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IGCSE CHEMISTRY: CHEMICAL BONDING

Total questions: 115

Worksheet time: 1hrs 26mins

Name
Class
Date
1.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

2.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

3.
Ionic bonds are between...
a)
nonmetals and nonmetals
b)
carbon and oxygen
c)
metals and nonmentals
d)
hydrogen and chlorine
4.
Covalent bonds are between...
a)
two or more nonmetals
b)
sodium and chlorine
c)
metals and metals
d)
metals and nonmetals
5.
If an atom loses two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
6.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
7.

What kind of bond forms when atoms transfer electrons?

a)
ionic
b)
covalent
c)

metallic

d)

molecular

8.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

9.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

10.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
11.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
12.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

13.
What is the proper name for CaCl2?
a)
Calcium dichloride
b)
Monocalcium dichloride
c)
Calcium chloride
d)
Calcium chlorine
14.
What is the proper name for S2O2?
a)
Sulfur oxide
b)
Sulfur dioxide
c)
sulfur (II) oxide
d)
disulfur dioxide
15.

Which two statements are correct about the figure shown?

a)

It is a covalent bond.

b)

Hydrogen atoms loss electrons and Carbon gains the atoms.

c)

It happens on metal and on another non-metal.

d)

The valence electrons are shared by both atoms.

16.

Check all that characterizes an ionic compound.

a)

Hard

b)

non-conductor of heat and electricity

c)

High melting and boiling points

d)

non-soluble in water

17.

Check two general properties of a molecular compound.

a)

Hard

b)

Soft

c)

Low melting point

d)

poor conductor of electricity when in solid state.

18.

Which two are ionic compounds?

a)

NaCl

b)

HCl

c)

CH4

d)

CaO

19.

Which two are molecular compounds?

a)

MgO

b)

Al2O3

c)

CO2

d)

H2O

20.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
21.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
22.

An atom with a different number of electrons than it should have (more or less) is called an ---

a)

isotope

b)

valence electron

c)

ion

d)

octet

23.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
24.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
25.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
26.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
27.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
28.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
29.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
30.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
31.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
32.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
33.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
34.
What happens when an atom loses an electron?
a)
Neutral (no charge)
b)
Positive charge
c)
Negative charge
35.
What happens when an atom gain an electron?
a)
Neutral(no charge)
b)
Positive charge
c)
Negative charge
36.
What charges attract?
a)
Opposite
b)
Same
37.
What charges repel?
a)
Same
b)
Opposite
38.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
39.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
40.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
41.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
42.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
43.
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.
44.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
45.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
46.
What is the number of valence electrons for Silicon?
a)
1
b)
2
c)
6
d)
4
47.
What is the number of valence electrons for Neon?
a)
6
b)
7
c)
8
d)
9
48.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
49.
What group would Ca like to join with
a)
5
b)
6
c)
7
d)
8
50.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
51.

What type of bond forms when many electrons are shared between many atoms?

a)

covalent

b)

ionic

c)

metallic

d)

all three

52.

What type of bond forms when electrons are shared between two atoms?

a)

covalent

b)

ionic

c)

metallic

d)

all three

53.

What type of bond forms between metals and nonmetals?

a)

covalent

b)

ionic

c)

metallic

d)

all three

54.

What type of bond forms between anions and cations?

a)

covalent

b)

ionic

c)

metallic

d)

all three

55.

What type of bond forms when there are charges?

a)

covalent

b)

ionic

c)

metallic

d)

all three

56.

What type of bond forms between nonmetals and other nonmetals?

a)

covalent

b)

ionic

c)

metallic

d)

all three

57.

What type of bond forms between metals and other metals?

a)

covalent

b)

ionic

c)

metallic

d)

all three

58.

What type of bond forms when there is an exchange or transfer of electrons between atoms?

a)

covalent

b)

ionic

c)

metallic

d)

all three

59.

What type of bond forms as a result of the interactions of electrons between atoms?

a)

covalent

b)

ionic

c)

metallic

d)

all three

60.

What is the charge of an electron?

a)

negative

b)

positve

c)

neutral

d)

there is no assigned charge to an electron

61.

What is the charge of the nucleus of an atom?

a)

negative

b)

positve

c)

neutral

d)

there is no assigned charge to an electron

62.

Which electrons are most loosely held to the nucleus of an atom? Check all that apply.

a)

The ones closest to the nucleus.

b)

The ones in the first energy level.

c)

The ones farthest from the nucleus.

d)

The valence electrons.

e)

The electrons in the middle of the electron cloud.

63.

If Cu bonds with Al, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

64.

If Cu bonds with O, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

65.

If O bonds with O, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

66.

If Ne bonds with Ne, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

67.

If N bonds with S, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

68.

If Fe bonds with F, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

69.

If H bonds with O, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

70.

If Fe bonds with Na, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

71.

How many valence electrons does Mg have?

a)

1

b)

2

c)

3

d)

4

72.

How many valence electrons does Br have?

a)

5

b)

6

c)

7

d)

8

73.

How many valence electrons does Al have?

a)

3

b)

4

c)

5

d)

6

74.

Lithium has 1 valence electron, to bond with iodine what would it do?

a)

share an electron with iodine.

b)

Give an electron to iodine.

c)

It depends on the temperature: if it is hot it will give its electron to iodine but if it is cold it will take an electron from iodine.

d)

Lithium and iodine will not react and form a bond.

75.

Which is an example of a diatomic molecule?

a)

H2O

b)

NaCl

c)

O2

d)

MgS

76.

Dot and cross diagram for O2

a)
b)
c)
d)
e)
77.

What is the chemical formula of magnesium chloride?

a)

MgCl

b)

MgCl2

c)

MgC

d)

MgC2

78.

Dot and cross diagram for CaF2

a)
b)
c)
79.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
80.

What type of bonding involves metals ONLY?

a)

Ionic

b)

Covalent

c)

Metallic

81.

What type of bonding involves non-metals ONLY?

a)

Ionic

b)

Covalent

c)

Metallic

82.

What type of bonding involves metals and non-metals?

a)

Ionic

b)

Covalent

c)

Metallic

83.

What type of bonding would you expect to see in SODIUM CHLORIDE?

a)

Ionic

b)

Covalent

c)

Metallic

84.

What type of bonding would you expect to see in CARBON DIOXIDE?

a)

Ionic

b)

Covalent

c)

Metallic

85.

Which statement correctly explains why metals conduct electricity?

a)

Metals contain delocalised electrons which can move throughout the structure

b)

Metals contain ions which are free to move throughout the structure

c)

Metals contain an electrical current

d)

Metals are magnetic

86.

Which statement correctly explains why ionic compounds conduct electricity as a LIQUID?

a)

Ionic compounds contain delocalised electrons which can move throughout the structure

b)

Ions are free to move

c)

Ions are fixed in position

d)

Ionic compounds contain an electrical current

87.

How are covalent bonds formed?

a)

Pairs of electrons are shared

b)

Electrons are transferred from one atom to another

c)

Strong attraction between negative delocalised electrons and positive ions

88.

How are ionic bonds formed?

a)

Pairs of electrons are shared

b)

Electrons are transferred from one atom to another

c)

Strong attraction between negative delocalised electrons and positive ions

89.

Which ion is formed by sodium (Na)?

a)

Na-

b)

Na+

c)

Na+7

d)

Na-7

90.

What is the chemical formula of magnesium chloride?

a)

MgCl

b)

MgCl2

c)

MgC

d)

MgC2

91.

Dot and cross diagram for O2

a)
b)
c)
d)
e)
92.

Dot and cross diagram for CaF2

a)
b)
c)
93.

Which is NOT a property of ionic compounds?

a)

solids with high melting and boiling points

b)

soft solids which are highly malleable

c)

when solid, the ions are held in place so the compounds cannot conduct electricity

d)

conduct electricity when dissolved or molten

94.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

95.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds which require a large amount of heat energy to overcome these strong bonds.

d)

They have weak bonds which require a little amount of heat energy to overcome these weak bonds.

96.

Substances such as  silica, diamond and graphite are

a)
simple covalent molecules
b)
metallic
c)

ionic substances

d)

giant covalent molecules

97.
Melting points are very high – a large amount of energy is needed to break all the covalent bonds
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
98.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)
Carbon fiber
d)
Carbon nanotubes
99.
Why is diamond strong?
a)
It's made of carbon
b)
It doesn't conduct electricity
c)
It forms 4 strong covalent bonds
d)
So it can cut glass
100.
Why is graphite so soft?
a)

The atoms are arranged in hexagons in layers that are held together strongly

b)

The atoms are arranged in hexagons in layers that are held together weakly

c)

Carbon is strongly bonded to 3 other carbon atoms.

d)

Carbon is weakly bonded to 3 other carbon atoms.

101.
What element are diamond and graphite made up of?
a)

Sodium

b)

Carbon

c)

Carbon dioxide

d)

Silicon

102.

Why does graphite conduct electricity?

a)

Ions are free to move to carry the charge

b)

Atoms can move

c)

Free electrons that can carry the charge

103.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)

Silica

d)

Salt

104.

Why is graphite so soft and slippery?

a)

It is made of layers of atoms with weak forces between them

b)

It is made of small molecules

c)

It is an ionic compound

d)

The covalent bonds are weak

105.

In which state are most simple covalent substances in at room temperature?

a)

solid

b)

liquid

c)

gas

106.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
107.
There are more metals than non metals in the periodic table.
a)
True
b)
False
108.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
109.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
110.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
111.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
112.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
113.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
114.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
115.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

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