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Chemistry Revision

Total questions: 125

Worksheet time: 2hrs 44mins

Name
Class
Date
1.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
2.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
3.
An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.
a)
20
b)
10
c)
5
d)
25
4.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
5.
The particles of the atom you can find by knowing the atomic number.
a)
neutrons
b)
protons and electrons
c)
protons and neutrons
d)
atomic mass
6.
What is the atomic mass of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
7.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
8.
What do the following properties describe? : shiny, ductile, good conductor, high melting point
a)
metal
b)
nonmetal
c)
metalloid
9.
Elements in the periodic table are arranged in order by their ...
a)
atomic number
b)
atomic mass (mass number)
c)
metal, nonmetal, or metalloid properties
10.
This particle determines what element you have - the elements identity.
a)
electron
b)
proton
c)
neutron
d)
valence shell
11.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
12.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
13.
Which element has an electron configuration of 2.8.8?
a)
Lead
b)
Flourine
c)
Neon
d)
Argon
14.

Which element has the electron configuration of 2.7?

a)

Krypton

b)

Iodine

c)

Fluorine

d)

Barium

15.

Which alkali metal is most reactive out of the following

a)

rubidium

b)

potassium

c)

sodium

d)

lithium

16.

How many electrons do the alkali metals have in their outer shell?

a)

1

b)

2

c)

8

d)

7

17.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

18.

Which gas is released when the alkali metals react with water?

a)

hydrogen

b)

oxygen

c)

hydroxide

d)

carbon dioxide

19.

What happens to the shielding affect as you go down the group?

a)

increases

b)

decreases

20.

Which of the following is TRUE about an isotope?

a)

same number of protons and neutrons

b)

same number of protons but different number of neutrons

c)

same atomic mass but different atomic number

d)

neutron and electron numbers are the same

21.

What is the charge on a magnesium ion?

a)

3+

b)

2+

c)

2-

d)

3-

22.

What is the charge on a oxygen ion?

a)

3+

b)

2+

c)

2-

d)

3-

23.

What is the charge on a beryllium ion?

a)

1+

b)

2+

c)

0

d)

1-

e)

2-

24.

What is the charge on a nitrogen ion?

a)

3+

b)

2+

c)

3-

d)

1-

e)

2-

25.

What is the charge on a sulfur ion?

a)

3+

b)

2+

c)

3-

d)

1-

e)

2-

26.

What is the charge on a potassium ion?

a)

1+

b)

2+

c)

1-

d)

2-

27.

Which of the following represents a sodium ion?

a)

Na⁻

b)

Na²⁻

c)

Na

d)

Na⁺

28.

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

29.

What is the name for an atom that has lost or gained one or more electrons?

a)

an ion

b)

an isotope

c)

an atom

30.

How does a sodium atom become a sodium ion?

a)

by gaining one electron

b)

by losing one electron.

c)

by gaining one proton

d)

by losing one proton

31.

Is a sodium ion (Na+) an anion or a cation?

a)

an anion

b)

a cation

32.

Is a chloride ion (Cl–) an anion or a cation?

a)

an anion

b)

a cation

33.

Which of the following represents a chloride ion?

a)

Cl⁻

b)

Cl²⁻

c)

Cl

d)

Cl⁺

34.

What is the charge on a chloride ion?

a)

1+

b)

1–

c)

0

35.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
36.
Ions that are made of more than one atom are called...
a)
ionic compounds
b)
crystals
c)

polyatomic ions

d)
ionic bonds
37.
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
38.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
39.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
40.

Calcium Oxide, CaO

a)

Covalent Bond

b)

Ionic Bond

41.

Calcium Chloride, CaCl2

a)

Covalent Bond

b)

Ionic Bond

42.

Why do ionic bonds form?

a)

so the number of protons equals the number of electrons

b)

to fill the outermost energy level to make the atom stable

c)

so an atom can become unstable

43.

If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?

a)

Al+3

b)

Al+13

c)

Al+10

d)

Al-10

44.

if NONMETALS are more likely to GAIN electrons, they will form ...

a)

anions

b)

neutral atoms

c)

cations

45.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
46.

In the chemical formula for an ionic compound, which item is written first?

a)

positive ion (cation)

b)

negative ion (anion)

c)

subscript

d)

it's alphabetical

47.
What element always has an oxidation number of +1?
a)
Hydrogen
b)
Fluorine
c)
Chlorine
d)
Iodine
48.

The transfer of Valence electrons from a metal to a non metal is known as

a)

Covalent Bonding

b)

Metallic bonding

c)

Molecular bonding

d)

Ionic Bonding

49.

A(n) _________ is an ion with a positive (+) charge.

a)

anion

b)

cation

c)

ion

d)

solute

50.

Covalent bonds are formed between...

a)

two or more metal atoms

b)

two or more non-metal atoms

c)

a metal and a non-metal atom

51.

Covalent bonds are formed when electrons are transferred between atoms.

a)

True

b)

False

52.

Atoms can only share electrons in the (a)   shell.

53.

Fluorine is a diatomic molecule. Fluorine is in Group 7. How many electrons are shared in this covalent bond?

(a)  

54.

Oxygen is a diatomic molecule. Oxygen is in Group 6. How many electrons are shared in this covalent bond?

(a)  

55.

The structure of ammonia is shown in the diagram. What is the formula for ammonia?

a)

NH3

b)

HN3

c)

N3H

d)

HN3

56.

What are the disadvantages of using displayed formulae, like the one shown?

a)

The 3D structure of the molecule is not shown.

b)

They can show how atoms are bonded in large molecules.

c)

They do not show which atom each electron comes from.

d)

They can be used to find the structural formula of the molecule.

57.

Select the properties of simple covalent substances.

a)

Low melting and boiling points.

b)

High melting and boiling points.

c)

Do not conduct electricity.

d)

Good conductors of electricity.

58.

Why do simple covalent substances not conduct electricity?

a)

They have low melting points.

b)

They have low boiling points.

c)

There are no delocalised electrons or free ions to carry the charge.

d)

The molecules are too large.

59.

Covalent structures have low melting and boiling points because it does not take much energy to break the _____ intermolecular forces.

a)

weak

b)

strong

60.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
61.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
62.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
63.
A chemical bond between oppositely charged ions.
a)
compound
b)
ion
c)
covalent bond
d)
ionic bond
64.
In this type of bond, electrons are delocalized in a "sea"
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nonpolar
65.

What is made when an atom gain an electron?

a)

Neutral(no charge)

b)

Positive ion

c)

Negative ion

66.

Which type of bond transfers electrons

a)

covalent bonds

b)

ionic bonds

c)

hydrogen bonds

67.

Identify the type of bonding between the oxygen and hydrogens in one water molecule.

a)

covalent bonding

b)

hydrogen bonding

c)

ionic bonding

68.

MgO is bonded together with what type of bond?

a)

ionic

b)

covalent

c)

metallic

d)

hydrogen

69.

C6H12O6 has what type of bond holding the atoms together?

a)

ionic

b)

covalent

c)

metallic

d)

Hydrogen

70.

Multiple Zn atoms are bonded together by what type of bond?

a)

ionic

b)

covalent

c)

metallic

d)

hydrogen

71.

Which of the following types of substance have a high melting point? (choose 2)

a)

metallic

b)

ionic

c)

covalent

d)

hydrogen

72.

Which of the following types of structure has a low melting point? (Choose 1)

a)

ionic

b)

covalent

c)

metallic

d)

hydrogen

73.
A positively or negatively charged particle.
a)
covalent bond
b)
compound
c)
ion
d)
chemical bond
74.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
75.
Which substance contains bonds that involve a transfer of electrons from one atom to another?
a)
CO2
b)
NH3
c)
KBr
d)
Cl2
76.
Which type of bond forms between two or more metals?
a)
Ionic
b)
Covalent
c)
Metallic
d)
Ironic
77.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1
78.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
79.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
80.

What is the size range of a nanoparticle?

a)

1-100 nm

b)

100-1000 nm

c)

1-10 nm

d)

10-1000 nm

81.

What is the approximate size of one nanometer in meters?

a)

0.000 000 001 m

b)

0.000 000 01 m

c)

0.000 000 1 m

d)

0.000 001 m

82.

What is a key difference between bulk materials and nanoparticles?

a)

Bulk materials consist of a few hundred atoms, while nanoparticles consist of huge numbers of atoms.

b)

Bulk materials consist of huge numbers of atoms, while nanoparticles consist of only a few hundred atoms.

c)

Bulk materials are smaller in size compared to nanoparticles.

d)

Bulk materials have a higher surface area to volume ratio compared to nanoparticles.

83.

What is the surface area of one side of a larger cube with dimensions 100 cm × 100 cm × 100 cm?

a)

1000 cm²

b)

10000 cm²

c)

60000 cm²

d)

100000 cm²

84.

What is the surface area to volume ratio of a smaller cube with dimensions 10 cm × 10 cm × 10 cm?

a)

0.06 : 1

b)

0.6 : 1

c)

6 : 10

d)

60 : 1

85.

Which of the following is a benefit of using nanoparticles of zinc oxide in sun creams?

a)

They are difficult to rub in.

b)

They are visible on the skin.

c)

They do not degrade on exposure to the sun.

d)

They provide less effective protection from UV rays.

86.

What is a potential risk of using nanoparticles in sun creams?

a)

They are too large to penetrate cell membranes.

b)

They are less reactive than bulk material.

c)

They may cause cell damage in the body.

d)

They have no harmful effects on the environment.

87.

How does the surface area to volume ratio change when the sides of a cube decrease by a factor of 10?

a)

It decreases by a factor of ten.

b)

It increases by a factor of ten.

c)

It remains the same.

d)

It decreases by a factor of one hundred.

88.

Which of the following is NOT a benefit of using nanoparticles in sun creams?

a)

Better skin coverage

b)

Clear and colourless appearance

c)

Effective protection from UV rays

d)

Harmful effects on the environment

89.

What is a formulation?

a)

A simple mixture designed as an useless product

b)

A complex mixture designed as a useful product

c)

A simple mixture

90.

Name some examples of formulations

a)

medicines

b)

pure gold

c)

pure acid

91.

What is the mobile phase?

a)

paper

b)

beaker

c)

ink

d)

water

92.

What is the stationary phase?

a)

paper

b)

water

c)

ink

d)

beaker

93.

Look the middle image. is it pure or impure?

a)

pure

b)

impure

94.

Look at the right image. Is it a a pure or impure substance?

a)

pure

b)

impure

95.

Why must the start line be drawn in pencil?

a)

pencil does not dissolve in to the water

b)

pencil dissolves in to the water

c)

pencil will separate out

96.

What is the test for oxygen?

a)

turns limewater cloudy

b)

relights a glowing splint

c)

bleaches damp litmus paper white

d)

makes a squeaky pop

97.

What is the test for carbon dioxide?

a)

turns limewater cloudy

b)

relights a glowing splint

c)

bleaches damp litmus paper white

d)

makes a squeaky pop

98.

What is the test for chlorine?

a)

turns limewater cloudy

b)

relights a glowing splint

c)

bleaches damp litmus paper white

d)

makes a squeaky pop

99.

What is the test for hydrogen?

a)

turns limewater cloudy

b)

relights a glowing splint

c)

bleaches damp litmus paper white

d)

makes a squeaky pop

100.
A leibeg condenser is used in
a)
Filtration
b)
Chromatography
c)
Evaporation
d)
Distillation
101.
Can you separate salt from water using filtration?
a)
yes
b)
no
102.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
103.
Jessica made a pitcher of lemonade. What can she do to dilute if she thinks it doesn't taste right?
a)
Add water
b)
Add sugar
c)
Boil the lemonade
d)
Put it in the refrigerator 
104.
Which one of the following solids is insoluble in water?
a)
sugar
b)
sand
c)
copper sulfate
d)
salt
105.
Dyes in water soluble markers may be separated by means of..
a)
crystallization
b)
sublimation
c)
chromatography
d)
sedimentation
106.
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
107.
Liquids that do not mix may be separated by using..
a)
an evaporating dish
b)
a separating funnel
c)
a loading
d)
a sedimentation
108.
Salt and water are
a)
compound
b)
mixture
c)
element
d)
solute
109.
If a solid disappears when added to a liquid (like when sugar is stirred in water)... it is said to have...
a)
Formed a solute
b)
Dissolved
c)
Formed a solvent
d)
Become insoluble
110.
KBr
a)
Soluble
b)
Insoluble
111.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
112.
What are always soluble?
a)
Nitrates
b)
Phosphates
c)
Carbonates
d)
Hydroxides
113.
uniform mixture of two or more substances
a)
solvent
b)
acid
c)
solution
d)
base
114.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
115.

What is the correct name for CaO?

a)

Carbon oxygen

b)

Carbon oxide

c)

Cadmium oxide

d)

Calcium oxide

116.

What is the correct name for CuCl2?

a)

Copper Chloride

b)

Copper (II) Chloride

c)

Copper 1 Chloride 2

d)

Copper (I) Chloride

117.

What is the formula for Aluminum oxide?

a)

AlO

b)

Al3O

c)

AlO3

d)

Al2O3

118.

What is the chemical formula for Copper (I) sulfate?

a)

CuSO4

b)

Cu(SO4)2

c)

Cu2SO4

d)

Cu2(SO4)2

119.

What is the formula for Sodium sulfate?

a)

NaSO4

b)

Na2SO4

c)

Na(SO4)2

d)

Na2(SO4)2

120.

What is the formula for Magnesium chloride?

a)

MgCl

b)

Mg2Cl

c)

MgCl2

d)

Mg2Cl3

121.

What is the name of Pb(NO2)2?

a)

Lead Nitrite

b)

Lead (I) Nitrite

c)

Lead (II) Nitrate

d)

Lead (II) Nitrite

122.

What is the name fo NaCl?

a)

Sodium chloride

b)

Sodium 1 chloride 1

c)

Sodium (I) Chloride

d)

Sodium chlorine

123.

What is the formula for a magnesium ion?

a)

Mg+

b)

Mg2+

c)

Mg2-

d)

Mg-

124.

Which is the correct formula for an ammonium ion?

a)

NH4

b)

NH4-

c)

NH42+

d)

NH4+

125.

What is the formula for lithium bromide?

a)

LiBr

b)

LiBr2

c)

Li2Br

d)

Li2Br2

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