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10 Chemistry term 1 revision

Total questions: 162

Worksheet time: 27hrs 0mins

Name
Class
Date
1.
If the reactant particles collide with less than the activation energy, the particles will be rebound, and no reaction will occur.
a)
True
b)
False
2.
With the increase in temperature, the average kinetic energy of the molecules increases, leading to a decrease in number of collisions per unit time.
a)
True
b)
False
3.
The collisions which bring about a chemical reaction are called: 
a)
Consistent collisions
b)
 Normal collisions 
c)
Effective collisions 
d)
None of the above
4.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
5.
Which of the following is/are the fundamental idea(s) of collision theory?
a)
Molecules react by colliding together
b)
The effective collisions must occur with certain minimum amounts of energy 
c)
In a large sample, the greater the number of effective collisions, and the faster the rate of reaction
d)
All of the above
6.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
7.
Under the collision theory, the particles must collide ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
8.

What is the correct formula for the oxide ion?

a)

Ox

b)

O2

c)

O2-

d)

O

9.

The correct name for the CO32- ion is

a)

carbon oxide

b)

nitrate

c)

sulphate

d)

carbonate

10.

What is the name of the compound whose formula is CuSO4 ?

a)

Copper sulphate

b)

Copper sulphide

c)

Copper(II) sulphate

d)

Culcium sulphide

11.

The formula for Magnesium hydroxide is

a)

Mg(OH)2

b)

MgO

c)

HMgO

d)

Mg(OH)

12.

To balance the equation; SO2 + O2 -> SO3, the coefficient to be placed in front of the SO3 is a

a)

1

b)

3

c)

2

d)

1.5

13.

When sulphur dioxide and hydrogen sulphide react to produce sulphur and water, the correct equation is

a)

SO2 + H2S -> 2S + H2

b)

SO2 + 2H2S -> 3S + 2H2O

c)

SO2 + H2S -> S + H2O

d)

SO2 + 2H2S -> S + 2H2O

14.

What is the rate of reaction?

a)

How much energy is needed for a reaction to occur.

b)

The energy required to break a bond.

c)

The time it takes for a reaction to occur.

d)

Collision Theory

15.

What is the purpose of a catalyst?

a)

Helps to slow down a reaction

b)

Raises the activation energy

c)

Lowers the activation energy

d)

Is consumed by the reaction

16.

What factors effect rate of reaction?

a)

Temperature, Concentration, Pressure and Energy

b)

Surface Area, Concentration, Energy and Pressure

c)

Temperature, Pressure, Concentration and Surface area

d)

Pressure, Surface area, Density and Energy

17.

Increasing the temperature of your solution will.......

a)

Not affect the rate of reaction.

b)

Speed up the rate of reaction

c)

Slow down the rate of reaction

18.

Which has more surface area?

a)

Large chunks of chalk

b)

Cube of sugar

c)

Powdered sugar

d)

Small chunks of sugar

19.

How does concentration affect the rate of reaction?

a)

Increasing concentration increases the rate

b)

Increasing concentration decreases the rate

20.

Why does increasing concentration increase the rate of reaction? Tick all correct options.

a)

There is a lower activation energy

b)

There are more particles in the same volume

c)

There are more frequent collisions

d)

The particles have a higher surface area

21.

Why does increasing surface area increase the rate of reaction? Tick all correct options.

a)

There is a lower activation energy

b)

There are more particles in the same volume

c)

There are more frequent collisions

d)

The particles have a higher surface area

22.

This equipment could be used to measure the rate of what type of reaction?

a)

One that produces a gas

b)

One that produces a solid

c)

One that has a colour change

23.

Which of the following reactions occurs at the highest rate?

a)

Photosynthesis

b)

Rusting of iron

c)

Combustion of hydrogen in oxygen

d)

Combustion of magnesium in oxygen

24.

An experiment is carried out to study the effect of concentration on the rate of reaction between sodium thiosulphate and hydrochloric acid.


Graph of the concentration of sodium thiosulphate against 1/time is as shown.


Based on the graph, what is the value of t if the experiment is repeated using sodium

thiosulphate solution 0.025 mol dm-3.

a)

32.3 s

b)

50.0 s

c)

0.020 s

d)

0.031s

25.

Diagram 4 shows the graph of volume of carbon dioxide gas against time when 5 g of marble chips is added to

50 cm3 of 0.2 mol dm-3 hydrochloric acid.


At what time the rate of reaction the highest?

a)

t1

b)

t2

c)

t3

d)

t4

26.

Diagram 7 shows a graph of the volume of gas produced against time for the reaction between zinc granules and hydrochloric acid.


The gradient of the graph decreases with time because

a)

catalyst is not used

b)

volume of mixture decreases

c)

temperature of reaction decreases

d)

concentration of hydrochloric acid decreases

27.

What does the "thermal" in thermal decomposition mean?

a)

sulfur

b)

catalyst

c)

heat

d)

oven

28.

copper(II)carbonate → ___________ + carbon dioxide

a)

copper(I) oxide

b)

copper(II) oxide

c)

copper oxide

d)

copper(III) oxide

29.

What happens when CO2 is bubbled through limewater

a)

It changes from pink to blue

b)

It goes pop

c)

It goes cloudy

d)

It gets hot

30.
What is the chemical formula of calcium carbonate
a)
Ca2CO3
b)
Ca(CO)3
c)
CaCO3
d)
CaCO
31.
How is calcium oxide formed?
a)
thermal decomposition of calcium carbonate
b)
Displacement of calcium carbonate
c)
combustion of calcium carbonate
d)
reaction of calcium and water
32.
What are the products of thermal decomposition of calcium carbonate
a)
calcium oxide only
b)
calcium hydroxide and water
c)
calcium oxide and carbon dioxide
d)
Calcium hydroxide only
33.
General name of chemical that is mainly a building material and is quarried
a)
Limestone
b)
calcium oxide
c)
calcium hydroxide
d)
limewater
34.
How is calcium hydroxide solution produced?
a)
Calcium carbonate and water
b)
Calcium oxide and water
c)
Calcium carbonate and acid
d)
calcium oxide and acid
35.
I add some limestone to hydrochloric acid and I see bubbles given off. What gas is it?
a)
Oxygen
b)
Hydrogen
c)
Carbon dioxide
d)
Chlorine
36.
Why does limestone lose mass as it is heated
a)
Oxygen is given off
b)
Carbon dioxide is given off
c)
The limestone is shrinking
d)
The limestone is evaporating
37.
an aqueous soln turns red lithmus blue . excess addition of which of the following would reverse the change
a)
baking powder
b)
lime
c)
ammonium hydroxide solution
d)
HCL
38.

True or false: a neutral solution has equal amounts of H+ and OH-.

a)

True

b)

False

39.

HCl is found in household products, including some toilet bowl cleaners. Is HCl an acid or a base?

a)

Acid

b)

Base

c)

Neither (Neutral)

40.
hydrochloric acid
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
41.

sulfuric acid

a)

HSO3

b)

H2SO3

c)

H2SO4

d)

H3SO4

42.

sulfuric acid

a)

HSO3

b)

H2SO3

c)

H2SO4

d)

H3SO4

43.
Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide
44.
In a neutralization reaction, what are the products of a reaction between an acid and a base?
a)
Another acid and base
b)
Carbon dioxide and a salt
c)
Water and a salt
d)
Either two acids or two bases
45.

Basic oxide

a)

BaO

b)

P2O5

c)

ZnO

d)

CO2

46.
How are metal oxides formed?
a)
When metals react with oxide.
b)
When metals react with water.
c)
When metals react with air.
d)
When metals react with oxygen.
47.

Which is NOT an amphoteric oxide?

a)

zinc oxide

b)

aluminium oxide

c)

lead (II) oxid

d)

sodium oxide

48.

Which of the followings is an acidic oxide?

a)

SO2

b)

H2O

c)

CO

d)

ZnO

49.

Acids are substances that release H+ ions when dissolved in water.

a)

True

b)

False

50.

Sulfuric acid reacts with sodium carbonate to form

a)

hydrogen gas

b)

carbon dioxide gas

c)

sodium sulfate

d)

water

51.

How are alkalis related to bases?

a)

It refers to strong bases.

b)

It refers to soluble bases.

c)

It refers to bases which react with acids.

d)

It is another name for bases.

52.

Which of the following substances will not react with sodium hydroxide?

a)

sulfuric acid

b)

chlorine

c)

aqueous ammonia

d)

ammonium sulfate

53.

Choose two suitable reactants that can be used to make barium sulfate.

a)

lead(II) sulfate

b)

potassium sulfate

c)

barium nitrate

d)

barium metal

54.

Which of the following is an acid given below?

a)

C2H5OH

b)

CH3COOH

c)

C2H5CHO

d)

All the above

55.
An acid that does not break apart completely.
Range from 4-7 on the pH scale.
a)
Strong Acid
b)
Strong Base
c)
Weak Acid
d)
Weak Base
56.
An acid that breaks apart completely. 0-4 on the pH scale,
a)
Strong Acid
b)
Weak Acid
c)
Weak Base
d)
Strong Base
57.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
58.

aluminium oxide has both acidic and basic properties, therefore it is

a)

a base oxide

b)

an acid oxide

c)

a metalloid oxide

d)

an amphoteric oxide

59.

when a non-metal oxide dissolves in water, the solution formed is a/an

a)

acid

b)

base

c)

alkali

d)

neutral solution

60.

which of the following solutions can turn blue litmus red?

a)

sulphur dioxide in benzene

b)

ammonia in water

c)

hydrogen chloride in methylbenzene

d)

carbon dioxide in water

61.

Metals and acids react to form .....

a)

Salt and hydrogen

b)

Salt and water

c)

Carbon dioxide, salt and water

d)

Hydrogen only

62.

Magnesium + hydrochloric acid-->

a)

Magnesium chloride + water

b)

Magnesium chloride + hydrogen

c)

Magnesium hydrochloride + hydrogen

d)

Magnesium chloride + water + carbon dioxide

63.

Metal carbonates react with acid to form....

a)

Salt, carboxylic acid and water

b)

Salt, carbon dioxide and water

c)

Salt and carbonated water

d)

Salt and hydrogen

64.

Calcium carbonate + hydrochloric acid -->

a)

Calcium chloride + hydrogen

b)

Calcium choride + water

c)

Calcium chloride + carbon dioxide + water

d)

Calcium sulfate + carbon dioxide + water

65.
Which of these is not a noble gas?
a)
Helium
b)
Argon
c)
Nitrogen
d)
Krypton
66.

6.15: Which of these is not a property of noble gases?

a)

Colourless

b)

Odourless

c)

Flammable

d)

Gas at room temperature

67.
The blue atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
68.

What is the trend in boiling point for noble gases?

a)

There is no trend.

b)

Boiling point decreases down the group.

c)

Boiling point increases down the group.

d)

All the boiling points are the same.

69.

What is the percentage composition of nitrogen in air?

a)

78%

b)

75%

c)

86%

70.

Acid rain can be traced back to

a)

the burning of fossil fuels.

b)

the use of electrostatic precipitators.

c)

thermal inversions.

d)

the release of particulate matter into the atmosphere.

71.
Increase in which gas is primarily responsible for increased global warming?
a)
Carbon dioxide
b)
Water vapor
c)
Methane
d)
Nitric oxides
72.
A metallic element that can cause brain damage
a)
Lead
b)
Particulate matter
c)
Ground-level ozone
d)
Nitrogen oxides
73.

During the purification process, filtration separates the

a)

Solid purities

b)

Solid impurities

74.
What does chlorination do to the water?
a)
Removes microorganisms
b)
Cleans the water
c)
Makes the water taste nice
d)
Removes twigs and sediment
75.

Steel generally speaking is made of

a)

iron and carbon

b)

copper and iron

c)

tin and carbon

d)

aluminum and nickel

76.
Definite shape and a definite volume.
a)
Gas
b)
Liquid
c)
Solid
77.
When the temperature of matter decreases the particles ...
a)
speed up and move farther apart
b)
speed up and move closer together
c)
slow down and move farther apart
d)
slow down and move closer together
78.

What happens to the average kinetic energy of matter when it is heated?

a)

It increases

b)

It stays the same

c)

It decreases

d)

It cannot be determined

79.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

80.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

81.

How many valence electrons does Mg have? (use the PTable)

a)

1

b)

2

c)

3

d)

4

e)

5

82.

Atoms are most stable when their outer shell is complete.

a)

True

b)

False

83.

Why do elements form chemical bonds?

a)

Because they're friendly

b)

To create a new element

c)

To become stable

d)

Because they all need to gain more electrons

84.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

85.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

86.

Write the chemical formula for K and Br (potassium bromide).

a)

KBr

b)

K2Br

c)

KBr3

d)

KBr2

87.

Metals (like Na) typically _____ electrons in the formation of ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

88.

Write the chemical formula for Na and S (sodium sulfide).

a)

NaS

b)

S2S2

c)

Na2S

d)

NaS2

89.

Why are there two sodiums (Na), in the formation of this ionic compound?

a)

There always has to be 2 metals

b)

The overall charge needs to add up to 4

c)

The overall charge has to be 0

d)

It needs to have more metal atoms than nonmetal

90.

How does oxygen become an oxide ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

c)

it shares electrons

d)

it releases energy

91.

Aluminum will react spontaneously with oxygen in the air to form aluminum oxide. Write the formula for the compound that is produced in this reaction.

a)

AlO

b)

Al2O3

c)

O3Al2

d)

Al6O3

92.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
93.

Correct diagram for HF

a)
b)
c)
d)
94.

Correct diagram for CF4

a)
b)
c)
95.

Correct diagram for  N2N_2  

a)
b)
c)
d)
96.

Name the following: C3H8

a)

Tricarbon octahydride

b)

Carbon hydride

c)

Carbon octahydride

d)

Tricarbon hydride

97.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

98.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
99.

Ionic bond is formed between _____________________________.

a)

metal atom with metal atom

b)

metal atom with non-metal atom

c)

non-metal atom with non-metal atom

100.
How many "valance electrons" are in chlorine?
a)
7
b)
2
c)
17
d)
8
101.
Carbon-12, Carbon-13, and Carbon-14 are...
a)
ions
b)
isotopes
c)
electronegative
d)
radioactive
102.
How many Protons does Bromine have?
a)
45
b)
79.904
c)
80
d)
35
103.
A particle with a negative charge inside of an element is called
a)
isotope
b)
neutron
c)
proton
d)
electron
104.
Nitrogen has 5 valence electrons
a)
True
b)
False, it has 7
c)
False, it has 14
d)
False, it has 7.01
105.
An isotope has...
a)
the same number of protons but different number of electrons
b)
same number of protons but different number of neutrons
c)
same number of electrons and neutrons
d)
same number of electrons, protons, and neutrons
106.
Elements that are gases, brittle, and not conductive are
a)
Metals
b)
Metalloids
c)
Transition Metals
d)
Non-metals
107.
The atomic mass of Boron is 10.81, which means Boron has..
a)
5 electrons and 6 protons, each weigh 1 amu
b)
5 neutrons and 6 electrons, each weigh 1 amu
c)
6 neutrons and 5 protons, each weigh 1 amu
d)
10.81 protons each weighing around 1 amu
108.

I am usually a good conductor and shiny/lustrous

a)

Metal

b)

Metalloid

c)

Non-metal

109.

I am Chlorine many electrons to I need to be complete?

a)

8

b)

7

c)

1

d)

0

110.

Elements in the same group or family have _____________.

a)

the same number of valence electrons and different properties.

b)

the same number of valence electrons and similar properties

c)

different number of valence electrons and similar properties.

d)

different number of valence electrons and different properties.

111.

A column of the periodic table is a ________.

a)

group

b)

period

c)

range

112.

A row on the periodic table is a _______.

a)

group

b)

period

c)

range

113.

Group 1 metals that react quickly with other elements are ___________.

a)

metals

b)

alkaline earth metals

c)

alkali metals

d)

nonmetals

114.

Oxygen (O) has a greater mass than chlorine (Cl).

a)

True

b)

False

115.
Sodium (Na) is found in period 
a)
3
b)
2
c)
4
d)
1
116.
Sodium (Na) is found in group 
a)
1
b)
2
c)
3
d)
4
117.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
118.
What is the atomic mass equal to?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
119.

Going across Period 3, the properties of the oxides changes from

a)

acidic to basic to amphoteric

b)

amphoteric to basic to acidic

c)

acidic to amphoteric to basic

d)

basic to amphoteric to acidic

120.
Which of the following is the most reactive in water?
a)
Lithium
b)
Sodium
c)
Potassium
121.
What is formed when sodium reacts with water?
a)
sodium oxide and hydrogen
b)
sodium hydroxide and hydrogen
c)
sodium hydroxide and oxygen
d)
sodium hydroxide and carbon dioxide
122.
What is the symbol equation for the reaction between sodium hydroxide and water?
a)
2Na + 2H2O → 2NaOH + H2
b)
Na + H2O → NaOH + H
c)
Na + H20 → NaCl + CO2
d)
2Na + 2H2O → 2NaH2 + O2
123.
What is another name for the elements in group 7?
a)
The Halogens
b)
The Noble gases
c)
The Oxides
d)
The Alkali Metals
124.

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

a)

Flourine

b)

Astatine

c)

Iodine

d)

Bromine

125.
At room temperature, iodine is a....
a)
Gas
b)
Liquid
c)
Solid
126.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

127.

Which halogens can displace bromide ions to make bromine?

a)

Fluorine and iodine.

b)

Fluorine and bromine.

c)

Fluorine and chlorine

d)

Chlorine and iodine.

128.
What type of ions do the Group 7 elements make?
a)
positive 2 (+2)
b)
positive 1 (+1)
c)
negative 1 (-1)
d)
negative 2 (-2)
129.

Would a displacement reaction occur for Bromine + Potassium Iodide?

a)

Yes

b)

No

c)

Maybe

130.
The physical separation of mixtures into individual components is..
a)
chromatography
b)
opacity 
c)
latent
d)
trace evidence 
131.
On the chromatogram given -------------- is mixture.
a)
red
b)
orange
c)
green
d)
black
132.
A pure substance shows ------------------ spot on chromat gram
a)
0
b)
1
c)
2
d)
3
133.
The diagram shows the chromatogram for three colouring dyes and that for a brown marker. What dye(s) are contained in the marker's ink?
a)
purple and green
b)
purple and yellow
c)
purple only
d)
green and yellow
134.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
135.
Why must the base line be drawn in pencil and not pen?
a)
a) Pencil is good at keeping substances in place.
b)
b) Pencil is soluble in water
c)
c) Pencil is insoluble in water
d)
d) Pencil is not coloured
136.
In chromatography, if a solute does not separate and remains on the start line ....
a)
the solute is insoluble in the solvent
b)
the solute is soluble in the solvent
c)
the solvent is insoluble in the solute
d)
the solvent is soluble in the solute
137.
The retention factor is used
a)
to zero the chromatography scale
b)
to identify unknown compounds in a sample
c)
to retain solvent
d)
as a starting tool for chromatography
138.
The diagram shows the apparatus for separating soil and water. What are the labelled parts?
a)
A = distillate, B = filtrate
b)
A = filtrate, B = residue
c)
A = residue, B = filtrate
d)
A = residue, B = distillate
139.
a)

Ethanol has a higher boiling point than water.

b)

Ethanol has a lower melting point than water.

c)

Ethanol has a higher melting point than water.

d)

Ethanol has a lower boiling point than water.

140.
a)

A

b)

B

c)

C

d)

D

141.

What allows us to know when the end point has been reached?

a)

Bubbles

b)

Feels warm

c)

indicator changing color

d)

Turns to a solid

142.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
143.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

144.

What are some things we will need for a titration?

a)

A solution of known concnetration

b)

A burette

c)

indicator

d)

mass balance

e)

a bunsen burner

145.

What is the reading on this burette?

a)

24.0cm3

b)

25.8cm3

c)

24.2cm3

d)

23.9cm3

146.

What is the colour of methyl orange an acid ?

a)

Pink

b)

Yellow

c)

Orange

d)

Colourless

147.

What is the colour of phenolphthalein an acid?

a)

Pink

b)

Yellow

c)

Orange

d)

Colourless

148.

How do you remove the water to leave solid copper sulfate crystals?

a)

Filter

b)

Evaporate

c)

Distill

149.

What is the name of the practical technique to neutralise an alkali?

a)

Neutralisation

b)

Titration

c)

Using a burette

d)

Telestration

150.

What does the word insoluble mean?

a)

Does dissolve

b)

Doesn't dissolve

c)

Is part of a solid

151.
Salts that are made with hydrochloric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
152.

How do you separate an excess insoluble reactant from a solution?

a)

Filtration

b)

Precipitation

c)

Crystalisation

d)

Evaporation

153.
Salts that are made with nitric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
154.
Identify the 'evaporating basin' from the diagrams.
a)
A
b)
B
c)
C
d)
D
155.

Why do you add excess of the insoluble reactant when making a soluble salt?

a)

To make sure all the acid is used up

b)

To separate the solid from the solution

c)

To make sure a reaction occurs

d)

To have the reaction happen faster

156.

When producing a soluble salt in a reaction between an acid and an alkali, how can you prepare dry solid crystals from the solution?

a)

Filtration

b)

Neutralisation

c)

Condensation

d)

Evaporation/crystallisation

157.

When a soluble salt is formed from reacting an acid and with an insoluble base, how do you know when an excess of a base has been added?

a)

There is effervescence

b)

When the reactant all dissolves

c)

When some of the reactant is left unreacted/undissolved

d)

When a colour change happens

158.

Which method is used to produce an insoluble salt?

a)

Neutralisation reaction

b)

Precipitation reaction

c)

Titration reaction

d)

Adding excess insoluble base to an acid

159.

Which of the following is NOT part of the definition of salt?

a)

Ionic compound

b)

when hydrogen ion of an acid

c)

is replaced by a metal cation or ammonium ion

d)

contains hydrogen ions

160.

Which of the following statements best define the term ‘salt’?

a)

Salt is formed when metal reacts with an alkali.

b)

Salt contains sodium ions and chloride ions.

c)

Salt is formed from a weak Van der Waals’ forces of attraction.

d)

Salt is formed when the hydrogen ions in an acid is replaced by metal or ammonium ions.

161.

What is the best method for removing water from a hydrated compound?

a)

freezing

b)

filtration

c)

distillation

d)

heating

162.

What is the colour of hydrated Copper (II) sulphate?

a)

White

b)

Blue

c)

Pink

d)

Brown

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