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IMF AP Chemistry Review

Total questions: 28

Worksheet time: 23mins

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.
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.
Does H2O have hydrogen bonding?
a)
yes
b)
no
4.
Does HF have hydrogen bonding?
a)
yes
b)
no
5.
Does HCl have hydrogen bonding?
a)
yes
b)
no
6.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
7.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
8.
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
9.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

10.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

11.
Determine the type of intermolecular force present in SiO2.
a)
dipole dipole
b)
dispersion
c)
ionic
d)
covalent network
12.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
13.

Which type of IMF is pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

14.

Rank these in order of strength:

covalent bond

dispersion force

hydrogen bond

dipole-dipole attraction

a)

dipole-dipole > covalent bond > hydrogen bond > dispersion

b)

dispersion > dipole-dipole > hydrogen bond > covalent bond

c)

covalent bond > hydrogen bond > dipole-dipole > dispersion

d)

hydrogen bond > dipole-dipole > dispersion > covalent bond

15.

Which line segment represents ONLY the solid state?

a)

A-B

b)

B-C

c)

C-D

d)

D-E

16.

Which molecule will have hydrogen bonds with other molecules in the sample?

a)

a) CO2

b)

b) HCN

c)

c) C2H2

d)

none of the above

17.

Crystalline solids _____

a)

have their particles arranged randomly

b)

have highly ordered structures

c)

are usually very soft

d)

exist only at high temperatures

18.

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

19.

Which type of solid has mobile electrons in the crystal (sea of electrons)?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

20.

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

21.

Which type of solid has strong covalent bonds between neighboring atoms?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

22.

Which is an example of an ionic crystal?

a)

SiO2

b)

NaCl

c)

SO3

d)

Li

23.

Which is an example of a molecular crystal?

a)

SiO2

b)

NaCl

c)

NH3

d)

Mg

24.

Which is an example of an covalent network crystal?

a)

SiO2

b)

NaCl

c)

NH3

d)

Fe

25.

What is the name of the three-dimensional pattern that forms when ions bond?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

an ionic chalice

26.
Which of these typically increases when IMF's increase?
a)
boiling point
b)
melting point
c)
viscosity
d)
all of these 
27.
When the atmospheric pressure equals the equilibrium vapor pressure ___ occurs.
a)
freezing
b)
melting
c)
boiling
d)
sublimation
28.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

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