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G11 Q2 Final exam revision 2026

Total questions: 131

Worksheet time: 3hrs 17mins

Name
Class
Date
1.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
2.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
3.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
4.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
5.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
6.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
silver + oxygen
7.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
8.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
9.
What is the formula for calcium carbonate?
a)
CaCO
b)
CaCO2
c)
CaCO3
d)
Ca3CO3
10.
Name this compound: 
NH4F
a)
Ammonia fluoride
b)
Ammonium fluorite
c)
Ammonia fluorate
d)
Ammonium fluoride
11.
The name for CrN:
a)
Chromium nitride
b)
Chromium (I) nitride
c)
Chromium (III) nitride
d)
Chromium nitride (III)
12.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
13.
Which is the Roman Numeral for +3?
a)
I
b)
II
c)
III
d)
+III
14.
What oxidation number is Roman Numeral (IV)?
a)
5
b)
4
c)
1
d)
3
15.
The oxidation number for copper in Cu2S:
a)
+1
b)
+2
c)
-1
d)
-2
16.
The oxidation number for Fe in Fe2O3:
a)
+2
b)
+3
c)
+1
d)
-2
17.
What do Roman Numerals represent in the name of a transition metal compound?
a)
how many atoms of the metal there are
b)
the oxidation number of the nonmetal
c)
the oxidation number of the metal
d)
the mass number
18.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
19.

K + and N-3 form...

a)

KN

b)

KN3

c)

K3N3

d)

K3N

20.
What are the electrons in the highest energy level of an atom called?
a)
orbital electrons
b)
valence electrons
c)
anions
d)
cations
21.

A phosphorus atom needs to gain ___ electrons to achieve a full octet. [P=15]

a)
3
b)
4
c)
6
d)
5
22.

What is the formula for aluminum phosphide?

a)

AlP

b)

AlP3

c)

Al3P3

d)

Al3P2

23.
What is the correct name for MgI₂?
a)
Manganese IV iodide
b)
Manganese diiodide
c)
Magnesium iodide
d)
Magnesium diiodide
24.

What group of elements do not take a charge because they are stable and do not want to gain or lose electrons?

a)

Transition Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

25.

Rb+1 S-2 --> These ions would have what formula?

a)

Rb1S2

b)

Rb2S

c)

Rb2S1

d)

Rb2S4

26.

Ionic bonds require which of the following? select what is needed.

a)

metal

b)

nonmetal

c)

noble gas

d)

transition metal

27.

Which of the following is an example of an IONIC COMPOUND?

a)

NaCl

b)

H2O

c)

CO2

d)

NO

28.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
29.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
30.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
31.
The prefix for 4 is?
a)
quatro
b)
tetra
c)
quarto
d)
tri
32.

SiCl6

a)

Monosilicon hexachloride

b)

Silicon hexachloride

c)

Silicon heptachloride

d)

Monosilicon heptachloride

33.

P3N5

a)

phosphorus pentanitride

b)

triphosphorus pentanitrogen

c)

triphosphide pentanitrogen

d)

triphosphorus pentanitride

e)

phosphorus nitride

34.

pentacarbon decahydride

a)

CH

b)

C5H10

c)

CH10

d)

C6H10

35.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
36.
What is the formula for Hexaboron Monosilicide
a)
B6Si
b)
BSi
c)
BSi6
d)
B6Si6
37.

Mark any statement(s) that are false

a)

Covalent bond is formed when atoms share electrons.

b)

Covalent bond is formed when the atoms gain or lose electrons.

c)

Covalent bond is formed when the atoms unequally share electrons.

d)

Covalent bond is formed when 2 electron pairs are shared.

38.

Water which is polar likes to dissolve:

a)

ionic compounds

b)

polar molecules

c)

nonpolar molecules

d)

metallic compounds

39.

What kind of bonds are shown here?

a)

Covalent

b)

Ionic

40.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
41.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

42.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
43.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
44.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
45.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
46.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
47.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
48.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
49.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
50.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

51.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
52.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
53.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
54.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

55.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
56.

What is the bond angle for the CH4 molecule?

a)

120°

b)

107°

c)

109.5°

d)

90°

57.
How many lone pairs are in this molecule's structure?
a)
6
b)
2
c)
0
d)
4
58.

Which one of the following is the correct bond angle between atoms adopting a trigonal planar geometry?

a)

180°

b)

109.5°

c)

90°

d)

120°

59.

The atoms in a molecule of water adopt what kind of geometry?

a)

Linear

b)

Tetrahedral

c)

Bent

d)

Trigonal planar

60.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

61.

How many bonding pairs and lone pairs of electrons are present in a molecule with trigonal planar molecular geometry?

a)

1 bonding pair and 2 lone pairs

b)

3 bonding pairs and 0 lone pairs

c)

4 bonding pairs and 1 lone pair

d)

2 bonding pairs and 1 lone pair

62.

What is the molecular geometry of a molecule with three bonding pairs and one lone pair of electrons?

a)

Tetrahedral

b)

Linear

c)

Trigonal pyramidal

d)

Octahedral

63.

How many bonding pairs and lone pairs of electrons are present in a molecule with tetrahedral molecular geometry?

a)

2 bonding pairs and 2 lone pairs

b)

3 bonding pairs and 1 lone pair

c)

5 bonding pairs and 0 lone pairs

d)

4 bonding pairs and 0 lone pairs

64.

CH4 is

a)

polar

b)

non-polar

65.

NH3 is

a)

polar

b)

non-polar

66.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

67.

Which of these atoms is the most electronegative?

a)

Bromine

b)

Fluorine

c)

Hydrogen

d)

Potassium

68.

Electronegativity refers to an atom's ability to _____________ shared electrons in a covalent bond.

a)

attract

b)

donate

69.

H2O is

a)

polar 

b)

non-polar

70.

More electronegative atoms in covalent compounds are likely to have:

a)

Partial positive charge

b)

Partial negative charge

71.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

72.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

73.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

74.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

75.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

76.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

77.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

78.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

79.

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

80.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
81.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
82.

Polar and nonpolar are two types of the ... bond

a)

Ionic

b)

Covalent

83.

CH4 is a nonpolar molecule because ...

a)

It is NOT symmetrical

b)

It is symmetrical

c)

It has polar bond between its atoms

d)

It dissolves in water

84.

F2

a)

Polar 

b)

Nonpolar 

85.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

86.

Molecules that contain whole number charges on atoms (+1,-3, etc.) must be...

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

d)

Polar Covalent or Ionic

87.

Hydrogen bonds are attraction forces between hydrogen atom, H bonded with high electronegativity atom such as ...in other molecules

a)

Fluorine

b)

Oxygen

c)

Sodium

d)

Nitrogen

88.

Which label shows hydrogen bond in between water molecule?

a)

X

b)

Y

c)

Z

89.

Bond Y is called...

a)

Hydrogen bond

b)

Dative bond

c)

Covalent bond

d)

Ionic bonf

90.

Oxygen atom with label X has

a)

High electronegativity

b)

High electropositivity

91.

Polar molecules

a)

have even charge density

b)

are symmetric

c)

form hydrogen bonds

d)

have 10 atoms per molecule

92.

How many hydrogen bonds can a water molecule form?

a)

One

b)

Two

c)

Three

d)

Four

93.

What is the basis of hydrogen bond?

a)

Attraction forces between hydrogen atom bonded with another hydrogen atom

b)

Attraction forces between hydrogen atom bonded with a high electronegativity atom (F, O, N)

c)

Attraction forces between hydrogen atom bonded with a high electronegativity atom (F, O, N) with atom (F, O, N) of another molecule

d)

Attraction forces between hydrogen atom with another hydrogen atom of another molecule

94.

Which type of physical bond is formed in Aluminum wire?

a)

Metallic

b)

Ionic

c)

Covalent

d)

Dative

95.

Molar mass of NaOH is ______________________ [Na= 23, O=16, H=1] g/mol.

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

96.

The elements present in sodium hydroxide are

a)

sodium oxygen and hydrogen

b)

sodium , oxygen and chlorine

c)

sodium, oxygen and boron

d)

sodium, oxygen and carbon

97.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
98.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
99.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
100.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

101.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

102.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
103.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
104.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
105.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
106.

If there is the maximum amount of solute in a solution, it is said to be

a)

saturated

b)

unsaturated

c)

supersaturated

d)

concentrated

107.
If there is more than the maximum amount of solute particles in a solution, it is said to be
a)
saturated
b)
unsaturated
c)
supersaturated
d)
concentrated
108.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Mixture
d)
Homogeneous solution
109.
Which of the following kind of compounds would be expected to NOT dissolve in water?
a)
Polar covalent solid
b)
Ionic solid
c)
Purely covalent solid (nonpolar)
110.
Because of their charges, ionic substances are most likely to dissolve into what kind of solvents?
a)
Polar covalent solvent
b)
Nonpolar covalent solvent
111.
Solid solutes are _______ soluble in a solvent when the solvent's temperature increases.
a)
more
b)
less
c)
just as
112.
Gaseous solutes are  _______ soluble in a solvent when the solvent's temperature increases.
a)
more
b)
less
c)
just as (no change)
113.
Increasing pressure makes gases _______ soluble in a solvent.
a)
more
b)
less
c)
just as (no change)
114.
Increasing pressure makes liquids and solids _______ soluble in a solvent.
a)
more
b)
less
c)
just as (no change)
115.

Dissociation and Ionization are parts of the _________

a)

Mixture Process

b)

Suspension Process

c)

Solution Process

d)

Emulsion Process

116.

the maximum amount of solute that will dissolve in a given amount of solvent at a given temperature

a)

Soluble

b)

Insoluble

c)

Solubility

117.

temperature and pressure affect _______

a)

rate of mixing

b)

rate of suspension

c)

rate of solution

d)

rate of solubility

118.

The least soluble substance at 10 degrees Celcius is

a)

KClO3KClO_3  

b)

Ce2(SO4)3Ce_2\left(SO_4\right)_3  

c)

K2Cr2O7K_2Cr_2O_7  

d)

NaClNaCl  

119.

Which substance is MOST soluble at 0 ºC?

a)

KI

b)

NaNO3

c)

NaCl

d)

Ce2(SO4)3

120.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

121.

H2OH_2O  has a difference in electronegativity of 1.4. Based on the table, what kind of bond is 

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

122.

In the following lewis structure, how many lone pairs of electrons are around the central atom?

a)

0 lone pairs of electrons

b)

1 lone pair of electrons

c)

3 lone pairs of electrons

d)

4 lone pairs of electrons

123.

In the following lewis structure, how many lone pairs of electrons are around the central atom?

a)

0 lone pairs of electrons

b)

1 lone pair of electrons

c)

2 lone pairs of electrons

d)

4 lone pairs of electrons

124.

In the following lewis structure, how many lone pairs of electrons are around the central atom?

a)

0 lone pairs of electrons

b)

1 lone pair of electrons

c)

3 lone pairs of electrons

d)

4 lone pairs of electrons

125.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
126.
How many pi bonds does this have? 
a)
1
b)
2
c)
3
d)
4
127.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
128.
How many sigma and pi bonds does this have?
a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
129.

Which of the following molecules is the least polar? [Calculate the electronegativity difference]

a)

H − N

b)

H − Si

c)

H − O

d)

H − C

130.

Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

131.

How many sigma and pi bonds are found in the following molecule?

H—C— — —C—CH2—CH2—CH— —CH2

a)

There are 3 pi bonds and 13 sigma bonds.

b)

There are 12 sigma bonds and 5 pi bonds.

c)

There are 12 sigma bonds and 2 pi bonds.

d)

There are 2 pi bonds and 4 sigma bonds.

e)

There are 8 sigma bonds and 2 pi bonds.

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