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Worksheets

Revision - IGCSE Edexcel Chemistry G10

Total questions: 150

Worksheet time: 2hrs 11mins

Name
Class
Date
1.

What is the name of the alkane with two carbon atoms?

a)

Ethane

b)

Methane

c)

Butane

d)

Propane

2.

What chemicals are found in crude oil?

a)

Methane only

b)

A mixture of compounds, which are mostly hydrocarbons

c)

A mixture of elements

d)

Carbon only

3.

What is the definition of a hydrocarbon?

a)

A compound made of hydrogen and carbon only

b)

A compound that includes hydrogen or carbon

c)

A mixture that includes hydrogen and carbon

d)

A mixture of hydrogen and carbon only

4.

Q. 

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

a)

distillation

b)

sedimentation

c)

chromatography

d)

filtration

5.

Which of the dyes was a pure substance?

a)

1

b)

2

c)

3

d)

4

6.

Calculate the Rf value

(a)  

7.

(a)   can be used to separate an insoluble solid from a soluble liquid.

8.

solute + solvent =

a)

solution

b)

equation

9.

Saturated solution is

a)

A solution which contains the maximum amount of solute that can be dissolved in the solvent. If any more solute is added, it will not dissolve in the solution.

b)

A solution that contains a huge amount of solute that can be dissolved in the solvent. It can still dissolve more

c)

A solution that contains a small amount of solute that can be dissolved in the solvent. It can still dissolve more

d)

is a fed up solution

10.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

11.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
12.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
13.

A pure substance boils at a

a)

Sharp temperature

b)

range of temperature

14.

What is empirical formula?

a)

True formula

b)

Smallest whole-number ratio of atoms present in a molecule

c)

Total number of atoms present in one molecule

d)

All of the above

15.

The number of electrons for an ion A2-, is 18. Calculate the number of proton in the ion.

a)

16

b)

18

c)

20

d)

22

16.

Calculate the number of atoms in 1 g of He.

a)

1.5 x 1023

b)

0.25

c)

4

d)

4.15 x 10-25

17.

The molecular weight of phosphorus oxide is 283.886 g/mol. Determinethe molecular formula of the phosphorus oxide if the empirical formula is P2O5.

a)

P6O15

b)

P8O20

c)

P4O10

d)

P10O25

18.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
19.
Which is most likely to form a negative ion...
a)

an element from Group 7

b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
20.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

21.

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

a)

NaS

b)

S2S2

c)

Na2S

d)

NaS2

22.

Nonmetals (like Cl) typically ____ electrons when they form ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

23.

Melting point: -196⁰C

Boling point: -152⁰C

Conductivity: Does not conduct

a)

Ionic

b)

Simple covalent

c)

Giant covalent

d)

Metallic

24.

Melting point: 732⁰C

Boling point: 1037⁰C

Conductivity: Not as a solid but does conduct when molten

a)

Ionic

b)

Simple covalent

c)

Giant covalent

d)

Metallic

25.

Melting point: 1984⁰C

Boling point: 2510⁰C

Conductivity: Does not conduct

a)

Ionic

b)

Simple covalent

c)

Giant covalent

d)

Metallic

26.

Melting point: 1083⁰C

Boling point: 2595⁰C

Conductivity: Conducts as both a solid and when molten

a)

Ionic

b)

Simple covalent

c)

Giant covalent

d)

Metallic

27.

Melting point: 3652⁰C

Boling point: 4827⁰C

Conductivity: Conducts as a solid. This substance does not melt.

a)

Ionic

b)

Simple covalent

c)

Giant covalent

d)

Metallic

28.

2.Which product is formed when calcium carbonate undergoes thermal decomposition?

a)

calcium

b)

calcium hydroxide

c)

calcium oxide

d)

calcium silicate

29.

3. Which process does not produce carbon dioxide?

a)

combustion of a hydrocarbon

b)

photosynthesis

c)

reaction between an acid and a metal carbonate

d)

respiration

30.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

31.

In the modern day atmosphere, what is the approximate percentage of nitrogen?

a)

0.04%

b)

21%

c)

78%

d)

1%

32.
At room temperature, chlorine is...
a)
a yellow-green gas
b)
a brown gas
c)
a yellow-green liquid
33.

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

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

34.

What are the two conditions that caused iron to rust ?

a)

Air and Oxygen

b)

Oxygen and Water

c)

Water and Carbon dioxide

d)

Carbon dioxide and Air

35.

Halogens exist as .....

a)

atoms

b)

ions

c)

diatomic molecules

d)

triatomic molecules

36.

In which group of the periodic table is alkali metals found?

a)

group 2

b)

group 7

c)

group 10

d)

group 1

37.

Which of the following is the most reactive in water?

a)

Rubidium

b)

Potassium

c)

Caesium

d)

Sodium

38.

Which of the following indicators show the pH value of a substances?

a)

A. I and II

b)

B. III and IV

c)

C. II and III

d)

D. I and IV

39.

A Brønsted-Lowry acid is defined as a ____ and a Brønsted-Lowry base is defined as a ____.

a)

proton acceptor, proton donor

b)

proton donor, proton donor

c)

proton acceptor, proton acceptor

d)

proton donor, proton acceptor

40.

Ammonium nitrate

a)

soluble in water

b)

insoluble in water

c)

almost insoluble (slightly soluble)

41.

Barium sulfate

a)

soluble in water

b)

insoluble in water

c)

almost insoluble (slightly soluble)

42.

Calcium chloride

a)

soluble in water

b)

insoluble in water

c)

almost insoluble (slightly soluble)

43.

Calcium carbonate

a)

soluble in water

b)

insoluble in water

c)

almost insoluble (slightly soluble)

44.

Copper(II) sulfate

a)

soluble in water

b)

insoluble in water

c)

almost insoluble (slightly soluble)

45.

Silver carbonate

a)

soluble in water

b)

insoluble in water

c)

almost insoluble (slightly soluble)

46.

A solution of one salt was made and some dilute nitric acid was added. Drops of silver nitrate solution were added. A yellow precipitate formed. This test shows the anion in the salt is

a)

bromide, Br-

b)

chloride, Cl-

c)

iodide, I-

d)

sulfate, SO42-

47.

Solid C is dissolved in water. When sodium hydroxide solution is added to the solution of C, a red-brown precipitate is formed. This test shows that the ion present in solid C is

a)

copper, Cu2+

b)

iron (II), Fe2+

c)

iron (III), Fe3+

d)

sodium, Na+

48.

If a flame test is carried out on copper chloride, the colour in the flame is

a)

red-brown

b)

yellow

c)

lilac

d)

blue-green

49.

What colour does litmus paper turn in the presence of chlorine?

a)

Red

b)

Blue

c)

Red then White

d)

Yellow

50.

The test for chloride ions was carried out on a solution. Dilute nitric acid was added to the solution, followed by a few drops of silver nitrate solution. A white precipitate formed. Why is it necessary to add dilute nitric acid in this test?

a)

To neutralise the solution

b)

Nitrate ions are needed for the test to work

c)

To make sure that no carbonate ions are present

d)

The test only work in alkaline conditions

51.

What is the best test for sulfate ions?

a)

add hydrochloric acid followed by barium chloride solution

b)

add sodium hydroxide followed by barium chloride solution

c)

add barium chloride solution

d)

add barium sulfate solution

52.
Name this alkane
a)
Methane
b)
Ethane
c)
Propane
d)
Butane
53.

What physical property allows Fractional Distillation to separate different fractions of crude oil?

a)

Melting point

b)

Boiling point

c)

Diffusion rate

d)

Condensation rate

54.
The longer the hydrocarbon, the _______ the boiling point
a)
Lower
b)
Higher
55.

For surfacing roads and roofs

a)

petrol

b)

bitumen

c)

fuel oil

d)

kerosene

56.

Check all that apply: Which of the following molecules are ISOMERS?

a)

A and B

b)

A and C

c)

C and D

d)

B and D

57.

What is the IUPAC name of this organic molecule?

a)

3-chlorobutane

b)

2-chlorobutane

c)

3-chloropentane

d)

2-chloropentane

58.

This reaction is an example of which type of organic reaction?

a)

addition

b)

fermentation

c)

polymerization

d)

substitution

59.

Large molecules made up of small monomers are called

a)

polymers

b)

monomer

c)

allotrope

d)

functional group

60.

What is fractional distillation?

a)

a process used to separate crude oil

b)

a process used to burn up fuels

c)

a way to make different products

d)

how oil is extracted from the ground

61.

Is this hydrocarbon saturated or unsaturated?  HINT: Look at the bonds.

a)
saturated
b)
unsaturated
62.
The longer the hydrocarbon, the _________ the viscosity?
a)
Lower
b)
Higher
63.

Complete the equation C16H34 ---> __________ + C2H4

a)

C16H34

b)

C2H30

c)

C10H20

d)

C14H30

64.
What is kerosene used for?
a)
Fuel for ships
b)
Fuel for lorries
c)
Fuel for airplanes
d)
Making roads
65.

CH4 + O2 --> CO + 2H2O

a)

complete combustion

b)

incomplete combustion

66.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
67.

Particles in a ______________________ move quickly and are far apart.

a)

gas

b)

solid

c)

liquid

68.

Particles of a liquid

a)

are tightly packed together and stay in a fixed position.

b)

are free to move around one another but still touch.

69.

What is condensation?

a)

gas to solid

b)

gas to liquid

c)

liquid to solid

70.

Phase change from solid to gas is called:

a)

Freezing

b)

Condensation

c)

Vaporization

d)

Sublimation

71.

How many grams of NaCl are in 450 g

of water at 30∘C if the solubility is 39 g

per 100 g of water?

a)

8.67 g

b)

39 g

c)

100 g

d)

175.5 g

72.

A saturated solution is______

a)

No more solute can be dissolved

b)

The solvent and solution

c)

More solute can be dissolved

73.

The separation of a mixture of two miscible liquids such as ethanol and water takes placed by

a)

Distillation

b)

Evaporation

c)

Fractional distillation

d)

Crystallization

74.

The process of fractional distillation depends on a difference in the

a)

Rate of evaporation of two liquids

b)

Boiling points of two liquids at the same pressure

c)

Solubilities of two solids in the same solvents

d)

Densities of two substances at the same temperature

75.

In the distillation apparatus shown, what are the parts labelled A and B?

a)

A = funnel, B = thermometer

b)

A = thermometer, B = funnel

c)

A = condenser, B = flask

d)

A = condenser, B = thermometer

76.

Which one of the following is the name for separation technique in the picture below

a)

evaporation

b)

seiving

c)

decanting

d)

distillation

77.
How can pure substances be distinguished from impure ones?
a)
Melting/boiling points
b)
Colour
c)
Smell
d)
Temperature
78.
Describe the melting and boiling points of impure substances
a)
Fixed
b)
Range of temperature
c)
Different temperature
d)
One very specific temperature
79.
In paper chromatography, what is the mobile phase?
a)
Pencil line
b)
Paper
c)
Ink
d)
Solvent e.g. water
80.
How can chromatography show pure or impure substances?
a)
Impure = no dots
b)
Pure = many dots
c)
Impure = single dot
d)
Pure = single dot
81.
In chromatography, why is a pencil used to draw the line?
a)
It’s insoluble
b)
It's soluble
c)
It's sharper
d)
Neutral colour
82.
A squeaky-pop when a gas is lit shows the presence of which gas?
a)
Oxygen
b)
Hydrogen
c)
Chlorine
d)
Carbon Dioxide
e)
Helium
83.
What type of gas is able to relight a glowing splint?
a)
Oxygen
b)
Hydrogen
c)
Chlorine
d)
Carbon Dioxide
e)
Helium
84.
A gas that turns limewater from colourless to cloudy is?
a)
Oxygen
b)
Hydrgogen
c)
Carbon Dioxide
d)
Chlorine
e)
Helium
85.
A gas that turns damp blue litmus paper from blue to red and then white is?
a)
Oxygen
b)
Hydrogen
c)
Carbon Dioxide
d)
Chlorine
e)
Helium
86.
On the chromatogram given -------------- is mixture.
a)
red
b)
orange
c)
green
d)
black
87.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
88.
The Rf value  for the red component is 
a)
0.3
b)
0.7
c)
10
d)
7
89.

What kind of elements are shown in red?

a)

Metal

b)

Nonmetal

c)

Metaloid

90.
What is the electron configuration of calcium?
a)
2.8.8.2
b)
2.8.10
c)
20
d)
2.18.2
91.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
92.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
93.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

94.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
95.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
96.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
97.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
98.

Reactant and products might adhere to containers causing actual yield to be less than theoretical yield.

a)

true

b)

false

99.

Competing reactions might occur forming other products causing your actual yield to be less than your theoretical yield.

a)

true

b)

false

100.

Some product may be lost during filtering causing your actual yield to be less than your theoretical yield.

a)

true

b)

false

101.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
102.
What is the molar mass of Carbon?
a)
6
b)
12
c)
20
d)
40
103.
How many moles is 4 grams of Calcium?
a)
0.10 moles
b)
10 moles
c)
44 moles
d)
160 moles
104.
What is Avogadro's Number?
a)
602,000
b)
23 x 106
c)
10 x 1023
d)
6.02 x 1023
105.

In the image, which reactant is limiting?

a)

The white molecules, because there are extra.

b)

The black atoms, because they are completely used up.

c)

The white molecules, because they are completely used up.

d)

The black atoms, because there are extra.

106.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
107.
7. The amount of product that actually forms when a chemical reaction is carried out in a laboratory is called the _________ yield.
a)
actual
b)
theoretical
c)
percent
108.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
109.
All chemical bonds involve two atoms sharing electrons.
a)
True
b)
False
110.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
111.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
112.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
113.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

114.

A Cation is an ion with a __________ charge.

a)

positive

b)

negative

c)

neutral

115.

An Anion is an ion with a ________ charge.

a)

positve

b)

negative

c)

neutral

116.

How does Lithium become an ion?

a)

Lose 1 electron

b)

Gain 7 electrons

c)

Lose 3 electrons

d)

Gain 1 electron

117.

How does Fluorine become an ion?

a)

Gain 1 electron

b)

Lose 1 electron

c)

Lose 7 electrons

d)

Lose 2 electrons

118.

In Metallic bond, electrons _______________ between atoms.

a)

are shared

b)

are transferred

c)

flow freely

119.

Atom 2 has a full outer shell.

a)

True

b)

False

120.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

121.

Which of the following is true about Covalent (non-polar) bonds? (select ALL true options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

122.

Potassium Chloride is...

a)

Ionic

b)

Covalent

123.

Ammonium (NH4) is...

a)

Ionic

b)

Covalent

124.

What happens to limewater when carbon dioxide is bubbled through it?

a)

Turns from white to blue.

b)

Turns from colourless to milky.

c)

The carbon dioxide bubbles give a squeaky pop sound.

d)

It freezes.

125.

What colour does sulfur burn in oxygen?

a)

Blue

b)

White

c)

Orange

d)

Lilac

126.

Which gas makes up approximately 0.9% of dry, unpolluted air?

a)

Carbon dioxide

b)

Neon

c)

Hydrogen

d)

Argon

127.

What is the appearance of copper oxide?

a)

White solid

b)

Colourless gas

c)

Blue-green liquid

d)

Black solid

128.

Which of the following has basic character?

a)

Nitrogen oxide

b)

Sulfur dioxide

c)

Magnesium oxide

d)

Carbon dioxide

129.

How do we solve for the percentage change?

a)

original quantity - new quantity

b)

increase ÷ original quantity

c)

decrease ÷ original quantity

d)

change ÷ original quantity

130.

Which of the following does not prevent rusting of iron?

a)

Painting , Oiling , Galvinising

b)

Attach to a piece of copper

c)

connect to a piece of magnesium with wire

d)

cover entirely with copper

131.

What is the chemical name given to Rust ?

a)

Iron II oxide

b)

Iron III oxide

c)

Steel dioxide

d)

Carbon dioxide

132.

Magnesium + hydrochloric acid-->

a)

Magnesium chloride + water

b)

Magnesium chloride + hydrogen

c)

Magnesium hydrochloride + hydrogen

d)

Magnesium chloride + water + carbon dioxide

133.

Calcium carbonate + hydrochloric acid -->

a)

Calcium chloride + hydrogen

b)

Calcium choride + water

c)

Calcium chloride + carbon dioxide + water

d)

Calcium sulfate + carbon dioxide + water

134.

Sulphur dioxide causes which environmental problem

a)

global warming

b)

acid rain

c)

eutrophication

d)

ozone layer depletion

135.

What is the volume of 5 moles of oxygen gas at

room temperature and pressure?

a)

12 dm3

b)

22.4 dm3

c)

120 dm3

d)

24 dm3

136.

How many moles of methane gas (CH4), are in 12 dm3 of methane

at room temperature and pressure?

a)

312 moles

b)

0.5 moles

c)

2 moles

d)

24 moles

137.

What type of reaction produced an insoluble salt?

a)

Neutralisation reaction

b)

Precipitation reaction

c)

Titration reaction

d)

Insoluble reaction

138.

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

139.

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

140.

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

a)

Filtration

b)

Precipitation

c)

Crystalisation

d)

Evaporation

141.

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

142.
Salts that are made with hydrochloric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
143.
Salts that are made with nitric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
144.
What salt is produced if you react sodium hydroxide with hydrochloric acid?
a)
sodium hydroxide
b)
sodium sulfate
c)
sodium nitrate
d)
sodium chloride
145.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
146.

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

a)

indicator

b)

neutraliser

c)

corrosive

d)

electricity

147.
What color does litmus paper turn in the presence of an acid?
a)
blue
b)
black
c)
green
d)
red
148.
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
149.

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

150.

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

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