Quiz

Total questions: 64

Worksheet time: 1hrs 22mins

Name
Class
Date
1.
Which grouping lists the states of matter in order of increasing distance between particles?
a)
gas, liquid, solid
b)
liquid, solid, gas
c)
solid, gas, liquid
d)
solid, liquid, gas
2.
A gas has a no definite shape and ________.
a)
a definite shape
b)
a definite volume
c)
no definite shape
d)
no definite volume
3.
A liquid has no definite shape and ________.
a)
a definite shape
b)
a definite volume
c)
no definite shape
d)
no definite volume
4.
A solid has ________ and a definite volume.
a)
a definite shape
b)
a definite volume
c)
no definite shape
d)
no definite volume
5.

Changing from a liquid to a gas

a)

condensation

b)

vaporization

c)

sublimation

d)

melting

6.

Changing from a gas to a liquid

a)

condensation

b)

vaporization

c)

sublimation

d)

melting

7.

Changing directly from a solid to a gas

a)

condensation

b)

vaporization

c)

sublimation

d)

melting

8.
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 
9.

Strongest type of intermolecular force present in HF.

a)

dipole dipole

b)

dispersion

c)

H-bond

d)

ionic

10.

H2S has what strongest kind of intermolecular force?

a)

dipole dipole

b)

dispersion

c)

H-bond

d)

ionic

11.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
12.
Which of the following will take the longest to evaporate?
a)
CH3CH2OH
b)
CH3OH
c)
CH3CH3
13.

Strongest intermolecular force present in HCl?

a)

dipole dipole

b)

dispersion

c)

H-bond

d)

ionic

14.

Strongest intermolecular force present in Cl2?

a)

dipole dipole

b)

H-bond

c)

dispersion

d)

metallic

15.
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.
16.

The measure of the resistance to the flow of a liquid is called:

a)

vapor pressure.

b)

sublimation.

c)

viscosity.

d)

condensation.

17.

The tendency of a liquid to minimize its surface area is called:

a)

capillary action.

b)

viscosity.

c)

surface tension.

d)

vaporization.

18.

Which statement about boiling point is FALSE?

a)

The boiling point is higher for compounds with strong intermolecular forces.

b)

The boiling point is higher for compounds with a high viscosity.

c)

The boiling point of a compound is an absolute constant.

d)

The boiling point of a compound is higher for nonvolatile compounds

19.

Which intermolecular force is present in all molecules and atoms?

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

20.

Which intermolecular force is due to the formation of an instantaneous dipole?

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

21.

Which substance below has dispersion forces?

a)

CH4

b)

CO2

c)

F2

d)

H2S

e)

All above

22.

Which noble gas has the highest boiling point?

a)

Ne

b)

Ar

c)

Kr

d)

Xe

23.

Which molecule below has hydrogen bonding?

a)

CH4

b)

HCl

c)

H2

d)

CH3CH2OH

24.

Which compound in liquid form will have the highest vapor pressure?

a)

CH4

b)

CH3CH3

c)

CH3COCH3

d)

CH3CH2OH

25.

What types of forces exist between I2 molecules?

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

ion-dipole forces

26.

Which substance would be expected to have the highest boiling point?

a)

N2

b)

O2

c)

CO

d)

not enough information

27.
What line segment represents only the solid state?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
28.
In which segment is the kinetic energy remaining constant?
a)
A-B
b)
B-C
c)
C-D
d)
E-F
29.
What state(s) of matter are present at D-E?
a)
Solid-liquid
b)
Liquid
c)
Liquid-gas
d)
Gas-Solid
30.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
31.
True or false: melting and freezing occur at the same temperature!
a)
True
b)
False
c)
I don't know
32.
A substance's heating curve is shown in the graph.  What is its boiling point?
a)
100 C
b)
60 C
c)
80 C
d)
20 C
33.
In which region(s) of the graph does a phase change occur?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
34.
In which region(s) of the graph would the substance be a liquid and a gas?
a)
Region 2
b)
Region 3
c)
Region 4
d)
Region 5
35.

Which of these conditions is always true for an endothermic process?

a)

They leave the surroundings feeling hot

b)

They release energy into the surroundings.

c)

They absorb energy from the surroundings

d)

The reactants lose energy

36.

Which container will have a lower pressure?

a)

left

b)

right

c)

they both have the same pressure

37.
Which is an example of an ionic crystal?
a)
Quartz
b)
NaCl
c)
Ammonia
d)
Iron
38.
The Strongest intermolecular force is ...
a)
Dipole-Dipole
b)
Ionic
c)
Hydrogen Bonding
d)
London Dispersion
39.
Ionic bonds are between _______ and ________. 
a)
nonmetals and nonmetals 
b)
metals and metals 
c)
metals and nonmetals
d)
none
40.

Intermolecular forces are

a)

the relationship between protons and electrons of an element.

b)

the attraction between two molecules.

c)

the bond that two or more elements make.

d)

the reacting of elements.

41.

Which of these is not a type of intermolecular force?

a)

Dipole-Dipole

b)

Helium "Bonds"

c)

(London) Dispersion Forces

d)

Debye (Induced) Dipole

42.

Intermolecular forces are responsible for:

a)

the shape of protein molecules.

b)

the function of DNA.

c)

the existence of liquids and solids.

d)

all of the above

43.

Hydrogen bonding occurs when a hydrogen atom bonded to N, O, or F is attracted to another molecule's N, O or F atom. Which of the following can participate in hydrogen bonding?

a)

CBr4

b)

NO2

c)

H2S

d)

NH3

44.

All molecules can exhibit London dispersion forces, but dipole-dipole and hydrogen bonding are stronger attractions for molecules with similar masses/numbers of electrons when they are present. Which of these can ONLY exhibit London dispersion forces?

a)

I2

b)

NH3

c)

OCl2

d)

CH3Cl

45.

Dipole-dipole attractions occur between polar molecules. Which of these molecules is polar?

a)

H2

b)

HCl

c)

Cl2

d)

Br2

46.

A Lewis structure for acetone is shown above. (There is a carbon atom at the center that isn't shown) 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 dispersion forces

47.

The weaker the intermolecular forces of a substance, the _____________ the boiling point.

a)

higher

b)

lower

48.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
49.

Which of the following explains the relatively high melting and boiling point of water?

a)

Strong dipole-dipole attractions between water molecules

b)

Strong hydrogen bonds between water molecules

c)

London dispersion forces between water molecules

d)

Dipole-induced dipole attractions between water molecules

50.

London dispersion forces are stronger in more massive atoms or molecules, and weaker in less massive atoms or molecules. Which of the following has the strongest London dispersion forces?

a)

F2

b)

Br2

c)

I2

d)

Cl2

51.

Which of the following intermolecular forces can all types of particles exhibit?

a)

London dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

52.

A Lewis structure for carbon dioxide is shown below. What types of intermolecular attractions can be present between molecules of carbon dioxide in a pure CO2 sample? Select all that apply

a)

London dispersion forces

b)

dipole-dipole attractions

c)

hydrogen bonds

d)

ion-dipole attractions

53.

Which of these molecules can participate in dipole-dipole attractions? Select all that apply.

a)

Br2

b)

CF4

c)

I2

d)

PCl3

e)

CO

54.
Which of the following molecules would have the lowest boiling point?
a)
CH4
b)
C2H6
c)
C3H8
d)
C4H10
55.

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

56.

Which numbered arrow in the image above points to a hydrogen bond?

a)

1

b)

2

c)

3

d)

4

57.

What is the strongest type of intermolecular force one H2S molecule will exhibit?

a)

dipole-dipole attraction

b)

London dispersion forces

c)

H-bonds

d)

ionic bonds

58.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
59.

What is the strongest intermolecular force present between HCl molecules?

a)

dipole dipole attractions

b)

London dispersion forces

c)

H-bonds

d)

ionic bonds

60.

Which of the following would best remove Sharpie marker from your wall if this marker is known to be non-water soluble?

a)

salt water

b)

ammonia (nitrogen trihydride)

c)

acetone (finger nail polish remover)

d)

distilled water

61.

Which of the following is NOT a kind of intermolecular force?

a)

hydrogen bonding

b)

covalent bond

c)

London dispersion forces

d)

dipole-dipole attraction

62.
Which kinds of substances are held together by intermolecular forces?
a)
metallic substances
b)
ionic substances
c)
molecules (covalent) in solid and liquid phases
d)
molecules (covalent) in the gas phase
63.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
64.

Rank these in order of strength:

covalent bond

London dispersion 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

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