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Q2 Revision

Total questions: 94

Worksheet time: 2hrs 41mins

Name
Class
Date
1.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
2.
Ions that are made of more than one atom are called...
a)
ionic compounds
b)
crystals
c)
polyatomic atoms
d)
ionic bonds
3.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
4.
Which is most likely to form a negative ion...
a)
an element from Group 17
b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
5.
Which of the following is the correct name for MgCl2....
a)
Magnesium Clorine
b)
Magnesium Dicholorine
c)
Magnesium Cloride
d)
Magnesium Dichloride
6.
The attraction between oppositely charged ions is called a(n) _______________.
a)
ionic bond
b)
polyatomic ion
7.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
8.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
9.
In order to have a stable arrangement of 8 valence electrons, metal atoms are likely to _________electrons.
a)
gain
b)
lose
10.
In an ionic compound, the total positive charge of all the positive ions ___________ the total negative charge of all the negative ions.
a)
equals
b)
is more than
11.
Because the force of attraction between the positive and negative ions is so strong, ionic compounds have _________ melting points.
a)
high
b)
low
12.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

13.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

14.

Select all of the statements below that are correct to describe the structure and properties of ionic compounds...

a)

They have high melting and boiling points

b)

They have a lattice structure

c)

The ions are held together by intermolecular forces

d)

They can conduct electricity when molten

e)

They can conduct electricity when solid

15.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

16.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

17.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

18.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

19.
 Which of the following is the correct formula for these two ions:
Al+3 +  S-2
a)
AlS3
b)
Al2S3
c)
Al3S2
d)
Al3S
20.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
21.

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

22.

What type of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids?

23.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
24.

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

25.

What is an ionic bond?

a)

A bond formed by the sharing of electrons.

b)

A bond formed by the transfer of electrons.

c)

A bond formed by the attraction of nuclei.

d)

A bond formed by the overlapping of atomic orbitals.

26.

Boron, B, will ____ valence electrons when forming an ionic bond.

a)

lose three

b)

gain three

c)

lose 5

d)

gain 5

27.

How many electrons are needed in the outer energy levels of an atom to be stable?

a)

2

b)

4

c)

6

d)

8

28.

In the chemical formula for an ionic compound, which item is written first?

a)

positive ion

b)

negative ion

c)

subscript

d)

the female

29.

Boron is in column 13 & has a charge of _. Potassium is in column 1 & has a charge of _.

a)

-3; +1

b)

+3; -1

c)

-3; -1

d)

+3; +1

30.

What is the charge on an Aluminium ion?

a)

3

b)

+3

c)

+2

d)

+1

31.

What is the charge on a chloride ion?

a)

-1

b)

1

c)

+2

d)

+1

32.

What is the formula of calcium oxide?

a)

CaO2

b)

CaO

c)

Ca2O

d)

CO

33.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
34.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
35.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
36.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
37.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
38.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
39.
The chemical bond formed when two atoms share electrons  is called a(an) IONIC bond. 
a)
True
b)
False
40.
Covalent bonds usually form when a nonmetal combines with a(an) METAL.
a)
True
b)
False
41.
A(n) ION is a neutral group of atoms joined by covalent bonds.
a)
True
b)
False
42.
If a molecule contains polar bonds, the molecule MAY OR MAY NOT be polar overall. 
a)
True 
b)
False
43.
In a(an) POLAR bond, one atom pulls on the shared electrons more than the other atom. 
a)
True
b)
False
44.
The forces between molecules are much STRONGER than the forces between ions. 
a)
True
b)
False
45.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

46.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

47.

A Metal + Nonmetal compound is a(n)...

a)

ionic compound

b)

covalent compound

48.

A bond between two atoms that share one pair of electrons.

a)

Double covalent bonds

b)

Triple covalent bonds

c)

Covalent bonds

d)

Single covalent bond

49.
What would you name this molecule?
a)
SNa3
b)
H3O
c)
NaCl
d)
H2O
50.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
51.

How many pairs of valence electrons are being shared in a single ammonia molecule?

a)

0 pair - 0 valence electrons

b)

1 pair - 2 valence electrons

c)

2 pair - 4 valence electrons

d)

3 pair - 6 valence electrons

52.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
53.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
54.

What type of bond would form between O and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

55.

What type of bond would form between O and H?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

56.

The bond between C and Cl is polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

57.

The bond between C and H is non-polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

58.
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.
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.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
62.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
63.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
64.
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
65.

What are some benefits of alloys? (choose all that apply)

a)

they can be stronger than pure metal

b)

they may not rust/corrode as easily

c)

they don't have electrons

d)

they form covalent bonds

66.

A solid mixture of a metal with one or more other elements is a(n)

(a)  

67.

A structure formed by metallic bonding is known as a

(a)  

68.

What is the one thing responsible for a metal being malleable, ductile, and conductive?

a)

metal atoms

b)

its covalent bonds

c)

its valence electrons

d)

its sea of free-floating electrons

69.

A metallic bond is a bond between ________.

a)

nonmetals

b)

metals

c)

transition metals

d)

metalloids

70.

Why are metals good conductors of electricity?

a)

The electric current can easily travel along the surface of the metal because it is smooth.

b)

A negative charge can easily push the sea of electrons in one direction, making a current.

c)

Metals attract electricity.

d)

Metals are malleable.

71.
Why are alloys generally used to make everyday objects?
a)
Alloys are often stronger and less active than pure metals.
b)
Alloys have higher melting point than pure metals.
c)
Alloys are less expensive to produce than pure metals.
d)
Alloys have ionic bonds instead of metallic bonds.
72.
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.
73.
What do metals conduct?
a)
heat
b)
electricity
c)
both
d)
neither
74.
Any change that alters a substance without changing it into another substance is a(n) ____________ change. 
a)
Physical
b)
Chemical
75.
A reaction that release energy in the form of heat is called a(n) _______________ reaction.
a)
Exothermic
b)
Endothermic
76.
A(n) ______________ reaction is a reaction in which energy is absorbed. 
a)
Endothermic
b)
Exothermic
77.
A chemical change is also referred to as a(n) _____________.
a)
Chemical Reaction
b)
Physical Reaction
78.
A(n) ____________ is a solid formed from liquid reactants during a chemical reaction.
a)
precipitate
b)
product
79.
Substances that enter into a chemical reaction are called products. 
a)
True
b)
False
80.

In an endothermic reaction, energy is

a)

absorbed

b)

released

c)

converted to mass

d)

synthesized

81.

Which of the following is NOT a physical property?

a)

melting point

b)

state of matter

c)

density

d)

flammability

82.

Substances formed as a result of a chemical reaction are called

a)

catalysts

b)

precipitates

c)

products

d)

reactants

83.

Breaking glass is a

a)

physical change

b)

chemical change

84.

Fireworks exploding is a

a)

physical change

b)

chemical change

85.

produces one or more new substances

a)

physical changes

b)

chemical changes

86.

Substances formed as a result of a chemical reaction are called

a)

catalysts

b)

precipitates

c)

products

d)

reactants

87.
Evidence that a reaction has occurred includes
a)
change of color
b)
formation of a precipitate
c)
release of gas bubbles
d)
all of these
88.
Cooking is a great example of 
a)
exothermic reactions
b)
endothermic reactions
c)
no chemical reactions have occurred
d)
the production of precipitates
89.
H2 + Cl reacts to form HCl. In this reaction:
H:H +Cl → HCl. This can be described as
a)
Hydrogen bonds break and H and Cl bonds form
b)
Chlorine bonds break and hydrogen bonds form
c)
No bonds break or form
d)
energy is released
90.
What are the reactants in this chemical equation?
6O2 + C6H12O6 -> 6CO2 + 6H2O + ENERGY
a)
CO2 + H2O
b)
O2 + C6H12O6
c)
O2 _ CO2
d)
C6H12O6 + H2O
91.

Frying an egg is an example of a _______.

a)

physical change

b)

chemical change

c)

transformational change

d)

material change

92.

Chemical changes occur when existing bonds break and _______.

a)

the same bonds reform again

b)

no new bonds form

c)

everything disappears

d)

new bonds form

93.

A characteristic of a substance that describes its ability to change into another substance is a _______.

a)

chemical property

b)

physical property

c)

material property

d)

transformational property

94.

A characteristic of a substance that can be observed without changing the substance into another substance is a _______.

a)

chemical property

b)

physical property

c)

chemical reaction

d)

physical malleability

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