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Chapter 11 Review for Test

Total questions: 55

Worksheet time: 39mins

Name
Class
Date
1.
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.
2.
Does HCl have hydrogen bonding?
a)
yes
b)
no
3.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
4.
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
5.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

6.

main intermolecular force for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

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.

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

a)

higher

b)

lower

9.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

10.
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
11.
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
12.
What forces will the following molecule have?
a)
dispersion
b)
dipole
c)
hydrogen bonding
13.

Which substance will have the highest vapor pressure? Hint: the weaker the intermolecular forces the faster it vaporizes.

a)

CH3CH2CH2CH2CH2CH3

b)

H2O

c)

CH4

d)

CH3F

14.

What is vapor pressure

a)

the amount of energy required to evaporate

b)

the amount of energy required to boil

c)

the force per unit area exerted by the gaseous layer above a liquid

d)

the force per unit area exerted by a liquid on the gaseous layer above it

15.
a)

CRYSTALLINE

b)

AMORPHOUS

16.
a)

CRYSTALLINE

b)

AMORPHOUS

17.
a)

CRYSTALLINE

b)

AMORPHOUS

18.

This type of soilds have ordered internal structures.

a)

Crystalline solids

b)

Amorphous solids

c)

Pseudo solids

d)

Supercooled liquids

19.

It is the smallest repeating structure of solids

a)

Unit cell

b)

lattice

c)

crystal

d)

cell

20.

It is the network formed from the combination of unit

cells.

a)

Unit cell

b)

Crystal Lattice

c)

Shape

d)

Rigidity

21.

What is an amorphous solid?

a)

Solid that does not has ordered internal structure

b)

Solid that has a crystal lattice

c)

Solid that cannot change its state

22.

Halite is a crystalline solid. Which means

a)

Its structure is not symmetrical

b)

It exhibits isotropy

c)

It can be compressed

d)

It has a sharp melting point

23.

What does it mean when a solid has a sharp melting point?

a)

It will turn into a gaseous state at a defined value of temperature

b)

It will melt over a range of temperature

c)

It will completely melt at a fixed value of temperature

d)

It will have sharp edges before it turns to liquid

24.

An amorphous solid has a definite melting point.

a)

True

b)

False

25.

An allotrope is defined as _____.

a)

different forms of a pure element

b)

different forms of two different elements

c)

similar forms of different elements

d)

two pure elements bonded together

26.

Which of the following allotropes of carbon can be used to cut glass?

a)

graphite

b)

graphene

c)

buckyball

d)

diamond

27.

Surface tension is the property of water in which...

a)

water molecules at the surface tend to stick together.

b)

water spills easily.

c)

water tends to be see-through.

28.

Refer to the picture of water sticking to a leaf; this is occurring because of:

a)

Adhesion

b)

Cohesion

29.

Describe COHESION.

a)

Water molecules attracted to other substances.

b)

Water molecules climbing upwards against the force of gravity.

c)

Water molecules dissolving many substances because of its polarity.

d)

Water molecules attracted to other water molecules.

30.
Which characteristic of water will allow a paperclip to remain floating on water when the paperclip is gently placed on top of the water?
a)
adhesion
b)
surface tension
c)
solvent properties
d)
nonpolar
31.
Rain drops are spherical in shape because of
a)
low temperature
b)
Surface Tension
c)
Viscosity
d)
External forces
32.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
33.
What state of matter is X?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
34.
What state of matter is Y?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
35.
What state of matter is Z?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
36.
What change occurs from F to E?
a)
sublimation
b)
deposition
c)
melting
d)
condensation
37.
What change occurs from E to C?
a)
sublimation
b)
freezing
c)
melting
d)
boiling
38.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
39.

What is the normal melting point of this substance at standard pressure?

a)

150 °C

b)

100 °C

c)

-50 °C

d)

0 °C

40.
What is point A?
a)
triple point
b)
critical point
c)
equilibrium point
d)
normal melting point
41.
At 0.10 atm, what phase(s) can exist?
a)
solid, liquid or gas
b)
liquid or gas
c)
solid only
d)
gas only
42.
Water exists as a _____________ at 3 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
43.
Which phase change increases the molecule's freedom of movement?
a)
Melting
b)
Freezing
c)
Condensing
44.

What happens to molecules when the temperature drops or lowers?

a)

The molecules get closer together

b)

The molecules start moving faster.

c)

The molecules stop moving.

d)

The molecules become smaller.

45.

A substance has a melting point of 25 oC and a boiling point of 235 oC. What state is it at 5oC?

a)

Solid

b)

Liquid

c)

Gas

46.

A substance has a melting point of -125 oC and a boiling point of -35 oC. What state is it at 15oC?

a)

Solid

b)

Liquid

c)

Gas

47.

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

a)

higher

b)

lower

48.

What are the intermolecular forces for CF4CF_4 ?

a)

dispersion

b)

dispersion and dipole-dipole

c)

dispersion, dipole-dipole, and hydrogen bonding

d)

ionic bonding

49.

What are the intermolecular forces for CHBr3CHBr_3 ?

a)

dispersion

b)

dispersion and dipole-dipole

c)

dispersion, dipole-dipole, hydrogen bonding

d)

ionic bonding

50.

What are the intermolecular forces for CH3OHCH_3OH ?

a)

dispersion

b)

dispersion, dipole-dipole

c)

dispersion, dipole-dipole, hydrogen bonding

d)

ionic bonding

51.

Molecule A has a low melting point. It is likely

a)

polar and has dipole-dipole IMFs

b)

non-polar and has strong dispersion forces

c)

non-polar and weak dispersion forces

d)

polar and has hydrogen bonds

52.

Match the following

a)

vaporization

1.

liquid to gas at any temperature

b)

evaporation

2.

liquid to gas below the boiling point

c)

boiling

3.

vaporization at the boiling point

d)

condensation

4.

gas to liquid

e)

deposition

5.

gas to solid

53.

In order to ​ ​ (a)   , vapor pressure must equal​ (b)   .

Choose from the below words
boil
atmospheric pressure
evaporate
sublimate
condense
54.

Lattice energy is always ...........

a)

endothermic

b)

exothermic

c)

can be both endothermic or exothermic

55.

Lattice energy is the energy​ (a)   when gas particles form crystals.

Choose from the below words
released
gained

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