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Review for Friday 3/15 Test

Total questions: 110

Worksheet time: 5hrs 56mins

Name
Class
Date
1.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
2.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
3.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
4.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
5.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
6.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
7.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

8.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
9.
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
10.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
11.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
12.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
13.
What is the molecular shape of a silicon dioxide molecule?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
14.
Determine the molecular shape of carbon tetrafluoride.
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
15.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
16.
Will this molecule be polar or nonpolar? CS2
a)
polar
b)
nonpolar
17.

How many unshared pairs of electrons will a bent molecule have?

a)

0

b)

2

c)

3

d)

4

18.
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
19.

Match the following shapes to their Names

a)
1.

Trigonal Planar

b)
2.

Tetrahedral

c)
3.

Trigonal Pyrimidal

d)
4.

Linear

e)
5.

Bent

20.
 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
21.

Both Carbon Dioxide and water have ​ (a)   atoms bonded to the central atom. Carbon Dioxide (CO2) is a ​ (b)   Molecule while water (H2O) is a ​ (c)   molecule because water has ​ (d)   on the central atom.

Choose from the below words
two
Linear
Bent
Lone Pairs
Three
Double Bonds
Trigonal Planar
22.

Think about how many electron groups are around the central atom. Place these structures in order from LEAST groups to MOST groups.

a)

Linear

b)

Trigonal Planar

c)

Tetrahedral

1)
2)
3)
23.

Think about how many electron groups are around the central atom. Place these structures in order from LEAST groups to MOST groups.

a)

Linear

b)

Bent

c)

Trigonal Pyramidal

1)
2)
3)
24.

Which Lewis Structure would be linear? Mark all that apply

a)
b)
c)
d)
25.

Which Structure has a different shape than the others?

a)
b)
c)
d)
26.

When determining molecular geometry, how many electron groups are around the central atom of this structure?

a)

1

b)

2

c)

3

d)

4

27.

What is the AXE # of this molecule?

a)

AX2

b)

AX2E2

c)

AX2E

d)

AX2E4

28.

What is the AXE # of this molecule?

a)

AX2

b)

AX2E2

c)

AX2E

d)

AX2E4

29.

What is the AXE # of this molecule?

a)

AX

b)

AXE

c)

AX3E

d)

AX3

30.
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
a)
True
b)
False
31.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
32.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
33.
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.
34.

Does the following reference Polar, Nonpolar, or both:

"affected by an electrical charge"?

a)

Polar

b)

Nonpolar

c)

Both

35.

Does the following reference Polar, Nonpolar, or both:

"equal sharing of electrons"?

a)

Polar

b)

Nonpolar

c)

Both

36.

True or False


Attractions between polar molecules are Weaker than attractions between nonpolar molecules.

a)

True

b)

False

37.
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
38.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
39.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)
CCl4
40.
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.
41.
Does HCl have hydrogen bonding?
a)
yes
b)
no
42.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
43.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
44.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

45.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

46.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
47.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
48.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

49.

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

a)

higher

b)

lower

50.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

51.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
52.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
53.
What will be the state of the following molecule?
a)
gas
b)
liquid
c)
solid
54.
What type of forces will the following molecule have?
a)
dispersion forces
b)
dipoles
c)
hydrogen bonding
55.
What forces will the following molecule have?
a)
dispersion
b)
dipole
c)
hydrogen bonding
56.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
57.

Which substance will have the highest vapor pressure

a)

CH3CH2CH2CH2CH2CH3

b)

H2O

c)

CH4

d)

CH3F

58.

What is vapor pressure

a)

the amount of energy required to evaporate

b)

the amount of energy required to boil

c)

the force per unit area exerted by the gaseous layer above a liquid

d)

the force per unit area exerted by a liquid on the gaseous layer above it

59.

Which of the following molecules would have Van der Waals Forces

a)

CH4

b)

SCO

c)

PCl3

d)

SO2

60.

Which force is only found between polar covalent molecules?

a)

Ionic bond

b)

Dipole Dipole

c)

London Dispersion Force

d)

Covalent bond

61.

In this force, electron movement cause a slight charge at a single instant. This charge is temporary.

a)

Hydrogen bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

62.

In ionic solids, what holds the ions together?

a)

Hydrogen Bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

63.

Which is not a bond, but is an intermolecular force?

a)

Covalent Bond

b)

Ionic Bond

c)

Hydrogen Bond

d)

These are all bonds

64.

All polar covalent molecule samples contain:

(Check all that apply)

a)

Hydrogen bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

65.

Samples of H2O, NH3, and HF all contain:

(Check all that apply)

a)

Hydrogen Bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

66.

Nonpolar molecule samples all contain

(Check all that apply)

a)

Hydrogen Bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

67.

When one polar molecule attracts another polar molecule it is called:

a)

Hydrogen Bonds

b)

Dipole Dipole

c)

London Dispersion Force

d)

Ionic Bond

68.

Which of these forces is always the strongest?

a)

Hydrogen bonds

b)

Dipole Dipole force

c)

London Dispersion force

d)

Ionic bonds

69.

Intermolecular forces are responsible for which of the following properties?

a)

State of matter

b)

Color

c)

Odor

d)

Conductivity

70.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

71.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

72.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

73.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

74.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

75.
The bond formed between atoms of the same element:
a)
nonpolar covalent
b)
polar covalent
c)
ionic bond
d)
hydrogen bond
76.

Match the Following

a)

Hydrogen Bond

1.

Present in Polar involving N, O, F

b)

London Dispersion Forces

2.

Present in both Polar and Non Polar Molecules

c)

Dipole- Dipole

3.

Polar Substances only

77.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

covalent bonding

78.

Which intramolecular force has the greatest strength?

a)

ionic bond

b)

nonpolar covalent

c)

polar covalent

79.

Which of these is the weakest intermolecular force [IMF]?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

80.

Which intermolecular force [IMF] do all molecules have?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

81.

Which intermolecular force [IMF] requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

82.

Which intermolecular force [IMF] is characterized by partial charges?

a)

Dipole-dipole forces

b)

Hydrogen bonding

c)

London dispersion forces

83.

Which intermolecular force [IMF] causes water to have an elevated boiling point?

a)

London dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

84.

Which of these molecules are polar? (Select ALL that apply.)

a)

SO₂

b)

F₂

c)

PCl₃

d)

CH₄

85.

Melting and boiling points depend on thermal energy and the strength of ________

a)

intramolecular forces

b)

intermolecular forces

c)

polar covalent bonds

d)

metallic bonds

86.
The EM spectrum increases from left to right in________________.
a)
Wavelength
b)
Frequency
c)
Amplitude
d)
Height
87.
The relationship between wavelength and frequency is λ=c/f.  Calculate the wavelength of light that has a frequency of 5.2 x 1012 1/s. The speed of of light is 3.0x 108 m/s.
a)
5.8 x 10 -5 m
b)
5.8 x 10 -7 m
c)
5.19 x 10 14 m
d)
1.56 x 10 23 m
88.
Solve this problems using the equation: 
C = λν
If an AM radio station broadcasts at
9.95 x 105 Hz, what is the wavelength of this radiation?
a)
6.59 x 10-28 m
b)
1.01 x 10-6 m
c)
3.32 x 10-3 m
d)
302 m
89.

Calculate the wavelength of light that has a frequency of 5.2 x 1012 1/s.

a)

5.8 x 10 -5 m

b)

5.8 x 10 -7 m

c)

5.19 x 10 14 m

d)

1.56 x 10 23 m

90.
What are the units of frequency?
a)
m/s
b)
s
c)
Hz
d)
m
91.

A common infrared laser operates at 1.06 x 103 nm. What is the energy of a photon with this wavelength? (1 x 109 nm = 1m)

a)

7.02 x 10^-40 J

b)

6.25 x 10^-28 J

c)

3.54 x 10^-15 J

d)

1.87 x 10^-19 J

92.
What is the frequency of a photon whose energy is 3.4x10-19J?
a)
8.8x1026 Hz
b)
5.1x1014 Hz
c)
1.9x10-15 Hz
d)
2.3x10-52 Hz
93.

A wave has a frequency of 10 hz and a wavelength of 4 m. What is the velocity of the wave?

a)

24 m/s

b)

40 m/s

c)

2.5 m/s

94.
What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 
a)
2.32 x 109 Hz
b)
3.60 x 1015 Hz
c)
1.58 x 10-51 Hz
d)
3 x 108  m/s
95.
Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 × 10 10 1/s.
a)
6.63 x 10-34 J
b)
5.25 x 1014 J
c)
5.24 x 10-23 J
d)
1.19 x 1044 J
96.
What is the energy of an X-ray with a frequency of 1.0 x 1017 Hz?
a)
6.63 x 10-34 J
b)
6.63 x 10-17 J
c)
1.51 x 1016 J
d)
1.51 x 10-16 J
97.
A joule is: 
a)
A SI unit of measurement for distance
b)
a SI unit of measurement for energy
c)
a SI unit of measurement for speed
d)
something shiny
98.
The equation that shows the relationship between the energy of light and frequency is: 
a)
c= λ⋅f
b)
E=h⋅f
99.

What is the electron doing in this image?

a)

Absorbing Energy

b)

Releasing Energy

100.

Does the energy released by this photon have high or low energy?

a)

High

b)

Low

101.

Does the photon released in this image have high or low energy?

a)

High

b)

Low

102.

Electrons (attract/repel) each other.

a)

Attract

b)

Repel

103.

Protons and Electrons (attract/repel) each other.

a)

Attract

b)

Repel

104.

What is happening with the electron in this image?

a)

Absorbing Energy

b)

Releasing Energy

105.

Which Danish physicist proposed an atomic model that described electrons as moving in circular orbits around the nucleus?

a)

Niels Bohr

b)

Tycho Brahe

c)

Stephen Hawking

d)

Carl Sagan

106.

The amount of energy required to move an electron from one energy level to another is a _______ of energy. 

a)

atomic emission spectrum

b)

energy level

c)

quantum

d)

Ground State

107.

What is the lowest possible energy level that an electron can occupy?

a)

Lower energy level

b)

Ground State

c)

Excited State 

d)

Depressive State

108.

How does an electron get from a lower energy level to an excited state (higher energy level)? 

a)

It absorbs light

b)

It emits light 

c)

it simply can do whatever it wants

d)

that's how the statistics describe it

109.

Which of the following electronic transitions in the oxygen atom will result in light emission?

a)

ni=1⟶nf=2n_i=1⟶n_f=2

b)

ni=1⟶nf=3n_i=1⟶n_f=3  

c)

ni=3⟶nf=2n_i=3⟶n_f=2  

d)

ni=2⟶nf=3n_i=2⟶n_f=3  

110.

How many electrons can occupy the lowest energy level? 

a)

1 only

b)

up to 2

c)

up to 4

d)

up to 8

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