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Intermolecular forces (Chemical Bonding)

Total questions: 40

Worksheet time: 30mins

Name
Class
Date
1.

Identify the IMF exist in CH4

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

2.

Identify the IMF exist in NH3

a)

london dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

3.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

4.

Which of the following molecules is the weakest?

a)

F2

b)

H2O

c)

HCl

d)

SO2

5.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

6.

Forces that holds atoms together within the molecule

a)

intermolecular forces

b)

intramolecular forces

7.

Which of the following has the lowest boiling point?

a)

PH3

b)

H2O

c)

BF3

d)

NH3

8.
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.
9.
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
10.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

11.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

12.

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

a)

higher

b)

lower

13.

Which of the following compounds can form intermolecular hydrogen bonds?

a)

CH4

b)

CH3-O-CH3

c)

CH3OH

d)

HCN

14.

The effect of hydrogen bonding can be observed from the following phenomena EXCEPT

a)

Solubility of NH3 in water

b)

Density of ice is lower than water

c)

Boiling point of CH3OH is lower than CH3CH2OH

d)

Vapour pressure of CH4 is higher than H2O

15.

Arrange the following compounds in the order of increasing boiling points: HF, HCl, Cl2

a)

HCl < HF < Cl2

b)

HCl < Cl2 < HF

c)

HF < HCl < Cl2

d)

Cl2 < HCl < HF

16.

Boiling points of Br2 and I2 are 58.8oC and 184.3oC respectively. The difference in the boiling points of these molecules is due to

a)

Molecular size

b)

Molecular shape

c)

Molecular polarity

d)

Molecular formula

17.

Factor (s) that influence(s) the value of boiling points of simple covalent molecules with comparable relative molecular mass is/are

a)

molecular geometry

b)

polarity of molecule

c)

types of intermolecular forces

18.

What is the basis of hydrogen bond?

a)

Attraction forces between hydrogen atom bonded with another hydrogen atom

b)

Attraction forces between hydrogen atom bonded with a high electronegativity atom (F, O, N)

c)

Attraction forces between hydrogen atom bonded with a high electronegativity atom (F, O, N) with atom (F, O, N) of another molecule

d)

Attraction forces between hydrogen atom with another hydrogen atom of another molecule

19.

The boiling points of water and ammonia are 373 K and 240 K respectively. The boiling point of water is higher than that of ammonia because

a)

oxygen is less electronegative than nitrogen

b)

the O-H bond in H2O is stronger than the N-H bond in NH3

c)

the hydrogen bonds between water molecules are stronger than the hydrogen bonds between ammonia molecules

d)

a water molecule has a larger size than an ammonia molecule

20.

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

21.

All matter can participate in London forces, but dipole-dipole and hydrogen bonding are so much stronger that when they are present, we can effectively ignore London forces. Which of these can ONLY participate in London forces?

a)

I2

b)

NH3

c)

OCl2

d)

CH3Cl

22.

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

a)

H2

b)

HCl

c)

Cl2

d)

Br2

23.

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

24.

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

a)

higher

b)

lower

25.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
26.

Which of the following explains the very 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

27.

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)

ion-dipole attractions

e)

dipole-induced dipole attractions

28.

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 forces

b)

dipole-dipole attractions

c)

hydrogen bonds

d)

dipole-induced dipole attractions

29.

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

a)

Br2

b)

P4

c)

I2

d)

PCl3

e)

CO

30.

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

31.

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

a)

1

b)

2

c)

3

d)

4

32.

The stronger the intermolecular forces of a substance, the _____________ the melting point.

a)

higher

b)

lower

33.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-dipole attraction

b)

Ion-dipole attraction

c)

Hydrogen bonds

d)

Covalent bond

e)

Ionic bond

34.

NH3 molecules can form...

(select all that apply)

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

35.

London forces are stronger in atoms or molecules with more electrons in the electron cloud, and weaker in atoms or molecules with fewer electrons in the electron cloud. Which of the following has the strongest London forces?

a)

F2

b)

Br2

c)

I2

d)

Cl2

36.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
37.

What type of intermolecular forces are due to the attraction between temporary dipoles and induced temporary dipoles?

a)

dipole-dipole

b)

hydrogen bond

c)

London forces

d)

ion-dipole

38.

Which of species does not exhibit hydrogen bonding among themselves?

a)

H2O

b)

HCl

c)

NH3

d)

CH3CH2OH

39.

How will the following molecule bond with itself?

a)

London forces

b)

Dipole-dipole

c)

Hydrogen bond

40.

The molar masses of C2H6, CH3OH and CH3F are very similar. How do their boiling points compare?

a)

C2H6 < CH3OH < CH3F

b)

CH3F < CH3OH < C2H6

c)

CH3OH < CH3F < C2H6

d)

C2H6 < CH3F < CH3OH

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