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Unit 1 - N5 Chemistry

Total questions: 100

Worksheet time: 3hrs 51mins

Name
Class
Date
1.

Organise these options into the right categories

Categorize the following

Increasing temperature

Decrease particle size

increase concentration

Decrease temperature

Incerase particle size

Decrease concnentration

Add a suitable catalyst

Increase rate of reaction
Decrease rate of reaction
2.

The correct formula for sulfur dioxide is?

a)

SO

b)

S2O

c)

SO2

d)

SiO2

3.

Organize these options into the right categories

Categorize the following

Bubbling

Colour change

Precipitate

Energy change

Change of shape

Boiling

Dissolving

Melting

Sign of a chemical reaction
Not a sign of a chemical reaction
4.

Identify the metal

a)

Carbon

b)

Calcium

c)

Silicon

d)

Iodine

5.

A substance that increases the rate of a reaction without being used up during the reaction is called a

a)

catalyst

b)

product

c)

reactant

d)

solute

6.

When a catalyst is added to a reaction the rate of reaction...

a)

Increases

b)

Decreases

c)

Does not change

7.

A catalyst

a)

is used up

b)

is never used up

8.

In an exothermic reaction, heat is_____

a)

taken in

b)

given out

9.

In an endothermic reaction, heat is_____

a)

taken in

b)

given out

10.

The mass of zinc used in Experiment 1 was 1.00 g. What mass the mass of zinc used in Experiment 3?

a)

0.50 g

b)

1.00 g

c)

2.00 g

d)

3.00 g

11.

In a reaction, the mass lost in 30 seconds was 2 g. What is the average rate of reaction, in g s−1, over this time?

a)

1/30

b)

30/2

c)

1/2

d)

2/30

12.

The volume of gas collected in 2 minutes was 5cm3.


What was the average rate of reaction over this time?

a)

0.2

b)

0.4

c)

2.5

d)

5

13.

The volume of gas collected in 2 minutes was 5cm3.


What are the units for the average rate of reaction?

a)

cm3/min-1

b)

cm3min-1

c)

min/cm3

d)

min cm-3

14.

Which reaction is the fastest?

a)

A

b)

B

15.

The table shows the results obtained in an experiment carried out to measure the volume of ethyne gas produced.


Calculate the average rate of reaction between 60 and 90 seconds.

(a)  

16.

Label the groups correctly.

a)

Noble Gases

b)

Transition Metals

c)

Alkali metals

d)

Alkali earth metals

e)

Halogens

1
2
3
4
5
1)
2)
3)
4)
5)
17.

Organise these options into the right categories

Categorize the following

positively charged

located in nucleus

mass of 1 amu

no charge

located in nucleu

mass of 1 am

negatively charged

orbits the nucleus

on energy shells

mass of almost zero

Protons
Neutrons
Electrons
18.

Match the group with the valency

a)

Group 2

1.

Valency 2

b)

Group 7

2.

Valency 1

c)

Group 5

3.

Valency 3

d)

Group 8

4.

Valency 0

e)

Group 4

5.

Valency 4

19.

Atoms have this charge...

a)

negative

b)

positive

c)

neutral

20.

Slowest reaction is?

A
B
C
21.

The orange reaction was repeated with smaller particles, which graph would be produced?

A
B
C
22.

The orange graph was produced using magnesium chunks. Which graph is for magnesium powder

A
B
C
23.

Elements in sodium nitrate

a)

Sodium and nitrogen

b)

Sodium and oxygen

c)

Sodium and nitrate

d)

Sodium and nitrogen and oxygen

24.

Fastest part of reaction at this point of the graph.

A
B
C
25.

Organize these options into the right categories

Categorize the following

molecules

lattice

share electrons

lose and gain electrons

conduct when melted or dissolved

never conduct

Ionic
Covalent
26.

Organize these options into the right categories

Categorize the following

Metal and non metal

non metals only

high melting points

low melting points

molecules

lattice

Ionic
Covalent
27.

Organize these options into the right categories

Categorize the following

Feels cold

heat absorbed

Heat released

Feels hot

Candle burning

Cool pack for sore wrist

Endothermic
Exothermic
28.

Why does the mass of the reaction change?

a)

Reactants get used up

b)

The products are lighter

c)

A gas is produced

d)

The solid disappears

29.

Number of protons in atom

a)

17

b)

35

c)

52

d)

18

30.

Number of neutrons in atom

a)

17

b)

35

c)

52

d)

18

31.

Mass of atom

a)

17

b)

35

c)

52

d)

18

32.

Atomic number

a)

17

b)

35

c)

52

d)

18

33.
Question Image

Match the following

a)

17

1.

Protons (atomic number)

b)

35

2.

Mass (protons + neutrons)

c)

18

3.

Neutrons

d)

Element

4.

Chlorine

34.

Atoms are neutral (have no charge) because

a)

Protons and electrons cancel each other out

b)

Same number of protons and neutrons

c)

Same number of protons and electrons

d)

Same number of electrons and neutrons

35.

Correct formula for calcium nitride

a)

CaN

b)

Ca2N3

c)

Ca3N2

d)

CaN3

36.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
37.

When an atom loses an outer electron, it becomes a _____________ ion.

a)
positive
b)
negative
c)
neutral
d)
polyatomic
38.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
39.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
40.

What is the charge on a magnesium ion, electron arrangement

2, 8, 2?

a)

3+

b)

2+

c)

2-

d)

3-

41.

What is the charge on a oxygen ion

electron arrnagement 2, 6?

a)

3+

b)

2+

c)

2-

d)

3-

42.

What is the charge on a nitrogen ion

electron arrangment 2,5 ?

a)

3+

b)

2+

c)

3-

d)

1-

e)

2-

43.

What is the charge on a flourine ion

electron arrangement 2, 7 ?

a)

3+

b)

2+

c)

3-

d)

1-

e)

2-

44.

What is the charge on a potassium ion

electron arrangment 2,8,8,1?

a)

1+

b)

2+

c)

1-

d)

2-

45.

Which of the following represents a sodium ion?

a)

Na⁻

b)

Na²⁻

c)

Na

d)

Na⁺

46.

How does a chlorine atom become a chloride ion?

a)

by gaining one electron

b)

by losing one electron

c)

by gaining one proton

d)

by losing one proton

47.

The 2nd and 3rd shells can hold a maximum of...

a)

One electron

b)

2 electrons

c)

8 electrons

d)

10 electrons

48.

Use your Periodic Table to identify this atom.

a)

Lithium

b)

Nitrogen

c)

Sodium

d)

Oxygen

49.

Why do atoms form ions during chemical reactions?

a)

To get a full first shell

b)

To empty their inner shells

c)

To get a full outer shell

d)

To become more reactive

50.

This atom, neon is a member of the group called the noble gases. Why are the noble gases unreactive?

a)

Because they already have full outer shells

b)

Because they have an even number of electrons

c)

Because they only need to gain one electron

51.

Metals (a)   electrons to become stable.

52.

Non metals (a)   electrons to become stable.

53.

Metals become (a)   ions.

54.

Non metals become -------- ions.

(a)  

55.

Match the following

a)

1.

Covalent Molecule

b)

2.

Covalent Network

c)

3.

Metallic Lattice

d)

4.

Ionic Lattice

56.

Organise these options into the right categories

Categorize the following

only contains strong bonds

made from positive & negative ions

positive ions and delocalised electrons

conducts as solid a

graphite is the only one that conducts

never conduct electricity

low melting and boiling points

conduct electricity when molten/dissolved

Metallic
Covalent network
Ionic
Covalent molecule
57.

What is the formula for lithium bromide?

a)

LiBr

b)

LiBr2

c)

Li2Br

d)

Li2Br2

58.

What is the formula for iron(II) oxide?

a)

FeO2

b)

FeO

c)

Fe2O

d)

Fe2O3

59.

What is the formula for aluminium hydroxide?

a)

AlOH

b)

AlOH3

c)

Al(OH)3

d)

(Al)3OH

60.

The formula for ammonium sulfate is

a)

(NH4)2S

b)

NHSO4

c)

NH42SO4

d)

(NH4)2SO4

61.

Order the prefixes from largest to smallest

a)

oct-

b)

hex-

c)

tetra-

d)

di-

e)

mon-

1)
2)
3)
4)
5)
62.


S ​ (a)  

V ​ (b)   ​

S ​ (c)  

D ​ (d)  

F​ ​ (e)   ​​

Choose from the below words
Formulae
swap
divide
Symbol
valency
63.

mass is measured in ​ (a)  

volume is measured in ​ (b)  

concentration is measured in​ (c)  

Choose from the below words
grams
litres
moles per litre
64.

Solutions that have more OH– ions than H+ ions are

a)

acidic

b)

alkaline

c)

spectator ions

d)

neutral

65.

Solutions that have more H+ ions than OH- ions are

a)

acidic

b)

alkaline

c)

spectator ions

d)

neutral

66.
What is the pH of an extremely strong acid?
a)

pH 1

b)
pH 7
c)

pH 10

d)

pH 14

67.
Which has a pH below 7?
a)
Acid
b)
Base
68.

When mixed with water, insoluble metal oxides e.g. CuOCuO  or ZnOZnO  make a _____ solution

a)

Acidic

b)

Alkaline

c)

Neutral

69.

When mixed with water, soluble metal oxides e.g. K2OK_2O  , Na2ONa_2O  , Li2OLi_2O  make a _____ solution

a)

Acidic

b)

Alkaline

c)

Neutral

70.

What happens to the pH of an acid during neutralisation?

a)

It stays the same

b)

It moves toward pH 1

c)

It moves towards pH 7

d)

It moves towards pH 14

71.
Acids react with
a)
water to produce bases and salts
b)
salts to produce bases and water
c)
neither bases, salts nor water
d)
bases to produce salts and water
72.
The products of a neutralisation reaction are lithium sulfate and water. What is the name of the acid used to neutralise the alkali lithium hydroxide?
a)
hydrochloric acid
b)
sulfuric acid
c)
nitric acid
d)
phosphoric acid
73.
Which reactants are used to produce sodium chloride (salt and water)
a)
sodium hydroxide and nitric acid
b)
sodium hydroxide and sulfuric acid
c)
sodium hydroxide and phosphoric acid 
d)
sodium hydroxide and hydrochloric acid
74.

Match the following

a)

Hydrochloric Acid

1.

HCl

b)

Sulfuric Acid

2.

H2SO4

c)

Nitric Acid

3.

HNO3

d)

Phosphoric Acid

4.

H3PO4

e)

Ethanoic Acid

5.

CH3COOH

75.

Substance that is most acidic

a)

Milk

b)

Drain cleaner

c)

Lemon

d)

Blood

76.

Substance that has highest pH

a)

Stomach acid

b)

Drain cleaner

c)

Coffee

d)

Soap

77.

What will happen to the pH of ammonia if it is diluted?

a)

No change

b)

Increase

c)

Decrease

d)

Soap

78.

What will happen to the pH of vinegar if it is diluted?

a)

No change

b)

Increase

c)

Decrease

d)

Soap

79.

Correct equation for neutralisation is​ (a)   + alkali -> ​ (b)   + water

Choose from the below words
Acid
Salt
80.

Calculate the formula mass of CaCO3

a)

18

b)

100

c)

102

d)

53.5

81.

Balance this equation:

H2 + Cl2 ---> HCl

a)

It is balanced.

b)

H2 + Cl2 ---> 2HCl

c)

3H2 + Cl2 ---> 6HCl

d)

H2 + 3Cl2 ---> 6HCl

82.

What is the total number of atoms present in 5Na3PO4?

a)

5

b)

55

c)

40

d)

8

83.

Calculate the formula mass of H2O

a)

18

b)

100

c)

102

d)

53.5

84.

Calculate the formula mass of potassium carbonate

a)

18

b)

100

c)

138

d)

53.5

85.

Calculate the formula mass of ammonium chloride

a)

18

b)

100

c)

102

d)

53.5

86.

Calculate the mass of 0.25 mol of Mg(NO3)2

a)

46g

b)

37.13 g

c)

46 kg

d)

37.1 kg

87.

Calculate the mass of 2 mol of sodium

a)

46g

b)

4.6g

c)

46 kg

d)

46 l

88.

Calculate the number of moles in 5.6 g KOH

a)

3 mol

b)

0.2 mol

c)

0.1 mol

d)

0.02mol

89.

Calculate the number of moles of potassium hydroxide that is dissolved to make 500 cm3 of 1 mol/l.

a)

0.5 mol

b)

0.1 mol

c)

0.01 mol

d)

0.5 mol

90.

Calculate the number of moles of potassium hydroxide that is dissolved to make 200 cm3 of 0.5 mol/l.

a)

0.5 mol

b)

0.1 mol

c)

0.01 mol

d)

0.5 mol

91.

Calculate the volume of a 0.4 mol l-1 solution containing 0.1 mol of solute

a)

2 l

b)

0.05 l

c)

5 l

d)

0.25 l

92.

Calculate the volume of a 0.1 mol l-1 solution containing 0.5 mol of solute

a)

2 l

b)

0.05 l

c)

5 l

d)

0.25 l

93.

Calculate the concentration of 1.38 g K2CO3 dissolved to make 100 cm3 of solution

a)

0.4mol/l

b)

0.02mol/l

c)

0.005 mol/l

d)

0.1 mol/l

94.

What is the meaning of standard solution?

a)

A solution of which its concentration does not accurately known.

b)

Measurement that shows the quantity of solute in one unit of volume of solution

c)

A solution of which its concentration is accurately known.

d)

Concentration that shows the number of mol of solute

95.

Calculate the concentration of 1.27g of iron (II) chloride dissolved to make 2 litres of solution

a)

0.4mol/l

b)

0.02mol/l

c)

0.005 mol/l

d)

0.1 mol/l

96.

Calculate the number of grams of substance required to make 200cm3 of calcium nitrate solution, concentration 0.25 mol/l

a)

10.6 g

b)

0.345 g

c)

33g

d)

8.2 g

97.

Balance this equation
​ (a)   Zn + ​ (b)   HCl --> ZnCl2 + ​ H2

​ ​

Choose from the below words
1
2
98.

(a)   Al + ​ (b)   FeO → Al2O3 + ​ (c)   Fe

Choose from the below words
2
3
99.

Which equation is balanced?

a)

PbO2 + 2H2--> H2SO4

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

d)

2Na + 2H2O --> 2NaOH + H

100.

What is the mass of 0.75 moles of (NH4)3PO4?

a)

0.0044 g

b)

91 g

c)

110 g

d)

74 g

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