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Review Activity 4 - Ionic Bonding

Total questions: 50

Worksheet time: 50mins

Name
Class
Date
1.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
2.

An ionic bond forms when

a)

Valence electrons are shared

b)

a sea of mobile electrons surround the cations

c)

valence electrons completely move from a metal to a non-metal

d)

none of the above

3.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
4.

a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

a)

compound

b)

ion

c)

chemical bond

d)

ionic bond

5.
How many atoms of Oxygen are in this compound?
a)
4
b)
1
c)
12
d)
7
6.

What elements generally make a covalent bond?

a)

metal and nonmetal

b)

nonmetal to nonmetal

c)

metal

d)

none of the above

7.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
8.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
9.
When forming an ionic bond, a metal atom
a)
Gains electrons to form a cation
b)
Loses electrons to form a cation
c)
Gains electrons to form an anion
d)
Loses electrons to form an anion
10.

What type of compound will conduct electricity when melted or dissolved in water?

a)

ionic

b)

covalent

c)

metallic

d)

molecule

11.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

12.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

Bonds result from sharing valence electrons

c)

Electrons are transferred between atoms

d)

Electrons move freely creating a sea of electrons

13.

Why do atoms form bonds?

a)

to increase their potential energy by filling up their valence shell

b)

atoms are more stable bonded together

c)

to increase their atomic number

14.

Which of the following describes metallic bonds?

a)

Bonds form because of opposite charges

b)

Bonds result from sharing valence electrons

c)

Electrons are transferred between atoms

d)

Electrons move freely creating a sea of electrons

15.

What elements generally make a metallic bond?

a)

metal and nonmetal

b)

nonmetal to nonmetal

c)

metal to metal

d)

none of the above

16.

Characteristics of a covalent bond include all of the following except which one?

a)

share electrons

b)

non metal to non metal

c)

forms a compound called a molecule

d)

forms in a sea of electrons

17.

Characteristics of an ionic bond include all of the following except which one?

a)

metal to non metal

b)

electrons completely move to form ions

c)

creates a compound called a molecule

d)

is composed of positive and negative ions

18.

What is defined as highly mobile electrons absorb and re-emit light to make a metal appear shiny

a)

sea of electrons

b)

luster

c)

molecule

d)

formula unit

19.

The sea of electrons which allow metal layers to slide past one another can be found where?

a)

ionic compounds

b)

polyatomic ions

c)

metallic compounds

d)

covalent compounds

20.

Which type of compound can be a gas, liquid or solid at room temperature?

a)

ionic compounds

b)

polyatomic ions

c)

metallic compounds

d)

covalent compounds

21.

Which type of compound has a crystal structure made of ions?

a)

ionic compounds

b)

polyatomic ions

c)

metallic compounds

d)

covalent compounds

22.

Which type of compound is a poor electrical conductor in all phases?

a)

ionic compounds

b)

polyatomic ions

c)

metallic compounds

d)

covalent compounds

23.

All of the following are common types of ionic compounds except what?

a)

oil

b)

salt

c)

rust

d)

antacid tablets

24.

All of the following are common types of metallic compounds except what?

a)

steel

b)

bronze

c)

alloys

d)

rust

25.

All of the following are common types of covalent compounds except what?

a)

oil

b)

bronze

c)

sugar

d)

carbon dioxide

26.

Which of the following elements have four valence electrons?

a)

Lead(IV)

b)

Uranium(VI)

c)

Selenium

d)

Beryllium

27.

Group 17 elements will have how many valence electrons?

a)

17

b)

1

c)

2

d)

7

28.

Group 2 elements will have how many valence electrons?

a)

8

b)

1

c)

2

d)

0

29.

How many valence electrons does Silver have?

a)

1

b)

2

c)

11

d)

47

30.

How many valence electrons does Cadmium have?

a)

1

b)

2

c)

12

d)

48

31.

The number of valence electrons in a transition metal is identified by what?

a)

group number

b)

roman numeral

c)

atomic number

d)

period number

32.

How many valence electrons does Copper(II) have?

a)

11

b)

1

c)

2

d)

29

33.

Ca+2 and N-3 create...

a)

Ca2N3

b)

Ca3N2

c)

CaN3

d)

Ca2N

34.

Potassium and Sulfur create...

a)

KS

b)

KS2

c)

K2S

d)

K2S2

35.

The chemical formula of Iron (III) and bromine is

a)

FeBr

b)

Fe(III)Br

c)

FeBr₃

d)

Fe₂Br₃

36.

The formula of calcium and phosphate is

a)

CaPO4

b)

Ca2(PO4)3

c)

Ca3PO4

d)

Ca3(PO4)2

37.

What is the formula for copper(I) and sulfate?

a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

38.

Which of the following will form an ion with a -2 charge?

a)

Ca

b)

Se

c)

Ge

d)

N

39.
Which is the charge that results when oxygen becomes an ion?
a)
+3
b)
+2
c)
-2
d)
-3
40.

Sodium carbonate

a)

So2CO3

b)

NaCO3

c)

K2CO3

d)

Na2CO3

41.

Zinc Oxide

a)

ZnO2

b)

Zn2O

c)

Zn4O

d)

ZnO

42.

How many Hydrogen atoms are in 4H2O?

a)

6

b)

8

c)

2

d)

4

43.

Number of C's in 2Na2CO3

a)

1

b)

2

c)

3

d)

5

44.
How many total atoms are in the compound C2H8O ?
a)
11
b)
2
c)
8
d)
1
45.

How many Aluminum are in Al2O3?

a)

3

b)

2

c)

5

d)

1

46.

What is the formula mass of NaCl

a)

58.5

b)

23

c)

35.5

d)

67.6

47.

What is the formula mass of Pr(OH)3

a)

191.9

b)

157.1

c)

160.9

d)

81.1

48.

What is the formula mass of magnesium fluoride

a)

62.3

b)

43.3

c)

67.6

d)

30.0

49.

What is the formula mass of copper (II) nitrate

a)

187.6

b)

125.6

c)

91.0

d)

173.5

50.

What is the formula mass of Cadmium Bromide

a)

304.72

b)

272.21

c)

192.31

d)

118.0

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