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Total questions: 75

Worksheet time: 4hrs 36mins

Name
Class
Date
1.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

2.

The negative ions tend to _____________ electrons.

a)

lose

b)

gain

3.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

4.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

5.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
6.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
7.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
8.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
9.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
10.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
11.

What type of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids?

12.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

13.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

14.

How does calcium become an calcium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

15.

How does magnesium become an magnesium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

16.

How does oxygen become an oxide ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

17.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
18.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
19.
An electron has what kind of charge?
a)
no charge
b)
positive 
c)
negative
d)
it depends
20.

What is responsible for bringing cations and anions together?

a)

the size of the ions

b)

the opposite charges are attracted to one another

c)

the similar charges are attracted to one another

d)

depends on what period they're in

21.

When ionic compounds form what is the overall charge?

a)

neutral

b)

positive

c)

negative

22.

In the compound aluminum oxide, which is the cation?

a)

[ Al ] +3

b)

Al

c)

[ O ] -2

d)

O

23.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

24.

Looking at the periodic table, when the halogens form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

25.

Looking at the periodic table, when the alkaline earth metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

26.

Looking at the periodic table, when the alkali metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

27.

If I had an anion with a charge of 3- how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 3 electrons

d)

lost 3 electrons

28.

If I had a cation with a charge of 2+ how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

29.

An ionic bond is the attraction between: (Select ALL that apply)

a)

oppositely charged ions

b)

similarly charged ions

c)

metals and nonmetals

d)

neutral atoms

e)

cations and anions

30.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

31.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
32.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
33.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
34.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
35.

Covalent bonds are formed between...

a)

two or more metal atoms

b)

two or more non-metal atoms

c)

a metal and a non-metal atom

36.

Covalent bonds are formed when electrons are transferred between atoms.

a)

True

b)

False

37.

The structure of ammonia is shown in the diagram. What is the formula for ammonia?

a)

NH3

b)

HN3

c)

N3H

d)

HN3

38.
In a(an) POLAR bond, one atom pulls on the shared electrons more than the other atom. 
a)
True
b)
False
39.
A(n) ION is a neutral group of atoms joined by covalent bonds.
a)
True
b)
False
40.
Covalent bonds usually form when a nonmetal combines with a(an) METAL.
a)
True
b)
False
41.
The chemical bond formed when two atoms share electrons  is called a(an) IONIC bond. 
a)
True
b)
False
42.

This type of bonding occurs when atoms share electrons.

a)

chemical

b)

covalent

c)

ionic

d)

metallic

43.

Single bonds are formed when ____ pair(s) of valence electrons are shared.

a)

one

b)

three

c)

two

d)

four

44.

Triple bonds are formed when atoms share _____ pairs of valence electrons.

a)

two

b)

four

c)

three

d)

six

45.

What is a diatomic molecule?

a)

Two atoms that are the same and share one or more electrons.

b)

Two atoms that share a different valence electron.

c)

Two atoms that share protons.

d)

Two ions that share a completed outer energy level.

46.

Many _____ exist as diatomic molecules.

a)

alkali metals

b)

alkali earth metals

c)

metalloids

d)

nonmetals

47.

Except for noble gases, elements on the right side of the table have a greater attraction to

a)

elements that are metalloids.

b)

elements that are halogens.

c)

elements that are in the transition zone of the table.

d)

elements that are on the left side of the table.

48.

A covalent bond in which electrons are not shared equally is called a(n)

a)

polar covalent bond.

b)

metallic covalent bond.

c)

ionic bond.

d)

unequal bond.

49.

When atoms form polar covalent bonds, atoms with the greater attraction for electrons has a(n)

a)

slight positive charge.

b)

slight negative charge.

c)

neutral charge.

d)

opposite charge.

50.

The type of atom and its shape are factors in determining

a)

if a molecule is covalent or polar.

b)

whether a molecule is polar or nonpolar.

c)

if the atoms are negative or positive.

d)

whether the molecule has valence electrons.

51.

The shape of the carbon dioxide molecule allows it to be classified as

a)

polar.

b)

linear.

c)

nonpolar.

d)

charged.

52.

Which of these elements do not bond to form molecules?

a)

helium

b)

chlorine

c)

oxygen

d)

neon

53.

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

54.

What is the correct formula for this molecule?

a)

CH

b)

C1H4

c)

CH4

d)

C4H

55.

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

56.

How many electrons are involved in a double bond?

a)

One pair of electrons

b)

Two pairs of electrons

c)

6 electrons

d)

8 electrons

57.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
58.
There are more metals than non metals in the periodic table.
a)
True
b)
False
59.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
60.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
61.

What is the ability of a substance to be pulled into a wire?

a)

Malleability

b)

Ductility

c)

Conductivity

d)

Solubility

62.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
63.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
64.
Metallic bonding is...
a)
a type of covalent bond.
b)
a type of ionic bond.
c)
an attraction between positive ions and electrons.
65.
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
66.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

67.
I can hit a metal with a hammer without the metal shattering because of its __________.
a)
Ductility
b)
Malleability
c)
Conductivity
d)
Lustrousness
68.

X is a solid at room temperature.

X has a high melting point.

Solid X conducts electricity.


Which diagram shows how the particles are arranged in solid X?

a)
b)
c)
d)
69.

Iron is a metal.

Its structure consists of a giant lattice of positive ions in a ‘sea of electrons’.


Which statements about solid iron are correct?

a)

Iron conducts electricity because the electrons are free to move

b)

Iron conducts heat because the positive ions are free to move.

c)

Iron has a high melting point due to the strong covalent bonds.

d)

Iron is malleable because the layers of ions can slide over one another.

70.

Metals are malleable. Which statement explains why metals are malleable?

a)

Metallic bonding is very strong.

b)

Metals are good conductors of electricity.

c)

Positive metal ions are arranged in a regular lattice structure

d)

The layers of positive metal ions can slide over each other.

71.

The diagram represents the general structure of a solid Z.


What is Z?

a)

aluminium

b)

iodine

c)

silicon dioxide

d)

sulfur

72.

True or False: Metals can be shaped into thin sheets

a)

True

b)

False

73.

Metal ions are surrounded by a "sea" of POSITIVE charge

a)

True

b)

False

74.

True or False: A metallic bond may form between a metal and any other element

a)

True

b)

False

75.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

positive ions are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

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