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CP Chem Unit 2A Practice Test

Total questions: 23

Worksheet time: 12mins

Name
Class
Date
1.

Which of the following compounds contains ionic bonds?

a)

SO2

b)

CO2

c)

AsBr3

d)

CaBr2

e)

SBr2

2.

Which of the following would contain only nonpolar bonds?

a)

N2

b)

OF2

c)

PCl3

d)

HCN

e)

CO2

3.

Which of he following would be the least polar, yet still have polar covalent bonds?

a)

Na-Cl

b)

S-Cl

c)

B-Cl

d)

Cl-Cl

e)

Fe-Cl

4.

Which of he following would be the most polar, without being considered to be ionic?

a)

Na-Cl

b)

S-Cl

c)

B-Cl

d)

Cl-Cl

e)

Fe-Cl

5.

Rank the following bonds from least polar to most polar.

a)

O-F < N-F < P-F < H-F

b)

N-F < P-F < H-F < O-F

c)

H-F < P-F < N-F < O-F

d)

H-F < O-F < N-F < P-F

6.

Which of the following bonds would not have a dipole moment?

a)

C-N

b)

C-Cl

c)

C-O

d)

C-Br

e)

C-C

7.

In which case is the bond polarity incorrect?

a)

δ+ B-O δ-

b)

δ- S-Se δ+

c)

δ+ F-N δ-

d)

δ- Cl-P δ+

e)

δ+ Si-P δ-

8.

The electron pair in a S-Cl bond could be considered_______.

a)

closer to the Cl because Chlorine has a higher electronegativity than S.

b)

closer to the S because Sulfur has a lower electronegativity than Chlorine.

c)

closer to the S because S has a larger atomic radius and exerts greater control over shared electrons.

d)

equally shared between the S and Cl.

e)

an inadequate model since the bond is ionic.

9.

Draw Lewis structures for the following compounds to assist you in answering the following questions.

( CHCl3, SCl2, PF3, SiO2, CF4)

How many of these compounds are nonpolar?

a)

1

b)

2

c)

3

d)

4

e)

5

10.

Draw Lewis structures for the following compounds to assist you in answering the following questions.

( CHCl3, SCl2, PF3, SiO2, CF4)

Which compound does not have bond angles of 109.5 degrees?

a)

CHCl3

b)

SCl2

c)

PF3

d)

SiO2

e)

CF4

11.

The number of polar covalent bonds in SiO2 is

a)

1

b)

2

c)

3

d)

4

12.

Draw Lewis structures for the following compounds to assist you in answering the following questions.

( CHCl3, SCl2, PF3, SiO2, CF4)

Which compound has the greatest total number of lone pairs (include all lone pairs, even on outside atoms)?

a)

CHCl3

b)

SCl2

c)

PF3

d)

SiO2

e)

CF4

13.

Draw Lewis structures for the following compounds to assist you in answering the following questions.

( CHCl3, SCl2, PF3, SiO2, CF4)

Which compound has at least one double bond?

a)

CHCl3

b)

SCl2

c)

PF3

d)

SiO2

e)

CF4

14.

Which of the following has a tripple bond?

a)

F2

b)

O2

c)

N2

d)

PF3

e)

CO32-

15.

What is the molecular geometry (VSEPR Shape) of PCl3?

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

e)

bent

16.

What is the molecular geometry (VSEPR Shape) of CCl4?

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

e)

bent

17.

What is the molecular geometry (VSEPR Shape) of SO2?

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

e)

bent

18.

What is the formula for carbon tetrafluoride?

a)

CaF3

b)

CF3

c)

CaF4

d)

CF4

e)

CF5

19.

According to the VSEPR model, the bond angles of NH3 and CH4 are ______________

a)

different because they have a different number of lone pairs around the central atom.

b)

the same because the sum of bonding pairs and lone pairs is equal for both molecules

c)

different because they have different numbers of bonding pairs around the central atom

d)

different or the same, depending on the conditions leading to the maximum repulsion.

20.

True or False: Intramolecular forces are the forces inside a molecule that hold atoms of a molecule together.

a)

True

b)

False

21.

Which compound will have hydrogen bonding intermolecular forces?

a)

CH4

b)

NH3

c)

SH2

d)

HCl

22.

What are the major attractive forces exerted between molecules of H2?

a)

dipole-dipole

b)

london dispersion

c)

hydrogen bonding

d)

ionic

e)

none of these

23.

What are the major attractive forces exerted between molecules of HCl?

a)

dipole-dipole

b)

london dispersion

c)

hydrogen bonding

d)

ionic

e)

none of these

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