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Sumer term review

Total questions: 121

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

Chemical reactions occur when reacting particles....

a)

collide

b)

pass

c)

interact

d)

are mixed

2.

The minimum energy particles must have to react is the

a)

acting energy

b)

active energy

c)

activation energy

3.

A reaction profile shows....

a)

the relative difference in temperature of reactants and products

b)

the relative difference in amounts of reactants and products

c)

the relative difference in energy of reactants and products

d)

the relative difference in volume of reactants and products

4.

Bond making is

a)

Endothermic

b)

Exothermic

5.

Bond breaking is..

a)

Endothermic

b)

Exothermic

6.

Which letter shows the activation energy

a)

A

b)

B

c)

C

7.

What is the definition of activation energy? Two answers are required.

a)

The energy needed to start a reaction

b)

The temperature needed to start a reaction

c)

The minimum energy that particles must have to react

d)

The maximum energy that particles must have to react.

8.

In a reaction the energy required to break bonds is less than the energy released when bonds are made. What type of reaction is this?

a)

Exothermic

b)

Endothermic

9.

What would be the product at the negative electrode in the electrolysis of Sodium Chloride solution

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

10.

What would be the product at the positive electrode in the electrolysis of Sodium Chloride solution

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

11.

What would be the product at the negative electrode in the electrolysis of molten Sodium Chloride

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

12.

What would be the product at the positive electrode in the electrolysis of molten Sodium Chloride

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

13.

What would be the product at the negative electrode in the electrolysis of Silver Nitrate solution

a)

Silver

b)

Nitrogen

c)

Hydrogen

d)

Oxygen

14.

What would be the product at the positive electrode in the electrolysis of Silver Nitrate solution

a)

Silver

b)

Nitrogen

c)

Hydrogen

d)

Oxygen

15.

What is the name given to the negative electrode

(a)  

16.

What name is given to the positive electrode

(a)  

17.

What is the third product produced in the electrolysis of Silver Nitrate solution

a)

Silver Nitrate

b)

Water

c)

Nitric Acid

d)

Silver Hydroxide

18.

What is the product at the negative electrode in the electrolysis of Copper Iodide solution

a)

Copper

b)

Iodine

c)

Hydrogen

d)

Oxygen

19.

What is the product at the positive electrode in the electrolysis of Copper Iodide solution

a)

Copper

b)

Iodine

c)

Hydrogen

d)

Oxygen

20.

What is the third product produced in the electrolysis of Copper Iodide solution

a)

Copper Iodide

b)

Copper Hydroxide

c)

Water

d)

Hydrogen Iodide

21.

What particles carry the electrical charge through the electrodes

a)

Electrons

b)

Ions

c)

Atoms

d)

Molecules

22.

What particles carry the electrical charge through the electrolyte

a)

Electrons

b)

Ions

c)

Atoms

d)

Molecules

23.

What would you observe at the negative electrode in the electrolysis of Sodium Chloride solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

24.

What would you observe at the positive electrode in the electrolysis of Sodium Chloride solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

25.

What would you observe at the positive electrode in the electrolysis of Copper Sulphate solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

26.

What would you observe at the negative electrode in the electrolysis of Copper Sulphate solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

27.
What is an ore?
a)
a solid metal
b)
a rock cantaining a metal combined with other elements
c)
an element
d)
an object used to row a boat
28.
What is the name of the positive electrode?
a)
cathode
b)
anode
29.
What is the name of the negative electrode?
a)
cathode
b)
anode
30.
The negatively charged ions migrate toward the ________.
a)
anode
b)
cathode
31.
The negatively charged ions migrate toward the ________.
a)
anode
b)
cathode
32.

What is the ore of aluminium called?

a)

Baxite

b)

Bauxite

c)

Cryolite

d)

Malachite

33.

The electrodes in electrolysis of aluminium are made of

a)

Steel

b)

Anodes

c)

Graphite

d)

Plastic

34.

What do you add to aluminium ore to reduce its melting temperature?

a)

Dendrite

b)

Malachite

c)

Bauxite

d)

Cryolite

35.
What is electrolysis?
a)
breaking down of a compound using a current
b)
making a compound using a current
36.
When NaCl solution is electrolysed what has forms at the anode?
a)
Hydrogen
b)
Oxygen
c)
Chlorine
d)
Sodium
37.
What is the equation to show what happens to Cl ions at the anode.
a)
Cl- --> Cl + e-   
b)
2Cl- --> Cl2 + 2e-   
c)
Cl2 + 2e-   2Cl- 
d)
Cl2 + 2e-  -->  2Cl- 
38.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

a)

Bromine atoms in lead(II) bromide are converted to ions when it is melted

b)

Electrons flow through the lead(II) bromide when it is melted

c)

The ions in lead(II) bromide are mobile charge carriers in the molten state.

d)

There are no ions in solid lead(II) bromide

39.

In electrolytic cell that uses aqueous copper(II) sulfate as electrolyte and copper plates as electrodes, what is the product at the anode?

a)

Oxygen gas and water

b)

Copper metal

c)

Copper(II) ions

d)

Hydrogen gas

40.

Anions get discharged by ________ electrons at the ___________

a)

gaining, cathode

b)

losing, anode

c)

gaining, anode

d)

losing, cathode

41.

What is the gas produced at the anode during the electrolysis of very dilute hydrochloric acid?

a)

water

b)

oxygen

c)

hydrogen

d)

chlorine

42.

Choose the half-equation that shows the discharge of aluminium ion.

a)

Al3+ - 3e- --> Al

b)

Al2+ + 3e- --> Al

c)

Al3+ + 3e- --> Al

d)

Al3+ --> Al + 3e-

43.

What is the half-equation for the discharge of hydroxide ions?

a)

2O2- --> O2 + 4e-

b)

OH- --> OH + e

c)

4OH- --> 2H2O + O2 + 4e-

d)

2H2O + O2 + 4e- --> 4OH-

44.

What factors do not affect the products of electrolysis in the electrolysis of aqueous magnesium chloride using graphite electrodes?

a)

position of ions in the electrochemical series

b)

concentration of ions in the solution

c)

type of electrodes

45.

What ions are present in molten aluminium oxide?

a)

Al3+, O2-, H+, OH-

b)

Al3+, O2-

c)

Al3+, OH-

46.

If the fork is to be electroplated with silver metal, what electrolyte should be used?

a)

Molten silver chloride

b)

Aqueous silver nitrate

c)

Sodium chloride solution

d)

Copper(II) sulphate solution

47.
In an exothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released
48.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
49.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
50.
Is photosynthesis an exothermic or endothermic reaction?
a)
Endothermic
b)
Exothermic
c)
Neither
51.
Baking bread and cooking an egg are examples of....?
a)
Endothermic processes
b)
Exothermic processess
c)
None of these 
52.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
53.
Have you ever eaten sherbet sweets candy? They fizz in your mouth and your tongue feels cold. Why do you think that is?
a)
It is an exothermic reaction
b)
It is an endothermic reaction
c)
It is made of ice
d)
It is dissolving your mouth
54.
Alka-seltzer in water is an example of a 
a)
Endothermic reaction
b)
Exothermic reaction
c)
Dissolving a salt
d)
physical change 
55.
When you freeze water, it turns to ice.  What kind of change is this?
a)
 Physical
b)
Chemical
56.
Sugar dissolves in water.  This is an example of....
a)
Physical Change
b)
Chemical Change
57.
A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true? 
a)
The temperature changed 
b)
It is an endothermic reaction
c)
It is an exothermic reaction 
d)
Two of the answers are correct 
58.
After you mix two substances together, a new substance forms.  This is an example of:
 
a)
 Physical Change
b)
 Chemical Change
59.

What instrument would you use to detect an endothermic or exothermic reaction?

a)

triple beam balance

b)

ruler

c)

thermometer

60.

Metal A is more reactive than Metal B. The following displacement reaction takes place.


Metal A + Metal B in compound ---> Metal B + Metal A in compound.


True or False.

a)

True

b)

False

61.

A more reactive metal will displace a less reactive metal from a metal compound. Which metal is more reactive - copper or iron?

a)

copper

b)

iron

62.

Copper is less reactive than iron. What do you expect to happen when copper is placed inside a solution of iron(II) sulfate?

a)

No reaction takes place.

b)

A reaction takes place. And a colour change is observed.

63.

Copper is less reactive than iron. What do you expect to happen when iron is placed inside a solution of copper(II) sulfate?

a)

No reaction takes place.

b)

A reaction takes place. And a colour change is observed on the iron nail.

64.
Acid + Metal --> ?
a)
Salt + Water
b)
Salt + Hydrogen
c)
Salt
d)
Hydrogen
65.

Iron + Hydrochloric acid --> ?

a)

iron(II) sulfate + water

b)

iron + hydrogen

c)

iron(II) chloride + hydrogen

d)

iron(II) chloride + water

66.

Which gas gives out a 'squeaky pop' when a lighted splint is placed in it?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

d)

nitrogen

67.

Which equation correctly shows the displacement of copper from copper(II) sulfate by zinc?

a)

copper + zinc sulfate --> copper(II) sulfate + zinc

b)

zinc sulfate + copper --> copper(II) sulfate + zinc

c)

copper(II) sulfate + zinc --> zinc sulfate + copper

d)

copper(II) sulfate + zinc --> zinc sulfate + water

68.

Which equation correctly shows magnesium displacing copper from it copper(II) sulfate?

a)

2Mg + O2 --> 2MgO

b)

Mg + CuSO4 --> MgSO4 + Cu

c)

Mg + MgSO4 --> MgSO4 + Mg

69.

A copper coil is placed inside a solution of silver nitrate. What would you expect to see after 5 minutes? Choose 2 options.

a)

There is no visible change because no displacement reaction took place. Copper, being less reactive than silver, cannot displace silver from silver nitrate.

b)
c)
d)

Silver crystals were formed on copper coil, because copper (being more reactive than silver) displaced silver from silver nitrate.

70.

What is the most likely identity of the metal on the filter paper?

a)

Copper, because it is grey.

b)

Potassium, because it can be cut with a knife showing it is soft.

c)

Iron, because it looks grey and all iron looks grey.

71.

Read the underlined words carefully. Rank the metals according to decreasing reactivity (most reactive to least reactive).

a)

Metal A, B, C, D

b)

Metal A, C, B, D

c)

Metal B, C, D, A

d)

Metal D, B, C, A

72.

Alkali metal + Water —> _____________ + ____________

a)

metal hydroxide and oxygen gas

b)

metal hydroxide and hydrogen gas

c)

metal oxide and oxygen gas

d)

metal oxide and hydrogen gas

73.

Lithium + Oxygen —> _________________

a)

Lithium hydroxide

b)

Lithium oxide

c)

Hydrogen gas

d)

Oxygen gas

74.

What is the correct decreasing order of metal reactivity with water ?

a)

Mg > Na > Li > K

b)

Mg > Li > Na > K

c)

Na > Li > Mg > K

d)

K > Na > Li > Mg

75.

Which of the following does not react with water?

a)

Copper

b)

Lithium

c)

Sodium

d)

Potassium

76.

Which of the following metals is the most reactive in dilute sulfuric acid?

a)

Magnesium

b)

Lead

c)

Zinc

d)

Potassium

77.

Name the products formed when zinc reacts with hydrochloric acid?

a)

zinc oxide and water

b)

zinc oxide and water

c)

zinc chloride and hydrogen gas

d)

zinc hydroxide and hydrogen gas

78.

Which one of the following metals reacts slowly with cold water?

a)

Lithium

b)

Copper

c)

Silver

d)

Calcium

79.

Aluminium carbonate + Sulfuric acid —> _______________ + __________________ + water

a)

Aluminium sulfide + Oxygen

b)

Aluminium sulfate + Hydrogen

c)

Aluminium sulfate + Carbon dioxide

d)

Aluminium sulfide + Carbon dioxide

80.

Which of the following metals easily get rusted to form brown deposits on it?

a)

Lead

b)

Gold

c)

Aluminium

d)

Iron

81.

Which of the following metals does not displace hydrogen gas when reacts with dilute HCl or dilute H2SO4?

a)

Lithium

b)

Sodium

c)

Magnesium

d)

Copper

82.

Arrange these metals in decreasing order of reactivity with dilute hydrochloric acid.

Mg, Fe, Ca, Zn, Cu

a)

Ca > Mg > Zn > Fe > Cu

b)

Ca > Mg > Zn > Fe > Mg

c)

Fe > Mg > Zn > Ca > Mg

d)

Zn > Fe > Mg > Ca > Mg

83.

A reaction in which more reactive metal displaces less reactive metal is called ________________ reaction.

a)

Endothermic reaction

b)

Exothermic reaction

c)

Displacement reaction

d)

Combination reaction

84.

Which of the following metals is kept under oil ?

a)

Copper

b)

Gold

c)

Zinc

d)

Potassium

85.

Which of the following metals sink in the container filled with water and react to form hydrogen gas?

a)

Potassium

b)

Sodium

c)

Lithium

d)

Calcium

86.

which of the following reaction would be possible ?

a)

Zinc + Copper sulphate

b)

Copper + Zinc sulphate

c)

Silver + Zinc chloride

d)

Lead + Iron nitrate

87.
The alkali metals are in group 1, on the far left of the periodic table. Which of these is NOT an alkali metal?
a)
Lithium
b)
Iron
c)
Potassium
d)
Francium
88.
How can you tell that a metal is reacting with water?
a)
Colour change
b)
Bright light
c)
Fizzing
d)
It gets colder
89.
What gas is always produced when a metal reacts with water?
a)
Oxygen
b)
Carbon Dioxide
c)
Hydrogen
d)
Carbon Monoxide
90.
What else is produced when a metal reacts with water? (HINT: Water has the formula H2O)
a)
Metal Oxide
b)
Metal Carbonate
c)
Metal Hydride
d)
Metal Hydroxide
91.
When the alkali metals react with water, which reacts most vigorously?
a)
Francium
b)
Rubidium
c)
Potassium
d)
Sodium
92.
Metals can also react with acids. This produces a gas. What is the name of this gas?
a)
Hydrogen
b)
Carbon Dioxide
c)
Nitrogen
d)
Oxygen
93.
As well as a gas, there is another product made when an acid reacts with a metal. What is the name for this?
a)
Salt
b)
Water
c)
Alkali
d)
Carbon
94.
When sodium reacts with hydrochloric acid, what is the name of the salt formed?
a)
Sodium Hydride
b)
Sodium Chloride
c)
Sodium Hydrochloric
d)
Sodium Chlorine
95.
When potassium reacts with sulphuric acid, what is the name of the salt produced?
a)
Potassium Sulphide
b)
Potassium Sulphur
c)
Potassium Sulphuric
d)
Potassium Sulphate
96.
When a metal salt reacts with a more reactive salt, what sort of reaction occurs?
a)
Displacement
b)
Neutralisation
c)
Combustion
d)
No Reaction
97.
When magnesium reacts with copper sulphate, there are two products. What are they?
a)
Magnesium  and Copper
b)
Magnesium Sulphate and Copper
c)
Magnesium Sulphate and Copper Sulphate
d)
Magnesium and Copper Sulphate
98.
When copper and magnesium sulphate are mixed together, there is no reaction. Why?
a)
Magnesium is more reactive than copper
b)
Copper is more reactive than magnesium
c)
Copper never reacts with metal salts
d)
Magnesium Sulphate never reacts with metals
99.
In nature, metals normally react with other compounds to form minerals. What is the metal that is found in the mineral Haematite?
a)
Copper
b)
Aluminium
c)
Iron
d)
Zinc
100.
Metals have many useful properties. For example, they...
a)
...conduct electricity
b)
...are malleable
c)
...are good thermal conductors
d)
All of these
101.
Another useful property of metals is that they are ductile. What does this mean?
a)
The conduct heat well
b)
They can be bent into shape
c)
They have high melting points
d)
They can be stretched into wires
102.
In order to make use of the many useful properties of metals, we need to extract them so that they are in their pure form. A common way of extracting many of the less reactive metals is to heat their minerals with what?
a)
Carbon
b)
Helium
c)
Oxygen
d)
Silicon
103.
Which statement correctly describes the 2 electrodes?
a)
The anode is negative and the cathode is positive
b)
The anode and cathode are both positive
c)
The anode is positive and the cathode is negative
d)
The anode and cathode are both negative.
104.

___________ electrode is an inert electrode.

a)

Copper

b)

Iron

c)

Carbon

d)

Zinc

105.
Positive ions (cations) will move towards the cathode (-) where they will discharge by....
a)
Breaking apart
b)
Losing electrons
c)
Clumping together.
d)
Gaining electrons
106.

Choose the half-equation that shows the discharge of aluminium ion.

a)

Al3+ - 3e- --> Al

b)

Al2+ + 3e- --> Al

c)

Al3+ + 3e- --> Al

d)

Al3+ --> Al + 3e-

107.

Which equation shows what happen to chloride ions at the anode.

a)

Cl- --> Cl + e-

b)

2Cl- --> Cl2 + 2e-

c)

Cl2 - -> 2e- + 2Cl-

d)

Cl2 + 2e- --> 2Cl-

108.

Ionic compounds do not conduct electricity when they are solid because,

a)

their electrons are not free to move

b)

their ions are free to move

c)

their ions are not free to move

d)

their electrons are free to move

109.

Oxidation is loss of electron. Where does oxidation take place during electrolysis.

a)

At anode

b)

In the electrolyte

c)

At the circuit

d)

At cathode

110.
When NaCl solution is electrolysed what has forms at the anode?
a)
Hydrogen
b)
Oxygen
c)
Chlorine
d)
Sodium
111.
What does the Cathode (-) do to ions?
a)
Give electrons to the Positive ions to turn them back into atoms
b)
Take electrons from the positive ions?
c)
Turn ions back into atoms by removing electrons
d)
Turn atoms into ions by adding electrons
112.
What is an ore?
a)
a solid metal
b)
a rock cantaining a metal combined with other elements
c)
an element
d)
an object used to row a boat
113.

The negatively charged ions are attracted to the ________.

a)

anode

b)

cathode

114.
What is the name of the negative electrode?
a)
cathode
b)
anode
115.
What state must the ionic compound be in to be electrolysed?
a)
aqueous only
b)
solid only
c)
solid or aqueous only
d)
molten or aqueous only
116.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

a)

Bromine atoms in lead(II) bromide are converted to ions when it is melted

b)

Electrons flow through the lead(II) bromide when it is melted

c)

The ions in lead(II) bromide are mobile charge carriers in the molten state.

d)

There are no ions in solid lead(II) bromide

117.

What is the half-equation for the discharge of hydroxide ions?

a)

2O2- --> O2 + 4e-

b)

OH- --> OH + e

c)

4OH- --> 2H2O + O2 + 4e-

d)

2H2O + O2 + 4e- --> 4OH-

118.

What ions are present in molten aluminium oxide?

a)

Al3+, O2-, H+, OH-

b)

Al3+, O2-

c)

Al3+, OH-

119.

Electroplating is an industrial process where objects are coated by a thin layer of a nonreactive metal by electrolysis. What should be used as the cathode in this process?

a)

Graphite electrode

b)

The electroplating metal

c)

The object to be electroplated

d)

Magnesium ribbon

120.

If the fork is to be electroplated with silver metal, what electrolyte should be used?

a)

Molten silver chloride

b)

Aqueous silver nitrate

c)

Sodium chloride solution

d)

Copper(II) sulphate solution

121.

What factors do not affect the products of electrolysis in the electrolysis of aqueous magnesium chloride using graphite electrodes?

a)

position of ions in the electrochemical series

b)

concentration of ions in the solution

c)

type of electrodes

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