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MIDTERMS_IGCSE Chemistry

Total questions: 205

Worksheet time: 3hrs 38mins

Name
Class
Date
1.

1 A method used to make copper(II) sulfate crystals is shown. 1 Place dilute sulfuric acid in a beaker.

2 Warm the acid.

3 Add copper(II) oxide until it is in excess.

4 Filter the mixture.

5 Evaporate the filtrate until crystals start to form.

6Leave the filtrate to cool. What are the purposes of step 3 and step 4?

a)

A

b)

B

c)

C

d)

D

2.

What is the correct sequence of steps for the preparation of a pure sample of copper(II) sulfate crystals from copper(II) oxide and sulfuric acid?

a)

A dissolving → crystallisation → evaporation → filtration

b)

B dissolving → evaporation → filtration → crystallisation

c)

C dissolving → filtration → crystallisation → evaporation

d)

D dissolving → filtration → evaporation → crystallisation

3.

Four stages in the preparation of a salt from an acid and a solid metal oxide are listed.

1 Add excess solid.

2Evaporate half the solution and leave to cool.

3 Filter to remove unwanted solid.

4 Heat the acid. In which order should the stages be carried out?

a)

A 1 → 3 → 4 → 2

b)

B 2 → 1 → 3 → 4

c)

C 4 → 1 → 3 → 2

d)

D 4 → 2 → 1 → 3

4.

Zinc sulfate is a soluble salt and can be prepared by reacting excess zinc carbonate with dilute sulfuric acid. Which piece of equipment would not be required in the preparation of zinc sulfate crystals?

a)

A beaker

b)

B condenser

c)

C evaporating dish

d)

D filter funnel

5.

Four steps to prepare a salt from an excess of a solid base and an acid are listed.

1 crystallisation

2 evaporation

3 filtration

4 neutralisation

In which order are the steps carried out?

a)

A 2 →

b)

B 3 →

c)

C 4 →

d)

D 4 →

6.

Which method is used to make the salt copper sulfate?

a)

dilute acid + alkali

b)

dilute acid + carbonate

c)

dilute acid + metal

d)

dilute acid + non-metal oxide

7.

Which two processes are involved in the preparation of magnesium sulfate from dilute sulfuric acid and an excess of magnesium oxide?

a)

neutralisation and filtration

b)

neutralisation and oxidation

c)

thermal decomposition and filtration

d)

thermal decomposition and oxidation

8.

Hydrochloric acid is used to clean metals. The acid reacts with the oxide layer on the surface of the metal, forming a salt and water. Which word describes the metal oxide?

a)

A alloy

b)

B base

c)

C element

d)

D indicator

9.

Which statement is not correct?

a)

A When a base reacts with an ammonium salt, ammonia is given off.

b)

When an acid reacts with a base, neutralisation takes place.

c)

When an acid reacts with a carbonate, carbon dioxide is given off.

d)

When the acidity of a solution increases, the pH increases.

10.

Which reaction is not characteristic of an acid?

a)

It dissolves magnesium oxide.

b)

It produces ammonia from ammonium compounds

c)

It produces carbon dioxide from a carbonate.

d)

It produces hydrogen from zinc metal.

11.

What type of reaction produced an insoluble salt?

a)

Neutralisation reaction

b)

Precipitation reaction

c)

Titration reaction

d)

Insoluble reaction

12.

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

a)

When bubbles of gas appear

b)

When the reactant all dissolves

c)

When some of the reactant is left unreacted/undissolved

d)

When a colour change happens

13.

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

14.

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

a)

Filtration

b)

Precipitation

c)

Crystalisation

d)

Evaporation

15.

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

16.

What is the purpose of a titration when making pure salts?

a)

To test if reactants react.

b)

To determine the exact quantities needed for neutralisation

c)

To calculate the concentration of the salt

d)

To test quality of reactants.

17.

Complete the following word equation:

Metal + Acid -->

a)

Salt + water

b)

Salt + hydrogen

c)

Salt + Water + Carbon dioxide

18.
Salts that are made with hydrochloric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
19.
Salts that are made with nitric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
20.
What salt is produced if you react sodium hydroxide with hydrochloric acid?
a)
sodium hydroxide
b)
sodium sulfate
c)
sodium nitrate
d)
sodium chloride
21.

pH is the measure of the concentration of ______.

a)

Acids

b)

H+ ion

c)

OH- ion

d)

Bases

22.

What is the definition of an ACID?

a)

a substance that contains hydroxide and ionizes to produce OH-

b)

a substance that contains hydrogen and ionizes to produce H+

c)

a substance that contains hydrogen and ionizes to produce OH-

d)

a substance that contains hydroxide and ionizes to produce H+

23.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
24.

A substance that changes colour when mixed with an acid or base is a(n) ___.

a)

indicator

b)

neutraliser

c)

corrosive

d)

electricity

25.
What color does litmus paper turn in the presence of an acid?
a)
blue
b)
black
c)
green
d)
red
26.
Bases are located where on the pH scale?
a)
any number can be a base
b)
below 7
c)
above 7
d)
number 7 is a base
27.

When making an insoluble salt, why do we wash the filter paper with distilled water?

a)

to remove insoluble impurities

b)

to remove soluble impurities

c)

to rinse more product through the filter paper

d)

to make a more dilute solution

28.

When carrying out a titration, what is the name of the equipment used to add incremental amounts of acid to the conical flask?

a)

glass pipette

b)

measuring cylinder

c)

separating funnel

d)

burette

29.

What is the colour change observed with phenolphthalein when adding acid to alkali?

a)

pink --> colourless

b)

blue --> red

c)

orange --> pink

d)

green --> yellow

30.

Which of the following is the correct definition for a strong acid?

a)

Partially dissociates into ions when dissolved in water

b)

Fully dissociates into ions when dissolved in water

c)

a larger proportion of acid to water molecules

d)

a smaller proportion of acid to water molecules

31.

Three liquids, P, Q and R, are added to a mixture of hydrochloric acid and Universal Indicator solution.

The following observations are made.

P the colour of the indicator turns purple.

Q the colour of the indicator does not change.

R there is effervescence and the indicator turns blue.

What are P, Q and R?

a)

A P = sodium carbonate solution; Q= water; R = sodium hydroxide solution

b)

B P = sodium hydroxide solution; Q= water; R = sodium carbonate solution

c)

C P = water; Q= sodium carbonate solution; R = sodium hydroxide solution

d)

D P = water ; Q= sodium hydroxide solution ; R = sodium carbonate solution

32.

What does the word insoluble mean?

a)

Does dissolve

b)

Doesn't dissolve

c)

Is part of a solid

33.

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

a)

When bubbles of gas appear

b)

When the reactant all dissolves

c)

When some of the reactant is left unreacted/undissolved

d)

When a colour change happens

34.

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

35.

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

a)

Filtration

b)

Precipitation

c)

Crystalisation

d)

Evaporation

36.

Which is NOT a step when making insoluble salts?

a)

mix

b)

filter

c)

rinse

d)

crystallise

37.

In the diagrams, circles of different sizes represent atoms of different elements. Which diagram represents hydrogen chloride gas?

a)

A

b)

B

c)

C

d)

D

38.

The diagram shows part of the Periodic Table. AA

a)

A

b)

B

c)

C

d)

D

39.

3 The diagram shows a section of the Periodic Table.

a)

V, W and X

b)

V, Y and W

c)

W, X and Z

d)

Y and Z

40.

4 Which statement is correct for the element of proton number 19?

a)

It is a gas that dissolves in water.

b)

It is a hard metal that is not very reactive with water.

c)

It is a non-metal that burns quickly in air.

d)

It is a soft metal that is highly reactive with water.

41.

5 The table shows the results of adding three metals, P, Q and R, to dilute hydrochloric acid and to water.

a)

A

b)

B

c)

C

d)

D

42.

6 Which two substances, when reacted together, would form a salt that contains two of the essential elements provided by fertilisers?

a)

potassium hydroxide and nitric acid

b)

potassium hydroxide and sulfuric acid

c)

sodium hydroxide and nitric acid

d)

sodium hydroxide and sulfuric acid

43.

7 Statement 1: Alloying iron with other materials to form stainless steel prevents iron from rusting by excluding oxygen.

Statement 2: Painting, oiling and electroplating are all methods of preventing iron from rusting. Which is correct?

a)

Both statements are correct and statement 2 explains statement 1.

b)

Both statements are correct but statement 2 does not explain statement 1.

c)

Statement 1 is correct but statement 2 is incorrect.

d)

Statement 2 is correct but statement 1 is incorrect.

44.

8 What is the main constituent of natural gas?

a)

carbon dioxide

b)

ethane

c)

hydrogen

d)

methane

45.

9 What is not essential for the formation of ethanol by fermentation?

a)

light

b)

sugar

c)

yeast

d)

water

46.

10 Which row describes the conditions used to make steel from the iron produced by a blast furnace?

a)

A

b)

B

c)

C

d)

D

47.

State the symbol of the element that has the atomic number of 12? (1)

4 lines
48.

State the symbol of the element that has a relative atomic mass of 12 (1)

4 lines
49.

State the number of the group that contains the noble gases. (1)

4 lines
50.

which group contains elements whose atoms form ions with a 2+ charge? (1)

4 lines
51.

Which group contains elements whose atoms form ions with a 1- charge? (1)

4 lines
52.

Sodium is a very reactive metal. It floats on water and reacts rapidly with water.

A small piece of sodium is placed in a trough of water. A reaction takes place and hydrogen gas is given off.


Give two observations, other than the sodium floating, that you could make during the reaction. (2)

4 lines
53.

Write a word equation for the reaction of sodium with water. (1)

4 lines
54.

Universal indicator is added to the water in the trough of sodium with water. State what colour it turns and explain why. (2)


Colour


Explanation

4 lines
55.

Give one observation that will be different if potassium is used in place of sodium when added to water. (1)

4 lines
56.

Three of the elements in Group 7 of the Periodic Table are chlorine, bromine and iodine.


Give the electronic configuration of chlorine (1)

4 lines
57.

How many electrons are there in the outer shell of an atom of iodine? (1)

4 lines
58.

Bromine reacts with hydrogen to form hydrogen bromide. The chemical equation for the reaction is:

Br2(g) + H2(g) → 2HBr(g)

Describe the colour change occurring during the reaction.

Colour change (1)

4 lines
59.

Hydrogen bromide and hydrogen chloride have similar chemical properties.


A sample of hydrogen bromide is dissolved in water. A piece of blue litmus paper is placed in the solution. State, with a reason the final colour of the litmus paper. (2)


Colour


Explanation

4 lines
60.

If a mixture of hydrogen and chlorine is exposed to sunlight a violent reaction takes place. The only product is hydrogen chloride.


Write a chemical equation for the reaction (1)

4 lines
61.
Which is a solid at room temperature?
a)
Fluorine
b)
Chlorine
c)
Bromine
d)
Iodine
62.
What happens to the reactivity as you go down group 1?
a)
Same
b)
Increase
c)
Decrease
d)
Yes
63.
Which is a solid at room temperature?
a)
Fluorine
b)
Chlorine
c)
Bromine
d)
Iodine
64.
What happens to the reactivity as you go down group 1?
a)
Same
b)
Increase
c)
Decrease
d)
Yes
65.
How many electrons are in the outer shell of halogens?
a)
110
b)
2
c)
7
d)
5
66.
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
67.
What group is Fluorine
a)
1
b)
5
c)
6
d)
7
68.
What is the color of chlorine?
a)
Yellow
b)
Green
c)
Red
d)
Brown
69.
State the electronic configuration for Fluorine
a)
2,7
b)
2,6
c)
2,8
d)
2,8,1
70.
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
71.
Which element is a halogen?
a)
Chlorine
b)
Potassium
c)
Gallium
d)
Titanium
72.
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
73.
Which group contains the alkali metals?
a)
7
b)
1
c)
5
d)
3
74.
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
75.
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
76.
Which is an alkali earth
a)
Magnesium
b)
Silicon
c)
Lithium
d)
Bohrium
77.
What is the charge of a Arsenic Ion
a)
+ 5
b)
-5
c)
Arsenic cannot form an ion
d)
Bruh
78.
Which alkali metal is the most reactive?
a)
Sodium
b)
Lithium
c)
Francium
d)
Rubidium
79.
Sodium burns with what colour flame to form sodium oxide?
a)
Yellow
b)
Red
c)
Lilac
d)
Blue
80.
what is the mass number of osmium
a)
136
b)
190
c)
137
d)
136.5
81.
What colour are Group 1 metal ions?
a)
Green
b)
Colourful in general
c)
Colourless
d)
Purple
82.
What is the meaning of “halogens” ?
a)
Very reactive
b)
Salt-producing
c)
Sun
d)
Very unreactive
83.
Which halogen is the most reactive?
a)
Chlorine
b)
Bromine
c)
Fluorine
d)
Iodine
84.
What gas is Caesium stored in?
a)
Argon
b)
Tungsten
c)
Livermorium
d)
Fluorine
85.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
86.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
87.
Which element could be lustrous and brittle?
a)
A
b)
B
c)
G
d)
L
88.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

89.
Which element has a full valence shell?
a)
F
b)
D
c)
C
d)
E
90.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

91.
Which elements have the same number of valence electrons?
a)
A & C
b)
E & C
c)
F & A
d)
F & B
92.
Which element belongs to the group that is made up of only gases?
a)
D
b)
L
c)
E
d)
A
93.
Which elements are in the same period?
a)
A & F
b)
F, B & D
c)
E & D
d)
F & B
94.
Is silicon a metal, nonmetal or metalloid?
a)
Metal
b)
NonMetal
c)
Metalloid
95.
Is this a metal, nonmetal or metalloid?
a)
Metal
b)
Nonmetal
c)
Metalloid
96.
In which group does this atom belong?
a)
1
b)
3
c)
13
d)
11
97.
How many energy levels does an atom of Chlorine have?
a)
2
b)
3
c)
4
d)
7
98.
Which element has the same number of valence electrons as this element?
a)
Bromine (Br)
b)
Nitrogen (N)
c)
Calcium (Ca)
d)
Boron (B)
99.
How many valence electrons does an atom of oxygen have?
a)
2
b)
5
c)
6
d)
16
100.
List the two most reactive families on the periodic table.
a)
Alkali metals & Transition Metals
b)
Noble gases & Oxygen Family
c)
Halogens & Alkali metals
d)
Halogens & Noble gases
101.

Which element is located in period 4?

a)

Zirconium (Zr)

b)

Silicon (Si)

c)

Beryllium (Be)

d)

Iron (Fe)

102.

Which element is located in group 3?

a)

Yttrium (Y)

b)

Carbon (C)

c)

Sodium (Na)

d)

Lithium (Li)

103.

Two elements that have similar physical and chemical properties are most likely in the same...

a)

period

b)

row

c)

group

104.

In which group would an element that is not reactive most likely be located?

a)

1

b)

2

c)

16

d)

18

105.

In which group would an element that is very reactive most likely be located?

a)

1

b)

5

c)

15

d)

18

106.

Which of the following elements is most likely a poor conductor of electricity?

a)

Beryllium (Be)

b)

Gold (Au)

c)

Phosphorus (P)

d)

Copper (Cu)

107.

Which trends in physical properties are correct for the alkali metals down Group I?

a)

A

b)

B

c)

C

d)

D

108.

The diagram shows a sack containing a mixture of three minerals. Which element is not present in the mixture?

a)

Cobalt

b)

Copper

c)

Iron

d)

Tin

109.

An element is in Group VI of the Periodic Table. What information does this give about the element?

a)

the number of protons in the nucleus

b)

the number of outer electrons

c)

the reactivity of the element

d)

the relative atomic mass of the element

110.

An atom has 2 electrons in its outer shell. Which element could this atom be?

a)

A

b)

B

c)

C

d)

D

111.

It is unusual for a hot drink to be served in a metal cup. Why is this?

a)

Metals are usually hard.

b)

Metals are usually strong.

c)

Metals have high porosity.

d)

Metals have high thermal conductivity.

112.

Which trends in physical properties are correct for the alkali metals down Group 1?

a)

A

b)

B

c)

C

d)

D

113.

Which Group I metal and which Group VII non-metal react together most vigorously?

a)

A

b)

B

c)

C

d)

D

114.

How many atoms of metals and of non-metals are shown in the formula Na2SO4?

a)

A

b)

B

c)

C

d)

D

115.

What is the trend for atomic radius (radii)?

a)

It increases left to right on the Periodic Table and decreases down a group.

b)

It decreases left to right on the Periodic Table and increases down a group.

c)

It increases left to right on the Periodic Table and increases down a group.

d)

It decreases right to left on the Periodic Table and decreases down a group.

116.

Where are metalloids located on the Periodic Table?

a)

In the s block.

b)

In the f block.

c)

In the d block.

d)

The elements that touch the staircase except aluminum.

117.

Why does the atomic radius decrease across a period?

a)

There are more protons in the nucleus that pull electrons closer.

b)

There are more electrons in the nucleus that pull protons closer.

c)

There are more protons in the nucleus that pull neutrons closer.

d)

There are more neutrons in the nucleus that pull protons closer.

118.

What does the atomic radius increase down a group?

a)

There are more electrons and energy levels.

b)

There are fewer electrons and energy levels.

c)

There are more protons that need more energy levels.

d)

There are more neutrons that need more energy levels.

119.

What element has the largest atomic radius?

a)

oxygen

b)

neon

c)

carbon

d)

sodium

120.

What is the trend for ionization energy?

a)

Across a period (left to right) it increases and down a group it decreases.

b)

Across a period (left to right) it decreases and down a group it increases.

c)

Across a period (left to right) it decreases and down a group it decreases.

d)

Across a period (left to right) it increases and down a group it increases.

121.
a)
Periods
b)
Groups
122.
a)
Periods
b)
Groups
123.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
124.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
125.
a)
Same group
b)
Same period
126.
Which element could be lustrous and brittle?
a)
A
b)
B
c)
G
d)
L
127.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

128.
Which element has a full valence shell?
a)
F
b)
D
c)
C
d)
E
129.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

130.
Which elements have the same number of valence electrons?
a)
A & C
b)
E & C
c)
F & A
d)
F & B
131.
Which element belongs to the group that is made up of only gases?
a)
D
b)
L
c)
E
d)
A
132.
Which elements are in the same period?
a)
A & F
b)
F, B & D
c)
E & D
d)
F & B
133.
Is silicon a metal, nonmetal or metalloid?
a)
Metal
b)
NonMetal
c)
Metalloid
134.
Is this a metal, nonmetal or metalloid?
a)
Metal
b)
Nonmetal
c)
Metalloid
135.

To which group does this atom belong?

a)

1

b)

3

c)

13

d)

11

136.
How many energy levels does an atom of Chlorine have?
a)
2
b)
3
c)
4
d)
7
137.
What is the group number of this atom?
a)
2
b)
7
c)
14
d)
15
138.
Which element has the same number of valence electrons as this element?
a)
Bromine (Br)
b)
Nitrogen (N)
c)
Calcium (Ca)
d)
Boron (B)
139.
How many valence electrons does an atom of oxygen have?
a)
2
b)
5
c)
6
d)
16
140.
List the two most reactive families on the periodic table.
a)
Alkali metals & Transition Metals
b)
Noble gases & Oxygen Family
c)
Halogens & Alkali metals
d)
Halogens & Noble gases
141.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)
Sodium is less electronegative than potassium. 
b)
Sodium has fewer energy levels than potassium. 
c)
Sodium has a larger ionic radius than potassium. 
d)
Sodium has lower ionization energy than potassium. 
142.
How can you tell that a metal is reacting with water?
a)
Colour change
b)
Bright light
c)
Fizzing
d)
It gets colder
143.
How can you test to show that when a metal reacts with water, hydrogen gas is produced?
a)
Relights a glowing splint
b)
A lit splint produces a squeaky pop
c)
Puts out a burning splint
d)
Is cold to the touch
144.

Complete the general equation:

Metal + Acid ->

a)

Salt + Water

b)

Salt + Hydrogen

c)

Salt

145.

Complete the general equation:

Metal + Water ->

a)

Salt + Water

b)

Metal Hydroxide + Hydrogen

c)

Metal hydroxide + Water

d)

Salt + Hydrogen

146.

Complete the equation:

Sodium + Hydrochloric Acid ->

a)

Sodium Hydroxide + Hydrogen

b)

Sodium Chloride + Hydrogen

c)

Chloric Sodium + Hydrogen

d)

Sodium Chloride + Water

147.

Complete the equation:

Potassium + Nitric Acid ->

a)

Potassium Hydroxide + Hydrogen

b)

Potassium Chloride + Hydrogen

c)

Potassium Nitrate + Hydrogen

d)

Nitric Potassium + Hydrogen

148.
What gas is produced when sodium reacts with water?
a)
Hydrogen
b)
Carbon dioxide
c)
Carbon monoxide
d)
Water vapour
149.

Complete the equation:

Potassium + Water ->

a)

Potassium Hydroxide + Hydrogen

b)

Potassium Chloride + Hydrogen

c)

Potassium Hydroxide + Water

d)

Nitric Potassium + Hydrogen

150.
Which salt will be produced if magnesium react with hydrochloric acid?
a)
Magnesium oxide
b)
Magnesium sulfate
c)
Magnesium sulfide
d)
Magnesium chloride
151.

Will a displacement reaction occur?

Copper Oxide + Magnesium ->

a)

Yes

b)

No

152.

Will a displacement reaction occur?

Magnesium Sulphate + Zinc ->

a)

Yes

b)

No

153.

Will a displacement reaction occur?

Iron Sulphate + Calcium ->

a)

Yes

b)

No

154.
What are the reactants for the reaction of metal with water?
Metal + water ---> metal hydroxide + hydrogen
a)
Metal
b)
Water
c)
Metal and water
d)
Metal hydroxide and hydrogen
155.
What metal hydroxide is produced when magnesium reacts with water?
a)
Copper hydroxide
b)
Magnesium oxide
c)
Magnesium
d)
Magnesium hydroxide
156.

Choose the most reactive metal

a)

calcium

b)

magnesium

c)

iron

d)

copper

157.

Aluminium + Iron oxide -->

a)

aluminium

b)

oxide

c)

aluminium oxide and iron

d)

iron

158.

gold + copper iodide-->

a)

gold iodide and copper

b)

No reaction

c)

gold copper

d)

gold iodide

159.
Metals that react quickly/strongly with water and acids are called?
a)
Reactive
b)
Unreactive
c)
Dangerous
d)
Corrosive
160.
How can you tell that a metal is reacting with water?
a)
Colour change
b)
Bright light
c)
Fizzing
d)
It gets colder
161.
How can you test to show that when a metal reacts with water, hydrogen gas is produced?
a)
Relights a glowing splint
b)
A lit splint produces a squeaky pop
c)
Puts out a burning splint
d)
Is cold to the touch
162.
What gas is produced when a metal reacts with an acid?
a)
Water vapour
b)
Acidic gas
c)
Hydrogen
d)
Nitrogen
163.
When sodium reacts with hydrochloric acid, what is the name of the salt formed?
a)
Sodium Hydride
b)
Sodium Chloride
c)
Sodium Hydrochloric
d)
Sodium Chlorine
164.
When potassium reacts with sulphuric acid, what is the name of the salt produced?
a)
Potassium Sulphide
b)
Potassium Sulphur
c)
Potassium Sulphuric
d)
Potassium Sulphate
165.

Steel is made of

a)

iron and carbon

b)

copper and iron

c)

tin and carbon

d)

aluminum and nickel

166.

Brass is an alloy made of

a)

copper and zinc

b)

copper and tin

c)

copper and nickel

d)

copper and aluminum

167.

Steel can become stainless when alloyed with _____.

a)

chromium and nickel

b)

copper and zinc

c)

tin and lead

d)

iron aand carbon

168.

What structure do metals have?

a)

lattice

b)

bit wobbly

c)

some metals, some non-metals joined together

169.

Which of these is a property of a metal?

a)

a good insulator

b)

always liquid at room temp

c)

conducts electricity

d)

rude

170.

What does malleable mean?

a)

drawn in to wires

b)

conducts heat

c)

can be bent in to shapes

d)

conducts electricity

e)

sonorous

171.

An alloy is a

a)

mixture which always has at least one metal

b)

compound

c)

mixture with no metals in it

172.

When selecting materials for constructing a bridge, what is the main difference to consider between ferrous and non-ferrous metals?

a)

Non-ferrous metals cannot be recycled.

b)

Non-ferrous metals are always magnetic.

c)

Ferrous metals contain iron, non-ferrous do not.

d)

Ferrous metals are lighter than non-ferrous metals.

173.

Imagine you're selecting materials for outdoor furniture that needs to withstand various weather conditions without rusting. Which metal would you choose for its ability to resist rust and stains?

a)

Copper

b)

Aluminium

c)

Mild Steel

d)

Stainless Steel

174.

Which of the following is a property of lead?

a)

High conductivity

b)

Soft and heavy

c)

High tensile strength

d)

Lightweight

175.

Why is copper commonly used in household electrical wiring?

a)

Malleability

b)

Ductility and conductivity

c)

Brittleness

d)

Resistance to rust

176.

During a science fair, a group of students presented a project on metals and their compositions. They displayed various samples, including Brass, Lead, Wrought Iron, and Stainless Steel. Which of these samples is not an alloy?

a)

Brass

b)

Lead

c)

Wrought Iron

d)

Stainless Steel

177.

What is the main use of wrought iron?

a)

Batteries

b)

Aircraft

c)

Ornamental gates and railings

d)

Cutlery

178.

Imagine you are an engineer tasked with designing a new line of commercial airplanes. Which metal would you primarily choose for the aircraft's structure due to its light weight?

a)

Lead

b)

Aluminium

c)

Copper

d)

Silver

179.

Why do engineers prefer using tube steel sections over solid steel sections for constructing a bridge?

a)

Reduced weight

b)

Better aesthetic appeal

c)

Increased weight

d)

Higher cost

180.

A craftsman is working on a new musical instrument and needs a durable yet malleable metal. He decides to create an alloy by mixing copper with another metal to produce brass. Which metal should he mix with copper?

a)

Zinc

b)

Nickel

c)

Chromium

d)

Iron

181.

Why is mild steel a common choice for manufacturing school furniture?

a)

Non-conductivity

b)

Lightweight

c)

Ability to resist rust

d)

High tensile strength

182.

Which of the following is more reactive?

a)

Calcium

b)

Magnesium

c)

Zinc

d)

Magnesium

183.

Will the following reaction take place?


Ni + NaCl ->

a)

NO

b)

YES

184.

Which one of the following combinations result in a displacement reaction?

a)

Iron with magnesium chloride

b)

magnesium with iron chloride

c)

Iron with Zinc Sulphate

d)

gold with silver nitrate

185.

What are the products when magnesium reacts with hydrochloric acid?

a)

magnesium nitrate and hydrogen gas

b)

magnesium sulfate and hydrogen gas

c)

magnesium oxide and oxygen gas

d)

magnesium chloride and hydrogen gas

186.
Which is not a Alkali Metal?
a)
Lithium
b)
Sodium
c)
Gold
d)
Potassium
187.
A displacement (single replacement) reaction will occur when...
a)
a more reactive metal displaces a less reactive metal from its compound.
b)
A less reactive metal displaces a more reactive metal from its compound
c)
Displacement only occurs when two of the same metals are reacted 
d)
Displacement reactions will only occur in metals above iron in the reactivity series
188.

What is the oxidation number of Cl2?

a)

0

b)

+1

c)

+2

d)

-1

189.

What is the oxidation number of Sulfide ion, S2-?

a)

-2

b)

-1

c)

0

d)

+2

190.

What is the oxidation number of oxygen in H2O?

a)

0

b)

+1

c)

+2

d)

-2

191.

What is the oxidation number of phosphorus in phosphate ion, PO43-?

a)

0

b)

+1

c)

+5

d)

-5

192.

What is the oxidation number of sulfur in H2SO4?

a)

0

b)

+1

c)

+4

d)

+6

193.

Which of these chemical reactions is an oxidation-reduction reaction?

a)

CO2 + H2O -> H2CO3

b)

Fe + S -> FeS

c)

AgNO3 + NaCl ->AgCl + NaNO3

d)

H2SO4 + 2NaOH -> Na2SO4 + 2H2O

194.

In which substance does bromine have an oxidation number of +1?

a)

Br2

b)

HBr

c)

HBrO

d)

HBrO2

195.

What happens to the oxidising agent in an oxidation-reduction reaction?

a)

It is oxidised as it gains electrons.

b)

It is oxidised as it loses electrons.

c)

It is reduced as it gains electrons.

d)

It is reduced as it loses electrons.

196.
Is calcium oxidized or reduced in the following reaction? 
2 CaO--> 2 Ca + O2
a)
Oxidized
b)
Reduced
197.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
198.

Reduction is the ___________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

199.

Which of the following represents oxidation?

a)

C → CH4

b)

Fe3+ → Fe2+

c)

Cl2 → 2Cl-

d)

Zn → ZnO

200.

In the reaction Zn + 2HCl --> ZnCl2 + H2

which element, if any, is oxidized?

a)

Zinc

b)

Hydrogen

c)

Chlorine

d)

None

201.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
202.

The following chemical equation represents the extraction of silicon from quartz using coke.

SiO2 + C → Si + CO2

What is the change in oxidation number of silicon?

a)

+2 to 0

b)

+4 to 0

c)

0 to +2

d)

0 to +4

203.

charge on cation is

(a)  

204.

Which of the following cannot occur during oxidation?

a)

Gain of oxygen

b)

Donation of electrons

c)

Loss of hydrogen

d)

Decrease in oxidation number

205.

What is the oxidation number of oxygen in oxygen gas, O2O_2  ?

a)

-2

b)

0

c)

-1

d)

+1

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