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Worksheets

YEAR 9 SCIENCE-CHEMISTRY

Total questions: 136

Worksheet time: 1hrs 19mins

Name
Class
Date
1.

To prepare copper sulfate using sulfuric acid, the sample that should be used is?

a)

copper carbonate

b)

copper metal

2.

Calcium carbonate reacts with nitric acid to form?

a)

calcium oxide

b)

calcium nitrate

c)

calcium chloride

d)

calcium sulfate

3.

Magnesium reacts with dilute sulfuric acid to form?

a)

magnesium oxide

b)

magnesium carbonate

c)

magnesium sulfate

d)

magnesium nitrate

4.

Acid react with metal to form

a)

salt+ carbon dioxide

b)

salt + hydrogen

c)

Salt + Water

d)

Salt + metal oxide

5.

Acid reacts with metal carbonate to form

a)

Salt + hydroxide + water

b)

Salt + carbon dioxide

c)

salt + water

d)

Salt + carbon dioxide + water

6.

What products are produced when we react an acid with an alkali?

a)

salt + water

b)

salt + carbon dioxide + water

c)

salt + hydrogen

d)

salt + water + hydrogen

7.

What salt is produced if you react sodium hydroxide with hydrochloric acid?

a)

sodium hydroxide

b)

sodium sulfate

c)

sodium nitrate

d)

sodium chloride

8.

A salt is formed when nitric acid combines with sodium hydroxide. What is the name of the salt?

a)

Sodium chloride

b)

Sodium nitrate

c)

Hydrogen Nitrate

d)

Nirate

9.

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

10.

Name the salt produced when reacting potassium hydroxide and phosphoric acid?

a)

Potassium chloride

b)

potassium nitrate

c)

potassium sulfate

d)

potassium phosphate

11.

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 hydrochloric acid

d)

sodium hydroxide and phosphoric acid

12.

Sodium hydroxide + sulfuric acid —> ...?

a)

sodium carbonate

b)

sodium sulfate

13.

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

14.

Iron + Hydrochloric acid --> ?

a)

iron sulfate + water

b)

iron + hydrogen

c)

iron chloride + hydrogen

d)

iron chloride + water

15.

Salts that are made with carbonic acid are called ______________.

a)

chlorides

b)

sulfates

c)

nitrates

d)

carbonates

16.

Which metal is the least reactive out of: copper, magnesium, zinc and iron?

a)

copper

b)

magnesium

c)

zinc

d)

iron

17.

In a reaction between an acid and a carbonate gas bubbles will appear. What is that gas?

a)

helium

b)

hydrogen

c)

oxygen

d)

carbon dioxide

18.

How do you know when a reaction between a metal and an acid is complete?

a)

All the metal is dissolved

b)

There is a color change in the acid

c)

Bubbles don't form when more metal is added

d)

All the acid evaporates

19.

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

a)

Filtration

b)

Evaporation

c)

Distillation

d)

Dissolving

20.

Which element reacts with dilute sulfuric acid to produce hydrogen?

a)

carbon

b)

copper

c)

zinc

d)

chlorine

21.
Salts that are made with hydrochloric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
22.
Salts that are made with sulfuric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
23.
Salts that are made with nitric acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
24.
Salts that are made with carbonic acid are called ______________.
a)
chlorides
b)
sulfates
c)
nitrates
d)
carbonates
25.
acid + metal ----->
a)
salt + hydrogen
b)
salt + water + carbon dioxide
c)
salt + water
d)
salt + carbon dioxide
26.
acid + carbonate ----->
a)
salt + hydrogen
b)
salt + water + carbon dioxide
c)
salt + water
d)
salt + carbon dioxide
27.
acid + alkali ----->
a)
salt + hydrogen
b)
salt + water + carbon dioxide
c)
salt + water
d)
salt + carbon dioxide
28.
What reactants are needed to prepare (make) copper carbonate?
a)
copper and hydrochloric acid
b)
copper and sulfuric acid
c)
copper and nitric acid
d)
copper and carbonic acid
29.
What reactants are needed to prepare (make) magnesium nitrate?
a)
magnesium and hydrochloric acid
b)
magnesium and sulfuric acid
c)
magnesium and nitric acid
d)
magnesium and carbonic acid
30.
What reactants are needed to prepare (make) lead sulfate?
a)
lead and hydrochloric acid
b)
lead and sulfuric acid
c)
lead and nitric acid
d)
lead and carbonic acid
31.
How do you know when a reaction between a metal and an acid is complete?
a)
All the metal is dissolved
b)
There is a color change in the acid
c)
Bubbles don't form when more metal is added
d)
All the acid evaporates
32.
Why is burning a salt one way to determine the metal used in preparing it?
a)
Each metal burns a different color.
b)
Some metals burn and some don't.
c)
Each metal has a different colored smoke.
d)
Burning salts is not will not help determine the metal.
33.
In a reaction between an acid and a metal gas bubbles will appear. What is that gas?
a)
oxygen
b)
hydrogen
c)
helium 
d)
carbon dioxide
34.
In a reaction between an acid and a carbonate gas bubbles will appear. What is that gas?
a)
helium
b)
hydrogen
c)
oxygen
d)
carbon dioxide
35.

Iron + copper oxide =

a)

Iron + copper oxide

b)

Iron oxide + copper oxide

c)

Iron oxide + copper

d)

Magic

36.
the starting materials in a chemical reaction
a)
Products
b)
Reactants
c)
Starters
d)
Enders
37.
a substance that is formed as the result of a chemical reaction
a)
Product 
b)
Reactant
c)
Starters
d)
Enders
38.

Which of the following is more reactive?

a)

Calcium

b)

Magnesium

c)

Zinc

d)

Magnesium

39.

Will the following reaction take place?


Ni + NaCl ->

a)

NO

b)

YES

40.

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

41.
A displacement 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
42.

What will the products of this reaction be?

calcium + zinc nitrate --------->

a)

Calcium + zinc nitrate

b)

Zinc + calcium nitrate

c)

there will be no reaction

d)

Zinc + calcium chloride

43.

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

44.
Which of the following will not undergo reaction?
a)
zinc metal  +  zinc oxide 
b)
iron metal  +  copper oxide
c)
zinc metal +  iron oxide
d)
magnesium  +  iron oxide
45.
Which two groups on the Periodic Table are the MOST reactive?
a)
Group 1 and Group 17
b)
Group 2 and Group 16
c)
Group 13 and Group 15
d)
Group 17 and Group 18
46.
How many valence electrons are elements trying to reach in their outer shells?
a)
1
b)
2
c)
5
d)
8
47.
What determines the reactivity of an element?
a)
Size of its nucleus
b)
Number of total electrons
c)
Number of valence electrons
d)
Number of shells
48.
How do you determine the number of valence electrons an element has?
a)
Look at its period
b)
Look at its group
c)
Look at its atomic number
d)
Look at its atomic mass
49.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

50.

Magnesium can be burned in oxygen to produce solid magnesium oxide.

a)

Mg + O2→ MgO

b)

Mg+ O→ MgO

c)

Mg + CO2 → MgO + C

d)

Mg + O2→ Mg2O2

51.

Sodium reacts with chlorine gas to produce sodium chloride.

a)

NaCl→ Cl + Na

b)

Na+ CO2 → NaCO2

c)

Na + Cl2→ NaCl

d)

Na + Cl → NaCl

52.

Magnesium + ________ --> magnesium oxide


What is missing?

a)

Hydrogen

b)

Sulphur

c)

Oxygen

d)

Oxide

53.

Copper oxide + _______________ -> copper sulphate + water


What is missing?

a)

sulphuric acid

b)

hydrochloric acid

c)

hydrogen

d)

oxygen

54.

Identify the product(s) in this word equation

a)

Sodium

b)

Sodium chloride

c)

Sodium and Chlorine

d)

Sodium and sodium chloride

55.

The products in this reaction are?

a)

Two solids

b)

One solid and one gas

c)

Three solids and a gas

d)

Two solids and a gas

56.

The new substances formed in a chemical reaction are called

a)

Reactants

b)

Atoms

c)

Products

d)

Reagents

57.

What are the reactants in this word equation?

a)

Carbon dioxide and oxygen

b)

Carbon dioxide and water

c)

Oxygen and glucose

d)

Oxygen and water

58.

What state of matter is this substance?

a)

solid

b)

liquid

c)

gas

d)

aqueous

59.

What state of matter is this substance?

a)

solid precipitate

b)

dissolved in water

c)

released as a gas

d)

liquid

60.

What does the symbol CaCO3 represent?

a)

An element

b)

A compound

c)

An atom

d)

None of the above

61.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
62.

Which factors affect the rate of a reaction?

a)

temperature

b)

concentration

c)

size

d)

pressure

e)

catalyst

63.

Increase in temperature causes the particles to

a)

slow down

b)

move faster

c)

stay apart from each other

d)

move in the correct order

64.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of reactant particles

d)

it increases the frequency of collision

65.

Why does a higher temperature increase the rate of a reaction?

a)

It increases both the frequency collision and energy of reactant particles

b)

It only increases the frequency of collision

c)

It only increases the energy of reactant particles

d)

It reduces the activation energy of the reaction

66.

Grinding an effervescent tablet into powder increases the rate of reaction due to increase of

a)

concentration

b)

total surface area

c)

temperature

d)

size

67.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing total surface area

d)

All of these

68.

Increasing the temperature gives particles more __________.

a)

time

b)

energy

c)

space

d)

frequency

69.

Why does breaking up a solid reactant increase the rate of reaction?

a)

it creates more solid

b)

it creates more energy

c)

it increases the total surface area

d)

it increases the concentration

70.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of collisions

71.

Which graph shows the effect of increasing temperature on the rate of reaction of calcium carbonate with dilute hydrochloric acid?

a)
b)
c)
d)
72.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

73.
Order the letters from highest to lowest rate of reaction.
a)
A > B > C > D
b)
A > BC > D (B and C have the same rate)
c)
A > B > CD (C and D have the same rate)
d)
D > C > B > A
74.

Grinding a effervescent tablet into powder increases the rate of reaction due to increased

a)

concentration

b)

surface area

c)

temperature

d)

reactants

75.

Increasing the temperature gives particles more __________.

a)

Time

b)

Energy

c)

Space

d)

Frequency

76.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

77.

Substance that changes the rate of a chemical reaction without being consumed in the reaction

a)

bonding

b)

catalyst

c)

chemical reaction

d)

activation energy

78.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

79.

Covalent bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

It depends on the situation

80.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
81.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
82.
A bond that forms when electrons are transferred is called a/an
a)
ionic bond
b)
covalent bond
c)
hydrogen bond
83.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
84.

An atom that gains or loses an electron becomes

a)

an isotope

b)

a new element

c)

an ion

d)

a molecule

85.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

86.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

87.
What type of bond is formed when electrons are transferred (stolen, or given) from one atom to another?
a)
Ionic Bond
b)
Covalent Bond
c)
Metallic Bond
d)
Acidic Bond
88.
What type of bond forms when atoms share electrons?
a)
Ionic Bond
b)
Covalent Bond
c)
Metallic Bond
d)
Gold Bond Medicated Powder
89.
What does an atomic number tell you about an atom?
a)
Number of Protons in an atom or ion
b)
Number of Neutrons in an atom or ion
c)
Number of Nuclei in an atom or ion
d)
Number of fingers on a hand
90.

Is H2O2 an element or a compound?

a)

element

b)

compound

91.

An atom that gains or loses an electron becomes

a)

an isotope

b)

a new element

c)

an ion

d)

a molecule

92.

When an atom gains an electron it becomes

a)

negatively charged

b)

positively charged

c)

neurtal

93.

Ionic bonds happen when valence electrons are

a)

shared

b)

too heavy

c)

transferred

94.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

95.

Which type of bonds create compounds?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all type of bonds

96.

Which type of bond occurs between non metals?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

97.

How many valence electrons does Oxygen have?

a)

0

b)

16

c)

6

d)

8

98.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

99.

How many total atoms are in C6H1206

a)

3

b)

6

c)

12

d)

24

100.

What type of bond forms CaF2

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all answers are correct

101.

Which type of bond is creates MgFe?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all the bonds

102.

What is the charge of an aluminum ion that has 13 protons and 10 electrons?

a)

3+

b)

3 -

c)

no charge

103.

Is this equation balanced? C3H8 + 5O2 = 4H2O + 3CO2

a)

yes

b)

no

104.

How many oxygen atoms on each side of C3H8 + 5O2 = 4H2O + 3CO2

a)

2

b)

3

c)

5

d)

10

105.

In order for a chemical reaction to occur,

a)

there must be an explosion or fire

b)

bubbling or gas must be produced

c)

a new substance must be formed

d)

the substance must turn color

106.

After a chemical reaction occurs, atoms are not created nor destroyed,

a)

just rearranged into a new substance

b)

just changed into different elements

c)

just turned into unstable elements

107.

Most elements bond to create compounds because

a)

their outer electron level is full

b)

they are unstable

c)

they are positively charged

108.

Compounds that share specific valence electrons are formed by

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

109.

Compounds or elements that share their pooled valence electrons are

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

110.

A column of the periodic table is a ________.

a)

group

b)

period

c)

range

111.

A row on the periodic table is a _______.

a)

group

b)

period

c)

range

112.

All _________ share properties that include luster, conductivity, malleability, and ductility.

a)

gases

b)

nonmetals

c)

metalloids

d)

metals

113.

Elements on the periodic table are arranged in rows and columns according to their _________.

a)

properties

b)

categories

c)

atomic number

d)

boiling point

114.

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

a)

metals

b)

alkaline earth metals

c)

alkali metals

d)

nonmetals

115.

In the periodic table, the elements are classifies acording to...

a)

The atomic number

b)

The mass number

c)

The electronic number

d)

The number of neutrons

116.

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

a)

True

b)

False

117.

Which of these is a noble gas?

a)

Chlorine (Cl)

b)

Hydrogen (H)

c)

Neon (Ne)

d)

Fluorine (F)

118.

Which of these is NOT a gas found in the Earth's atmosphere?

a)

Nitrogen (N)

b)

Oxygen (O)

c)

Argon (Ar)

d)

Gold (Au)

119.
Sodium (Na) is found in period 
a)
3
b)
2
c)
4
d)
1
120.
Sodium (Na) is found in group 
a)
1
b)
2
c)
3
d)
4
121.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
122.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
123.
These are found on the Periodic Table.
a)
Compounds
b)
Elements
c)
Mixtures
124.

The horizontal (side to side) rows in the Periodic Table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

125.

Which of the following is found in the nucleus of an Atom?

a)

Protons

b)

Electrons

c)

Shells

d)

negative

126.

Which of the following's number is equal to the numbers of electrons.

a)

Neutrons

b)

Shells

c)

Protons

d)

Nucleus

127.

Which of the following particles is negatively charged?

a)

Protons

b)

Neutrons

c)

Shells

d)

Electrons

128.

Which of the following particles has no charge?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Shells

129.

The total sum of Protons and Neutrons is equal to the ....

a)

Nucleon Number

b)

Atomic number

c)

Neutron Number

d)

Electron number

130.

Electrons in an atom are always organized in

a)

the nucleus

b)

the shell

c)

the neutrons

d)

None

131.

The picture below shows element Neon. What is the Mass Number of Neon?

a)

10

b)

20

c)

19

d)

11

132.

The picture below shows the element Neon. What is the Number of protons of its atom?

a)

10

b)

20

c)

19

d)

11

133.

The picture below shows the element Neon. What is the Number of electrons of its atom?

a)

10

b)

20

c)

19

d)

11

134.

You are provided with the Figure in this question that represents an atom of an element. How many shells does this atom has?

a)

1

b)

2

c)

3

d)

4

135.

You are provided with the Figure in this question that represents an atom of an element. How many Neutrons does this element has?

a)

10

b)

26

c)

11

d)

13

136.

The atom of an element has the electron configuration of 2:8:8:2. How many shells doe this atom have?

a)

1

b)

2

c)

3

d)

4

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