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SJC S3 Exam Revision HW

Total questions: 87

Worksheet time: 2hrs 2mins

Name
Class
Date
1.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
2.

What is the reason why Noble gases are so stable?

a)

They have an even number of electrons

b)

They have no electrons

c)

They have a full outer shell of electrons

d)

They bond with other atoms

3.

Covalent bonds are formed between...

a)

2 non-metals

b)

a metal and a non-metal

c)

2 metals

d)

2 ions

4.

How many electrons are involved in a double bond?

a)

One pair of electrons

b)

Two pairs of electrons

c)

2 electrons

d)

6 electrons

5.

Which of these is not a covalent molecule?

a)

MgO

b)

CO2

c)

HCl

d)

CH4

6.

Chlorine has 7 electrons in it's outer shell. How many covalent bonds does it need to make to complete it's outer shell electrons?

a)

1

b)

2

c)

3

d)

4

7.

Oxygen has 6 electrons in it's outer shell. How many covalent bonds does it need to make to complete it's outer shell electrons?

a)

1

b)

2

c)

3

d)

4

8.

Carbon has 4 electrons in it's outer shell. How many covalent bonds does it need to make to complete it's outer shell electrons?

a)

1

b)

2

c)

3

d)

4

9.

What is the valency of an element?

a)

The total number of electrons in the atom

b)

The number of electrons the atom needs to lose

c)

The number of electrons needed to obtain a complete outer shell

d)

The number of electrons closest to the nucleus

10.

Why do atoms have an overall neutral charge?

a)

So that they can't react

b)

Because they have neutrons in their nucleus

c)

Because they have electrons arranged in shells

d)

Because they have the same number of protons and neutrons

11.

What is the correct formula for this molecule?

a)

CH

b)

C1H4

c)

CH4

d)

C4H

12.

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

13.

Which of the following is a Diatomic Molecule

a)

Potassium

b)

Carbon

c)

Sulfur

d)

Nitrogen

14.
What is the name of this Molecule shape
a)
Tetrahedral
b)
Trigonal Pyramidal 
c)
Trigonal bipyramidal
d)
Bent
15.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
16.

Conducts electricity well when dissolved in water

a)

Ionic lattice

b)

Covalent molecule

c)

Covalent Network

d)

Metallic lattice

17.

Can be a solid, liquid, or gas at room temperature

a)

Ionic lattice

b)

Covalent molecule

c)

Covalent Network

d)

Metallic lattice

18.

Very high melting and boiling points, does not conduct in any state

a)

Ionic lattice

b)

Covalent molecule

c)

Covalent Network

d)

Metallic lattice

19.

Conducts in solid form

a)

Ionic lattice

b)

Covalent molecule

c)

Covalent Network

d)

Metallic lattice

20.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
21.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
22.
In general, what can be said of the melting points of metals?
a)
They are low.
b)
They are high.
c)
They are lower than nonmetals.
d)
They do not have melting points.
23.
Carbon dioxide
a)
C2O2
b)
C20
c)
CO
d)
CO2
24.

How are compounds with metallic bonds similar to ionic compounds?

a)

Both tend to have double and triple bonds.

b)

Both tend to have low boiling point

c)

Both tend to have poor conductivity.

d)

Both tend to have high melting points.

25.

Which of the following would have the lowest melting point?

a)

MgCl2

b)

Al2O3

c)

CO2

d)

AlP

26.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
27.

Atoms joined together by sharing electrons are?

a)
Ionic bonds
b)
Covalent bonds
c)
Metallic Bonds
d)
James Bonds
28.

The temperature at which a liquid turns into a gas describes

a)

Malleability

b)

Boiling point

c)

Thermal conductivity

d)

Melting point

29.

Which of the following is an example of a covalent compound?

a)
H2S
b)
KI
c)
CaCl2
d)
MgO
30.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

31.

What are diatomic elements?

a)

Elements that form two-atom molecules when not combined in a compound.

b)

Two elements that combine with one atom from each element.

c)

Elements that are always in pairs no matter what.

32.
The definition: an expression which states the number and type of atoms present in a molecule of a substance, best describes 
a)
chemical formula
b)
chemical symbol
c)
chemical equation
d)
group or family
33.
In Cl2, the 2 is known as
a)
the subscript.
b)
the coefficient.
c)
the molecular mass.
d)
the number of protons.
34.
In what form is Nitrogen commonly found in nature?
a)
gas-N2
b)
solid-N
c)
unknown
35.
Chlorine, bromine, fluorine, and iodine are all 
a)
nonmetals and good conductors.
b)
nonmetals and halogen gases.
c)
metals and bad conductors.
d)
metals and malleable.
36.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
37.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
38.
An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.
a)
20
b)
10
c)
5
d)
25
39.
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
40.
The particles of the atom you can find by knowing the atomic number.
a)
neutrons
b)
protons and electrons
c)
protons and neutrons
d)
atomic mass
41.
What is the electron configuration of sodium?
a)

2,8

b)

2,8,2

c)

2,8,1

d)
11
42.

Which element has an electron configuration of 2,5?

a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
43.

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

a)

1

b)

2

c)

8

d)

7

44.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

45.

What happens to the reactivity of the halogens as you move down the group?

a)

increases

b)

decreases

46.

What is a subatomic particle with a positive charge that is in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

47.

What is a subatomic particle without an electric charge, located in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

48.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

49.

What term describes a structure where a large number of atoms join together to form a giant lattice held together by strong covalent bonds?

a)

Covalent molecule

b)

Ionic lattice

c)

Metallic lattice

d)

Covalent network

50.

What is the shape called when a central atom has 4 bonds, as shown in the diagram?

a)

Tetrahedral

b)

Angular

c)

Trigonal pyramidal

d)

Linear

51.

What is the shape called when a central atom has 3 bonds, as shown in the diagram?

a)

Tetrahedral

b)

Angular

c)

Trigonal pyramidal

d)

Linear

52.

What is the shape called when a central atom has 2 bonds, as shown in the diagram?

a)

Tetrahedral

b)

Angular

c)

Trigonal pyramidal

d)

Linear

53.

What is the shape called when a central atom has 1 bond, as shown in the diagram?

a)

Tetrahedral

b)

Angular

c)

Trigonal pyramidal

d)

Linear

54.

What is an atom or molecule that has gained or lost electrons, resulting in a positive or negative charge, called?

a)

Ion

b)

Compound

c)

Molecule

d)

Atom

55.

What term is used to describe the number of electrons an atom needs to gain or lose to achieve a stable electron configuration?

a)

Molecule

b)

Ionic Bonding

c)

Synthesis

d)

Valency

56.

What is a group ion?

a)

A family of compounds

b)

Ion with no charge

c)

Ion with a positive and negative charge

d)

An ion that consists of more than one atom

57.

What is the force of attraction between particles with opposite electric charges called?

a)

Metal

b)

Electrostatic attraction

c)

Ionic bond

d)

Covalent bond

58.

Which term refers to conductive materials used to make contact with a nonmetallic part of an electrical circuit?

a)

Cathode

b)

Electrolysis

c)

Electrodes

d)

Neutrons

59.

What does the term 'electron configuration' refer to?

a)

The distribution of electrons in the energy levels or orbitals of an atom or ion.

b)

The number of neutrons in an atom.

c)

The number of valence electrons in an atom.

d)

The arrangement of electrons around the nucleus of an atom.

60.

What is the process called that uses an electric current to decompose ionic compounds into their constituent elements?

a)

Solubility

b)

Filtration

c)

Electrolysis

d)

Distillation

61.

What is a diagram that represents all of the electrons and shells of an atom called?

a)

Target diagram

b)

Dot-cross diagram

62.

What is the term for a diagram that represents covalent bonding by showing the sharing of electrons between atoms?

a)

Target diagram

b)

Dot-cross diagram

63.

What is the assumed valency of silver?

a)

1

b)

2

c)

3

d)

0

64.

What is the assumed valency of a transition metal if there are no Roman numerals given?

a)

1

b)

2

c)

3

d)

4

65.

Which of the following best describes how atoms form ionic bonds?

a)

By sharing electron pairs equally between atoms

b)

By transferring electrons from one atom to another

c)

By increasing the distance between the nuclei of two atoms

d)

By creating a magnetic attraction between two atoms

66.

What is the structure of ionic substances typically like?

a)

A random arrangement of ions

b)

A single line of ions

c)

A repeating three-dimensional lattice structure

d)

A layered structure like graphite

67.

Which of the following is a property of ionic compounds?

a)

They have low melting and boiling points

b)

They conduct electricity when solid

c)

They are typically soluble in water

d)

They are composed of only non-metal elements

68.

How many protons does a sodium ion (Na+) have?

a)

10

b)

11

c)

12

d)

9

69.

What is the total charge of a sodium ion (Na+)?

a)

0

b)

+1

c)

-1

d)

+2

70.

Why do noble gases not form ions?

a)

They have no electrons.

b)

They already have a full outer shell of electrons.

c)

They have a negative charge.

d)

They have 5, 6, or 7 electrons in their outer shell.

71.

Which of the following is the correct ion formula for chlorine?

a)

Cl2+

b)

Cl2-

c)

Cl+

d)

Cl-

72.

Which equation is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

73.
Which number should go in the blank?
Mn + _ HNO3 → Mn(NO3)2 + H2
a)

1

b)

2

c)

3

d)

0

74.

Which of the following elements exists as a covalent network?

a)

silicon

b)

oxygen

c)

chlorine

d)

hydrogen

75.

What is the gram formula mass of nitrogen?

a)

14

b)

7

c)

21

d)

4

76.

Which of the following structures is never found in compounds?

a)

monatomic

b)

diatomic

c)

covalent network

d)

ionic lattice

77.

What is the chemical formula of calcium carbonate

a)

CaCO

b)

CaCO2

c)

CaC

d)

CaCO3

78.

Why do ionic substances conduct electricity when molten and in solution?

a)

they have delocaised electrons

b)

their ions are free to move

c)

their electrons are free to move

d)

they do not conduct

79.

Why do covalent networks have high melting and boiling points?

a)

weak forces need to be broken

b)

strong covalent bonds need to be broken

80.

Why do covalent molecules have low melting and boiling points?

a)

weak forces need to be broken

b)

strong covalent bonds need to be broken

81.

What is the mass of one mole of sodium sulfate (Na2SO4)?

a)

71

b)

142

c)

284

82.

What is the ionic formula for lithium fluoride?

a)

Li-F+

b)

Li+7F-

c)

Li+F-

d)

L+Fl-

83.

Which of these always happens during a chemical reaction?

a)

A new substance is formed

b)

Heat energy is released

c)

Heat energy is taken in

d)

Gas is produced

84.

Is this chemical equation balanced?

a)

Yes

b)

No

85.

What is the test for Carbon Dioxide?

a)

Relights a glowing splint

b)

Lime water turning milky

c)

Burns with a squeaky pop

86.

What is the test for Oxygen?

a)

Relights a glowing splint

b)

Lime water turning milky

c)

Burns with a squeaky pop

87.

What is the test for Hydrogen?

a)

Relights a glowing splint

b)

Lime water turning milky

c)

Burns with a squeaky pop

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