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Yr 10 Chemistry - Chemical Energy

Total questions: 76

Worksheet time: 6hrs 20mins

Name
Class
Date
1.

The minimum amount of energy that is required to break the chemical bonds of atoms or molecules is:

a)

kinetic energy

b)

light energy

c)

activation energy

d)

potential energy

2.

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

a)

Ruler

b)

Thermometer

c)

Calorimeter

d)

Balance

3.

What type of reaction is this?

a)

endothermic

b)

combustion

c)

hydrocarbon

d)

exothermic

4.

True or false: ΔH for an endothermic reaction is a positive value.

a)

True

b)

False

5.

During a chemical reaction, the chemical potential energy of a substance is released as heat.

a)

true

b)

false

6.

Potential energy is due to the composition or position of an object.

a)

true

b)

false

7.

Chemical potential energy is stored in the chemical bonds of a substance.

a)

true

b)

false

8.

How many joules of energy is required to raise the temperature of one gram of water by one degree Celcius?

a)

41.84 Joules

b)

4.184 Joules

c)

418.4 Joules

d)

4184 Joules

9.

Breaking chemical bonds takes in energy from the surroundings. This is an example of?

a)

endothermic

b)

making

c)

exothermic

d)

breaking

10.

Making chemical bonds gives out energy to the surroundings. This is an example of?

a)

endothermic

b)

exothermic

c)

energy level diagram

d)

combustion

11.

Way to show overall change in energy?

a)

table

b)

line graph

c)

pie chart

d)

energy level diagram

12.

In exothermic reaction the heat is

a)

taken in

b)

given out

13.

In endothermic reaction the heat is

a)

given out

b)

taken in

14.

Is photosynthesis an Exothermic or an Endothermic reaction?

a)

Exothermic

b)

Endothermic

15.

Which letter corresponds to the activation energy?

a)

A

b)

B

c)

C

d)

D

16.

What units are used to measure energy?

a)

Watts

b)

Newtons

c)

Joules

d)

Amps

17.

In an endothermic reaction the products have....

a)

more energy than the reactants

b)

less energy than the reactants

c)

the same energy as the reactants

d)

no energy

18.

In an exothermic reaction, the products have....

a)

more energy than the reactants

b)

the same energy as the reactants

c)

less energy than the reactants

d)

no energy

19.

Which equation is correct?

a)

Energy Change = bonds formed - bonds broken

b)

Energy Change = bonds made - bonds broken

c)

Energy Change = bonds broken - bonds formed

20.

What elements generally make an ionic bond ?

a)

Metal and nonmetal

b)

2 or more nonmetals

c)

2 or more metals

d)

2 elements

21.

What is a valence electron?

a)

an electron that is found in the outermost shell of an atom

b)

an electron found in the innermost shell of an atom

c)

an electron found in the middle shell

d)

an electon found in the nucleus

22.

What is the number of valence electrons of Oxygen?

a)

1

b)

2

c)

6

d)

8

23.

How many electrons are being shared between the two carbon atoms in the compound ethyne?

a)

1

b)

2

c)

3

d)

6

24.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
25.
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
26.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
27.

Why don't noble gases form bonds?

a)

Noble gases do form bonds

b)

They all have a full octet

c)

They only bond with each other

28.
What is a cation? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
29.
What is a anion? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
30.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

31.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) --> PCl5 (s) + energy

a)

endothermic

b)

exothermic

32.

A measure of a chemical bond's strength

a)

Enthalpy

b)

Heat

c)

Bond Energy

d)

Joule

33.

A chemical reaction that occurs between a fuel and an oxidizing agent that produces energy is...

a)

Heat

b)

Joule

c)

Combustion

d)

Thermal Energy

34.

The following equation shows the formation of magnesium oxide from magnesium metal. Which statement is correct for this reaction?

2Mg(s) + O2(g) → 2MgO(s) ΔH = -1204 kJ

a)

1204 kJ of energy are released for every mole of magnesium reacted

b)

602 kJ of energy are absorbed for every mole of magnesium oxide formed

c)

602 kJ of energy are released for every mole of oxygen reacted

d)

1204 kJ of energy are released for every two moles of magnesium oxide formed

35.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

36.

Which of the following represents an exothermic reaction?

a)
b)
37.

Which bond stores the least energy per mole?

a)

C-H

b)

N-H

c)

H-H

d)

C=C

38.

Which bond stores the most energy per mole?

a)

C-H

b)

N-H

c)

H-H

d)

C=C

39.

How many C-H bonds are present here?

a)

4

b)

5

c)

6

d)

7

40.

How many carbon-oxygen double bonds are present here?

a)

1

b)

2

c)

3

d)

4

41.

How many types of bonds are present in this molecule?

a)

3

b)

5

c)

6

d)

8

42.

Which of the following is NOT a type of bond present in this molecule?

a)

C-H

b)

C-C

c)

C=O

d)

C-O

43.

Calculate the total bond energy that exists within one molecule of water (H2O).

a)

467kJ

b)

467kJ/mol

c)

934kJ

d)

934kJ/mol

44.

What is the bond energy that exists within a hydrochloric acid molecule (HCl)?

a)

427 kj

b)

427kJ/mol

c)

427 cal

d)

427 cal/mol

45.
What is essential for a combustion reaction to begin?
a)
Carbon dioxide
b)
Fuel 
c)
Fuel, oxygen and heat
d)
Water and oxygen
46.
Complete combustion is when there is plenty of oxygen to react with. 
a)
True
b)
False
47.
Incomplete combustion is when there is a limited amount of oxygen.
a)
True
b)
False
48.

What are the products of combustion?

a)

Hydrogen + oxygen

b)

Carbon dioxide + water

c)

Carbon dioxide + hydrogen

d)

Carbon + water

49.
A compound that contains only carbon and hydrogen and that produces carbon dioxide and water when burned is called a(n)
a)
binary compound
b)
carbonate
c)
ionic compound
d)
hydrocarbon
50.

Which picture is NOT an example of chemical potential energy?

a)
b)
c)
d)
51.
What does incomplete combustion produce that complete combustion doesn't?
a)
Carbon monoxide
b)
Water
52.

In a Galvanic cell, the salt bridge...

a)

completes the circuit so that electrons can flow through the wire

b)

maintains charge balance

c)

is soaked in an unreactive electrolyte such as KNO3

d)

all of the above

53.

In the above Galvanic Cell, which half cell is undergoing reduction?

a)

Cu | Cu2+

b)

Zn | Zn2+

54.

Consider the galvanic cell reaction Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq) When the cell is running spontaneously, which is the only true statement?

a)

The copper electrode loses mass and the zinc electrode is the cathode.

b)

The copper electrode gains mass and the copper electrode is the cathode.

c)

The zinc electrode gains mass and the zinc electrode is the anode.

d)

The zinc electrode loses mass and the zinc electrode is the cathode.

Show answersExplanationPreviousNext

55.

In a redox reaction, the oxidising agent is...

a)

oxidised

b)

reduced

56.

What reaction occurs at the anode?

a)

Ag+ + e- →Ag

b)

Ag → Ag+ + e-

c)

Ni2+ + 2e- → Ni

d)

Ni → Ni2+ + 2e-

57.

WHAT DO WE CALL THE METAL COATING THE OUTSIDE LAYER OF ANOTHER METAL?

a)

SACRIFICIAL METAL

b)

ELECTROPLATED METAL

c)

DYING METAL

d)

OXIDISED METAL

58.

ANOTHER NAME FOR A SPONTANEOUS ELECTROCHEMICAL CELL

a)

SALT BRIDGE

b)

VOLTMETER

c)

ELECTROLYSIS CELL

d)

VOLTAIC CELL

59.

WHERE IS THE ANODE?

a)

COPPER ELECTRODE

b)

ZINC ELECTRODE

c)

ZINC SULFATE SOLUTION

d)

SALT BRIDGE

60.

In a Galvanic cell, the electrons flow from the...

a)

anode to the cathode

b)

cathode to the anode

61.

In a Galvanic cell, the cations in the salt bridge...

a)

flow the same way as the electrons flow in the wire

b)

flow the opposite way to the electron flow in the wire

c)

stay in the salt bridge

62.

Oxidation is the _________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

63.

Reduction is the _________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

64.

.................................................. process is any conversion between chemical energy and electrical energy.

a)

An electrochemical

b)

A biochemical

c)

A geochemical

65.

A typical half-cell consists of a piece of ................... immersed in a solution of its ions.

a)

metal

b)

nonmetal

66.

Which combination would electroplate an object with copper?

a)

A

b)

B

c)

C

d)

D

67.

In an electrochemical cell, which particles carry the electrical charge through the electrodes?

a)

Electrons

b)

Ions

c)

Atoms

d)

Molecules

68.

In an electrochemical cell, which particles carry the electrical charge through the electrolyte?

a)

Electrons

b)

Ions

c)

Atoms

d)

Molecules

69.

______ allows organisms to liberate the energy stored in the chemical bonds of glucose.

a)

redox reaction

b)

oxidizing agent

c)

photosynthesis

d)

Cellular respiration

70.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
71.

What is another name for oxidation-reduction

a)

Redox

b)

chemical reaction

c)

experiment

d)

chemical change

72.

The following ionic equation represents a redox reaction

Al + 3Ag+ -----> Al3+ + 3Ag

Which statement is correct?

a)

Silver ion is oxidized

b)

Silver ion is a reducing agent

c)

Aluminium atom undergoes oxidation

d)

Aluminium atom receives electrons

73.

What are the two conditions that caused iron to rust ?

a)

Air and Oxygen

b)

Oxygen and Water

c)

Water and Carbon dioxide

d)

Carbon dioxide and Air

74.

Rust is also known as

a)

hydrated iron

b)

iron oxide

c)

copper carbonate

d)

hydrated iron oxide

75.

Which diagram shows the most favourable conditions for rust to appear on the nail?

a)

A

b)

B

c)

C

d)

D

76.

To protect iron against corrosion, the most durable metal plating on it, is:

a)

Zinc plating

b)

Nickel plating

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