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Chemistry paper 1 Revision

Total questions: 111

Worksheet time: 3hrs 37mins

Name
Class
Date
1.
What is the relative formula mass of CO2?
a)
44
b)
32
c)
16
d)
56
2.
Calculate the number of gold atoms in a 4 mole sample of gold.
a)
2.41x1024
b)
3.01x1023
c)
4.82x1024
d)
6.02x1023
3.
Calculate the % composition by mass of oxygen present in H2SO4.
a)
16.3%
b)
65.25%
c)
32.6%
d)
57.14%
4.
Calculate the mass of oxygen present in a 55g sample of Aluminum oxide, Al2O3.
a)
29.28
b)
19.95
c)
11.36
d)
32.33
5.
Which represents the greatest mass of sulfur?
a)
1 gram of sulfur
b)
1 molecule of sulfur
c)
0.5 mole of sulfur
d)
6.02 x 1023 atoms of sulfur
6.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
7.
Formula mass of KBr
a)
119
b)
117g
c)
54
d)
62g
8.
Moles of Al2O3 in 40g
a)
40%
b)
0.39
c)
4080
d)
2.55
9.
How much CO2 could you make from 6g of C?
C + O2 --> CO2
a)
12g
b)
44g
c)
22g
d)
32g
10.
Mass of one mole of Mg(OH)2
a)
58g
b)
42g
c)
82g
d)
41g
11.

What amount (in moles) is present in 2.0 g of sodium hydroxide, NaOH?

a)

0.050

b)

0.10

c)

20

d)

80

12.

Lithium hydroxide reacts with carbon dioxide as follows.


2LiOH + CO2 → Li2CO3 + H2O


What mass (in grams) of lithium hydroxide is needed to react with 11 g of carbon dioxide?

a)

6

b)

12

c)

24

d)

48

13.

What is the law of conservation of mass?

a)

Mass of products is more than mass of reactants

b)

Mass of reactants is less than mass of products

c)

Mass of reactants is equal to mass of products

14.

1 dm3 is equal to how many cm3 ?

a)

100

b)

500

c)

1000

d)

2000

15.

Choose a correct unit for concentration.

a)

g

b)

gdm

c)

g/dm3

d)

mol

16.

A high mass of solute dissolved in a low volume of liquid would result in what type of solution?

a)

Low Concentration

b)

High Concentration

17.

50g of sodium hydroxide is dissolved in water to make up 200cm3 . What is the concentration in dm3.

a)

0.25 g/dm3

b)

2.5 g/dm3

c)

25 g/dm3

d)

250 g/dm3

18.

Give the equation for calculating concentration from the mass of substance and volume of solution.

a)

Concentration = mass x volume

b)

Concentration = mass ÷ volume

19.

Which element is graphene made from?

a)

Carbon

b)

Copper

c)

Hydrogen

d)

Sodium

20.

Which structure is a fullerene?

a)

A

b)

B

c)

C

d)

D

21.

What type of forces act between the ions in an ionic compound?

a)

Electrostatic

b)

Frictional

c)

Gravitational

d)

Magnetic

22.

What are TWO properties of ionic compounds?

a)

Conducts electricity when molten

b)

High melting point

c)

Low melting point

d)

Small molecules

e)

Weak bonds between particles

23.

Each carbon atoms in graphite is joined to _______ other carbon atoms

a)

Two

b)

Three

c)

Four

24.

What type of bonding holds together the atoms in graphite?

a)

ionic

b)

covalent

c)

metallic

25.

Why is graphite so soft and slippery?

a)

It is made of layers of atoms

b)

It is made of small molecules

c)

It is an ionic compound

26.

Diamond is made from what type of atoms?

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Silicon

27.

The atoms in diamond are joined together by which type of bonds?

a)

Ionic

b)

Covalent

c)

Metallic

28.

In diamond each atom is joined to _______ others

a)

two

b)

three

c)

four

29.

Diamond is suitable for the cutting end of a drill bit because it is

a)

hard

b)

shiny

c)

soft

30.

Which structure has a very low boiling point?

a)

A

b)

B

c)

C

d)

D

e)

E

31.

What type of bond is in a molecule of hydrogen chloride?

a)

Ionic

b)

Covalent

c)

Metallic

32.

Give TWO reasons why hydrogen chloride is a gas at room temperature

a)

Hydrogen chloride has a low boiling point

b)

Hydrogen chloride has a high melting point

c)

Hydrogen chloride is made of simple molecules

d)

Hydrogen chloride does not conduct electricity

e)

Hydrogen chloride has a giant structure

33.

What type of bonding is preset in calcium oxide?

a)

Ionic

b)

Covalent

c)

Macromolecular

d)

Metallic

34.

What type of particle is this?

a)

An ion

b)

A lattice

c)

A molecule

d)

A polymer

35.

What type of structure is C60?

a)

Diatomic

b)

Giant ionic

c)

A Fullerene

d)

Giant Metallic

36.

What type of bond is labelled A?

a)

Metallic

b)

Double

c)

Ionic

d)

Covalent

37.

This is propane. What type of bonding holds the atoms together?

a)

Ionic

b)

Covalent

c)

Metallic

38.

In silicon dioxide the bonds between atoms are

a)

Easily broken

b)

Very strong

c)

Weak

39.

What type of structure does this diagram represent?

a)

Ionic

b)

Metallic

c)

Alloy

d)

Covalent

40.

Which term would NOT apply to a metallic structure?

a)

High melting point

b)

Good insulator

c)

Delocalised electrons

d)

Malleable

41.

When can ionic substances conduct electricity?

a)

Never

b)

As a solid

c)

As a liquid

d)

As a solution

42.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
43.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
44.

4. What usually forms the positive ion?

a)

Metal

b)

Nonmetals

c)

None

45.

6. What usually forms the negative ion?

a)

Nonmetals

b)

Metal

c)

None

46.

What does the image represent?

a)

A ionic compound

b)

A simple covalent compound

c)

A polymer

d)

A metallic structure

47.

What type of structure is H20 ?

a)

Simple Covalent

b)

Giant Covalent

48.

What are the limitations of using dot and cross diagrams to represent covalent bonds? Choose 2

a)

Does not show the bond angles

b)

Does not show the shape of the molecule

c)

Is simple to draw

d)

Represents the electrons as being shared

49.

What is the arrangement of particles in a metal? Choose 2

a)

Arranged in near rows

b)

Electrons are shared between particles

c)

Sea of delocalised electrons

d)

Particles are arranged in a random pattern

50.

What are the properties of giant covalent structures?

a)

Low melting and boiling points

b)

Can conduct electricity

c)

Cannot Conduct electricity

d)

High melting and boiling points

51.

Why are metals malleable?

a)

The particles are not able to slide over each other

b)

The particles are able to slide over each other

52.

Why are alloys harder than pure metals?

a)

The different sized atoms distort the layers in the structure making it easier for them to slide over each other.

b)

The different sized atoms distort the layers in the structure making to more difficult for them to slide over each other.

c)

There is no difference in hardness.

53.

Why do small molecules have low melting and boiling points?

a)

Weak forces between molecules

b)

Strong forces between molecules

c)

The covalent bonds are broken more easily than giant molecules.

d)

Weak ionic bonds

54.

Which state of matter contains particles in fixed positions?

a)

Liquid

b)

Gas

c)

Solid

55.

What change of state can occur at the boiling point?

a)

Freezing

b)

Melting

c)

Boiling

d)

Condensing

56.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
57.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
58.

Since covalent compounds do not have free charges, they are

a)

good conductors

b)

poor conductors

c)

ionic

d)

metallic

59.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
60.
Protons have a charge of:
a)
-1
b)
+1
c)
-2
d)
+2
61.
Electrons have a charge of:
a)
-1
b)
-2
c)
+1
d)
+2
62.
If a you saw the following, K+; what does it tell you about the  the ion.
a)
it has lost one electron 
b)
it has lost one proton 
c)
it has lost two electrons 
d)
it is a negative ion 
63.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

64.

Why are dots and crosses used to show the electrons in the bonds?

a)

To show which atoms the electrons belong to

b)

Because this is what electrons looks like

c)

To show if the electron came from a metal

d)

To show if the electrons are gained or lost

65.

Predict the bond between Mg and Cl

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

66.
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.
67.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
68.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
69.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

70.
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
71.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
72.

How are elements organized in the periodic table ?

a)

Alphabetically

b)

Based on physical and chemical properties

c)

Increasing number of electrons

d)

Most reactive to least reactive

73.

Most elements on the periodic table are classified as ____________.

a)

Gases

b)

Metalloids

c)

Metals

d)

Nonmetals

74.

Groups on the periodic table are arranged...

a)

Vertically

b)

Horizontally

c)

Diagonally from bottom right corner

d)

Diagonally from top right corner

75.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

76.

Which group on the periodic table is the most reactive?

a)

Group 1

b)

Group 2

c)

Group 13

d)

Group 18

77.

What is the chemical symbol for Sodium?

a)

S

b)

So

c)

Na

d)

Ca

78.

A neutral atom of _____________ has 52 electrons.

a)

Chromium

b)

Tellurium

c)

Manganese

d)

Antimony

79.

Each horizontal row on the periodic table is called a what?

a)

Group

b)

Row

c)

Period

d)

Family

80.

Who arranged the periodic table of elements by the atomic mass (or mass number)?

a)

Democritus

b)

John Dalton

c)

Henry Moseley

d)

Dmitri Mendeleev

81.

Identify the unknown atom.

a)

Flourine

b)

Beryllium

c)

Boron

d)

Helium

82.

Choose ALL of the alkali metals (group 1) from the list below:

a)

lithium

b)

copper

c)

mercury

d)

potassium

e)

sodium

83.

What ions do Metals form when they react?

a)

Positive Ions

b)

Negative Ions

84.

Select all the properties of a Metal:

a)

Strong

b)

Malleable

c)

Conductive

d)

Brittle

85.

Select the 3 things that describe Group 1 Elements as you go DOWN the group:

a)

More Reactive

b)

Lower Melting/Boiling Point

c)

Higher relative atomic mass

d)

Less Reactive

e)

Higher Melting/Boiling Point

86.

Select the 3 things that describe Group 7 Elements as you go DOWN the group:

a)

More Reactive

b)

Lower Melting/Boiling Point

c)

Higher relative atomic mass

d)

Less Reactive

e)

Higher Melting/Boiling Point

87.

Which one describes a reaction between a Group 1 metal and Water?

a)

Vigorous Reaction to produce Hydrogen Gas and a Metal Hydroxide

b)

Vigorous Reaction when Heated to form Metal Chloride Salts

c)

Reacts to form a Metal Oxide

88.

Which one describes a reaction between a Group 1 metal and Oxygen?

a)

Vigorous Reaction to produce Hydrogen Gas and a Metal Hydroxide

b)

Vigorous Reaction when Heated to form Metal Chloride Salts

c)

Reacts to form a Metal Oxide

89.

What happens to the Boiling point of Nobel Gases as you go Down the Group?

a)

Increases

b)

Decreases

90.
What is formed when sodium reacts with water?
a)
sodium oxide and hydrogen
b)
sodium hydroxide and hydrogen
c)
sodium hydroxide and oxygen
d)
sodium hydroxide and carbon dioxide
91.
What is the symbol equation for the reaction between sodium hydroxide and water?
a)
2Na + 2H2O → 2NaOH + H2
b)
Na + H2O → NaOH + H
c)
Na + H20 → NaCl + CO2
d)
2Na + 2H2O → 2NaH2 + O2
92.
What is another name for the elements in group 7?
a)
The Halogens
b)
The Noble gases
c)
The Oxides
d)
The Alkali Metals
93.
When an alkali metal reacts with water, the hydroxide produced dissolves to form and alkaline solution, True or False?
a)
True
b)
False
94.
At room temperature, chlorine is...
a)
a yellow-green gas
b)
a brown gas
c)
a yellow-green liquid
95.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

96.

Which halogens can displace bromide ions to make bromine?

a)

Fluorine and iodine.

b)

Fluorine and bromine.

c)

Fluorine and chlorine

d)

Chlorine and iodine.

97.

A displacement reaction involves...

a)

a solution turning brown or yellow.

b)

a less reactive element taking the place of a more reactive element.

c)

a dislocated hip.

d)

a more reactive element taking the place of a less reactive element.

98.
What type of ions do the Group 7 elements make?
a)
positive 2 (+2)
b)
positive 1 (+1)
c)
negative 1 (-1)
d)
negative 2 (-2)
99.

Would a displacement reaction occur for Bromine + Potassium Iodide?

a)

Yes

b)

No

c)

Maybe

100.

How many electrons do the halogens all have in their outer shells?

a)

1

b)

2

c)

7

d)

8

101.

Would a displacement reaction occur for Iodine + Potassium Bromide?

a)

Yes

b)

No

c)

Maybe

102.

As you go down the group, how does the boiling point of the halogen elements change?

a)

Increases

b)

Decreases

c)

They're all about the same

103.
Which of these is not a noble gas?
a)
Helium
b)
Argon
c)
Nitrogen
d)
Krypton
104.

6.15: Which of these is not a property of noble gases?

a)

Colourless

b)

Odourless

c)

Flammable

d)

Gas at room temperature

105.
Name the group that contains inert (nonreactive) elements.
a)
noble gases
b)
halogens
c)
alkali metals
d)
alkaline earth metals
106.
Which of the following is a noble gas that is heavier than air?
a)
Hydrogen
b)
Helium
c)
Argon
d)
Sodium
107.

Which of the following has the lowest boiling point?

a)

Argon

b)

Krypton

c)

Xenon

d)

Helium

e)

Neon

108.

All noble gases have 8 electrons in their outer shell.

a)

True

b)

False

109.

What is the trend in boiling point for noble gases?

a)

There is no trend.

b)

Boiling point decreases down the group.

c)

Boiling point increases down the group.

d)

All the boiling points are the same.

110.
Another term for being chemically inactive is...
a)
Inert
b)
Inbert
c)
Insert
d)
Inmert
111.
Group 0 elements are non-metals - true or false?
a)
True
b)
False

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