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National 5 Chemistry- Unit 1 Revision

Total questions: 68

Worksheet time: 3hrs 24mins

Name
Class
Date
1.

What type of elements form Covalent Bonds?

a)

Metals only

b)

Non-metals only

c)

Metals and non-metals

2.

Covalent bonds are formed when

a)

positive and negative ions are attracted to each other

b)

positive metal ions are attracted to delocalised electrons

c)

positive nuclei are attracted to a shared pair of electrons

d)

none of the above

3.

Diamond is an example of a

a)

covalent molecule

b)

covalent network

c)

metallic lattice

d)

ionic lattice

4.

What type of elements form ionic bonds?

a)

metals

b)

non-metals

c)

non-metals and metals

5.

Ionic bonds are the attraction between

a)

positive nuclei and shared electrons

b)

positive metal ions and delocalised electrons

c)

positive and negative ions

6.

Metals form (blank) ions.

a)

positive

b)

Negative

7.

Non-metal form (blank) ions.

a)

positive

b)

negative

8.

Ionic substances have which type of structure?

a)

covalent molecular

b)

covalent network

c)

ionic lattice

d)

metallic lattice

9.

Metallic bonds occur in which elements?

a)

metals

b)

non-metals

c)

metals and non-metals

10.

Metallic bonds are the attraction between

a)

positive nuclei and shared electrons

b)

positive and negative ions

c)

positive ions and delocalised electrons

11.

Which structure will have low melting and boiling points?

a)

metallic lattice

b)

ionic lattice

c)

covalent molecular

d)

covalent network

12.

Do covalent compounds conduct electricity?

a)

Yes

b)

No

13.

Why can't covalent substances conduct electricity?

a)

They have delocalised electrons

b)

The ions are trapped in the bond

c)

The electrons are trapped in the bond

d)

They can conduct electricity

14.

Why can metals conduct electricity?

a)

They have positive and negative ions

b)

The have delocalsied ions

c)

They can't conduct electricity

d)

They have delocalised electrons.

15.

Why do covalent molecular substances have low melting and boiling points?

a)

The covalent bonds need to be broken

b)

The weak inter-molecular forces need to be broken

16.

Why do ionic substances conduct when they are molten or in solution?

a)

The ions are trapped in the ionic lattice

b)

They have delocalised electrons

c)

The ions are free to move

17.

Which line in the table shows the properties of a covalent network compound?

a)

A

b)

B

c)

C

d)

D

18.

Which line in the table shows the properties of an ionic compound?

a)

A

b)

B

c)

C

d)

D

19.

Which term can be used to describe the shape of chloromethane?

a)

Linear

b)

Tetrahedral

c)

Trigonal pyrimidal

d)

V-shaped

20.

Which term can be used to describe the shape of phosphorous hydride?

a)

Trigonal pyrimidal

b)

Tetrahedral

c)

Linear

d)

V-Shaped

21.

Which of the following diagrams can be used to show the structure of Copper?

a)
b)
c)
d)
22.

Which of the following diagrams can be used to show the structure of sodium chloride?

a)
b)
c)
d)
23.

Which of the following diagrams can be used to show the structure of silicon dioxide (sand)?

a)
b)
c)
d)
24.
Which two subatomic particles are found in the NUCLEUS of at atom?
a)
protons & nuetrons
b)
protons & electrons
c)
neutrons & electrons
d)
electrons & protons
25.
The subatomic particle with a neutral charge is:
a)
protons
b)
electrons
c)
neutrons
d)
cloud
26.
If an element has 6 protons, 7 neutrons, and 6 electrons, what type of charge does the element have?
a)
positive
b)
negative
c)
neutral
d)
imaginary
27.
What gives an atom mass?
a)
Protons & electrons in the nucleus
b)
electrons in the cloud
c)
protons & neutrons in the nucleus
d)
Protons & electrons in the cloud
28.
If an atom has 24 protons and 24 electrons, what is the atomic number of this element?
a)
24
b)
48
c)
0
d)
42
29.
The number of protons is equal to 
a)
the atomic number
b)
the number of neutrons
c)
the energy levels
d)
the periodic table groups
30.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
31.
The second energy level can hold up to how many electrons?
a)
2
b)
8
c)
10
d)
12
32.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

33.
a)

A

b)

B

c)

C

d)

D

34.

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 particle collisions

35.

What can be said about the green line?

a)

it is a faster rate of reaction

b)

It produces same volume of product as red line

c)

Half the volume of reactants has been used

36.

Which would not speed up a chemical reaction?

a)

Using a large beaker

b)

Increasing the concentration

c)

Decreasing particle size

d)

adding a catalyst

37.

Which would have the slowest rate of reaction

a)

Magnesium ribbon 1M HCl at 20 degrees

b)

Magnesium powder 1M HCl at 20degrees

c)

Magnesium ribbon 0.5M HCl at 10degrees

d)

Magnesium powder 0.5M HCl at 10degrees

38.

Increasing the temperature gives particles more __________.

a)

Time

b)

Energy

c)

Space

d)

Frequency

39.

When surface area is decreased the rate of reaction...

a)

Decreases, because there are LESS possible sites for correct collisions

b)

Increases, because there are LESS possible sites for correct collisions

c)

Decreases, because there are MORE possible sites for correct collisions

d)

Increases, because there are MORE possible sites for correct collisions

40.
Which ion determines a base?
a)
H+
b)
OH-
c)
OH+
d)
CO32-
41.
What is the pH of an extremely strong acid?
a)
pH 0
b)
pH 7
c)
pH 13
d)
pH 2
42.

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

a)

acids

b)

bases

c)

enzymes

d)

neutral

43.

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

a)

acids

b)

bases

c)

enzymes

d)

neutral

44.
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
45.

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

46.
What salt is produced if you react sodium hydroxide with hydrochloric acid?
a)
sodium hydroxide
b)
sodium sulfate
c)
sodium nitrate
d)
sodium chloride
47.
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
48.
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
49.
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
50.
sulfuric acid
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
51.

A student made some statements about particles found in atoms. Identify the 2 statements that apply to both a proton and a neutron.

a)

Relative mass almost zero

b)

charge = 1+

c)

charge = 0

d)

Found inside the nucleus

e)

Relative mass = 1

52.

A student made some statements about particles found in atoms. Identify the 2 statements that apply to both an electron.

a)

charge = -1

b)

charge = 1+

c)

charge = 0

d)

Found outside the nucleus

e)

Relative mass = 1

53.

Identify the 2 particles which are isotopes.

a)

Protons = 11, neutrons = 12, electrons = 11

b)

Protons = 9, neutrons = 10, electrons = 9

c)

Protons = 11, neutrons = 13, electrons = 11

d)

Protons = 19, neutrons = 20, electrons = 18

e)

Protons = 9, neutrons = 10, electrons = 10

54.

Identify the compound that produces a green flame colour (use page 6 of your data book).

a)

strontium chloride

b)

lithium oxide

c)

calcium oxide

d)

barium fluoride

e)

sodium fluoride

55.

Identify the compound that produces a green flame colour (use page 6 of your data book).

a)

strontium chloride

b)

lithium oxide

c)

calcium oxide

d)

barium fluoride

e)

potassium chloride

56.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

57.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
58.
a)

A

b)

B

c)

C

d)

D

59.
a)

A

b)

B

c)

C

d)

D

60.
a)

A

b)

B

c)

C

d)

D

61.
a)

A

b)

B

c)

C

d)

D

62.
a)

A

b)

B

c)

C

d)

D

63.
a)

A

b)

B

c)

C

d)

D

64.

The correct formula for finding moles is:

a)

Moles x molar mass

b)

molar mass / mass

c)

mass / molar mass

d)

6.02214076×1023

65.

Find the molar mass of calcium carbonate (CaCO3) to the nearest gram.

a)

100 g

b)

68 g

c)

84 g

d)

112 g

66.

Find the mass of 5 moles of water (H2O).

a)

18.02 g

b)

36.04 g

c)

90.1 g

d)

25.0g

67.

How many moles are in 225g of CO (carbon monoxide)?

a)

8.03 mole

b)

28.01 mole

c)

4.82x1024 mole

d)

7.50 mole

68.

What is the mass in grams of 5.90 mol octane (C8H18)?

a)

673 g

b)

0.0512 g

c)

389 g

d)

E) 3.55 x 1024 g

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