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Unit 6 Test Review

Total questions: 139

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

a term used to describe the shape of molecules that have one central atom with two other atoms bonded to it at a 104⁰ bond angle; the central atom has one or two lone pairs of electrons.

a)

bent

b)

tetrahedral

c)

trigonal planar

d)

linear

2.

an attractive force between atoms, ions, or molecules that results in the formation of compounds

a)

bond

b)

single bond

c)

tetrahedral

d)

bent

3.

a chemical bond resulting from the sharing of electron between two bonding atoms

a)

covalent bond

b)

single bond

c)

double bond

d)

nonpolar covalent bond

4.

a chemical bond resulting from the sharing of two pairs of electrons between two atoms

a)

double bond

b)

triple bond

c)

single bond

d)

bond

5.

International Union of Pure and Applied Chemistry

a)

IUPAC system

b)

molecular geometry

c)

VSEPR theory

d)

single bond

6.

a diagram where dots or other small symbols are placed around the symbol of an element to illustrate the valence electrons

a)

lewis dot diagram

b)

linear

c)

molecular geometry

d)

VSEPR theory

7.

a term used to describe the shape of molecules that resemble a straight line; there is a 180° bond angle between bonded pairs of electrons

a)

linear

b)

single bond

c)

bent

d)

tetrahedral

8.

the arrangement of atoms, not lone pair electrons, around the central atom of a molecule or a polyatomic ion

a)

molecular geometry

b)

VSEPR theory

c)

single bond

d)

lewis dot diagram

9.

a type of bond that has an even distribution of charge due to an equal sharing of electrons

a)

nonpolar convalent bond

b)

polar covalent bond

c)

covalent bond

d)

double bond

10.

a type of bond that has an uneven distribution of charge due to an unequal sharing of electrons

a)

polar covalent bond

b)

nonpolar covalent bond

c)

bond

d)

single bond

11.

a chemical bond resulting from the sharing of one pair of electrons between two atoms

a)

single bond

b)

bond

c)

triple bond

d)

double bond

12.

a term used to describe molecules and polyatomic ions that have a central atom bonded to four other atoms in the form of a tetrahedron; there is a 109.5° bond angle between bonded pairs

a)

tetrahedral

b)

trigonal planar

c)

linear

d)

trigonal pyramidal

13.

a term used to describe molecules and polyatomic ions that have a central atom bonded to three other atoms in the form of a flat, triangular shape; there is a 120° bond angle between bonded pairs

a)

trigonal planar

b)

trigonal pyramidal

c)

tetrahedral

d)

polar covalent bond

14.

a term used to describe molecules and polyatomic ions that have a central atom bonded to three other atoms in the form of a pyramid with lone pairs of electrons on the central atom; there is a 107° bond angle between bonded pairs

a)

trigonal pyramidal

b)

triple bond

c)

trigonal planar

d)

tetrahedral

15.

a chemical bond resulting from the sharing of three pairs of electrons between two atoms

a)

triple bond

b)

single bond

c)

trigonal planar

d)

tetrahedral

16.

Valence Shell Electron Pair Repulsion Theory; a model used the predict the geometric arrangement of molecules based on minimizing the electrostatic repulsion of a molecule’s valence electrons around the central atom

a)

VSEPR theory

b)

IUPAC system

17.

What is this unit focusing on?

a)

Molecular Geometry

b)

The Water Cycle

c)

The Periodic Table of Elements

d)

Electronegativity

18.

What is the difference between Covalent and Ionic bonds?

a)

Electrons in Covalent bonds are shared, and Electrons in Ionic bonds are transferred

b)

Electrons in Covalent bonds are transferred, and Electrons in Ionic bonds are shared

c)

There is no difference

d)

Electrons in Covalent bonds disappear, and Electrons in Ionic bonds don't exist

19.

Do all compounds have a chemical formula?

a)

No!

b)

Yes!

20.

Which element is a useful building block of larger molecules?

a)

Oxygen

b)

Nitrogen

c)

Carbon

d)

Helium

21.

Up to how many atoms can Carbon bond with at one time?

a)

5

b)

2

c)

1

d)

4

22.

What rule do bonding atoms follow?

a)

The octopus rule

b)

The fourth rule

c)

The laws of electronegativity

d)

The octet rule

23.

What is bond length?

a)

The average distance between two bonded atoms.

b)

How long it takes to form a bond

c)

Where the bond information is stored

d)

The reason for the octet rule

24.

What is a single bond?

a)

1 pair of electrons (one line)

b)

2 pairs of electrons

c)

A bond that only applies to nitrogen

d)

2 lines

25.

What are multiple bonds?

a)

Bonds with one line

b)

Bonds with more than one line

26.

What is molecular geometry?

a)

The positions of the atomic nuclei in a molecule

b)

Geometry dealing with squares

c)

Geometry that is only concerned with carbon

d)

The specific three-dimensional arrangement of atoms in molecules

27.

What are non-bonded electrons shown by two dots called?

a)

molecules

b)

lone pairs

c)

double bonds

d)

triple bonds

28.

How many bonds does a tetrahedral have?

a)

4

b)

5

c)

3

d)

8

29.

What is the bond angle of a tetrahedral?

a)

90

b)

108.5

c)

109.5

d)

110.5

30.

Whats an atom that has two bonded pairs and no lone pairs called?

a)

Trigonal Planar

b)

Bent

c)

Tetrahedral

d)

Linear

31.

How many bonded pairs and lone pairs does a trigonal planar atom have?

a)

3 bonded pairs and no lone pair

b)

4 bonded pairs and 2 pairs

c)

5 bonded pairs and 1 lone pair

d)

3 bonded pairs and 5 lone pairs

32.

How many bonds and lone pairs does a bent molecule have?

a)

Three bonds and two lone pairs

b)

Four bonds and four pairs

c)

Two bonds and two lone pairs

d)

none

33.

What is the definition of trigonal pyramidal?

a)

a central atom bonded to three other atoms in the form of a pyramid with lone pairs of electrons

b)

A central atom bonded to 4 other atoms

c)

A central atom bonded by triangles to a pyramid shape

d)

Molecules in a straight line

34.

What is bent?

a)

One central atom with two other atoms bonded to it

b)

something ripped in half

c)

A faulty shape

35.

Whats a double bond?

a)

A chemical bond resulting from the sharing of two pairs of electrons between two atoms

b)

Three bonds

c)

A chemical bond resulting from the sharing of electron between two atoms

d)

a chemical bond resulting from the sharing of three pairs of electrons between two atoms

36.

What is a covalent bond?

a)

a type of bond that has an uneven distribution of charge due to an equal sharing of electrons

b)

IUPAC system

c)

a chemical bond resulting from the sharing of electrons between two bonding atoms

d)

VSEPR

37.

What is a triple bond?

a)

a chemical bond resulting from the sharing of one pair of electrons between two atoms

b)

A chemical bond resulting from the sharing of three pairs of electrons between two atoms

38.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

39.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
40.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
41.

What is the molecular geometry of CO2?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

42.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
43.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
44.

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

45.

Does the following reference Polar, Nonpolar, or both:

"affected by an electrical charge"?

a)

Polar

b)

Nonpolar

c)

Both

46.

Does the following reference Polar, Nonpolar, or both:

"equal sharing of electrons"?

a)

Polar

b)

Nonpolar

c)

Both

47.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
48.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
49.

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

50.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
51.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
52.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
53.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
54.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
55.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
56.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
57.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
58.

What is the correct shape of CHCl3?

a)

Bent

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Trigonal planar

59.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
60.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
61.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
62.

What molecule could this be? (Each purple cloud represents a lone pair of electrons.)

a)

CO2

b)

NH3

c)

H2S

d)

CH4

63.

What molecule could this be? (The purple cloud represents a lone pair of electrons.)

a)

H2O

b)

NH3

c)

CO2

d)

CH4

64.
 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
65.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
66.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
67.

What is this unit focusing on?

a)

Molecular Geometry

b)

The Water Cycle

c)

The Periodic Table of Elements

d)

Electronegativity

68.

What is the difference between Covalent and Ionic bonds?

a)

Electrons in Covalent bonds are shared, and Electrons in Ionic bonds are transferred

b)

Electrons in Covalent bonds are transferred, and Electrons in Ionic bonds are shared

c)

There is no difference

d)

Electrons in Covalent bonds disappear, and Electrons in Ionic bonds don't exist

69.

Do all compounds have a chemical formula?

a)

No!

b)

Yes!

70.

Which element is a useful building block of larger molecules?

a)

Oxygen

b)

Nitrogen

c)

Carbon

d)

Helium

71.

Up to how many atoms can Carbon bond with at one time?

a)

5

b)

2

c)

1

d)

4

72.

What rule do bonding atoms follow?

a)

The octopus rule

b)

The fourth rule

c)

The laws of electronegativity

d)

The octet rule

73.

What is bond length?

a)

The average distance between two bonded atoms.

b)

How long it takes to form a bond

c)

Where the bond information is stored

d)

The reason for the octet rule

74.

What is a single bond?

a)

1 pair of electrons (one line)

b)

2 pairs of electrons

c)

A bond that only applies to nitrogen

d)

2 lines

75.

What are multiple bonds?

a)

Bonds with one line

b)

Bonds with more than one line

76.

What is molecular geometry?

a)

The positions of the atomic nuclei in a molecule

b)

Geometry dealing with squares

c)

Geometry that is only concerned with carbon

d)

The specific three-dimensional arrangement of atoms in molecules

77.

What are non-bonded electrons shown by two dots called?

a)

molecules

b)

lone pairs

c)

double bonds

d)

triple bonds

78.

How many bonds does a tetrahedral have?

a)

4

b)

5

c)

3

d)

8

79.

What is the bond angle of a tetrahedral?

a)

90

b)

108.5

c)

109.5

d)

110.5

80.

Whats an atom that has two bonded pairs and no lone pairs called?

a)

Trigonal Planar

b)

Bent

c)

Tetrahedral

d)

Linear

81.

How many bonded pairs and lone pairs does a trigonal planar atom have?

a)

3 bonded pairs and no lone pair

b)

4 bonded pairs and 2 pairs

c)

5 bonded pairs and 1 lone pair

d)

3 bonded pairs and 5 lone pairs

82.

How many bonds and lone pairs does a bent molecule have?

a)

Three bonds and two lone pairs

b)

Four bonds and four pairs

c)

Two bonds and two lone pairs

d)

none

83.

What is the definition of trigonal pyramidal?

a)

a central atom bonded to three other atoms in the form of a pyramid with lone pairs of electrons

b)

A central atom bonded to 4 other atoms

c)

A central atom bonded by triangles to a pyramid shape

d)

Molecules in a straight line

84.

What is bent?

a)

One central atom with two other atoms bonded to it

b)

something ripped in half

c)

A faulty shape

85.

Whats a double bond?

a)

A chemical bond resulting from the sharing of two pairs of electrons between two atoms

b)

Three bonds

c)

A chemical bond resulting from the sharing of electron between two atoms

d)

a chemical bond resulting from the sharing of three pairs of electrons between two atoms

86.

What is a covalent bond?

a)

a type of bond that has an uneven distribution of charge due to an equal sharing of electrons

b)

IUPAC system

c)

a chemical bond resulting from the sharing of electrons between two bonding atoms

d)

VSEPR

87.

What is a triple bond?

a)

a chemical bond resulting from the sharing of one pair of electrons between two atoms

b)

A chemical bond resulting from the sharing of three pairs of electrons between two atoms

88.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

89.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
90.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
91.

What is the molecular geometry of CO2?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

92.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
93.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
94.

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

95.

Does the following reference Polar, Nonpolar, or both:

"affected by an electrical charge"?

a)

Polar

b)

Nonpolar

c)

Both

96.

Does the following reference Polar, Nonpolar, or both:

"equal sharing of electrons"?

a)

Polar

b)

Nonpolar

c)

Both

97.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
98.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
99.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
100.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
101.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

102.

Is this molecule polar?

a)

No

b)

Yes

103.

Is this molecule polar?

a)

Yes

b)

No

104.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

105.
Choose the correct shape for this molecule:
a)

Trigonal planar

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Linear

e)

Bent

106.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
107.

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

e)

Bent

108.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Bent

109.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

110.

What IMF are present

a)

Dipole Dipole

b)

London Dispersion Forces

c)

Hydrogen Bonding

111.

What IMF are present

a)

Dipole Dipole

b)

London Dispersion Forces

c)

Hydrogen Bonding

112.

What IMF are present

a)

Dipole Dipole

b)

London Dispersion Forces

c)

Hydrogen Bonding

113.

What IMF are present

a)

Dipole Dipole

b)

London Dispersion Forces

c)

Hydrogen Bonding

114.

What IMF are present

a)

Dipole Dipole

b)

London Dispersion Forces

c)

Hydrogen Bonding

115.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Bent

116.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Bent

117.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Bent

118.

Is this molecule polar?

a)

Yes

b)

No

119.

Is this a valid Lewis Structure?

a)

Yes

b)

No

120.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Bent

121.

What is the molecular geometry/shape of this molecule

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Bent

122.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
123.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
124.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
125.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)
attract elenece in the non-valence energy levels
126.
How many electrons are represented by a single straight line in a Lewis structure?
a)
1
b)
2
c)
4
d)
6
127.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
128.
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
129.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
130.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
131.
Which molecule contains bonds of GREATER polarity?
a)
H2O
b)
OF2
132.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)
CCl4
133.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
134.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
135.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
136.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
137.
When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom
a)
true
b)
false
138.
The electronegativity difference in the bonds of CH4 (methane) is:
a)
0.4
b)
5.9
c)
-0.4
d)
1.7
139.
The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:
a)
0.4
b)
0.5
c)
9.5
d)
5.5

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