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Bonding Review

Total questions: 159

Worksheet time: 3hrs 38mins

Name
Class
Date
1.

Sea of electrons

a)

Metallic Bonding

b)

Ionic Bonding

c)

Covalent Bonding

2.

valence electrons exist as a "sea of electrons" around positive ions pulling ions close together

a)

Metallic bond

b)

Ionic bond

c)

Covalent Bond

3.

Shares electrons in order to fill an energy level

a)

Metallic bond

b)

Ionic bond

c)

Covalent Bond

4.

Attraction of oppositely charged ions

a)

metallic

b)

covalent

c)

Ionic

5.

Generally occurs between metal and nonmetal

a)

Metallic

b)

Ionic

c)

Covalent

6.

Molecules

a)

Metallic Bond

b)

Ionic Bond

c)

Covalent Bond

7.

Completes the octet

a)

Metallic bond

b)

Ionic bond only

c)

Covalent bond only

d)

Ionic and Covalent bonds

8.

Electrons are shared equally

a)

ionic bond

b)

Polar covalent bond

c)

Nonpolar covalent bond

9.

Electrons are shared unequally

a)

ionic bond

b)

Polar covalent bond

c)

Nonpolar covalent bond

10.

Water

a)

Metal

b)

Ionic compound

c)

Polar molecule

d)

Nonpolar molecule

11.

molecules with partial charges

a)

Ionic compound

b)

Polar molecule

c)

Nonpolar molecule

12.

molecules with NO partial charges

a)

Metal

b)

Ionic compound

c)

Polar molecule

d)

Nonpolar molecule

13.

molecules that are attracted to each other because of partial charges

a)

Ionic compound

b)

Polar molecule

c)

Nonpolar molecule

14.

Forms large crystals with an ordered arrangement of oppositely charged ions

a)

Metallic

b)

Ionic

c)

Covalent

15.

Ion that has more protons than electrons

a)

Positive ion

b)

Negative ion

16.

Ion that has more electrons than protons

a)

Positive ion

b)

Negative ion

17.

Conducts electricity

a)

Metallic

b)

Ionic

c)

Covalent

18.

Any state at room temperature Low melting point

a)

metals

b)

ionic compounds

c)

molecular compounds (covalent bonds)

19.

Malleable

a)

metallic

b)

ionic

c)

covalent

20.

crystal structure

a)

metals

b)

ionic compounds

c)

molecular compounds (covalent bonds)

21.

Luster (shiny)

a)

metals

b)

ionic compounds

c)

molecular compounds (covalent bonds)

22.

Occurs between metal atoms.

a)

Metallic Bonding

b)

Ionic Bonding

c)

Covalent Bonding

23.

high melting point

a)

ionic compounds

b)

molecular compounds (covalent bonds)

24.

conduct electricity when dissolved in water

a)

ionic compounds

b)

molecular compounds (covalent bonds)

c)

metals

25.

Poor conductors of electricity even when dissolved in water

a)

metals

b)

ionic compounds

c)

molecular compounds (covalent bonds)

26.

Which of the following compounds is formed by ionic bonding?

a)

C₂H₆

b)

CO₂

c)

Na₂O

d)

F₂

27.

Which statement correctly describes what happens to Li and Cl atoms when they bond?

a)

Li loses 1 valence electron and becomes a negative ion, Cl gains 1 valence electron and becomes a positive ion.

b)

Li loses 1 valence electron and becomes a positive ion, Cl gains 1 valence electron and becomes a negative ion.

c)

Li gains 1 valence electron and becomes a negative ion, Cl loses 1 valence electron and becomes a positive ion.

d)

Li gains 1 valence electron and becomes a positive ion, Cl loses 1 valence electron and becomes a negative ion.

28.

When lithium and oxygen bond together

a)

Li forms a positive ion, O forms a negative ion.

b)

Li forms a negative ion, O forms a positive ion.

c)

Li and O share electrons.

d)

Li forms an anion, and O forms a cation.

29.

Which atom will form an anion when forming an ionic bond?

a)

Sr

b)

Li

c)

Ca

d)

O

30.

When an atom of hydrogen and an atom of fluorine bond together

a)

the H will be partially positive, because it has a higher electronegativity than F.

b)

the H will be partially negative, because it has a higher electronegativity than F.

c)

the F will be partially positive, because it has a higher electronegativity than H.

d)

the F will be partially negative, because it has a higher electronegativity than H.

31.

Which of the following molecules has the most polar bond between the bonded atoms, in term of greatest END?

a)

HF

b)

HCl

c)

HBr

d)

HI

32.

Which of the following compounds is formed by covalent bonding?

a)

Na2S

b)

AlCl3

c)

CH4

d)

LiCl

33.

Which of the following molecules contains a nonpolar covalent bond?

a)

H2O

b)

HF

c)

F2

d)

NH3

34.

Which of the following molecules contains a polar covalent bond?

a)

H2

b)

PH3

c)

F2

d)

NH3

35.

Using electronegativity differences, predict the type of bond present between the following: a. sodium and fluorine b. chlorine and hydrogen c. carbon and sulfur d. carbon and fluorine e. phosphorus and oxygen f. hydrogen and fluorine g. copper and sulfur h. iodine and bromine

a)

The question asks to predict the type of bond (ionic, covalent, or polar covalent) based on electronegativity differences for pairs of elements.

b)

The question asks to predict the type of bond (metallic, ionic, or covalent) based on electronegativity differences for pairs of elements.

c)

The question asks to predict the type of bond (hydrogen, ionic, or covalent) based on electronegativity differences for pairs of elements.

d)

The question asks to predict the type of bond (van der Waals, ionic, or covalent) based on electronegativity differences for pairs of elements.

36.

Identify the following bonds as polar covalent or nonpolar covalent—giving the END. For polar covalent bonds, label the δ+ and δ- ends of the molecule.

a)

H—H

1.

nonpolar covalent

b)

H—C

2.

polar covalent

c)

H—Cl

3.

polar covalent

d)

P—Cl

4.

polar covalent

e)

Cl—Cl

5.

nonpolar covalent

37.

Match the following to form true statements:

a)

When solid, ionic compounds

1.

cannot conduct electricity

b)

When melted ionic compounds

2.

can conduct electricity

c)

Ionic compounds have

3.

high melting and high boiling points

d)

There are many strong bonds

4.

between ions in an ionic compound.

e)

Elements in group 1 of the periodic table form ions

5.

with a charge of 1+

38.

Calculate ΔEN for Pb-S

a)

1.1

b)

-0.6

c)

0.6

d)

4.4

39.

Calculate ΔEN for Pb-S

a)

1.1

b)

-0.6

c)

0.6

d)

4.4

40.

Match the following

a)

valence electron

1.

energy level of an electron

b)

covalent

2.

sharing of electron pairs

c)

ionic

3.

transfer of electrons

d)

reactivity

4.

ability to undergo chemical reactions

e)

oxidation state

5.

charge of an atom

41.
A chemical bond resulting from electrostatic attraction between positive and negative ions is a(n)
a)
nonpolar covalent
b)
ionic
c)
polar covalent
d)
coordinate covalent
42.
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
43.

What is a covalent bond?

a)

A bond between atoms where electrons are shared.

b)

A bond between atoms where one atom gains an electron and another loses an electron.

c)

A bond where electrons dance in a 123 pattern.

d)

A bond between two atoms where they send each other special BFF messages.

44.

What part of the atom makes a bond?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Any subatomic particle

45.

8. Predict what type of bond would form between Mg and Cl.

a)

Ionic

b)

Covalent

c)

Metallic

d)

Polar Covalent

46.

13. How many valence electrons do elements in the group 14 contain?

a)

3

b)

4

c)

13

d)

14

47.

10. If an atom loses two electrons what charge will it have?

a)

+2

b)

-2

c)

+1

d)

-1

48.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
49.

MgCl2, this compound has ...

a)

ionic bond

b)

covalent bond

50.

CH4, this compound has ...

a)

ionic bond

b)

covalent bond

51.

What type of bond would form between Li and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

52.

Valence electrons are found

a)

in the innermost energy level of an atom

b)

in the middle energy levels of an atom

c)

in the outermost energy levels of an atom

53.
Which of the following is an ionic bond?
a)
H3N
b)
CaCl2
c)
NO2
d)
SCl
54.

Cl2

a)

Ionic Bond

b)

Covalent Bond

55.

NaO

a)

Ionic Bond

b)

Covalent Bond

56.

NH3

a)

Ionic Bond

b)

Covalent Bond

57.

The electrons in a POLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

58.

The electrons in a NONPOLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

59.

Electronegativity is...

a)

The ability for an atom to ATTRACT electrons

b)

the ability of an atom to LOSE electrons

c)

the energy required to remove an electron from an atom

d)

how easy it is to make friends.

60.

Which element is MORE electronegative?

a)

O

b)

Be

61.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

62.
Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 
a)
Fluorine has less energy levels.
b)
Chlorine has more electrons in its outer shell
c)
Fluorine has more protons.
d)
None of these
63.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
64.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

65.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

66.

What are the intermolecular attractions that form ionic compounds?

a)

Covalent bonds

b)

Hydrogen bonds

c)

Ionic bonds

d)

Van der Waals forces

67.

What are the intermolecular attractions that occur amongst molecules?

a)

Covalent bonds

b)

Ionic bonds

c)

Hydrogen bonds

d)

Metallic bonds

68.

What does the prefix 'Inter' mean?

a)

A) Within

b)

B) Between

c)

C) Inside

d)

D) Outside

69.

Fill in the blank: Forces between different substances are called ________ forces.

a)

intermolecular

b)

intramolecular

c)

gravitational

d)

nuclear

70.

What is the measure of the ability of an atom in a bond to attract electrons called?

a)

Ionization Energy

b)

Electronegativity

c)

Atomic Radius

d)

Electron Affinity

71.

The properties of a compound are very different from the properties of the elements that make up the compound.

a)

True

b)

False

72.

When a chemical reaction occurs, what happens with the valence electrons?

a)

They are destroyed

b)

They are transferred or shared

c)

They remain unchanged

d)

They disappear

73.

Fill in the blank: The chemical formula NaCl consists of 1 atom of sodium and 1 atom of ____.

a)

chlorine

b)

oxygen

c)

hydrogen

d)

nitrogen

74.

What is the chemical formula for ammonia?

a)

NH3

b)

H2O

c)

CO2

d)

O2

75.

What is the chemical formula for aluminum sulfate?

a)

A) Al2(SO4)3

b)

B) Al2O3

c)

C) Al(SO4)2

d)

D) AlSO4

76.

According to the Octet Rule, atoms will gain, lose, or share electrons in order to have how many electrons in their outer energy shell?

a)

6

b)

7

c)

8

d)

9

77.

What is the valence electron count of Sodium (Na) in the formation of NaCl?

a)

1

b)

2

c)

7

d)

8

78.

What happens to Sodium (Na) when it loses 1 valence electron in the formation of NaCl?

a)

It becomes unstable

b)

Its outermost energy level becomes full and it becomes stable

c)

It gains another electron

d)

It forms a covalent bond

79.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
80.

What are intramolecular forces

a)

Forces within a molecule

b)

Forces between two or more molecules

c)

Forces of the opposition

d)

Forces of your allies

81.

What is a compound?

a)

Two or more atoms of the same element combined

b)

Two or more elements physically combined

c)

Two or more elements chemically combined

d)

Two or more cheeses on a sandwich

82.

All compounds are molecules, but not all molecules are compounds

a)

True

b)

False

83.

A chemical formula tells us>>>>>

a)

in what order atoms are joined together

b)

absolutely nothing

c)

the way to bake a cake

d)

what elements and how many of each are in a unit of compound

84.

Elements form compounds to be ___________

a)

unstable

b)

ordinary

c)

stable

d)

different

85.

To be stable, an atom follows the ________ in order to have ____ electrons in their outer energy shell

a)

octet, 6

b)

octet, 8

c)

duplo, 2

d)

duplo 8

86.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
87.

When forming a covalent bond, a non-metal atom:

a)
Gains electrons to form a cation
b)
Loses electrons to form a cation
c)
Gains electrons to form an anion
d)
Loses electrons to form an anion
88.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
89.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
90.
An ionic bond forms when 
a)
Valence electrons are shared
b)
a sea of mobile electrons surround the cations
c)
valence electrons are transferred between atoms
d)
none of the above
91.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
92.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
93.
A chemical bond between oppositely charged ions.
a)
compound
b)
ion
c)
covalent bond
d)
ionic bond
94.
A chemical bond formed between shared atoms.
a)
chemical bond
b)
covalent bond
c)
oxidation #
d)
ionic bond
95.
Substance made from two or more combined atoms. 
a)
ion
b)
covalent bond
c)
ionic bond
d)
compound
96.
Force that holds together atoms in a substance.
a)
compound
b)
ion
c)
chemical bond
d)
ionic bond
97.

What type of energy is stored in a bond?

a)

potential energy

b)

kinetic energy

c)

thermal energy

98.

Why do atoms bond?

a)

to become more stable

b)

to get 8 valence electrons

c)

to gain more neurons

d)

to gain more protons

99.

when a bond is formed?

a)

energy is released

b)

energy is absorbed

c)

exothermic

d)

stability increases

100.

When a bond is BROKEN

a)

energy is absorbed

b)

energy is released

c)

endothermic

d)

stability decreases

101.

Why is there a transfer of electrons in ionic compounds?

a)

because the electronegativity difference is greater than 1.7

b)

because the electronegativity difference is greater than 1.0

c)

because the electronegativity difference is between 0.0 - 0.4

d)

because the electronegativity difference is between 0.5 - 1.7

102.

H2

a)

ionic

b)

covalent

103.

CH4

a)

ionic

b)

covalent

104.

CaCl2

a)

ionic

b)

covalent

105.

What type of energy is stored in a bond?

a)

chemical

b)

potential

c)

kinetic

d)

thermal

106.

C2O5

a)

Covalent

b)

Ionic

107.

CCl4

a)

Covalent

b)

Ionic

108.

PI3

a)

Covalent

b)

Ionic

109.

PI5

a)

Covalent

b)

Ionic

110.

S2Cl2

a)

Covalent

b)

Ionic

111.

S2F10

a)

Covalent

b)

Ionic

112.

CO

a)

Covalent

b)

Ionic

113.

F10O9

a)

Covalent

b)

Ionic

114.

FN

a)

Covalent

b)

Ionic

115.

I2Cl

a)

Covalent

b)

Ionic

116.

NaBr

a)

Covalent

b)

Ionic

117.

MgCl2

a)

Covalent

b)

Ionic

118.

K2Te

a)

Covalent

b)

Ionic

119.

Na3N

a)

Covalent

b)

Ionic

120.

Li2S

a)

Covalent

b)

Ionic

121.

MnS2

a)

Covalent

b)

Ionic

122.

Mg3P2

a)

Covalent

b)

Ionic

123.

CaCN

a)

Covalent

b)

Ionic

124.

RbOH

a)

Covalent

b)

Ionic

125.

AlPO4

a)

Covalent

b)

Ionic

126.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

127.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

128.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

129.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

130.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

131.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

132.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

133.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

134.

Which of these is incorrect?

a)
b)
135.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

136.
How many valence electrons does chlorine (Cl) have?
a)
2
b)
5
c)
6
d)
7
137.
How many valence electrons does carbon (C) have?
a)
3
b)
4
c)
5
d)
6
138.
Which of these elements has 8 valence electrons?
a)
P
b)
Be
c)
O
d)
Ar
139.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
140.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
141.
Which type of bonding leads to brittle substances?
a)
Metallic
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
142.
A mystery substance has a low melting point, does not dissolve in water, does not conduct electricity, and is made of nonmetals. This substance is soft. Which type of substance is it most likely to be?
a)
Metal
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
143.
A mystery substance has a high melting point, dissolves in water, does not conduct electricity when it is solid, and is made of metals and nonmetals. Which type of substance is it most likely to be?
a)
Metal
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
144.

a substance in an excellent conductor of electricity in a solution. The chemical bonds in this substance are most likely?

a)

ionic, because the valence electrons are mobile

b)

ionic, because the valence electrons are stationary

c)

covalent, because the valence electrons are stationary

d)

metallic, because the valence electrons are stationary

145.
Why do ionic bonds form?
a)
so the number of protons equals the number of electrons
b)
to fill the outermost energy level
c)
so an atom can become unstable
146.
An electron has what kind of charge?
a)
no charge
b)
positive 
c)
negative
d)
it depends
147.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
148.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
149.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
150.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
151.
The attraction between oppositely charged ions is called a(n) _______________.
a)
ionic bond
b)
polyatomic ion
152.
What is the charge on a noble gas & why?
a)
0; they don't exchange electrons
b)
+1; they give away an electron
c)
-1; they gain an electron
d)
1; they form only single bonds
153.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
154.
What type of elements will form an ionic bond?
a)
Metals + Metals
b)
Nonmetals + Nonmetals
c)
Metals + Nonmetals
d)
None of the above
155.
To form a charge of +2 an atom must _ electrons.  To form -3 it must _ electrons.
a)
Gain 2; Lose 3
b)
Gain 3; Lose 2
c)
Lose 2; Gain 3
d)
Lose 3; Gain 2
156.
What is the name given to the outermost electron(s)?
a)
outside electrons
b)
plutonian electrons
c)
ionic electrons
d)
valance electrons
157.
Ionic bonds form because
a)
Two ions of the same charge are attracted to each other
b)
Two ions of different charges are attracted to each other
c)
Two atoms share their electrons
d)
Two or more atoms share protons
158.
An ionic bond may or may not include a metal.
a)
True
b)
False
159.
An ionic bond involves two elements...
a)
Transferring electrons
b)
Sharing electrons

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160 questions

Y9 Bio & Chem

quiz

Worksheet

•

9th Grade

anh lớp 1

164 questions

anh lớp 1

quiz

Worksheet

•

10th Grade

Earth Science Spring 2025 Final Question Pool

160 questions

Earth Science Spring 2025 Final Question Pool

quiz

Worksheet

•

9th - 12th Grade

Chemistry C4-Revision

162 questions

Chemistry C4-Revision

quiz

Worksheet

•

9th Grade

Biology Topic 1

155 questions

Biology Topic 1

quiz

Worksheet

•

9th Grade

Enviro A Final Exam Review

158 questions

Enviro A Final Exam Review

quiz

Worksheet

•

7th - 12th Grade