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Chemistry Bonding Test Review

Total questions: 45

Worksheet time: 47mins

Name
Class
Date
1.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

2.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

3.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

4.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

5.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

6.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
d)
Carbon and Bromine
7.

Oxygen has (a)   valence electrons.

8.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
9.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
10.

Which of the following is the best representation of a molecule of fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

11.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
12.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
13.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
14.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
15.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
16.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
17.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
18.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
19.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

20.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

21.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

22.
Which of the following geometries could be nonpolar?
a)
bent
b)
tetrahedral
c)
trigonal pyrimidal
d)
none of the above
23.
A molecule containing polar covalent bonds is always polar.
a)
True
b)
False
24.
What is the formula for sodium nitrate?
a)
Na3(NO)
b)
Na(NO)
c)
Na3(NO3)
d)
Na(NO3)
25.
What is the formula for copper(I) sulfate?
a)
Cu(SO3)
b)
Cu(SO4)
c)
Cu2(SO3)
d)
Cu2(SO4)
26.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
27.
Name this compound: 
Ca(CO3)
a)
Calcium carbon oxide
b)
Calcium (II) carbonate
c)
Calcium carbonate
d)
Carbonate (I) calcide
28.
Carbon dioxide
a)
C2O2
b)
C20
c)
CO
d)
CO2
29.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCl
30.
Bromine monoflouride
a)
BaF
b)
BrF
c)
Br2F
d)
BrF2
31.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
32.
hydrochloric acid
a)
H(ClO3)
b)
H(ClO2)
c)
HClO
d)
HCl
33.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
34.
Which of the following molecules contains only London dispersion forces?
a)
CF4
b)
HCl
c)
H2O
d)
MgO(aq)
35.
Which of the following molecules would have the lowest boiling point?
a)
CH4
b)
C2H6
c)
C3H8
d)
C4H10
36.
Which of the following molecules has hydrogen bonding?
a)
HCl
b)
HI
c)
HF
d)
HBr
37.

Ca ionizes to a charge of _______.

a)

+1

b)

+2

c)

-1

d)

-2

38.

Which element has the following electron configuration:


1s2 2s2 2p6 3s2 3p2

a)

Mg

b)

Al

c)

Si

d)

P

39.

What is the correct condensed electron configuration for potassium (K)?

a)

[Ar] 4s1

b)

[Kr] 4s1

c)

[Ar] 4s2

d)

[Kr] 4s2

40.

What is the maximum number of electrons that can occupy an orbital?

a)

1

b)

2

c)

4

d)

6

e)

8

41.

A "p" sublevel can hold up to _______ electrons.

a)

2

b)

4

c)

6

d)

8

e)

10

42.

What sub-level will receive electrons after the 2p sub-level?

a)

1s

b)

1p

c)

2s

d)

3s

e)

3p

43.

How many orbitals make up a "s" sub-level?

a)

1

b)

3

c)

6

d)

8

44.

Count the total valence electrons in CH4.

a)

6

b)

12

c)

8

d)

10

45.

Count the total valence electrons in CO2.

a)

14

b)

16

c)

18

d)

10

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