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C2 GCSE Chemistry Revision Quiz

Total questions: 57

Worksheet time: 47mins

Name
Class
Date
1.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
2.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
3.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
4.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
5.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
6.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
7.
When electrons are shared unequally a/an ___________ bond is formed 
a)
ionic 
b)
hydrogen
c)
polar covalent 
d)
nonpolar covalent
8.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
9.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
10.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
11.
What is the chemical name for the compound with the formula Na₂S?
a)
sodium sulfide
b)
sodium fluoride
c)
magnesium sulfide
d)
lithium oxide
12.
What is the name of PS3?
a)
phosphorus trisulfide
b)
phosphorus chloride
c)
phosphide trisulfide
d)
phosphate
13.
The bonds in Na2O are best described as 
a)
a.  covalent, because valence electrons are shared.
b)
covalent, because valence electrons are transferred
c)
ionic, because valance electrons are shared.
d)
ionic, because valance electrons are transferred. 
14.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
15.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
16.
Which is the correct lewis dot structure for calcium chloride?
a)
A
b)
B
c)
C
17.
According to the diagram below, how many bonds will this atom need to make to be stable?
a)
1
b)
2
c)
3
d)
4
18.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
19.
How many more valence electrons does Oxygen need to be stable?
a)
6
b)
2
c)
4
d)
It's already stable with 8
20.
Name this compound:   MgS
a)
Sulfur Magnesium
b)
Magnesium Sulfate
c)
Magnesium Sulfur
d)
Magnesium Sulfide
21.

Atoms form ions because they want to have a (a)   outer shell.

22.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

23.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

24.

Select all of the statements below that are correct to describe the structure and properties of ionic compounds...

a)

They have high melting and boiling points

b)

They have a lattice structure

c)

The ions are held together by intermolecular forces

d)

They can conduct electricity when molten

e)

They can conduct electricity when solid

25.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

26.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

27.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

28.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

29.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

30.

Magnesium Hydroxide is an ionic compound made up from Mg2+ and OH- ions. Which is its correct formula?

a)

MgOH

b)

MgOH2

c)

Mg(OH)2

d)

MgO

31.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
32.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
33.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

34.

Carbon is in 4A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

35.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
36.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
37.

What bond is formed between a metal and a nonmetal?

a)

Covalent bond

b)

Ionic bond

c)

Hydrogen bond

d)

Metallic bond

38.

When two nonmetals do not share electrons evenly, the resulting covalent bond will be

a)

nonpolar

b)

polar

c)

ionic

d)

metallic

39.

Since covalent compounds do not have free charges, they are

a)

good conductors

b)

poor conductors

c)

ionic

d)

metallic

40.
Most covalent compounds are do not exist in which state?
a)
solid
b)
liquid
c)
gas
41.

Which would be the only situation where valence electrons would be shared evenly?

a)

metals and nonmetals

b)

different nonmetals

c)

nonmetals of the same element

d)

metalloids of the same element

42.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

43.

Silicon dioxide is the compound in sand. What is its formula?

a)

SO2

b)

NaO2

c)

SiO2

d)

SiO

44.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
45.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

P2O6

46.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
47.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
48.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
49.
There are more metals than non metals in the periodic table.
a)
True
b)
False
50.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
51.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
52.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
53.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
54.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
55.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
56.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
57.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

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