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End of Year 10 Chemistry Revision

Total questions: 184

Worksheet time: 2hrs 20mins

Name
Class
Date
1.

Which statement best describes the fact that gases can be compressed?

a)

The particles in a gas do not have a fixed volume.

b)

The particles in a gas are very far apart.

c)

The particles in a gas have no force of attraction (bonds) between them.

d)

The particles in a gas are constantly moving very rapidly.

2.

A substance has a boiling point of 90°C. What changes occur when it is heated from 50°C to 120°C?

a)

energy of particles increase; attractive forces decrease

b)

energy of particles decrease; attractive forces increase

c)

energy of particles increase; attractive forces increase

d)

energy of particles decrease; attractive forces decrease

3.

The three states of matter are represented by diagrams X, Y and Z. Which change occurs during condensation?

a)

X to Y

b)

X to Z

c)

Y to X

d)

Z to X

4.

In a solid, ___________________. (Select all that apply).

a)

Particles are packed closely together

b)

Particles have a fixed shape

c)

Particles vibrate about their fixed positions

d)

Particles slide across one another

e)

There are strong forces of attraction between particles.

5.

The particles of solids ________________

a)

vibrate about their fixed postions

b)

are able to slide over each other

c)

move about freely at high speeds and in random direction

d)

do not move

6.

Name the process which happens when a solid changes directly to gaseous state

(a)  

7.

Why solids and liquids cannot be compressed?

a)

The particles are closely packed together and there are no empty spaces.

b)

The particles are far apart from one another and there are empty spaces.

c)

The particles are arranged in an orderly manner.

d)

The particles are not arranged in an orderly manner.

8.

The three states of matter are represented by diagrams X, Y and Z. Which change occurs during condensation?

a)

X to Y

b)

X to Z

c)

Y to X

d)

Z to X

9.

The experiment shown in the diagram demonstrates the process of...

(a)  

10.

A 24 carat gold bar is an example of an element. This means it is made of...

a)

Only one atom

b)

Only gold atoms

c)

Only two different atoms

d)

A mixture of atoms

11.

Which two of these could represent an element?

a)
b)
c)
d)
12.

Which two of these are elements?

a)

Water (H2O)

b)

Hydrogen (H2)

c)

Salt 🧂 (NaCl)

d)

Iron (Fe)

e)

Carbon dioxide (CO2)

13.

Which two of these could represent a compound?

a)
b)
c)
d)
14.

Imagine I fill a balloon with some hydrogen gas, then some oxygen gas is added. They do not react. This is an example of..

a)

An element

b)

A mixture

c)

A compound

15.

Which two of these are true?

a)

In a mixture, all the chemicals have reacted together and bonded

b)

In a compound the elements have reacted together and bonded

c)

To make a mixture, the chemicals must be combined in the same amounts every time

d)

In a compound, the atoms are always combined in a specific ratio

16.

A mixture can easily be separated, a compound cannot. Which of these is a compound?

a)
b)
c)
d)

Salt water

17.

Which two of these common chemicals are not mixtures?

a)

Tap water

b)

Air

c)

Milk

d)

Copper

e)

Oxygen

18.

Which two of these mixtures could easily be separated using a filter?

a)

Coffee grinds and coffee

b)

Salt and water

c)

Sand and salt

d)

Sand and water

e)

Oil and water

19.

What is evaporation (or crystallisation) usually used for?

a)

To get clean water from dirty water

b)

To separate a soluble solid (like salt or minerals) from water

c)

To separate hydrogen from water

d)

To separate an insoluble solid (like sand) from water

20.

Which of the following do you think is s pure substance?

a)

Gold

b)

Al

c)

kool-aid

d)

milk

21.

Which of these substances can be a compound?

a)

CO2

b)

C

c)

O2

d)

Red Bull

22.

What is a pure substance that cannot be broken down chemically into simpler substances?

a)

mixture

b)

element

c)

compound

d)

formula

23.

An Element is made up of how many types of atoms?

a)

12

b)

36

c)

58

d)

1

24.

Choose the option that cannot be a chemical symbol.

a)

a

b)

H

c)

O

d)

Cl

25.

What is the result of a CHEMICAL change?

a)

mixture

b)

element

c)

compound

d)

pure substance

26.

What is the building block of all matter?

a)

legos

b)

symbols

c)

letters

d)

elements

27.

Ice melting into water is a ....

a)

chemical change

b)

physical change

28.

Which is NOT a compound?

a)

CO2

b)

H2O

c)

S

d)

SiO2

29.
Which is a solid at room temperature?
a)
Fluorine
b)
Chlorine
c)
Bromine
d)
Iodine
30.
What happens to the reactivity as you go down group 1?
a)
Same
b)
Increase
c)
Decrease
d)
Yes
31.
How many electrons are in the outer shell of halogens?
a)
110
b)
2
c)
7
d)
5
32.
Which 3 Alkali Metals have a density lower than water
a)
Sodium, Potassium, Rubidium
b)
Lithium, Potassium, Rubidium
c)
Rubidium, Caesium, Francium
d)
Lithium, Sodium, Potassium
33.
What group is Fluorine
a)
1
b)
5
c)
6
d)
7
34.
What is the color of chlorine?
a)
Yellow
b)
Green
c)
Red
d)
Brown
35.
State the electronic configuration for Fluorine
a)
2,7
b)
2,6
c)
2,8
d)
2,8,1
36.
What is the electronic configuration of Calcium?
a)
2,8,8,1
b)
2,8,8,3
c)
2,8,8,4
d)
2,8,8,2
37.
Which element is a halogen?
a)
Chlorine
b)
Potassium
c)
Gallium
d)
Titanium
38.
Why is potassium more reactive than lithium
a)
It's valence electron is further from the nucleus
b)
It's got a larger atomic radius
c)
It has more protons
d)
It has a lower density
39.
Which group contains the alkali metals?
a)
7
b)
1
c)
5
d)
3
40.
What are the elements in Group 1 of the periodic table called?
a)
Alkaline Earth Metals
b)
Transition metals
c)
Alkali metals
d)
Alkaline Metals
41.
If you test a solution of aqueous Sodium Hydroxide with universal indicator, what colour will the universal indicator go?
a)
Blue
b)
Green
c)
Red
d)
Orange
42.
Which alkali metal is the most reactive?
a)
Sodium
b)
Lithium
c)
Francium
d)
Rubidium
43.
Which halogen is the most reactive?
a)
Chlorine
b)
Bromine
c)
Fluorine
d)
Iodine
44.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
45.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
46.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
47.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
48.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
49.
What element is will have the most similar physical and chemical properties to the element Sulfur (S)?
a)
Carbon (C)
b)
Phosphorous (P)
c)
Oxygen (O)
d)
Neon (Ne
50.
What element is will have the most similar physical and chemical properties to the element Lithium (Li)?
a)
Sodium (Na)
b)
Magnesium (Mg)
c)
Beryllium (Be)
d)
Calcium (Ca)
51.
What element is will have the most similar physical and chemical properties to the element Bromine (Br)?
a)
Fluorine (F)
b)
Carbon (C)
c)
Krypton (Kr)
d)
Selenium (Se)
52.
Elements that are arranged in __________ have the most similar physical and chemical properties to each other.
a)
periods
b)
groups
53.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
54.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
55.

What do the vertical columns on the periodic table tell us?

a)

The number of orbitals

b)

The number of valence electrons (electrons on the outer most shell)

56.
What is the symbol for Potassium?
a)
P
b)
K
c)
Pb
d)
Pd
57.
What is the symbol for Carbon?
a)
C
b)
Ca
c)
Cl
d)
H
58.
What family is Sodium a part of?
a)
Transition Metals
b)
Halogens
c)
Alkali Metals
d)
Alkaline Earth Metals
59.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
60.
Who first developed the Periodic Table?
a)
Mendeleev
b)
Mosely
c)
Mendella
d)
Murphy
61.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
62.

Which of the following is an alkali metal?

a)

Tin

b)

Carbon

c)

Nitrogen 

d)

Lithium

63.

 Which of the following elements is a metal?

a)

H

b)

Ar

c)

Zn

d)

B

64.

Li, Cs, and Na belong to

a)

Transition metals

b)

Halogens

c)

Alkali metals

d)

Alkaline Earth metal

65.

Hydrogen can be classified as 

a)

Metal

b)

Nonmetal

c)

Alkali metal

d)

Transition metal

66.

As the atomic number increase, ______________ contributes to the increase in atomic size within a group in the periodic table.

a)

a. Electron repulsion 

b)

b. More shielding of the nucleus by electrons from inner to outer energy levels

c)

c. The proton number 

d)

d. The ionic energy

67.

What type of elements are poor conductors of heat and electricity?

a)

transition metals

b)

inner transition metals

c)

metals

d)

nonmetals

68.

Neutron are a sub-atomic particle that

a)

Is found in the nucleus

b)

flying around the nucleus

c)

have a positive charge

d)

have a negative charge

69.

What property is the same for every atom of an element?

a)

energy

b)

mass number

c)

atomic number

d)

number of neutrons

70.

I am a nonmetal

I am in period 2

I am in group 16

a)

Ba

b)

Si

c)

O

d)

S

71.
Boiling Point: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
72.

What is diffusion?

a)

when molecules move

b)

when molecules move from a high concentration to a low concentration

c)

no movement

d)

molecules move everywhere

73.
Atoms have no electric charge because they...
a)
have an equal number of charged and non charged particles
b)
have neutrons in their nuclei
c)
have an equal number of electrons and protons
d)
have an equal number of neutrons and protons
74.
Most of the mass in an atom is concentrated in the...
a)
electrons
b)
nucleus
c)
protons
d)
empty space
75.
What does the nucleus consist of?
a)
Protons + Electrons
b)
Neutrons + Electrons
c)
Atoms
d)
Protons + Neutrons
76.
What is the smallest?
a)
worm
b)
molecule
c)
galaxy
d)
atom
77.

Isotopes are the atoms of the same element with the same number of.............. but different number of............

a)

electrons/neutrons

b)

neutrons/protons

c)

protons/neutrons

d)

electrons/protons

78.
What is an example of an element?
a)
Oxygen
b)
Pure water
c)
Air
d)
Table salt
79.

How can you get salt from salty water?

a)

evaporate the water; then crystallisation

b)

condense the water; then crystallisation

c)

Filtration

80.

What separation method could you use to separate water from ink?

a)

filtration

b)

distillation

c)

electrolysis

81.

Mixtures can be separated using chromatography.

a)

True

b)

False

82.

Ink can be separated by a method of -----------------------------------------------

a)

distillation

b)

filtration

c)

chromatography

d)

sedimentation

83.
A pure substance shows ------------------ spot on chromat gram
a)
0
b)
1
c)
2
d)
3
84.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
85.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
86.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
87.

Nitrogen will ____ electrons to become stable (hint: nitrogen is in group 5).

a)

gain 1

b)

lose 1

c)

gain 3

d)

lose 3

88.

NaCl

a)

ionic bonding

b)

covalent bonding

89.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
90.

What two types of atoms make a covalent bond?

a)

2 Non-metals

b)

1 Non-metal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

91.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
92.

What is the mass number of magnesium?

a)

2

b)

4

c)

12

d)

24

93.

What is the relative molecular mass of fluorine gas, F2?

F = 19

a)

19

b)

38

c)

9

d)

18

94.

Which alkali metal is most reactive out of the following?

a)

lithium

b)

potassium

c)

sodium

95.

Which alkali metal reacts with water to produce a violet flame?

a)

K

b)

Na

c)

Li

d)

DuNo

96.

Which gas is released when the alkali metals react with water?

a)

hydrogen

b)

oxygen

c)

hydroxide

d)

carbon dioxide

97.

Which of the "Halogens" is found in liquid state at room temperature?

a)

Flourine

b)

Astatine

c)

Iodine

d)

Bromine

98.

Which of the "Halogens" has yellowish green color?

a)

Chlorine

b)

Bromine

c)

Flourine

d)

Iodine

99.

What is the electron configuration of the ion that this atom would form?

a)

2,8,2

b)

2,8,1

c)

2,8

d)

2,8,8

100.

What is the correct description of this atom?

a)

It has an atomic number of 3, and an atomic mass of 5

b)

It has an atomic mass of 6, and an atomic number of 6

c)

It has an atomic number of 3, and an atomic mass of 6

d)

It has an atomic mass of 6, and an atomic number of 9

101.

Which of these equations is correctly balanced?

a)

Mg + O2 → 2MgO

b)

2Mg + O2 → MgO

c)

2Mg + O2 → 2MgO

d)

Mg + O2 → MgO

102.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

103.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

104.

What type of elements will form an ionic bond?

a)

Metal + Metal

b)

Non-metal + Non-metal

c)

Metal + Non-metal

d)

None of the above

105.

Which picture is a mixture?

a)

A

b)

B

c)

C

d)

D

106.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
107.
What is the mass number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
108.

A substance that dissolves in a liquid is called the...

a)

Solvent

b)

Solute

c)

Solution

d)

Salient

109.

What is the correct formula of silver nitrate?

a)

AgNO3

b)

AgNO2

c)

Ag(NO3)2

d)

Ag2NO3

110.

What is the correct formula of magnesium sulphate?

a)

Mg(SO4)3

b)

MgSO4

c)

MnSO4

d)

Mg(SO4)2

111.

What is the correct formula of calcium hydroxide?

a)

Ca(OH)3

b)

Ca(OH)2

c)

CaOH

d)

Ca2OH

112.

Which of the following terms describes the structure of iodine, oxygen, and carbon dioxide?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

113.

A measuring cylinder is used to measure the volume of a liquid. What is the volume of the liquid?

a)

43 cm3

b)

46 cm3

c)

48 cm3

d)

54 cm3

114.

Isotopes are the atoms of the same element with the same number of.............. but different number of............

a)

electrons/neutrons

b)

neutrons/protons

c)

protons/neutrons

d)

electrons/protons

115.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

116.

Has a mass of 1/2000th the mass of a proton.

a)

electron

b)

neutron

c)

nucleus

d)

electron cloud

117.

What are valence electrons?

a)

electrons on the first orbital always

b)

nucleus

c)

the outermost shell

d)

electrons on the outermost orbital

118.

What do these isotopes of carbon all have in common?

a)

neutrons & mass number

b)

atomic number and neutrons

c)

atomic number

d)

protons, atomic number, and mass number

119.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
120.

Milk contains water, fat, salt and protein.


Milk is an example of ....

a)

an element

b)

a mixture

c)

a compound

121.

If you were using filtration, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

122.

If you were using simple evaporation, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

123.

If you were using distillation, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

124.

If you were using chromatography, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

125.

75% of naturally occurring chlorine is Cl-35. The remaining chlorine is Cl-37. Which of the below equations shows how to calculate the relative atomic mass of chlorine?

a)

(75x37) + (25x35) / 100 = 35.5

b)

(75x35) + (25x37) / 100 = 35.5

c)

(75x37) + (25x35) / 100 = 35

d)

(75x35) + (25x37) / 100 = 37

126.

Which of the following terms describes the structure of sand, graphite and diamond?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

127.

Which of the following terms describes the structure of sodium, steel, and iron?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

128.

Simple molecular substances have low melting and boiling points because... (tick all statements that help explain it)

a)

they have weak intermolecular forces

b)

it takes more energy to separate the molecules

c)

the covalent bonds are very strong

d)

it takes less energy to separate the molecules

129.

Simple molecular substances do not conduct electricity because... (tick all statements that help explain it)

a)

they have delocalised electrons

b)

they do not have delocalised electrons

c)

they do not contains ions

d)

the covalent bonds are very strong

130.

Diamond is very hard because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the intermolecular forces require a lot of energy to be broken

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that cannot slide over each other

131.

Diamond has a very high melting point because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the intermolecular forces require a lot of energy to be broken

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that cannot slide over each other

132.

Diamond does not conduct electricity because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

it does not have any delocalised electrons or ions

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that cannot slide over each other

133.

Graphite is soft because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the forces between the layers are weak

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that can slide over each other

134.

Graphite has a high melting point because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the forces between the layers are weak

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that can slide over each other

135.

Graphite can conduct electricity because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the electrons can move along the layers from one atom to the next

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that can slide over each other

136.

Which of these are properties of metals? (Tick all that apply)

a)

High densities

b)

High melting and boiling points

c)

Good conductors of heat and electricity

d)

Malleable

137.
Salts produced by the reactions of hydrochloric acid are known as... 
a)
chlorines
b)
nitrates
c)
chlorides
d)
bromides
138.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

139.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
140.

What kind of bond forms when atoms transfer electrons?

a)
ionic
b)
covalent
c)

metallic

d)

molecular

141.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
142.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
143.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

144.
What is the proper name for CaCl2?
a)
Calcium dichloride
b)
Monocalcium dichloride
c)
Calcium chloride
d)
Calcium chlorine
145.

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.

146.

Which two are ionic compounds?

a)

NaCl

b)

HCl

c)

CH4

d)

CaO

147.

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

148.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
149.
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
150.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
151.
What charges attract?
a)
Opposite
b)
Same
152.
What charges repel?
a)
Same
b)
Opposite
153.

What type of bond forms between anions and cations?

a)

covalent

b)

ionic

c)

metallic

d)

all three

154.

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

a)

covalent

b)

ionic

c)

metallic

d)

all three

155.

What is the charge of an electron?

a)

negative

b)

positve

c)

neutral

d)

there is no assigned charge to an electron

156.

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

a)

covalent

b)

ionic

c)

metallic

d)

none of these

157.

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

a)

covalent

b)

ionic

c)

metallic

d)

none of these

158.

Which is an example of a diatomic molecule?

a)

H2O

b)

NaCl

c)

O2

d)

MgS

159.

Dot and cross diagram for O2

a)
b)
c)
d)
e)
160.

What is the chemical formula of magnesium chloride?

a)

MgCl

b)

MgCl2

c)

MgC

d)

MgC2

161.

Dot and cross diagram for CaF2

a)
b)
c)
162.

What type of bonding involves metals ONLY?

a)

Ionic

b)

Covalent

c)

Metallic

163.

What type of bonding involves non-metals ONLY?

a)

Ionic

b)

Covalent

c)

Metallic

164.

What type of bonding involves metals and non-metals?

a)

Ionic

b)

Covalent

c)

Metallic

165.

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

166.

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

167.

Dot and cross diagram for O2

a)
b)
c)
d)
e)
168.

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.

169.

Substances such as  silica, diamond and graphite are

a)
simple covalent molecules
b)
metallic
c)

ionic substances

d)

giant covalent molecules

170.
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 
171.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)
Carbon fiber
d)
Carbon nanotubes
172.
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
173.
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.

174.
What element are diamond and graphite made up of?
a)

Sodium

b)

Carbon

c)

Carbon dioxide

d)

Silicon

175.

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

176.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)

Silica

d)

Salt

177.

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

178.
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.
179.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
180.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
181.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
182.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
183.
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
184.
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

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