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Lewis Structures, VSEPR, Polarity and IMFs

Total questions: 40

Worksheet time: 2hrs 0mins

Name
Class
Date
1.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
2.
How many electrons can be used in the Lewis Structure for : NO3 -
a)
23
b)
20
c)
18
d)
24
3.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
4.

Which image could be a representation of NH3?

a)

A

b)

B

c)

C

5.

Which of the following is the correct Lewis structure for a molecule of fluorine?

a)

A

b)

B

c)

C

d)

D

6.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

7.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
8.

Model the Lewis Structure for ClO4- where the central atom obeys the octet rule. How many unshared pairs, single bonds and double bonds are on the central atom?

a)

1, 3, 0

b)

1, 1, 1

c)

0, 4, 0

d)

0, 0, 2

e)

2, 2, 0

9.

Model the Lewis Structure for SF2 where the central atom obeys the octet rule. How many unshared pairs, single bonds and double bonds are on the central atom?

a)

1, 3, 0

b)

1, 1, 1

c)

0, 4, 0

d)

0, 0, 2

e)

2, 2, 0

10.

Model the Lewis Structure for NH4+ where the central atom obeys the octet rule. How many unshared pairs, single bonds and double bonds are on the central atom?

a)

1, 3, 0

b)

1, 1, 1

c)

0, 4, 0

d)

0, 0, 2

e)

2, 2, 0

11.

Model the Lewis Structure for ClF3 where the central atom has an expanded octet. How many unshared pairs, single bonds and double bonds are on the central atom?

a)

1, 3, 0

b)

1, 1, 1

c)

0, 4, 0

d)

0, 0, 2

e)

2, 3, 0

12.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
13.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
14.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
15.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
16.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
17.

Is this molecule polar?

a)

Yes

b)

No

18.

Is this molecule polar?

a)

Yes

b)

No

19.

Choose the correct molecular shape for SO3.

a)

trigonal planar

b)

trigonal pyramidal

c)

bent

d)

tetrahedral

20.

What molecular geometry would PBr3 have?

a)

trigonal pyramidal

b)

trigonal planar

c)

tetrahedral

d)

linear

21.

Choose the correct molecular shape for NH4+.

a)

trigonal planar

b)

trigonal pyramidal

c)

bent

d)

tetrahedral

22.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

23.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
24.
Which of the following geometries could be nonpolar?
a)
bent
b)
tetrahedral
c)
trigonal pyrimidal
d)
none of the above
25.
Which of the following molecules, based on the elements present, would be most polar?
a)
HF
b)
H2
c)
HCl
d)
HBr
26.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

27.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

28.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

29.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

30.
Does HCl have hydrogen bonding?
a)

yes

b)

no

31.
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
32.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

33.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
34.
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
35.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
36.

Intermolecular forces depend on the size of the charge

a)

true

b)

false

37.

In a water molecule, the bond between the hydrogen and the oxygen is best described as

a)

a hydrogen bond

b)

an intermolecular bond

c)

an ionic bond

d)

a covalent bond

38.

Does NH3 or PH3 have a higher boiling point?

a)

NH3 because it has the strongest intermolecular forces

b)

PH3 because it has the strongest intermolecular forces

c)

NH3 because it has the weakest intermolecular forces

d)

PH3 because it has the weakest intermolecular forces

39.

In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces

a)

Higher

b)

Lower

c)

Forces and boiling point are not related

40.

Which statement explains why Br2 is a liquid at STP and I2 is a solid at STP?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar

b)

Molecules of Br2 are nonpolar, and molecules of I2 are polar

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

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