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Y9 End of year review quiz

Total questions: 114

Worksheet time: 1hrs 27mins

Name
Class
Date
1.
Which of the following reactions is a combustion reaction ? 
a)
MgCO3 + O2 → MgO + CO2  
b)
C3H8 + 5O2 → 3CO2 + 4H2O 
c)
6CO2 + 6H2O → C6H12O6 + 6O2 
d)
6CO2 + 6H2O → C6H12O6 + 6O2 
2.
The compounds or elements present at the end of a reaction 
a)
reactants
b)
catalyst
c)
products
d)
energy 
3.
The compounds and elements that are present at the beginning of a reaction:
a)
reactants
b)
catalyst
c)
products
d)
energy 
4.
What kind of change is a change of state?
a)
Physical
b)
Chemical 
5.
Three alkali metals are...
a)
calcium, magesium, barium
b)
lithium, sodium, potassium
c)
gold, silver, platinum
d)
aluminium, cobalt, nickel
6.
Which of the following is NOT a mixture? 
a)
NaCl + H2O
b)
C6H12O6 + H2O
c)
C6H12O6
d)
SiO2 +H2O
7.
Which type of mixture is this? 
a)
Element only
b)
compounds only
c)
elements and compounds
d)
Concoction
8.
Which type of mixture is this?
a)
Element only
b)
Compound only
c)
Element and compound
d)
Miscellany
9.
Which of the following is a compound?
a)
sodium
b)
sea water
c)
carbon dioxide
d)
brass
10.
Which of the following is the correct name for MgCl2?
a)
magnesium chlorine
b)
magnesium dichlorine
c)
magnesium chloride
d)
magnesium dichloride
11.
What is an example of an element that doesn't like to react with anything?
a)
Neon
b)
Oxygen
c)
Hydrogen
d)

Carbon

12.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
13.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
14.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
15.
Balance this equation.
_CH4 + _O2 --> _CO2 + _H2O
a)
1,2,1,1
b)
2,1,2,1
c)
1,2,1,2
d)
0,2,0,2
16.
Magnesium can be burned in air to produce solid magnesium oxide.
a)
2Mg(s) + O2(g)→ 2MgO(s)
b)
Mg(s) + O(g) → MgO(s)
c)
2Mg(s) + CO2(g) → 2MgO(s) + C(s)
d)
2Mg(s) + O2(g) → Mg2O2(s)
17.

What are the three components found in an atom?

a)

Protons

b)

energy

c)

electrons

d)

neutrons

e)

nucleus

18.

Protons are..

a)

negative charged

b)

neutral charged

c)

positive charged

19.

a neutron is..

a)

positive charged

b)

neutral charged

c)

negative charged

20.

an electron is..

a)

negative charged

b)

positive charged

c)

neutral charged

21.

What is an isotope?

a)

A particle

b)

A poisonous dart frog

c)

Isotopes are variants of a particular chemical element which differ in neutron number.

d)

Dust

22.
The atomic number of an element tells you
a)
how many protons and neutrons it has
b)
how many protons and electrons it has
c)
its place on the periodic table
d)
the mass of the nucleus
23.
The mass of an atoms nucleus is the sum of 
a)
protons + neutrons
b)
electrons + neutrons
c)
electrons + protons
24.

Name this element and identify its atomic number.

a)

Carbon, 12.01

b)

Calcium, 6

c)

Carbon, 6

d)

Calcium 12.01

25.

Identify the group number and family name of these elements.

a)

Group 1 - Hydrogen Family

b)

Group 2 - Hydrogen Family

c)

Group 8 Hydrogen Family

d)

Group 1 - Alkaline Metals Family

26.

Suggest the group and period of Sodium simply by referring to it's electron configuration.

a)

Group 7, Period 3

b)

Group 1, Period 3

c)

Group 1. Period 1

d)

Group 7, Period 7

27.

Determine the Atomic Number of this element:

a)

6

b)

7

c)

8

d)

5

28.

Determine the number of neutrons.

a)

125

b)

82

c)

207

d)

207.2

29.

A stable carbon atom has an Atomic Mass of 12. Suggest the name of this.

a)

Carbon ion

b)

Carbon-14 radioisotope

c)

Carbon-6 radioisotope

d)

Carbonic acid

30.

Which of the statements below about the periodic table is true?

a)

All elements found in period 3 are metals

b)

The elements are arrange in increasing atomic number

c)

The elements in groups 17 and 18 are metals

d)

The elements are arranged in increasing atomic mass

31.

what is the atomic number?

a)

17

b)

35

c)

Cl

32.

What is the mass number?

a)

9

b)

4

c)

Be

33.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

8

34.

what would the electron configuration be for this element?

a)

2,6

b)

6,2

c)

2,4,2

d)

2,8

35.

What would the electron configuration be for this element?

a)

2,8,7

b)

2,6,8

c)

4,8,5

d)

7,8,2

36.

how many protons does this element have?

a)

12

b)

24

c)

45

d)

10

37.

Atoms that lose or gain electrons to become charged are called _________.

a)

atoms

b)

elements

c)

ions

d)

valences

38.

Outer shell electrons are also called _________________ electrons.

a)

atoms

b)

electrons

c)

valence

d)

inner most

39.

The arrangement of electrons in the shells is called the __________________ ___________________.

a)

atomic number

b)

atomic mass

c)

electron configuration

d)

electron diagram

40.

The number of electrons in a neutral atom is the same as the ______________ ________________.

a)

atomic number

b)

atomic mass

41.

The octet rule state an atom is stable when the outer shell is _________, usually containing 8 electrons

a)

full

b)

empty

42.
If an element has 5 protons and 5 electrons, what is its net charge?
a)
+5
b)
-5
c)
0
d)
-1
43.
The group of an element tells us...
a)
The number of protons
b)
The number of electron shells
c)
The number of valence electrons
d)
The number of total electrons
44.
Ionic Bonds are formed between...
a)
two metals
b)
two non-metals
c)
metal and a non-metal
d)
different every time
45.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
46.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
47.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
48.
When an atom gains a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
49.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
50.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
51.
How many neutron are in the atom "K"?
a)
7
b)
2
c)
39
d)
20
52.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
53.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
54.
What type of bond is this?
a)
ionic
b)
covalent
55.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
56.
LiF
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
57.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
58.
What is the mass number of this atom?
a)
4
b)
5
c)
9
d)
none of the above
59.
What is the atomic number of this atom?
a)
9
b)
10
c)
19
d)
27
60.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
61.
Atoms of the same element which have a different number of neutrons are called _________________.
a)
ions
b)
isotopes
c)
quarks
d)
molecules
62.
Changing the number of electrons in an atom changes its...
a)
element type.
b)
charge.
c)
isotope type.
d)
atom type.
63.
Changing the number of neutrons in an atom changes its...
a)
element type.
b)
mass (weight).
c)
charge.
d)
atom type.
64.
Why does K become positive when it bonds to Cl to form KCl?
a)
Because it loses an electron to have a full valence shell 
b)
Because it gains an electron to have 2 valence electrons
c)
Because it loses an electron to become negatively charged
d)
Because Cl gives away its 7 electrons to Na to form an equal charge 
65.
Ionic compounds tend to be _________ whereas covalent compounds tend to be ______ or _____
a)
solids // liquids or gases
b)
liquids // solids or gases
c)
gases // solids or liquids
d)
solids // solids or liquids 
66.
Why does CO2 not have a charge? 
a)
The metal gives away an electron to the non-metal
b)
The metal takes the electron from the non-metal
c)
The non-metals equally share electrons
d)
The metal and the non-metal equally share electrons
67.
The mass of an atoms nucleus is the sum of 
a)
protons + neutrons
b)
electrons + neutrons
c)
electrons + protons
68.

How are elements arranged in the modern Periodic Table?

a)

In rows called columns, by increasing mass number.

b)

In rows called periods, by increasing mass number.

c)

In rows called columns, by increasing atomic number.

d)

In rows called periods, by increasing atomic number.

69.

Mendeleev’s Periodic Table was revolutionary because (CHOOSE 2):

a)

He ordered elements by both their properties and their proton number

b)

He left gaps for undiscovered elements.

c)

He swapped some elements so they fit into a group with similar properties

70.

What group are the Halogens in?

a)

Group 1

b)

Group 2

c)

Group 7

d)

Group 0

71.

Elements in the same group in the Periodic Table have (CHOOSE 2):

a)

Similar reactivity

b)

The same melting and boiling points

c)

The same number of outer shell electrons

d)

The same mass

72.

Select the correct physical properties of the alkali metals (CHOOSE 2).

a)

Soft

b)

Brittle

c)

Dense

d)

Have relatively low melting points

73.

When potassium reacts with water, the following observations are true (CHOOSE 2):

a)

Melts into a ball and fizzes

b)

It sinks

c)

Burns with a lilac flame and floats

d)

It doesn't react

74.

Why do the alkali metals get more reactive down the group? (CHOOSE 3)

a)

They are smaller and have less electron shells

b)

They are larger and have more electron shells

c)

It is easier for them to lose their outer electron

d)

The attraction from the nucleus for the outer shell electron is less

75.

Chlorine is more reactive than bromine, so it ........................... it from a compound

a)

decomposes

b)

neutralises

c)

displaces

76.

What term is given to a compound which contains atoms of carbon and hydrogen only?

a)

alkene

b)

hydrocarbon

c)

alkane

d)

saturated

77.

Alkenes have the general formula:

a)

CnH2n

b)

CnH2n+1

c)

CnH2n+2

d)

CnHn

78.

What term describes alkene molecules that contain a C=C double bond?

a)

saturated

b)

unsaturated

79.

Alkanes have the general formula:

a)

CnH2n

b)

CnH2n+1

c)

CnH2n+2

d)

CnHn

80.

What term describes alkane molecules that contain C-C single bonds?

a)

saturated

b)

unsaturated

81.

What process is used to separate crude oil in hydrocarbons with different chain lengths?

a)

distillation

b)

fractional distillation

c)

cracking

d)

polymerisation

82.

Where in the fractionating column are shorter chain hydrocarbon molecules obtained?

a)

At the top

b)

At the bottom

83.

Fractional distillation separates crude oil based on the different __________ of the molecules in the mixture

a)

melting point

b)

boiling point

c)

freezing point

d)

chemical reactivity

84.

Molecules collected at the bottom of the fractionating column tend to be...

a)

more viscous, less flammable and less volatile

b)

less viscous, more flammable and more volatile

c)

more viscous, more flammable and less volatile

d)

less viscous, less flammable and more volatile

85.

Molecules collected at the top of the fractionating column tend to be...

a)

more viscous, less flammable and less volatile

b)

less viscous, more flammable and more volatile

c)

more viscous, more flammable and less volatile

d)

less viscous, less flammable and more volatile

86.

What are the 2 products of complete combustion?

a)

carbon dioxide + hydrogen

b)

carbon dioxide + water

c)

carbon monoxide + water

d)

carbon monoxide + hydrogen

87.

What are the products of incomplete combustion?

a)

carbon monoxide

b)

water

c)

carbon

d)

hydrogen

88.

What does a fuel react with when it burns?

a)

oxygen

b)

water

c)

carbon dioxide

d)

methane

89.

What is the term given to the process by which longer chain hydrocarbons are broken down into shorter length alkanes and alkenes?

a)

fractional distillation

b)

evaporation

c)

cracking

d)

polymerisation

90.

What conditions are needed for cracking?

a)

high temperature

b)

high pressure

c)

catalyst

d)

low temperature

91.

Name the following hydrocarbon

a)

alkane

b)

pentene

c)

pentane

d)

alkene

92.

Name the following hydrocarbon

a)

butane

b)

hexane

c)

heptane

d)

hexene

93.

C10H22 --> C5H12 + C3H6 + ?

a)

C2H4

b)

C3H4

c)

CO2

d)

CH4

94.

When testing for alkenes (unsaturation) bromine water turns from...

a)

orange --> blue/black

b)

colourless --> pink

c)

orange --> colourless

d)

orange --> clear

95.

Limewater turning cloudy is the test for...

a)

carbon dioxide

b)

water

c)

hydrogen

d)

oxygen

96.

What is the name of the alkane with two carbon atoms?

a)

Ethane

b)

Methane

c)

Butane

d)

Propane

97.

The alkanes are a homologous series.

What is the general formula of the alkanes?

a)

n carbon atoms, 2n hydrogen atoms

b)

2n carbon atoms, n hydrogen atoms

c)

n carbon atoms, n+2 hydrogen atoms

d)

n carbon atoms, 2n+2 hydrogen atoms

98.

Crude oil is finite because we use it before more can be formed.

How was crude oil formed?

a)

From the remains of an ancient biomass, consisting mainly of plankton, that was buried in mud

b)

Mostly from the remains of dinosaur bones

c)

By fractional distillation

d)

By cracking

99.

Hydrocarbons with shorter carbon chains are more flammable.

What does this make them useful for?

a)

Lubricants

b)

Fuels

c)

Plastics

d)

Feedstock

100.

What gas is produced when magnesium reacts with ethanoic acid?

a)

hydrogen

b)

carbon dioxide

c)

oxygen

d)

chlorine

101.

What gas is produced when potassium carbonate reacts with ethanoic acid?

a)

hydrogen

b)

carbon dioxide

c)

oxygen

d)

chlorine

102.

Ethanoic acid is described as a weak acid. Explain what this means in terms of ionisation

a)

fully ionised

b)

partially ionised

c)

deionised

103.

Complete the following equation, which show what happens when ethanoic acid dissolves in water.

CH3COOH(aq)⋚ CH3COO– (aq) + _______

a)

H

b)

H-

c)

H+

d)

H2

104.

Explain why the pH of 0.1 mol/dm3 hydrochloric acid is lower than the pH of 0.1 mol/dm3 ethanoic acid

a)

Hydrochloric acid is a strong acid so is fully ionised.It has a higher concentration of H+ ions, so a lower pH.

b)

Hydrochloric acid is a weak acid so is fully ionised.It has a higher concentration of H+ ions, so a lower pH.

c)

Hydrochloric acid is a strong acid so is partially ionised.It has a higher concentration of H+ ions, so a lower pH.

d)

Hydrochloric acid is a strong acid so is fully ionised.It has a lower concentration of H+ ions, so a lower pH.

105.

What is the role of sulfuric acid in the reaction to make esters?

a)

weak acid

b)

hydrogen ion acceptor

c)

catalyst

d)

partially ionises

106.

Esters have distinctive sweet smells, and are volatile liquids. What does volatile mean?

a)

flows easily

b)

catches fire easily

c)

evaporates easily

d)

colours easily

107.

What are some common uses of esters? (Select all that apply)

a)

perfumes

b)

flavourings

c)

clothing

d)

nappies

108.

What type of reaction is shown?

a)

Polymerisation

b)

Hydrogenation

c)

Hydration

d)

Bromination

109.
Which of the following undergoes addition reactions
a)
alkanes
b)
alkanes and alkenes
c)
alkanes and alkynes
d)
alkenes
110.

What would you make if you added Hydrogen to Ethene?

a)

Ethane

b)

Propane

c)

1,2 - dihydroethane

d)

Ethanol

111.

What is the general formula for alcohols?

a)

CnH2n+1OH

b)

CnH2nOH

c)

CnH2n+2OH

d)

CnH2n-1OH

112.

Which of the following is a property of alcohols?

a)

They are non-flammable

b)

They have high boiling points

c)

They are insoluble in water

d)

They do not react with sodium

113.

What is the product when ethanol is oxidized?

a)

Ethanoic acid

b)

Ethene

c)

Ethane

d)

Ethyl ethanoate

114.

What is the name of the ester formed from ethanol and ethanoic acid?

a)

Ethyl ethanoate

b)

Methyl ethanoate

c)

Propyl ethanoate

d)

Butyl ethanoate

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