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Y9 Bonding Questions

Total questions: 157

Worksheet time: 2hrs 35mins

Name
Class
Date
1.

Look at the diagram. How many covalent bonds does each carbon atom form in graphite?

(a)  

2.

Look at the diagram. How many covalent bonds does each carbon atom form in diamond?

(a)  

3.

Tick the properties of diamond

a)

Very hard

b)

Slippery

c)

Conducts electricity

d)

Soft

e)

Does not conduct electricity

4.

Tick the properties of graphite

a)

Very hard

b)

Slippery

c)

Conducts electricity

d)

Soft

e)

Does not conduct electricity

5.

What type of bonding involves metals ONLY?

a)

Ionic

b)

Covalent

c)

Metallic

6.

What type of bonding involves non-metals ONLY?

a)

Ionic

b)

Covalent

c)

Metallic

7.

What type of bonding involves metals and non-metals?

a)

Ionic

b)

Covalent

c)

Metallic

8.

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

a)

Ionic

b)

Covalent

c)

Metallic

9.

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

a)

Ionic

b)

Covalent

c)

Metallic

10.

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

11.

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

12.

Which statement correctly explains why ionic compounds DO NOT conduct electricity as a SOLID?

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 are not magnetic

13.

How many bonding pairs are present in this covalent molecule?

a)

1

b)

2

c)

3

d)

4

14.

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

15.

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

16.

Which statement correctly explains why metals are easily bent and shaped?

a)

The metal ions can be squashed

b)

The metal ions can move

c)

The metal ions are in layers which can slide over each other

d)

The metal ions are all the same size

17.

Which statement correctly explains why alloys are harder to shape than pure metals?

a)

The metal ions can be squashed

b)

The metal ions cannot move

c)

The metal ions are in layers which can slide over each other

d)

Different size metal ions disrupt the layers

18.

What is an alloy?

a)

Mixture of elements

b)

Mixture of metals

c)

Pure metal

d)

Mixture of metal and plastic

19.

What is a smart alloy?

a)

An alloy that can change colour

b)

An alloy that returns to its original shape

c)

An alloy that can be used for different purposes

20.

Which are examples of alloys?

a)

Stainless steel

b)

Iron

c)

Copper

d)

Brass

e)

Nitinol

21.

Which ONE is an example of a smart alloy?

a)

Stainless steel

b)

Iron

c)

Copper

d)

Brass

e)

Nitinol

22.

Which statement correctly explains why most covalent substances have low melting/boiling points?

a)

There are strong electrostatic attractions

b)

There are weak intermolecular forces

c)

Covalent bonds are weak

d)

There are no strong bonds

23.

Which statement correctly explains why ionic compounds have high melting/boiling points?

a)

There are strong electrostatic attractions

b)

There are weak intermolecular forces

c)

Ionic bonds are weak

d)

There are strong intermolecular forces

24.

What type of structure do ionic compounds have?

a)

Small, simple molecules

b)

Giant molecule

c)

Giant lattice

25.

Which ion is formed by sodium (Na)?

a)

Na-

b)

Na+

c)

Na+7

d)

Na-7

26.

Which ion is formed by magnesium (Mg)?

a)

Mg-

b)

Mg+

c)

Mg2+

d)

Mg2-

27.

Which ion is formed by oxygen (Mg)?

a)

O-

b)

O+

c)

O2+

d)

O2-

28.

Which ion is formed by Chlorine (Cl)?

a)

Cl-

b)

Cl+

c)

Cl2+

d)

Cl2-

29.

Choose the correct words to complete the sentence:

Ionic compounds can conduct electricity when ____________ or ____________.

a)

solid

b)

aqueous (dissolved)

c)

powdered

d)

squashed

e)

molten

30.

Choose the correct words to complete the sentence:

Metals are excellent conductors of ___________ and _____________.

a)

heat

b)

water

c)

electricity

d)

light

31.

What is the charge of a magnesium ion after it loses two electrons?

a)

-1

b)

+2

c)

-2

d)

+1

32.

How many valence electrons does sulfur have before it gains two electrons to form a sulfide ion?

a)

2

b)

4

c)

8

d)

6

33.

What is the final electron configuration of a sodium ion after it loses its valence electron?

a)

2,8

b)

2,8,2

c)

2,7

d)

2,8,1

34.

What type of bond forms between sodium and chlorine to create sodium chloride?

a)

Hydrogen bond

b)

Ionic bond

c)

Covalent bond

d)

Metallic bond

35.

What is the overall charge of an ionic compound?

a)

-1

b)

Varies

c)

0

d)

+1

36.

How many chloride ions are needed to balance the charge of one magnesium ion?

a)

3

b)

2

c)

1

d)

4

37.

What is the charge on a sulfide ion?

a)

-2

b)

+1

c)

+2

d)

-1

38.

What happens to the ions in an ionic compound when it is dissolved in water?

a)

They form covalent bonds

b)

They lose their charge

c)

They become immobile

d)

They are free to move

39.

What is the correct formula for magnesium chloride?

a)

Mg2Cl3

b)

Mg2Cl

c)

MgCl2

d)

MgCl

40.

What is the principle behind the formation of ionic bonds?

a)

Movement of neutrons

b)

Sharing of electrons

c)

Transfer of electrons

d)

Exchange of protons

41.

Which element typically does not form an ionic bond with chlorine?

a)

Sodium

b)

Magnesium

c)

Carbon

d)

Potassium

42.

In a dot and cross diagram for sodium chloride, what does a dot represent?

a)

An electron from sodium

b)

An electron from chlorine

c)

A shared electron pair

d)

A neutron

43.

How does the electron configuration of an oxygen atom change when it forms an oxide ion?

a)

It loses two electrons

b)

It gains two electrons

c)

It shares two electrons

d)

No change

44.

What is the electron configuration of a chloride ion?

a)

2,8,7

b)

2,8,8

c)

2,8,6

d)

2,8

45.

Which of the following elements is most likely to form an ionic bond with fluorine?

a)

Oxygen

b)

Lithium

c)

Carbon

d)

Nitrogen

46.

What is the correct formula for potassium oxide?

a)

K2O

b)

KO2

c)

K2O2

d)

KO

47.

Surname

4 lines
48.

First name

4 lines
49.
The diagram shows the electron configuration for calcium. How can you write the electron configuration for calcium?
a)
8,2,2,8
b)
2,8,8,2
c)
10,10
d)
2,10,8
50.
How many electrons does the outer shell of a lithium atom contain?
a)
1
b)
3
c)
4
d)
7
51.

Electrons are ____________ charged.

a)

positively

b)

neutrally

c)

negatively

52.

When atoms lose or gain electrons and become charged, we call them:

a)

an isotope

b)

a new atom

c)

an ion

d)

a bond

53.

An atom that loses an electron forms a positive ion.

a)

a positive

b)

a negative

c)

neither

54.

Sodium forms an ionic bond with Chlorine. What is the charge on the Sodium ion?

a)

-2

b)

+1

c)

-

d)

+

55.

Ionic bonding happens between a metal and a non-metal.

a)

metals

b)

non-metals

c)

a metal and a non-metal

56.

Covalent bonding happens between:

a)

metals

b)

non-metals

c)

a metal and a non-metal

57.

Metallic bonding is a bond between a metal and ________.

a)

a non-metal

b)

a metal

58.

What type of bonding is present in calcium oxide?

a)

Covalent

b)

Ionic

c)

Macromolecular

d)

Metallic

59.

What kind of force attracts oppositely charged ions to each other?

a)

electrostatic

b)

magnetic

c)

intermolecular

d)

attractive

60.

Ionic bonds are:

a)

Strong

b)

Weak

c)

Neither

61.
Covalent bonds are:
a)
Strong
b)
Weak
c)
Neither
62.
Forces between molecules - intermolecular forces - are:
a)
Strong
b)
Weak
c)
Neither
63.
What word describes the structure of an ionic compound?
a)
box
b)
molecule
c)
solid
d)
lattice
64.
What type of particle is shown in Figure 2?
a)
An ion
b)
A lattice
c)
A simple molecule
d)
A polymer
65.

Describe how the calcium atom and the oxygen atom form calcium oxide (4 marks)

4 lines
66.

Ionic compounds have a high melting and boiling point.

a)

High

b)

Mid range

c)

Low

67.
Simple molecular compounds have a _______ melting and boiling point.
a)
High
b)
Mid range
c)
Low
68.
Can covalent compounds like pure water or oxygen conduct electricity?
a)
yes
b)
no
69.

Copper conducts electricity because of the movement of delocalised ___________.

a)

atoms

b)

electrons

c)

ions

d)

molecules

70.

Explain why a sodium chloride solution conducts electricity.

4 lines
71.
Graphene, graphite, diamond are all different forms of:
a)
calcium
b)
carbon
c)
copper
d)
hydrogen
72.
Each carbon atom in graphene has __ covalent bonds.
a)
1
b)
2
c)
3
d)
4
73.
Graphene is a ________ layer of graphite?
a)
single
b)
double
c)
half
d)
triple
74.
Graphite conducts electricity.
a)
true
b)
false
c)
sometimes
75.

Having only 3 bonds between carbon atoms in graphite means that there are:

a)

free atoms

b)

empty bonds

c)

delocalised electrons

d)

inter-molecular forces

76.

Graphene and diamond are allotropes of carbon.

a)

true

b)

false

77.

Nanotubes can be used for medicine delivery.

a)

true

b)

false

78.

Diamond has: a high melting point, a high boiling point, strong covalent bonds, all the above.

a)

a high melting point

b)

a high boiling point

c)

strong covalent bonds

d)

all the above

79.

Buckminster fullerenes can be used as lubricant oils for engines. What element are they made of?

a)

calcium

b)

nitrogen

c)

copper

d)

carbon

80.

Diamond can conduct electricity.

a)

true

b)

false

c)

I don't know

81.

Balance the equation for the reaction of lithium with oxygen.

a)

2

b)

3

c)

4

d)

6

82.

What shape are carbon nanotubes?

a)

Pyramidal

b)

Cubic

c)

Cylindrical

d)

Spherical

83.

What is a limitation of the particle model?

a)

The particle model assumes that particles have no forces between them

b)

The particle model assumes that particles should be square

c)

The particle model assumes that there are more particles than in real life

d)

The particle model assumes that there are fewer particles than in real life

84.

In graphite, how many covalent bonds does each carbon atom form?

a)

1

b)

2

c)

3

d)

4

85.

Which one of these is NOT a property of a fullerene?

a)

A hollow shape

b)

Hexagonal carbon rings

c)

A molecule of carbon atoms

d)

Short length and large diameter

86.

Metals consist of giant structures of           arranged in a regular pattern.

a)

atoms

b)

neutrons

c)

molecules

d)

protons

87.

Non-metal atoms become negatively charged ions by…

a)

gaining electrons

b)

sharing electrons

c)

losing electrons

d)

gaining protons

88.

Which of these is NOT an example of a giant covalent substance?

a)

Graphite

b)

Sodium chloride

c)

Diamond

d)

Silicon dioxide

89.

Ionic bonding is the bonding between…

a)

metals and non-metals

b)

metals and metals

c)

non-metals and non-metals

d)

gold and silver

90.

Which of these statements is NOT true?

Ionic compounds can conduct electricity when…

a)

they are melted

b)

they are dissolved in water

c)

electrons are free to move

d)

ions are free to move

91.

In metallic bonding, the electrons are…

a)

stationary

b)

delocalised

c)

donated

d)

gained

92.

Simple covalent molecules have…

a)

weak intermolecular forces

b)

strong intermolecular forces

c)

weak electrostatic forces

d)

strong electrostatic forces

93.

In pure metals, atoms are arranged in…

a)

no order

b)

groups of 3

c)

layers

d)

circles

94.

Covalent bonding is the bonding between…

a)

metals and non-metals

b)

metals and metals

c)

non-metals and non-metals

d)

metals and gases

95.

What takes place at the boiling point?

a)

Freezing and boiling

b)

Melting and freezing

c)

Condensing and melting

d)

Boiling and condensing

96.

In a simple covalent bond diagram, a single covalent bond is represented using…

a)

a double line

b)

a dotted line

c)

a squiggle

d)

a single line

97.

Define the term 'alloy'.

a)

Non-metal and metal chemically bonded together

b)

More than one metal chemically bonded together

c)

A metal and rock

d)

Two non-metals chemically bonded together

98.

What is a nanometre?

a)

A billionth of a metre

b)

A hundredth of a metre

c)

A thousandth of a metre

d)

A millionth of a metre

99.

How many carbon atoms are there in a molecule of Buckminsterfullerene?

a)

60

b)

50

c)

40

d)

30

100.

In diamond, how many covalent bonds does each carbon atom form?

a)

3

b)

4

c)

2

d)

5

101.

A substance has a boiling point of 220 degrees Celsius and a melting point of −120 degrees Celsius.

What state will it be at room temperature?

a)

Solid

b)

Liquid

c)

Gas

d)

Aqueous

102.

What property does graphite have in common with most metals?

a)

It can conduct electricity

b)

It is magnetic

c)

It is hard

d)

It is ductile

103.

In covalent bonding, electrons are…

a)

swapped

b)

donated

c)

shared

d)

received

104.

At room temperature and pressure, what are the state symbols for hydrogen (H2) and sodium hydroxide (NaOH)?

a)

(g) & (s)

b)

(s) & (aq)

c)

(g) & (l)

d)

(l) & (s)

105.

When magnesium bonds with oxygen, the magnesium loses two electrons. What ion will be formed?

a)

[Mg]+

b)

[Mg]2-

c)

[Mg]2+

d)

[Mg]-

106.

What takes place at the melting point?

a)

Melting and freezing

b)

Freezing and boiling

c)

Boiling and condensing

d)

Condensing and melting

107.

In a molecule of ammonia, how many electrons need to be shared for nitrogen to have a full outer shell?

a)

5

b)

3

c)

1

d)

2

108.

[Mg]2+ and [O]2- ionically bond to form magnesium oxide. What is the correct empirical formula for this compound?

a)

MgO2

b)

2MgO

c)

Mg2O

d)

MgO

109.

Why are metals good conductors of electricity?

a)

Because delocalised electrons carry the charge

b)

Because atoms carry the charge

c)

Because they are arranged in layers of atoms

d)

Because ions carry the charge

110.

At room temperature, polymers are what state?

a)

Solid

b)

Liquid

c)

Gas

d)

Aqueous

111.

Which of these statements is INCORRECT?

The amount of energy needed to change state from a solid to liquid depends on…

a)

the type of bonding

b)

the strength of forces between particles

c)

the colour of the substance

d)

the structure of a substance

112.

What happens during reduction?

a)

Electrons are gained

b)

Electrons are shared

c)

Protons are lost

d)

Electrons are lost

113.

Atoms in a polymer are linked together by…

a)

strong ionic bonds

b)

strong covalent bonds

c)

weak ionic bonds

d)

weak covalent bonds

114.

What is graphene?

a)

A hollow shape

b)

A single layer of graphite

c)

A double layer of graphite

d)

A spherical shape

115.

Which of these statements is NOT characteristic of most metals?

a)

Able to conduct electricity

b)

High melting and boiling points

c)

Malleable

d)

Insulating

116.

Ionic compounds have a regular structure that is called a…

a)

giant ionic lettuce

b)

giant ionic lattice

c)

simple ionic structure

d)

simple ionic lattice

117.

Positive ions and negative ions are attracted by…

a)

intermolecular forces

b)

electrostatic forces

c)

strong covalent bonds

d)

sticky bonds

118.

Electrons are shared in…

a)

pairs

b)

triads

c)

groups of 3

d)

groups of 4

119.

Electron transfer can be shown using…

a)

dot diagrams

b)

cross diagrams

c)

dot and cross diagrams

d)

circle diagrams

120.

Why are alloys harder than metals?

a)

They have more ions

b)

The layers of atoms cannot be distorted

c)

The delocalised electons can move more freely

d)

The atoms are bigger

121.

Which one of these is INCORRECT?

The repeating unit of a polymer is drawn using…

a)

brackets

b)

single bonds

c)

the letter 'n'

d)

double bonds

122.

Complete the sentence. Nanoparticles have a…

a)

small surface area to volume ratio

b)

large surface area to volume ratio

c)

small surface area to length ratio

d)

large surface area to length ratio

123.

[Li]+ and [O]2- would ionically bond to form lithium oxide.

What is the correct empirical formula for this compound?

a)

LiO

b)

Li2O

c)

2LiO

d)

LiO2

124.

Why do ionic compounds have high melting and boiling points?

a)

Lots of energy is needed to break strong electrostatic bonds

b)

Lots of energy is needed to break strong intermolecular forces

c)

Lots of energy is needed to break weak electrostatic bonds

d)

Lots of energy is needed to break weak intermolecular forces

125.

Atoms are most stable when…

a)

they move around

b)

the electrons move

c)

they become charged

d)

they have full outer shells

126.

Which one of these properties of diamond is NOT correct?

a)

High melting point

b)

Hard

c)

Does not conduct electricity

d)

Malleable

127.

What is a polymer?

a)

A chain of monomers

b)

A chain of carbon atoms

c)

A large ionic compound

d)

A metal

128.

When metal atoms lose electrons they become…

a)

elements

b)

negatively charged ions

c)

positively charged ions

d)

chemical bonds

129.

In graphite, how many electrons from each carbon atom are delocalised?

a)

1

b)

2

c)

3

d)

4

130.

What happens during oxidation?

a)

Electrons are gained

b)

Electrons are shared

c)

Protons are lost

d)

Electrons are lost

131.

Most metals have high melting and boiling points because…

a)

they have strong ionic bonds

b)

they have strong intermolecular forces

c)

they have strong covalent bonds

d)

they have strong metallic bonds

132.

What is the process of ionic bonding?

a)

Sharing of electrons

b)

Transfer of electrons

c)

Loss of protons

d)

Gain of neutrons

133.

What is the charge of a nonmetal atom after gaining electrons?

a)

Neutral

b)

Negative

c)

Variable

d)

Positive

134.

How can the number of electrons in an ion be calculated?

a)

By multiplying the atomic number and mass number

b)

By using the charge of the ion

c)

By subtracting the atomic number from the mass number

d)

By adding the atomic number and mass number

135.

Which group of elements forms negative ions with the electronic structure of a noble gas?

a)

Group 5 and 6

b)

Group 1 and 2

c)

Group 3 and 4

d)

Group 6 and 7

136.

What does the ending -ide indicate in the names of compounds?

a)

Contains oxygen

b)

Contains a halide ion

c)

Contains at least 3 elements

d)

Contains a nonmetal negative ion

137.

Which ion is involved in the formation of sodium oxide?

a)

OH- ion

b)

O²- ion

c)

Cl- ion

d)

NO3- ion

138.

What holds together the ions in an ionic compound?

a)

Hydrogen bonds

b)

Ionic bonds

c)

Covalent bonds

d)

Metallic bonds

139.

What is the structure of an ionic compound?

a)

Single ion structure

b)

Random arrangement of ions

c)

Linear arrangement of ions

d)

Regular arrangement of ions

140.

What is the charge of Na+ ion?

a)

+1

b)

+2

c)

-1

d)

0

141.

What is the force that acts in all directions in the lattice of an ionic compound?

a)

Dipole-dipole forces

b)

Covalent bonding

c)

Ionic bonding

d)

Van der Waals forces

142.

What type of bonding occurs between non-metal atoms?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

143.

What type of bonding occurs between non-metal AND metal atoms?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

144.

What type of bonding occurs between metal atoms?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

145.

Are covalent bonds strong or weak?

a)

strong

b)

weak

146.

Covalently bonded substances consist of either simple molecules or giant covalent structures. What are simple molecules?

a)

molecules that contain only a few atoms held together by covalent bonds

b)

structures that contain many atoms, each joined to adjacent atoms by covalent bonds

147.

True of false? Simple molecular substances have low melting and boiling points.

a)

True

b)

False

148.

Why do simple molecular substances have low melting and boiling points?

a)

The intermolecular forces between simple molecules are weak.

b)

The covalent bonds holding the atoms together in a simple molecule are strong. A large number of covalent bonds hold the atoms together in simple molecules.

149.

What happens when a simple molecular substance melts or boils?

a)

The weak intermolecular forces between the molecules break.

b)

Strong covalent bonds between the atoms of the molecule break.

150.

Why do weak intermolecular forces between simple molecules result in low melting and boiling points?

a)

Little energy is needed to break the strong covalent bonds.

b)

Little energy is needed to break the weak intermolecular forces.

c)

Lots of energy is needed to break the weak intermolecular forces.

151.

Simple molecular substances are often ________ or ________ at room temperature because they have low melting and boiling points.

a)

solid

b)

liquid

c)

gas

152.

Do simple molecular substances conduct electricity?

Select yes or no and a reason.

a)

yes

b)

no

c)

Simple molecular substances are held together by weak intermolecular bonds that are easily broken, enabling the molecules to flow and carry charge.

d)

Simple molecular substances don't have any free electrons or an overall electric charge.

153.

Which of the following simple molecular substances conduct electricity?

a)

water

b)

oxygen

c)

carbon dioxide

d)

all of these simple molecular substances

e)

none of these simple molecular substances

154.

Covalently bonded substances consist of either simple molecules or giant covalent structures. What are giant covalent structures?

a)

molecules that contain only a few atoms held together by covalent bonds

b)

structures that contain many atoms, each joined to adjacent atoms by covalent bonds

155.

Which two of the following are examples of giant covalent structures?

a)

graphite

b)

silicon dioxide

c)

oxygen

d)

water

156.

True of false? Giant covalent structures have low melting and boiling points.

a)

true

b)

false

157.

Why do giant covalent structures have very high melting and boiling points?

a)

Giant covalent structures are held together by a large number of strong covalent bonds that require a lot of energy to break them.

b)

Giant covalent structures are held together by a large number of weak intermolecular forces that require a lot of energy to break them.

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