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Chemical Bonding, Molecular Shapes, and Intermolecular Force

Total questions: 37

Worksheet time: 3hrs 5mins

Name
Class
Date
1.
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
2.
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
3.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

4.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

5.

In the Lewis structure for sulfur dioxide, the molecular geometry is ________________.

a)

polar

b)

polar covalent

c)

bent

6.

What is a molecule that has a positive side and a negative side as a result of an uneven distribution of electrons?

a)

polar covalent

b)

polar molecule

c)

covalent bond

7.

The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom?

a)

H2S

b)

NH3

c)

CH4

d)

HCN

8.

Intermolecular force present in HCl?

a)

dipole dipole

b)

LDF

c)

H-bond

d)

ionic

9.

Type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

LDF

d)

metallic

10.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
11.

Type of intermolecular force present in HF.

a)

dipole dipole

b)

LDF

c)

H-bond

d)

ionic

12.

Intermolecular force present in CHF3

a)

H bond

b)

dipole dipole

c)

LDF

d)

ionic

13.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
14.

Which of these is not an intermolecular force?

a)

covalent bonding

b)

hydrogen bonding

c)

London dispersion forces

d)

dipole-dipole forces

15.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
The same
16.
Which of the following geometries could be nonpolar?
a)
bent
b)
tetrahedral
c)
trigonal pyrimidal
d)
none of the above
17.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
18.
Which of the following molecules, based on the elements present, would be most polar?
a)
HF
b)
H2
c)
HCl
d)
HBr
19.

Using electronegativity differences, what type of bond is formed by S and Br.

a)

ionic

b)

polar covalent

c)

non-polar covalent

20.

Using electronegativity differences, what type of bond is formed by Co and F.

a)

ionic

b)

polar covalent

c)

non-polar covalent

21.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
22.

Why do atoms bond?

a)

They typically don't bond

b)

To add or take away energy levels

c)

To have a full valance shell.

d)

To have a full inner shell

23.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
24.
How many electrons should Boron have around its Lewis dot model?
a)
1
b)
3
c)
5
d)
7
25.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
26.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
27.

Which geometric molecular shape is shown?

a)

trigonal planar

b)

linear

c)

bent

d)

trigonal pyramidal

28.
 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
29.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
30.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
31.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
32.
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
33.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
34.
Which of these molecules has nonpolar covalent bonding?
a)
H2O
b)
HCl
c)
I2
d)
NaCl
35.
In the HCl molecule which atom would have a slightly negative charge?
a)
H
b)
Both
c)
Cl
d)
Neither
36.
Why does H2O have a higher boiling point than H2Se?
a)
It has stronger bonding
b)
it has dipole-dipole forces
c)
it has london dispersion forces
d)
it has hydrogen bonding
37.

Which equation represents the breaking of intermolecular forces?

a)

NH3 (g) --> N2 (g) + H2 (g)

b)

NH3 (i) --> NH3 (g)

c)

K2CO3 (s) --> CO2 (g) + K2O (s)

d)

Mg (s) + O2 (g) --> MgO (s)

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