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G11 Q3 FINAL EXAM REVISION

Total questions: 137

Worksheet time: 3hrs 32mins

Name
Class
Date
1.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
2.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
3.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
4.

How many covalent bonds does carbon need to form in order to have a full octet? [C=6]

a)
2
b)
3
c)
4
d)
5
5.

What is a double bond?

a)

a bond between two atoms

b)

one pair of electrons shared between two atoms

c)

two pairs of electrons shared between two atoms

d)

three pairs of electrons shared between two atoms

6.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
7.

NH3 has how many lone pairs? [N=7 ,H=1]

a)

0

b)

1

c)

2

d)

3

8.

How many valence electrons does nitrogen have? [N=7]

a)
3
b)
2
c)
5
d)
1
9.

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

a)

Triple bond

b)

Trigonal bond

c)

Tri-bond

d)

Three bonds

10.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
11.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
12.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)
eight electrons
c)
the number of electrons needed to reach an octet
d)
the group number
13.

Which of these would be covalently bonded?

a)

Sodium, Na and potassium, K

b)

Magnesium, Mg and oxygen, O

c)

Fluorine, F and chlorine, Cl

d)

Helium, He and argon, Ar

14.

Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)? [F=9]

a)
A
b)
B
c)
C
d)
D
15.

Which is the correct molecular structure for carbon dioxide? [C=6 ,O=8]

a)

b)

c)

d)

16.

Which of the following is the correct Lewis structure for the compound PBr3? [P=15 ,Br=35]

a)
structure A
b)
structure B
c)
structure C
d)
structure D
17.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
18.

What is the correct structure for BF3? [B=5 ,F=9]

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

19.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
20.

Complete the sentence: In covalent bonds, electrons are _______________________

a)

Lost

b)

Gained

c)

Halved

d)

Shared

21.

Hydrogen needs _____ electrons in its valence shell to be stable. [H=1]

a)
4
b)
6
c)
8
d)
2
22.
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
23.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
24.

The electrons on the outermost energy level of the atom are called:

a)

extra electrons

b)

valence electrons

c)

ions

d)

elements

25.

As bond length increase the strength...

a)

increases

b)

decreases

c)

no change

26.

The reaction in which the energy released.

a)

endothermic

b)

exothermic

c)

none of these

27.

The number of covalent bonds form in group 17

a)

One

b)

Two

c)

Three

28.

Number of covalent bonds can form in group 16

a)

three

b)

two

c)

four

29.

Name the bond in which the orbitals overlap head to head

a)

Ionic bond

b)

sigma bond

c)

pi bond

30.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
31.
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
32.

How many sigma bonds are in the following molecule?

a)

0

b)

1

c)

2

d)

3

e)

5

33.

How many pi bonds are in the following compound?

a)

0

b)

1

c)

2

d)

3

e)

5

34.
How many pi bonds are there in a single bond? 
a)
0
b)
1
c)
2
d)
3
35.
How many sigma bonds are there in a triple bond? 
a)
0
b)
1
c)
2
d)
3
36.
How many pi bonds are there in a double bond? 
a)
0
b)
1
c)
2
d)
3
37.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

38.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

39.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

40.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number of electrons

41.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

42.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number of electrons

43.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

44.

Select the 3 exceptions to octet rule.

a)

Expanded octet

b)

Even number electron

c)

Incomplete octet

d)

Odd number electron

45.

Which of the following has the chemical formula of

carbon tetraflouride?

a)

CF

b)

CF2

c)

CF3

d)

CF4

46.

What is the formula of tetraphosphorous heptaflouride?

a)

PF7

b)

P2F6

c)

P4F5

d)

P4F7

47.

What is the chemical name for the compound with the formula Na2S?

a)

sodium fluoride

b)

magnesium sulfide

c)

lithium oxide

d)

sodium sulfide

48.
What is the chemical formula for CP ?
a)
Carbon phosphide
b)
Monocarbon phosphide
c)
Carbon monophosphide
d)
none of the above
49.
What is the chemical formula for Fluorine trisulfide ?
a)
S3F
b)
FS3
c)
FS
d)
none of the above
50.
What is the chemical formula for Tetraphosphorous Pentachloride ?
a)
4P5Cl
b)
PCl
c)

P4Cl5

d)
none of the above
51.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
52.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
53.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
54.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
55.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
56.

Which of these compounds is not an acid?

a)

HCl

b)

NaOH

c)

HNO3

d)

H2SO4

57.

Oxyacids will contain __________. Check all that apply.

a)

chlorine

b)

an oxoanion

c)

just hydrogen and a non-metal

d)

the O-2 ion

e)

the H+ ion

58.

What prefix is used to name binary acids?

a)

per-

b)

hydro-

c)

hypo-

d)

bi-

59.

The suffix -ite in the name of a polyatomic ion becomes ______ in the acid name.

a)

-ous

b)

-ate

c)

-ide

d)

-ic

60.

The suffix -ic in the name of an oxyacid, implies that the polyatomic ion in the acid has a ________ suffix.

a)

-ous

b)

-ate

c)

-ide

d)

-ite

61.

What is the formula for hydrobromic acid?

a)

HBrO

b)

HBrO2

c)

HBrO3

d)

HBr

62.

Which of the following are binary acids? Check all that apply.

a)

HCl

b)

HNO3

c)

H2S

d)

KCl

e)

H2CO3

63.
Hydroiodic acid
a)
H2I2
b)
H1I1
c)
HI
64.

Is H2S an oxyacid or Binary acid?

a)

Oxyacid

b)

Binary Acid

65.

Select all of the oxyacids from the list below.

a)

H2CO3

b)

HCl

c)

HCN

d)

HNO3

66.

HNO2 (nitrite ion)

a)

hydronitrogen

b)

hydrogen nitrogen oxygen

c)

nitrous acid

d)

nitric acid

67.

H2SO3 (sulfite ion)

a)

sulfuric acid

b)

hydrosulfuric acid

c)

sulfurous acid

d)

persulfuric acid

68.

Chlorous acid (chlorite ion)

a)

HClO3

b)

HClO2

c)

HClO

d)

HCl

69.

Oxyacids contain hydrogen, oxygen, and one other element?

a)

True

b)

False

70.

Name this acid: H2SO4 (sulfate ion)

a)

hydrogen sulfate

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

e)

hydrosulfurous acid

71.
Molecular compounds contain
a)
1 metal and 1 nonmetal
b)
only metals
c)
only nonmetals
d)
more than 2 elements (either metal or nonmetal)
72.

Name the acid: H3PO4 (phosphate ion)

a)

hydrophosphoric acid

b)

phosphorous acid

c)

phosphoric acid

d)

phosphoric hydroxide

73.

HIO3 (iodate ion)

a)

Iodic acid

b)

hydrogen iodine oxygen acid

c)

hydrogen iodide acid

74.

Of the oxyanions ClO4-, ClO3-, ClO2-, and ClO-, which is the perchlorate ion?

a)

ClO4-

b)

ClO3-

c)

ClO2-

d)

ClO-

75.
How many resonance structure for SO2 ?
a)
1
b)
2
c)
3
d)
4
76.

What bond is formed between a metal and a nonmetal?

a)

Covalent bond

b)

Ionic bond

c)

Hydrogen bond

d)

Metallic bond

77.

In a(n) ________ electrons are transferred from one atom to another

a)

ionic compound

b)

covalent compound

78.

What would be the bond angle between atoms in this molecule?

a)

180

b)

120

c)

90

d)

109.5

79.

What would be the bond angle between atoms in this molecule?

a)

109.5

b)

120

c)

180

d)

90

80.

What shape would a molecule have if it has 2 bonded pairs and 1 lone pair around its central atom? (It may help if you sketch this out)

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Bent

81.

What is the name of this molecule's shape?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

82.

What 3-D shape would this molecule have: H2S ?

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

83.

What is the name of this molecular shape?

a)

trigonal pyramid

b)

tetrahedral

c)

bent

d)

trigonal planar

84.

What 3-D shape would this molecule have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

85.

What 3-D shape would this molecule have?

a)

tetrahedral

b)

trigonal planar

c)

trigonal pyramid

d)

bent

86.

What would be the bond angle between atoms in this molecule?

a)

90

b)

120

c)

180

d)

109.5

87.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
88.

What shape is a hydrogen sulfide molecule (H2S)?

a)

linear

b)

tetrahedral

c)

bent

d)

trigonal pyramid

89.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
90.
 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
91.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
92.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
93.

A hybrid occurs when two things are combined and the result has characteristics of both is called

a)

Molecular geometry

b)

Molecular shapes

c)

Hybridization

d)

None of the above

94.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
95.

Two carbon atoms form a linear shaped ethene, C2H4, molecule when bonded with four other hydrogen atoms. Prior to bonding, the carbon atom

a)

does not hybridise

b)

undergoes sp hybridisation

c)

undergoes sp2 hybridisation

d)

undergoes sp3 hybridisation

96.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
97.

What is the hybridization of the carbon atom indicated by the arrow?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

sp3d hybridization

98.
Nitrogen atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
99.

What is the hybridization of this molecule shown above

a)

sp

b)

sp2

c)

sp3

d)

sp4

100.

Which of the following images represents a Trigonal Planar molecular geometry?

a)
b)
c)
d)
101.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

102.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
103.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

104.

What is the molecular geometry/shape of HCN?

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

105.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
106.

What is the molecular geometry/shape of a molecule with 3 shared pairs and 0 unshared pairs?

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

107.

What is the molecular geometry/shape of a molecule with 4 shared pairs and 0 unshared pairs?

a)

Linear

b)

Bent

c)

Trigonal Pyramidal

d)

Tetrahedral

108.

What is the molecular geometry/shape of a molecule with 2 shared pairs and 2 unshared pairs?

a)

Linear

b)

Bent

c)

Trigonal Pyramidal

d)

Tetrahedral

109.

Which of these is the shape of CO2?

a)
b)
c)
d)
e)
110.

Which of these is the shape of NH3?

a)
b)
c)
d)
e)
111.

Which of these is the shape of BF3?

a)
b)
c)
d)
e)
112.

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

a)

Ionic

b)

Covalent

113.

A polar bond happens between ...

a)

metal/ non metal

b)

Two non metals of the same strength

c)

Two non metals, one is stronger than the other

d)

Two metals

114.

... bond happens when electrons are shared EVENLY between the two bonded atoms.

a)

Covalent polar

b)

Covalent nonpolar

c)

Ionic

d)

Metallic

115.

The bond between two chlorine atoms in Cl2 molecule is ...

a)

Ionic

b)

Covalent polar

c)

Covalent pure

d)

metallic

116.

Chloroform (CHCl3) is a .... molecule.

a)

polar

b)

nonpolar

c)

ionic

117.

NH3 is a ... molecule

a)

Polar

b)

Nonpolar

118.

CCl4 is a ... molecule.

a)

polar

b)

nonpolar

c)

ionic

119.

What is the AXE # of this molecule ?

a)

AX3E3

b)

AX3E

c)

AXE3

d)

AX3E2

120.

What is the AXE # of the molecule shown?

a)

AX2E3

b)

AXE3

c)

AX4E

d)

AX3E2

121.

What is the AXE # of this molecule?

a)

AE4

b)

AX4

c)

AX3E

d)

AX3

122.

According to VSEPR theory, atoms and unshared pairs orient themselves so that

a)

they are all in the same plane.

b)

they are at 90 degree angles.

c)

they are as close to each other as possible.

d)

they are as far apart as possible.

123.

What is the significance of the VSEPR theory in chemistry?

a)

It helps predict the 3D arrangement of atoms in a molecule.

b)

It determines the boiling point of substances.

c)

It explains the color of chemical compounds.

d)

It identifies the types of chemical bonds present.

124.

What is the bond angle in a tetrahedral molecular geometry?

a)

90 degrees

b)

109.5 degrees

c)

120 degrees

d)

180 degrees

125.

What type of bond is depicted in the image?

a)

Covalent

b)

Polar Covalent

c)

Ionic

126.

Measure of the tendency of an atom to attract a bonding pair of electrons is known as...

a)

electronegativity

b)

bond polarity

c)

angular momentum

d)

valence electrons

127.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

128.

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

129.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts fewer electrons

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

130.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 2.0?

a)

Covalent

b)

Polar Covalent

c)

Ionic

131.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 0.3?

a)

Covalent

b)

Polar Covalent

c)

Ionic

132.

Hydrogen bonding occurs when a hydrogen atom bonded to N, O, or F is attracted to another molecule's N, O or F atom. Which of the following can participate in hydrogen bonding?

a)

CBr4

b)

NO2

c)

H2S

d)

NH3

133.

Dipole-dipole attractions occur between polar molecules. Which of these molecules is polar?

a)

H2

b)

HCl

c)

Cl2

d)

Br2

134.

Which of these molecules can participate in dipole-dipole attractions? Select all that apply.

a)

Br2

b)

CF4

c)

I2

d)

PCl3

e)

CO

135.

Which of the following is NOT a kind of intermolecular force?

a)

hydrogen bonding

b)

covalent bond

c)

dispersion forces

d)

dipole-dipole attraction

136.

Rank these in order of strength:

covalent bond

dispersion forces

hydrogen bond

dipole-dipole attraction

a)

dipole-dipole>covalent bond>hydrogen bond>dispersion

b)

dispersion>dipole-diple>hydrogen bond>covalent bond

c)

covalent bond>hydrogen bond>dipole-dipole>dispersion

d)

hydrogen bond>dipole-dipole>dispersion>covalent bond

137.

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

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