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Anne Chemistry revision 1

Total questions: 156

Worksheet time: 3hrs 48mins

Name
Class
Date
1.

How would you describe the movement of particles in a gas?

a)

Move randomly in all directions

b)

Stationary

c)

Vibrate around a fixed position

d)

Can flow

2.

What is the name of the change of state from solid to liquid?

a)

Sublimation

b)

Boiling

c)

Freezing

d)

Melting

3.

What is the name of the change of state from liquid to gas?

a)

Freezing

b)

Condensation

c)

Evaporation

d)

Melting

4.

What is the name of the change of state from gas to liquid?

a)

Condensation

b)

Evaporation

c)

Melting

d)

Freezing

5.
The ___ is the thing being dissolved.
a)
solute
b)
solvent
c)
mixture
d)
suspension
6.

Besides stirring, which of the following should be done to make this powder dissolve faster in the liquid?

a)

Add heat to the liquid

b)

Cool the liquid in a freezer

c)

Add more powder to the liquid

d)

Store the mixture in a dark place

7.

When you have added as much solute as can dissolve in the solvent, the solution is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

8.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
9.
salt water is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
10.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
11.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
12.

25 grams of NaCl are dissolved in 100 mL of water at 60 C. How many more grams need to be dissolved for the solution to be saturated?

a)

13 grams

b)

25 grams

c)

6 grams

d)

38 grams

13.

How many grams of K2Cr2O7, are soluble in 50 g of water at 90ºC?

a)

70 grams

b)

35 grams

c)

140 grams

d)

105 grams

14.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
15.

What causes diffusion?

a)

The constant, random motion of molecules

b)

Magnetic attraction between atoms

c)

The nuclear forces that hold atoms together

d)

The tendency of atoms to form chemical bonds with one another

16.

What is a substance made of two or more elements that are chemically combined called?

a)

A. element

b)

B. compound

c)

C. mixture

d)

D. solution

17.

Is salt (NaCI) a compound or an element?

a)

Compound

b)

element

18.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
19.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
20.

Which of the options below is the correct definition of an element?

a)

Elements have only two types of atom

b)

Elements have only two types of atom bonded together

c)

Elements have only one type of atom

d)

Elements have two types of atom not bonded together

21.

Which of the following example are elements

a)

Lithium

b)

Carbon Dioxide

c)

Helium

d)

Sodium Chloride

22.

Which diagram A, B, C or D represents a mixture?

a)

A

b)

B

c)

C

d)

D

23.

Choose the separating methods from the list

a)

Boling

b)

Evaporation

c)

Filtration

d)

Distillation

e)

Diffusion

24.

Distillation is

a)

a process of separating a solvent and a solute using evaporation and condensation using difference in boiling points

b)

a process of separating a soluble solid from a liquid by turning the liquid into a gas

c)

separation of dissolved colours

25.

In what states of matter can diffusion occur?

a)

Gas

b)

Liquid

c)

Solid

26.

Which part of a filtration is the "filtrate"?

a)

The filter paper

b)

The solid material left in the funnel

c)

The liquid that has gone through

d)

The conical flask

27.

How could you increase the concentration of a solution?

a)

Add more solute

b)

Add more solvent

c)

Remove some solute

d)

Remove some solvent

28.

When no more solid can be dissolved in a solution, it is now...?

a)

Unsaturated

b)

Full

c)

Saturated

d)

Soaked

29.

Dyes in water soluble markers may be separated by means of

a)

Simple distillation

b)

Crystallisation

c)

Chromatography

d)

Filtration

30.

The droplets of water that appear on the outside of a glass of cold water on a warm day are an example of?

a)

sublimation

b)

condensation

c)

evaporation

d)

sedimentation

31.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
32.
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
33.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
34.

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

35.

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

a)

anions

b)

neutral atoms

c)

cations

36.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
37.

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

a)

anion

b)

cation

c)

ion

d)

solute

38.

Which element(s) will form negative ions? Check all that apply.

a)

Potassium

b)

Sulfur

c)

Iodine

d)

Magnesium

39.
What is the charge on an Aluminium ion?
a)
3
b)
+3
c)
+2
d)
+1
40.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
41.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
42.
What colour is universal indicator in a strong alkali?
a)
Green
b)
Orange
c)
Purple
d)
Red
43.
What colour is universal indicator in a neutral solution?
a)
Green
b)
Orange
c)
Purple
d)
Red
44.
What colour is universal indicator in strong acid?
a)
Green
b)
Orange
c)
Purple
d)
Red
45.

Strong acids and strong alkalis are.......

a)

Able to turn blue litmus paper red

b)

Corrosive

c)

Sour

d)

Sweet

46.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-14
d)
1-20
47.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
48.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
49.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
50.
A solution with a pH of 8.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
51.
A neutralization reaction will always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
52.

Acids are source of

a)

hydrogen ions

b)

hydroxide ions

53.

Alkalis are source of

a)

hydrogen ions

b)

hydroxide ions

54.

A wasp sting is alkali. Which substance would neutralise the sting?

a)

Vinegar

b)

Bleach

c)

Baking soda

d)

Distilled water

55.

Acid + Alkali --> Salt + Water

a)

neutralization reaction

b)

synthesis

c)

decomposition

d)

single displacement

56.

what type of ions do alkalis form when dissolved in water?

a)

hydroxide ions (OH-)

b)

oxygen ions (O2-)

c)

hydrogen ions (H+)

57.

Which salt is produced during a neutralisation reaction using hydrochloric acid?

a)

chloride

b)

sulphate

c)

nitrate

d)

phosphate

58.

Which salt is produced during a neutralisation reaction using sulfuric acid?

a)

chloride

b)

sulphate

c)

nitrate

d)

phosphate

59.

A solution with more hydrogen ions than hydroxide ions will be more ......

a)

alkaline

b)

neutral

c)

acidic

60.

A solution turns blue litmus paper red, what is the chemical?

a)

An acid

b)

An alkali

c)

Neutral

d)

Cannot tell

61.

What salt is made in the reaction between sodium and sulfuric acid?

a)

silver sulfate

b)

sodium nitrate

c)

sodium sulfate

d)

sodium chloride

62.

How can we test a gas to see if it is hydrogen?

a)

A lit splint will make a squeaky pop sound

b)

Limewater will turn cloudy

c)

Damp blue litmus paper will be bleached

d)

A glowing splint will relight

63.

Which pH represents the solution with the highest Hydrogen ion concentration

a)

pH=1

b)

pH=3

c)

pH=7

d)

pH=11

64.

Which pH represents the solution with the lowest Hydroxide ion concentration

a)

pH=1

b)

pH=3

c)

pH=7

d)

pH=11

65.

Which compound represents an acid?

a)

NaOH

b)

HCl 

c)

CH2OH

d)

NaCl

66.

What is the chemical formula of sulfuric acid?

a)

SO3

b)

H2O2

c)

NaCl

d)

H2SO4

67.

What is the chemical formula of sodium hydroxide?

a)

H2O

b)

NaOH

c)

CO2

d)

CH4

68.

What is the chemical formula of potassium hydroxide?

a)

H2SO4

b)

NaOH

c)

KOH

d)

PO4

69.

Sodium hydroxide + Sulphuric acid --> X + Water


What will be the X

a)

Sodium sulphate

b)

Sodium sulphonate

c)

Sodium sulphurate

70.

Potassium hydroxide + Y -> potassium sulphate + water


What Y will be?

a)

Nitric acid

b)

Hydrochloric acid

c)

Sulphuric acid

71.

Where do long chain hydrocarbons collect?

a)

At the top

b)

In the middle

c)

At the bottom

72.

Where do short chain hydrocarbons collect?

a)

At the top

b)

In the middle

c)

At the bottom

73.

What process happens as the crude oil enters the fractionating column?

a)

Evaporation

b)

Condensation

c)

Combustion

74.

What process happens at each level in the fractionating column?

a)

Evaporation

b)

Condensation

c)

Combustion

75.

Which are more useful as fuels?

a)

Long chain hydrocarbons

b)

Short chain hydrocarbons?

76.

Gases/LPG are used for:

a)

Fuel in cars

b)

Fuel for large ships

c)

Roof and road surfacing

d)

Domestic heating and cooking

77.

Petrol is used for:

a)

Fuel in cars

b)

Fuel in aircraft

c)

Domestic heating and cooking

d)

Road surfacing

78.

Kerosene (paraffin) is used for:

a)

Fuel for cars

b)

Domestic heating and cooking

c)

Fuel in aircraft

d)

Fuel for large ships and in power stations

79.

Diesel oil is used for:

a)

Fuel in cars

b)

Fuel in aircraft

c)

Road and roof surfacing

d)

Fuel in some cars and larger vehicles

80.
Petroleum and natural gas form from...
a)
strong winds
b)
cooled magma
c)
radioactive materials
d)
remains of plants and animals 
81.
How does the temperature change from top to bottom?
a)
Increases
b)
Decreases
c)
It does not change
d)
Cannot be determined
82.
The longer the hydrocarbon, the ________ the flammability?
a)
Lower
b)
Higher
83.

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

84.

Fraction with the highest boiling point

a)

bitumen

b)

refinery gas

c)

petroleum

d)

diesel

85.

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

86.

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

a)

distillation

b)

fractional distillation

c)

cracking

d)

polymerisation

87.
Which of the following is not a use of the products from the fractional distillation of crude oil?
a)
a) Iron ore
b)
b) Petrol
c)
c) Asphalt
d)
d) Motor fuel
88.

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

a)

alkene

b)

hydrocarbon

c)

alkane

d)

saturated

89.

Alkanes have the general formula:

a)

CnH2n

b)

CnH2n+1

c)

CnH2n+2

d)

CnHn

90.

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

a)

saturated

b)

unsaturated

91.

Name the following hydrocarbon

a)

alkane

b)

pentene

c)

pentane

d)

alkene

92.

An atom that gains or loses an electron becomes

a)

an isotope

b)

a new element

c)

an ion

d)

a molecule

93.

When an atom gains an electron it becomes

a)

negatively charged

b)

positively charged

c)

neurtal

94.

Ionic bonds happen when valence electrons are

a)

shared

b)

too heavy

c)

transferred

95.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

96.

Which type of bond occurs between non metals?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

97.

How many valence electrons does Oxygen have?

a)

0

b)

16

c)

6

d)

8

98.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

99.

How many total atoms are in C6H1206

a)

3

b)

6

c)

12

d)

24

100.

What type of bond forms CaF2

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all answers are correct

101.

Is this equation balanced? C3H8 + 5O2 = 4H2O + 3CO2

a)

yes

b)

no

102.

How many oxygen atoms on each side of C3H8 + 5O2 = 4H2O + 3CO2

a)

2

b)

3

c)

5

d)

10

103.

After a chemical reaction occurs, atoms are not created nor destroyed,

a)

just rearranged into a new substance

b)

just changed into different elements

c)

just turned into unstable elements

104.

Compounds that share specific valence electrons are formed by

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

105.
Name this compound:   MgS
a)
Sulfur Magnesium
b)
Magnesium Sulfate
c)
Magnesium Sulfur
d)
Magnesium Sulfide
106.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
107.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
108.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
109.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
110.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
111.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
112.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
113.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
114.
Why do Hydrogen and Helium only need two valence electrons?
a)
The first electron shell can only hold two electrons.
b)
They are both metals.
c)
They both begin with H.
d)
They are both gases.
115.
How many valence electrons do elements in Group 1, the Alkali Metals, have?
a)
1
b)
2
c)
6
d)
7
116.
How many valence electrons do elements in Group 2, the Alkaline Earth Metals, have?
a)
1
b)
2
c)
6
d)
7
117.
Write the formula when Al and O bond?
a)
Al3O2
b)
AlO
c)
Al2O3
d)
O2Al3
118.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
119.
Metals tend to 
a)
gain electrons
b)
lose electrons
120.
Beryllium, Be, and chlorine, Cl, form an ionic compound. In order for the compound to be neutral, what must the formula look like?
a)
Be2Cl
b)
2BeCl
c)
BeCl2
d)
Be2Cl2
121.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

122.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
123.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
124.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
125.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
126.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
127.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
128.

The smallest particle of an element.

a)

Element

b)

Molecule

c)

Atom

129.

What is one way Neutrons are different from electrons?

a)

they both are negative

b)

neutrons have no charge, while electrons have a negative charge

c)

Both are in the nucleus( center of atom)

d)

Electrons are inside nucleus and neutrons are outside the nucleus.

130.

What is the atomic number?

a)

35

b)

18

c)

17

d)

52

131.

How many protons and electrons does this element have?

a)

35

b)

18

c)

17

d)

52

132.

How many neutrons does Chlorine have?

a)

18

b)

17

c)

35

d)

52

133.

What is the atomic mass of Neon?

a)

10

b)

20

c)

30

134.

How many neutrons does calcium have?

a)

20

b)

40

c)

60

d)

0

135.

What is the atomic mass of Arsenic?

a)

33

b)

107

c)

75

136.

What are any of the various self-contained units of matter or energy that are fundamental parts of all matter. These particles include electrons, protons, and neutrons.

a)

subatomic particles

b)

elements

c)

nucleus

d)

electron cloud

137.

What part of an atom has a mass of 1 and a charge of +1?

a)

Neutrons

b)

Protons

c)

Nucleus

d)

Electrons

138.

Where are electrons found?

a)

In neutrons

b)

In shells

c)

In the nucleus

d)

In protons

139.

What particles have a charge of -1 and a very small mass?

a)

protons

b)

neutrons

c)

electrons

d)

shells

140.

How many electrons can fit in the first shell?

a)

1

b)

2

c)

3

d)

4

141.

Elements in group 7 have how many electrons in their outer shell?

a)

1

b)

3

c)

5

d)

7

142.

The period (row) number determines the

a)

number of electrons

b)

number of neutrons

c)

number of shells

d)

number of protons in the nucleus

143.

Why are atoms neutrally charged?

a)

Balanced numbers of protons and neutrons

b)

Equal numbers of electrons and protons

c)

The neutrons have no charge

d)

Atoms always have a positive charge

144.

What element has the symbol N?

a)

Neon

b)

Nitrogen

c)

Nickel

d)

Sodium

145.

What element has the symbol Ca?

a)

Cobalt

b)

Carbon

c)

Copper

d)

Calcium

146.

Isotopes are atoms that have ...

a)

same number of protons but different number of electrons

b)

same number of neutrons but different number of protons

c)

same number of protons but different number of neutrons

d)

same number of electrons but different number of protons

147.
An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.
a)
20
b)
10
c)
5
d)
25
148.
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
149.
What is the atomic mass of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
150.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
151.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
152.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
153.
Which element has an electron configuration of 2.8.8?
a)
Lead
b)
Flourine
c)
Neon
d)
Argon
154.

Which element has the electron configuration of 2.7?

a)

Krypton

b)

Iodine

c)

Fluorine

d)

Barium

155.

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

a)

1

b)

2

c)

8

d)

7

156.

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

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