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Review: Ch. 10 Intermolecular Forces

Total questions: 63

Worksheet time: 5hrs 53mins

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.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, ion-dipole

b)

hydrogen bonding, london dispersion

c)

ion-dipole, london dispersion

8.

Hydrogen bonding is a special case of __________.

a)

london dispersion

b)

ion-dipole

c)

dipole-dipole

9.

Which of the following has the lowest boiling point?

a)

PH3

b)

H2O

c)

SiH4

d)

NH3

10.

Forces that holds molecules together

a)

intramolecular forces

b)

intermolecular forces

11.

NH3 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

12.

BH3 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

13.

SO2 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

14.

HF molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

15.

HCl molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

16.

BeCl2 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

17.

CH4 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

18.

CH3Cl molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

19.

CH2Cl2 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

20.

Which one has the highest boiling point?

a)

CH4

b)

SO2

c)

H2O

21.

Which one has the highest boiling point?

a)

BeCl2

b)

CO2

c)

SF4

22.

Factor(s) that influence the strength of London dispersion forces

a)

Molecular size

b)

Molecular shape

c)

Molecular polarity

23.

Which of the following non-polar molecules has the highest boiling point? (Recall, increasing molar mass means either more atoms or larger atoms. This will change the number of electrons present in the electron cloud.)

a)

CH4; molar mass = 16.04 g/mol

b)

CCl4; molar mass = 153.82 g/mol

c)

PF5; molar mass = 125.966 g/mol

d)

Rn; molar mass = 222.01758 g/mol

24.

H2O and NH3 are polar molecules that can form the strongest type of intermolecular force (hydrogen bonding). However, the boiling point of H2O is 100.00 °C whereas NH3 is -33.34 °C.

Why is that so?

a)

H2O can form more hydrogen bonds than NH3

b)

H2O can form less hydrogen bonds than NH3

c)

O on the H2O is more electronegative than N on the NH3

25.

Between HF and H2O... which one has a higher boiling point?

a)

H2O

b)

HF

26.

Select the species that is/are soluble in water.

a)

CH4

b)

BeCl2

c)

CO2

d)

NH3

e)

HF

27.

Why do the ice cubes float on liquid water?

a)

Due to the "open structure" of the arrangement of water molecules when cooled.

b)

Due to the "extensive structure" of the arrangement of water molecules when cooled.

c)

Due to the "open structure" of the arrangement of air when water is cooled.

28.

H2O and NH3 are polar molecules that can form the strongest type of intermolecular force (hydrogen bonding). However, the boiling point of H2O is 100.00 °C whereas NH3 is -33.34 °C.

Why is that so?

a)

H2O can form more hydrogen bonds than NH3

b)

H2O can form less hydrogen bonds than NH3

c)

O on the H2O is more electronegative than N on the NH3

29.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

30.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

31.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

32.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

33.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
34.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
35.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
36.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
37.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
38.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
39.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
40.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
41.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
42.

What is the molecular geometry for this molecule?

a)

Bent

b)

Trigonal pyramidal

c)

Trigonal planar

d)

Linear

43.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
44.

what is the intermolecular forces in H2 ?

a)

London dispersion forces

b)

Dipole - Dipole

c)

Hydrogen bonding

d)

covalent bonding

45.

what is the intermolecular forces in CH4 ?

a)

London dispersion forces

b)

Dipole - Dipole

c)

Hydrogen bonding

d)

covalent bonding

46.

what is the intermolecular forces in H2O ?

a)

London dispersion forces

b)

Dipole - Dipole

c)

Hydrogen bonding

d)

covalent bonding

47.

what is the intermolecular forces in NH3 ?

a)

London dispersion forces

b)

Dipole - Dipole

c)

Hydrogen bonding

d)

covalent bonding

48.

what is the intermolecular forces in HCl ?

a)

London dispersion forces

b)

Dipole - Dipole

c)

Hydrogen bonding

d)

covalent bonding

49.

what is the intermolecular forces in HF?

a)

London dispersion forces

b)

Dipole - Dipole

c)

Hydrogen bonding

d)

covalent bonding

50.

Which of the following has the highest boiling point?

a)

H2

b)

F2

c)

Cl2

d)

O2

51.

Which of the following has the lowest boiling point?

a)

H2

b)

F2

c)

Cl2

d)

O2

52.

Which of the following didn't have hydrogen bonding?

a)

protein

b)

DNA

c)

H2O

d)

amino acids

53.

Which of the following is the quantum number for p orbital ?

a)

0

b)

1

c)

2

d)

3

54.

the correct electronic configuration for carbon atom is ?

a)

1s2 2s2 2p2

b)

1s2 2s2 2p6

c)

1s2 2s2 2p4

d)

1s2 2s2 2p3

55.

the correct electronic configuration for Magnesium Mg atom is ?

a)

[Ne] 2s2

b)

[Ne] 3s2

c)

[He] 3s2

d)

[He] 2s2

56.

the correct electronic configuration for Chromium Cr atom is ? (atomic number = 24 )

a)

[Ne] 3s2 3p4

b)

[Ar] 4s13d5

c)

[Ar] 4s2 3d4

d)

[Ar] 3s2 3p4

57.

the correct electronic configuration for potassium K atom is ? (atomic number = 19)

a)

[Ne] 3s2 3p4

b)

[Ar] 3s1

c)

[Ar] 4s1

d)

[Ne] 3s1

58.

what is the maximum capacity for p orbital ?

a)

2 electrons

b)

6 electrons

c)

10 electrons

d)

14 electrons

59.

what is the maximum capacity for s orbital ?

a)

2 electrons

b)

6 electrons

c)

10 electrons

d)

14 electrons

60.

what is the maximum capacity for d orbital ?

a)

2 electrons

b)

6 electrons

c)

10 electrons

d)

14 electrons

61.

what is Quantum number for d orbital ?

a)

0

b)

1

c)

2

d)

3

62.

what is Quantum number for p orbital ?

a)

0

b)

1

c)

2

d)

3

63.

which of the following molecules has strong hydrogen bonding ?

a)

NH3

b)

CH4

c)

CH3Cl

d)

AlCl3

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