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Unit 3 Lesson 1 Practice Test

Total questions: 85

Worksheet time: 1hrs 4mins

Name
Class
Date
1.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

2.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

3.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

4.

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

5.

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

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

6.

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

a)

O-

b)

O+

c)

O2-

d)

O2+

7.

Lead(II) Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

8.

Which of the following could NOT form an ionic compound? Check all that apply.

a)

Li+ and Cl-

b)

F- and O2-

c)

Ba2+ and Ag+

d)

Mg2+ and S2-

9.

Which of the following could form an ionic compound? Check all that apply.

a)

Na+ and F-

b)

S2- and O2-

c)

Ca2+ and Fe3+

d)

Mg2+ and Cl-

10.

Which element(s) will lose valence electrons to form an ion? Check all that apply.

a)

Phosphorus

b)

Iron

c)

Barium

d)

Neon

11.

The following ionic crystal has 4 Sr ions (red) and 8 Br ions (blue). What is the formula for this ionic crystal?

a)

SrBr

b)

SrBr2

c)

Sr2Br

d)

Sr4Br8

12.

The following ionic crystal has 6 Fe ions (red) and 9 O ions (blue). What is the formula for this ionic crystal?

a)

FeO

b)

Fe2O3

c)

Fe3O2

d)

Fe6O9

13.
A cation is a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
14.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
15.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
16.

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

a)

N

b)

N-3

c)

N-5

d)

N+5

17.
How many electrons are needed in the outer energy levels of an atom to be stable?
a)
2
b)
4
c)
6
d)
8
18.

Sulfur, S, will ____ valence electrons when forming an ionic bond.

a)

gain 1

b)

lose 1

c)

gain 2

d)

lose 2

19.

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

a)

lose three

b)

gain three

c)

lose 5

d)

gain 5

20.
Write the formula for barium + nitrogen
a)
Ba2N3
b)
Ba3N2
c)
BaN
d)
BaN3
21.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
22.
Write the correct formula for an ionic compound formed from S2- and Rb1+.
a)
SRb2
b)
SRb
c)
Rb2S
d)
RbS2
23.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

24.

Molecules

a)

Ionic compounds

b)

Covalent compounds

25.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

26.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

27.

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

a)

Ionic compounds

b)

Covalent compounds

28.

What kind of bond does this show?

a)

Ionic

b)

Covalent

29.

Generally, atoms form bonds so that _______________.

a)

Each atom loses its electrons

b)

Each atom has a stable electron configuration

c)

Each atom has an unstable electron configuration

d)

Each atom gains electrons

30.

What kind of bonds are shown here?

a)

Covalent

b)

Ionic

31.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

32.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

33.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
34.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

35.

Which of the following is the best representation of a molecule of fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

36.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
37.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
38.

When two nonmetals do not share electrons evenly, the resulting covalent bond will be

a)

nonpolar

b)

polar

c)

ionic

d)

metallic

39.
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
40.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
41.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
42.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
43.

Which is the correct structure for NH3?

Pictures correspond with a-d.

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

44.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
45.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
46.

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

a)

one

b)

three

c)

two

d)

four

47.

In general, elements at the top of a group have a greater attraction for electrons than

a)

alkali metals.

b)

alkaline earth metals.

c)

elements at the bottom of a group.

d)

elements on the right side of a group.

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.

Attractions between polar molecules are weaker than attractions between nonpolar molecules.

a)

True

b)

False

51.
Fluorine (F₂) is a(n)  _________________                  molecule because the valence electrons are shared equally between the two fluorine atoms.
a)
polar
b)
nonpolar
c)
ionic
d)
crystal
52.
Which type of bond does Nitrogen and Hydrogen make?
a)
covalent
b)
metallic
c)
ionic
d)
James
53.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
54.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
55.
In the correct Lewis structure for CH4, how many unshared electron pairs surround the carbon?
a)
2
b)
8
c)
0
d)
4
56.
In CO2, how many UNSHARED pairs of electrons does each oxygen have?
a)
2
b)
1
c)
4
d)
6
57.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
58.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
59.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
60.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
61.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
62.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
63.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
64.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
65.

By replacing the element symbol, this could be a diagram of which element?

a)

Li

b)

Al

c)

C

d)

Be

66.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
67.

SO4

a)

Covalent

b)

Ionic

c)

Metallic

68.

O3

a)

Covalent

b)

Ionic

c)

Metallic

69.

Why is this Lewis Structure incorrect? Select all that appy.

a)

There should be a single bond between H and C.

b)

There should be a triple bond between C and N.

c)

Carbon has too many bonds around it.

d)

Hydrogen needs more electrons.

70.
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.
71.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
72.
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
73.

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

74.

Which of the following would react to form an ionic compound

a)

Copper & Zinc

b)

Boron and Carbon

c)

Fluorine and Lithium

d)

Carbon and Bromine

75.

The melting points of covalent molecules are:

a)

very high

b)

high

c)

medium

d)

low

76.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

77.

Which of the following is true about Covalent bonds? (select ALL true options)

a)

High melting point

b)

Low melting point

c)

Cannot conduct electricity

d)

Can conduct electricity

78.

Excellent conductors as solid and liquid due to a sea of delocalised electrons.

a)

simple covalent molecules

b)

metallic

c)

ionic

d)

giant covalent

79.

The particles responsible for chemical bonding are

a)

protons.

b)

cations.

c)

electrons.

d)

valence electrons.

80.

The melting points of covalent molecules are:

a)

very high

b)

high

c)

medium

d)

low

81.

Is this picture of the lewis dot stucture of Potassium Iodide correct?

a)

Yes

b)

No

82.

What is the correct formula for Calcium Oxide?

a)

CaO

b)

Ca2O

c)

CaO2

d)

CaO3

83.

Click on all the properties of Ionic Bonds.

a)

Brittle

b)

High Melting Point

c)

Hard

d)

Conducts electricity when dissolved in water

e)

Conducts electricity when melted (molten)

84.

Check all properties of covalent bonds.

a)

Low Melting Points

b)

Do not conduct electricity

c)

Generally softer

d)

Shares electrons

85.

Check all the properties of metallic bonding.

a)

Malleable

b)

Ductile

c)

Conducts electricity as a solid

d)

Shiny

e)

Good conductor of heat

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