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Ionic and Covalent Compounds Review

Total questions: 141

Worksheet time: 47mins

Name
Class
Date
1.

Which of these are oxides?

a)

Na₂O

b)

CaCl₂

c)

NaF

d)

MgO

e)

NO

2.

What charge does the magnesium ion (Mg) have after it forms an ionic bond with oxygen?

a)

Mg+

b)

Mg2+

c)

Mg3+

d)

Mg4+

3.

What charge does the oxygen ion (O) have after it forms an ionic bond with magnesium?

a)

O+

b)

O2+

c)

O2-

d)

O3-

4.

In the process of forming an ionic bond, magnesium donates two electrons to oxygen.

a)

True

b)

False

5.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
6.
In the process of ionic bonding, ions come together because
a)
opposite charges repel
b)
positive and negative ions attract
c)
salt is magnetic
d)
like charges attract each other
7.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
8.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
9.
Metals tend to 
a)
gain electrons
b)
lose electrons
10.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
11.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
12.
How do the following two elements bond together?
Pb4+  O2-       
a)
PbO
b)
Pb2O3
c)
PbO2
d)
Pb3O2
13.
If an ion has lost an electron and has more protons than electrons, what is its charge?
a)
Negative
b)
Positive
c)
Neutral
d)
This is impossible
14.
What is true about an ionic bond?
a)
the nonmetal transfers electrons to the metal
b)
the metal transfers electrons to the nonmetal
c)
no electrons are transferred
d)
both the nonmetal and metal transfer electrons to each other
15.
Which forms an ionic bond?
a)
When a metal and a nonmetal combine
b)
When 2 nonmetals react
c)
Gaining or losing an electron
d)
Gaining or losing a proton
16.
if METALS are more likely to LOSE electrons, they will form ...
a)
anions
b)
neutral atoms
c)
positive ions
d)
negative ions
17.

What compound is formed when Cr3+ bonds with O2- ?

a)

CrO

b)

Cr3O2

c)

Cr2O3

d)

CrO3

18.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
19.

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-

20.

In an ionic bond, the ions are held together because...

a)

the positive nucleus of each ion attracts the other ion's negatively charged electrons

b)

the ions have opposite charges

c)

as the electron moved from one atom to another it pulled the atom along with it

d)

electrons are being shared

21.

Aluminum forms a compound with a halogen (X). What will the formula of this ionic compound be?

a)

Al2X3Al_2X_3  

b)

Al3X2Al_3X_2  

c)

Al3XAl_3X  

d)

AlX3AlX_3  

22.

Oxygen will form an ionic compound with which of the following?

a)

Nitrogen

b)

Fluorine

c)

Boron

d)

Lithium

23.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
24.
Manganese II Oxide
a)
MnO
b)
Mn2O
c)
Mn2O4
d)
MnO2
25.

Which of the following Roman Numerals represents the charge on the copper in CuO?

a)
II
b)

III

c)

L

d)

I

26.

Name the ionic compound CuCl 2_2 .

a)

Copper chloride

b)

Copper (I) chloride

c)

Copper (II) chloride

d)

Cupric chloride

27.
Which of these is a characteristic of ionic compounds?
a)
They are gases at room temperature.
b)
They conduct an electric current when melted or dissolved.
c)
They have low melting points.
d)
They have the weakest bonds.
28.

Which is true of ionic compounds?

a)

They are electrically neutral when dissolved in a solution

b)

They are made by sharing electrons

c)

They are made of metals and nonmetals

d)

They are good conductors as solids

29.

In general, how many electrons does carbon have?

a)

2

b)

4

c)

6

d)

12

30.

Write the configuration for Phosphorus (P)

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

31.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
32.

Choose the Noble Gas that you would use to begin the shorthand configuration of the following element.

Plutonium (Pu)

a)

[Xe]

b)

[Ne]

c)

[Rn]

d)

[Kr]

33.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
34.
The electrons involved in the formation of a chemical bond are called
a)
dipoles
b)
s electrons
c)
Lewis electrons
d)
valence electrons
35.

What is this element?

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Lithium

36.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
37.

This is a Bohr Diagram of Aluminum. How many valence electrons does Aluminum have?

a)

3

b)

4

c)

5

38.

Where do you find electrons? Check all that apply.

a)

Nucleus

b)

Electrons cloud

c)

Outside the nucleus

39.

In general, how many electrons does carbon have?

a)

2

b)

4

c)

6

d)

12

40.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
41.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
42.

Choose the correct electron configuration for Chlorine (Cl).

a)

1s2 2s2 2p1

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 3p5

43.

Which noble gas is used in the shorthand electron configuration for Potassium (K)?

a)

Helium (He)

b)

Neon (Ne)

c)

Argon (Ar)

d)

Krypton (Kr)

44.

What is a key difference between ionic and covalent bonds?

a)

Ionic bonds occur only in organic compounds, while covalent bonds occur in inorganic compounds.

b)

Ionic bonds involve the sharing of electrons, while covalent bonds involve the transfer of electrons.

c)

Ionic bonds involve the transfer of electrons, while covalent bonds involve the sharing of electrons.

d)

Covalent bonds can only form between two metals, while ionic bonds can form between a metal and a nonmetal.

45.

Which of the following best describes the formation of an ionic bond?

a)

Two atoms share their valence electrons equally.

b)

An atom donates its valence electron to another atom, creating ions that attract each other.

c)

Two atoms exchange neutrons to achieve stability.

d)

Electrons are shared unequally between two atoms.

46.

Which of the following is a characteristic feature of substances with covalent bonds?

a)

High solubility in water.

b)

High electrical conductivity in solid form.

c)

Low boiling points.

d)

High melting points.

47.

What is the result of an atom achieving a full outer shell through ionic bonding?

a)

The atom becomes a stable molecule.

b)

The atom remains unchanged.

c)

The atom becomes an ion with a net charge.

d)

The atom becomes a covalent compound.

48.

Which of the following is a property of ionic compounds?

a)

Low melting and boiling points.

b)

Poor electrical conductivity in solid state.

c)

High melting and boiling points.

d)

Easily vaporized.

49.

Bonds between atoms in a molecule (covalent compound) form as a result of the sharing  of?

a)

formulas

b)

electrons

c)

atoms

d)

chemicals

50.

Name for NaH

a)

sodium hydrogen

b)

potassium hydride

c)

sodium hydride

d)

potassium hydrogen

51.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

52.

Formula for lead (II) chloride

a)

PbCl2

b)

Pb2Cl

c)

Pb2Cl3

d)

Pb3Cl2

53.

Name for PBr2

a)

phosphorus bromide

b)

phosphorus dibromide

c)

phosphorus dibromine

d)

phosphorus bromine

54.

Formula for Disilicon Heptasulfide

a)

SiS6

b)

SiS7

c)

Si2S6

d)

Si2S7

55.

Formula for iron (II) carbonate

a)

FeCO3

b)

Fe2CO3

c)

FeCO2

d)

Fe2CO2

56.

Formula for Cobalt (II) bromide

a)

CoBr

b)

Co2Br2

c)

Co2Br

d)

CoBr2

57.

Name the ionic compound, CaCO3

a)

calcium carbide

b)

calcium carbon trioxide

c)

calcium carbon oxide

d)

calcium carbonate

58.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
59.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
60.
What is the formula for Copper II Sulfide?
a)
CuS
b)
Cu₂S
c)
CuS₂
d)
CuSO₃
61.
How do the following two elements bond together?
Pb4+  O2-       
a)
PbO
b)
Pb4O2
c)
PbO2
d)
Pb2O4
62.

What is the name for As4O10?

a)

arsenic oxide

b)

arsenide decoxide

c)

tetraarsenic decoxide

d)

arsenic decoxide

63.

Hexaboron monosilicide

a)

B5S

b)

B6S

c)

B6Si

d)

Br6Si1

e)

Br6Si

64.

Antimony tribromide

a)

AnBr3

b)

AtBr3

c)

Sb1Br3

d)

SbBr3

65.

P4S5

a)

phosphorus sulfide

b)

quadphosphorus hexasulfide

c)

tetraphosphorus pentasulfur

d)

tetraphosphorus pentasulfide

66.

SeF6

a)

silicon fluoride

b)

selenium fluoride

c)

selenium hexafluoride

d)

selenium heptafluoride

67.

Si2Br6

a)

silicon bromide

b)

disilicide bromide

c)

disilicon hexabromide

d)

disilicide hexabromide

68.

NF3

a)

mononitrogen trifluorine

b)

mononitrogen trifluoride

c)

nitrogen trifluoride

d)

ammonia

69.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

70.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

71.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

72.

What is the name of this molecule's shape?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

73.

What is the name of this molecular shape?

a)

trigonal pyramid

b)

tetrahedral

c)

bent

d)

trigonal planar

74.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
75.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
76.
A roman numeral represent the charge for the ___________ in a chemical formula.
a)
cation
b)
anion
c)
ion
d)
atom
77.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
78.

Binary Naming

What is the name of CaCl2?

a)

calcium, chlorine

b)

calcium chloride

c)

calcide chlorine

d)

calcium dichloride

79.

Name the compound using appropriate rules: FeCl3

a)

Chloride Iron

b)

Iron III Chloride

c)

Chloride III Iron

d)

I have no clue

80.

What type of compound is cobalt (II) sulfate? Check all that apply.

a)

Ionic compounds

b)

Covalent compounds

c)

Transition Metals

d)

Acids

e)

Polyatomic compounds

81.

What is the formula for phosphorous acid?

a)

H3PO4

b)

H2PO4

c)

H3P

d)

H3PO3

82.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
83.

carbonic acid

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

84.

H3PO4

a)

hydrophsophorus acid

b)

phosphoric acid

c)

hydrogen phosphorous

d)

phosphori hydroxide

85.

Binary acids start with the prefix "____________"

a)

acid

b)

nitric

c)

hydraulic

d)

hydro

86.

When naming binary acids, the ending always changes to:

a)

-ate

b)

-ite

c)

-ic

d)

-ous

87.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

88.

Name this acid: HNO2

a)

hydronitrous acid

b)

hydrogen nitrogen oxygen

c)

nitrous acid

d)

hyponitrous acid

89.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
90.
chlorous acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
91.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
92.
Select the formula for the following acid: chloric acid
a)
HClO3
b)
HCl
c)
HClO4
93.
A _________ describes a chemical reaction
a)
chemical equation
b)
chemical symbol
c)
chemical formula
d)
product
94.

3KOH + H3PO4 --> K3PO4 + 3H2O

a)

Combustion

b)

Double Displacement

c)

Single displacement

d)

Neutralization

95.
In a chemical equation, the symbol that means dissolved in water is ____.
a)
(aq)
b)
(dw)
c)
(l)
d)
(s)
96.

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

97.

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.

98.

Indicate the correct diatomic molecule

a)

H2

b)

N2

c)

C2

d)

Br2

99.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

100.

Ionic compounds can conduct electricity

a)

always

b)

as long as they are dissolved in water

c)

as long as they are molten (melted)

d)

never

101.

A repeating pattern of alternating positive and negative charged ions is called a(n)

a)

crystal lattice

b)

crystal ladder

c)

table salt

d)

diamond

102.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

103.

Is the following compound ionic or covalent?

A material that has a low boiling point

a)

Ionic

b)

Covalent

104.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
105.
When dissolved in water, the solution does NOT conduct electricity.
a)
ionic compounds
b)
covalent compounds
106.
usually soft
a)
ionic compounds
b)
covalent compounds
107.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
108.

Metallic bonds are characterized by:

a)

The transfer of electrons from metal atoms to non-metal atoms.

b)

The sharing of electron pairs between non-metal atoms.

c)

A sea of delocalized electrons surrounding positively charged metal ions.

d)

The formation of hydrogen bonds between metal atoms.

109.

Which model describes metals as being composed of a collection of atoms that contribute their valence electrons to form a sea of electrons around them?

a)

A) Bohr model

b)

B) Electron cloud model

c)

C) Electron sea model

d)

D) Orbital model

110.

How can metals be modeled according to their atomic structure in metallic bonds?

a)

As isolated neutral atoms

b)

As anions surrounded by a sea of protons

c)

As cations surrounded by a sea of freely moving valence electrons

d)

As covalently bonded clusters

111.
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.
112.

Which of the following substances is an example of a material with metallic bonding?

a)

Water (H 2_2 O)

b)

Sodium chloride (NaCl)

c)

Copper (Cu)

d)

Methane (CH 4_4 )

113.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

114.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

115.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
116.
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.
117.

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

a)

nonpolar

b)

polar

c)

ionic

d)

metallic

118.
Is this image an example of covalent bonding?
a)
Yes
b)
No
119.
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
120.

How many PAIRS of electrons are shared in a triple bond?

(a)  

121.

How many PAIRS of electrons are shared in a double bond?

(a)  

122.

How many covalent bonds are created in a single water molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

123.

Chlorine is a diatomic element which means in nature, it is found in two's. (Cl2) Chlorine shares one pair of electrons to make sure each atom complete the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

124.
Which formula represents a substance that contains covalent bonds?
a)
LiCl
b)
CaCl2
c)
K2O
d)
CO2
125.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

126.

Molecules:

a)

have covalent bonds and are always polar

b)

have covalent bonds and are always non-polar

c)

have covalent bonds and can be polar or non-polar

d)

have ionic bonds and are always polar

127.

Which types of elements become cations?

a)

non-metals

b)

metals

c)

metalloids

128.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

129.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

130.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

131.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
132.

Is the following compound ionic or covalent?

A material with a high melting point

a)

Ionic

b)

Covalent

133.

Is the following compound ionic or covalent?

A material that is hard and brittle

a)

Ionic

b)

Covalent

134.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

135.
The reason that a sodium atom bonds with a chlorine atom is because
a)
Sodium transfers an electron to Chlorine
b)
oppositely charged ions form a strong electrostatic attraction
c)
ions are the same size
d)
the ions have a full outer shell
136.

Is the following a property of ionic or covalent compounds?

form molecules

a)

ionic

b)

covalent

137.
When electrons are shared unequally a/an ___________ bond is formed 
a)
ionic 
b)
hydrogen
c)
polar covalent 
138.

A small amount of NaCl is dissolved in water to make a solution. In this solution

a)

water is the precipitate

b)

water is the solute

c)

NaCl is the solvent

d)

NaCl is the solute

139.
A solution is a kind of ________. 
a)
mixture 
b)
compound 
c)
element 
d)
stuff 
140.
An example of a nonelectrolyte is
a)
sugar water
b)
salt water
c)
sodium chloride
d)
hydrogen chloride
141.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.

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Worksheet

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11th Grade