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Worksheets

Intramolecular & Intermolecular Forces

Total questions: 211

Worksheet time: 5hrs 39mins

Name
Class
Date
1.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
2.
What is the best explanation of VSEPR theory?
a)
It explains the shapes that electrons make around atoms when they repel
b)
It explains how many electrons fit into an element's valent shell
c)
It explains why electrons pair up
d)
It explains why electrons repel each other
3.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
4.

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

a)

Linear

b)

Tetrahedral

c)

Bent

d)

Trigonal planar

5.
 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
6.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
7.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
8.

The geometry of a molecule with 4 bonded pairs of electrons and 0 lone pairs of electrons, AB4

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

9.

What is molecular shape for this shape?

a)

Tetrahedral

b)

Trigonal planar

c)

Trigonal bipyramidal

d)

Trigonal pyramidal

10.
 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
11.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
12.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

13.

How many lone pairs of electrons are on the P atom in PF3?

a)
1
b)
2
c)
3
d)
0
14.
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
15.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
16.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
17.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
18.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
19.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
20.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
21.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
22.

The acronym VSEPR stand for

a)

very strong electron pair repulsion.

b)

varied symmetry electrostatic proton reaction.

c)

venomous snakes enjoy pink ribbons.

d)

valence shell electron pair repulsion.

23.

VSEPR theory is used to predict

a)

the number of unshared pairs of electrons in a Lewis structure.

b)

the number of multiple bonds in a Lewis structure.

c)

the three-dimensional geometry of a molecule.

d)

the three-dimensional crystal lattice structure of ionic compounds.

24.

Molecules such as boron trichloride that have three bonded atoms and no unshared pairs have what shape?

a)

trigonal planar

b)

trigonal pyramidal

c)

trigonal bipyramidal

d)

tetrahedral

25.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
26.

Ethanol is...

a)

polar

b)

nonpolar

27.

Butane is...

a)

polar

b)

nonpolar

28.

CF4 is...

a)

polar

b)

nonpolar

29.

What is the BOND and MOLECULE polarity of SiI4

a)

Bond: Polar

Molecule: Polar

b)

Bond: Polar

Molecule: Nonpolar

c)

Bond: Nonpolar

Molecule: Nonpolar

d)

Bond: Nonpolar

Molecule: Polar

30.

What is the BOND and MOLECULE polarity of H2O

a)

Bond: Polar

Molecule: Polar

b)

Bond: Polar

Molecule: Nonpolar

c)

Bond: Nonpolar

Molecule: Nonpolar

d)

Bond: Nonpolar

Molecule: Polar

31.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

32.

Which of these atoms is the most electronegative?

a)

Bromine

b)

Fluorine

c)

Hydrogen

d)

Potassium

33.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

34.

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

35.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

36.

Partial charges like the ones shown here are called:

a)

dipoles

b)

deltas

c)

ions

d)

magnetic poles

37.

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 an anion

38.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
39.

Identify the strongest IMF exist in CH4

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

40.

Identify the strongest IMF exist in NH3

a)

london dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

41.

Identify the strongest IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

42.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

43.

Forces that holds atoms together within the molecule

a)

intermolecular forces

b)

intramolecular forces

44.

Hydrogen bonding is a special case of __________.

a)

london dispersion

b)

ion-dipole

c)

dipole-dipole

45.
Does HCl have hydrogen bonding?
a)
yes
b)
no
46.
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
47.

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

a)

higher

b)

lower

48.
What state of matter consists of tightly packed atoms?
a)
Solid
b)
liquid
c)
gas
d)
plasma
49.
Liquid has a definite ___________, but a variable _____________.
a)
shape, volume
b)
mass, area
c)
smell, taste
d)
volume, shape
50.
Which of the following states of matter has the most kinetic energy?
a)
solid
b)
liquid
c)
gas
51.
Which of the following states of matter has the lowest kinetic energy? 
a)
solid
b)
liquid 
c)
gas
52.
To make a solid become a liquid, you must increase its________________.
a)
mass
b)
density
c)
kinetic energy
d)
potential energy
53.
Gas particles move around at __________ speeds. 
a)
low
b)
slow
c)
high
d)
unknown
54.
Adding thermal energy to matter casues its particles to _________________.
a)
move slower
b)
move faster
c)
melt
d)
feeze
55.
Which state of matter has particles that are loosely connected, and move freely past each other? 
a)
solid
b)
liquid
c)
gas
d)
plasm
56.

Anything that has mass and takes up space.

a)

Matter

b)

Atom

c)

Pure Substance

d)

Element

57.

Which phase of matter has no definite shape or volume?

a)

Solid

b)

Liquid

c)

Gas

d)

All of the above

58.
In which state does matter completely fill its closed container?
a)
Gas
b)
Liquid
c)
Solid
d)
Ice
59.

Order the following intermolecular forces from strongest to weakest

a)

Hydrogen Bonds

b)

Dipole-Dipole

c)

London Dispersion

1)
2)
3)
60.

Order the following intermolecular forces from weakest to strongest

a)

London Dispersion Forces

b)

Dipole-Dipole

c)

Hydrogen Bonds

1)
2)
3)
61.

London Dispersion Forces are the result of

a)

Permanent Dipoles

b)

Temporary dipoles

c)

No Dipoles

d)

Hydrogen bonds

62.

Dipole-Dipole interactions occur between both nonpolar and polar molecules

a)

True

b)

False

63.

Which of the following elements does NOT form hydrogen bonds?

a)

Oxygen

b)

Fluorine

c)

Carbon

d)

Nitrogen

64.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)

pairs of electrons are shared between two non-metal atoms.

d)

two non-metal atoms are attracted to each other by opposite charges.

65.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

66.

Identify the following compound as ionic or covalent: Ca(OH)2

a)

ionic

b)

covalent

67.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
68.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
69.

dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

70.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
71.

P₄S₁₀

a)

tetrapotassium decasulfide

b)

phosphorus decasulfide

c)

tetraphosphorus decasulfide

d)

phosphorus (X) sulfide

72.

SO₃

a)

sulfate

b)

sulfur oxide

c)

sulfur trioxide

d)

monosulfur trioxide

73.

tetraphosphorus heptoxide

a)

K₄O₁₀

b)

P₄O7

c)

KO

d)

P₁₀O₄

74.

chlorine dioxide

a)

ClO2

b)

ClO

c)

ClO3

d)

HClO2

75.

hexaboron monosilicide

a)

B6Si

b)

BSi

c)

BSi6

d)

B6Si6

76.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

77.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

78.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)

pairs of electrons are shared between two non-metal atoms.

d)

two non-metal atoms are attracted to each other by opposite charges.

79.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

80.

Identify the following compound as ionic or covalent: Ca(OH)2

a)

ionic

b)

covalent

81.

What is the chemical formula for dinitrogen tetraphosphide?

a)

NP

b)

N4P2

c)

N2P4

d)

N2P3

82.

What is the correct molecular formula for the compound tetraphosphorus trisulfide?

a)

P3S4

b)

K4S3

c)

P4S3

d)

PS

83.

What is the correct name for the compound, S2F10?

a)

sodium fluoride

b)

disodium decafluoride

c)

sulfur fluoride

d)

disulfur decafluoride

84.

What is the name of the following compound: CS2?

a)

Carbon Sulfide

b)

Monocarbon Sulfide

c)

Monocarbon disulfide

d)

Carbon disulfide

85.

A covalent bond is made of the 2 following kinds of elements:

a)

Metal and metal

b)

Nonmetal and nonmetal

c)

Metalloid and Metalloid

d)

Metal and nonmetal

86.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
87.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
88.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
89.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
90.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
91.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
92.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
93.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
94.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
95.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

96.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

97.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
98.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

99.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

100.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

101.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
102.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
103.
 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
104.

What is a cation?

a)

a metal with a negative (-) charge that gains electrons

b)

a non-metal with a negative (-) charge that loses electrons

c)

a metal with a positive (+) charge that loses electrons

d)

a non-metal with a positive (+) charge that loses electrons

105.

What is a anion?

a)

a metal with a negative (-) charge that loses electrons

b)

a non-metal with a negative (-) charge that gains electrons

c)

a metal with a positive (+) charge that gains electrons

d)

a non-metal with a positive (+) charge that loses electrons

106.

How many valence electrons does Silicon Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

107.

How many valence electrons does Phosphorus Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

108.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
109.

How many valence electrons does Potassium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

110.

If the charge becomes 2+ what does that indicate about an ion?

a)

It is stealing 2 electrons

b)

It is losing 2 electrons

c)

It is in period 2

d)

It has an atomic # of 2

111.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
112.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
113.

What is the overall charge of the ionic compound NaCl

a)

+1

b)

+2

c)

+3

d)

0

114.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
115.

What kind of Ion does Aluminum form?

a)

Al+3Al^{+3}  

b)

Al−3Al^{-3}  

c)

Al−1Al^{-1}  

d)

Al+2Al^{+2}  

116.

Anions...

a)

lose electrons

b)

lose protons

c)

gain electrons

d)

gain protons

117.

Key properties of ionic bonds are (choose all that apply)

a)

Thermal conductivity

b)

Electric conductivity

c)

high melting point

d)

low boiling point

118.

Cations...

a)

lose electrons

b)

lose protons

c)

gain electrons

d)

gain protons

119.

For an ionic compound formula, write

a)

Metal first

b)

Non-Metal first

c)

Cation first

d)

Anion first

120.

Losing electrons makes an atom

a)

a loser

b)

positively charged

c)

negatively charged

d)

happy

121.

Gaining electrons make an atom

a)

a hustler

b)

negatively charged

c)

atomic

d)

positively charged

122.

Which two elements would NOT form an ionic bond?

a)

calcium and lithium

b)

calcium and oxygen

c)

lithium and oxygen

d)

calcium and carbon

123.

A sodium ion has a charge of

a)

-1

b)

-2

c)

+1

d)

+2

124.

True or False: Sodium and Chloride ions have equal but opposite charges

a)

True

b)

False

125.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
126.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
127.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
128.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
129.
What is the correct name for MgI₂?
a)
Manganese IV iodide
b)
Manganese diiodide
c)
Magnesium iodide
d)
Magnesium diiodide
130.

Name for NaH

a)

sodium hydrogen

b)

potassium hydride

c)

sodium hydride

d)

potassium hydrogen

131.

Name for SrBr2

a)

strontium bromine

b)

strontium bromide

c)

strontium dibromide

d)

strontium dibromine

132.

Why don't noble gases form bonds?

a)

Noble gases do form bonds

b)

They all have a full octet

c)

They only bond with each other

133.

What charge will a Neon ion have?

a)

+1

b)

-1

c)

-8

d)

Neon does not form ions.

134.

Is this the correct Lewis Dot Structure for phosphorus?

a)

Yes

b)

No

135.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

136.

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

a)

nonpolar

b)

polar

c)

ionic

137.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

138.

When you have Ga-Se, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

139.

When you have I2, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

140.

The correct formula for copper (II) nitride is:

a)

CuNCuN  

b)

CuN2CuN_2  

c)

Cu3N2Cu_3N_2  

d)

Cu2N3Cu_2N_3  

141.

The correct name for CaCl2CaCl_2  is:

a)

calcium chlorine

b)

calcium chloride

c)

calcium dichloride

d)

calcium (II) chloride

142.

The correct formula for beryllium fluoride is:

a)

BeFBeF  

b)

BF2BF_2  

c)

Be2FBe_2F  

d)

BeF2BeF_2  

143.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

144.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

145.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

146.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

147.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

148.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

149.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

150.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

151.
Which of the following is the correct name for the chemical formula Ca(NO2)2?
a)
cadmium nitride
b)
calcium nitrate
c)
calcium nitrite
d)
cadmium nitrite
152.
Metals tend to 
a)
gain electrons
b)
lose electrons
153.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
154.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
155.

A chemical bond where electrons are taken/stolen

a)

Ionic Bond

b)

James Bond

c)

Covalent Bond

d)

Polar Bond

156.

When two or more different elements are chemically combined.

a)

Mixture

b)

Element

c)

Solution

d)

Compound

157.
When naming ionic compounds you always write the name of the positive element  _______ .
a)
first
b)
second
c)
with "ide"
d)
with a prefix
158.

Name the following compound: Zn3N2

a)

zinc nitride

b)

trizinc dinitride

c)

zinc (III) nitride

d)

zinc (II) nitide

e)

zinc nitrogen

159.
The name of Al₂(SO₄)₃ is
a)
aluminum sulfur oxide
b)
aluminum sulfate
c)
aluminum trisulfate
d)
aluminum (III) sulfate
160.

Name the following ionic compound: Li(NO3)

a)

lithium nitrate

b)

lithium III nitrate

c)

lithium nitride

d)

lithium oxide

161.

What is the name of the following compound: NaCl

a)

sodium chloride

b)

sodium (I) chloride

c)

sodium chlorine

d)

sodium (I) chlorine

162.

How many bonds can Carbon make in covalent bond?

a)

1

b)

2

c)

3

d)

4

163.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
164.

Which substances, in general, have the higher melting point?

a)

Metal

b)

Non-Metals

165.
Which of the following is NOT a characteristic of most metals?
a)
Brittle
b)
Good conductor
c)
Ductile
d)
Malleable
166.

How many electrons are in Aluminium?

a)

40

b)

27

c)

13

d)

14

167.

How many neutrons are in Magnesium?

a)

36

b)

12

c)

24

d)

6

168.

How many protons are in Sodium?

a)

11

b)

22

c)

12

d)

33

169.

How many protons are in Chlorine?

a)

35

b)

18

c)

17

d)

52

170.

How many electrons are in Sulfur?

a)

32

b)

16

c)

48

d)

8

171.

Metals are hard because metals have a

a)

sea of electrons that tightly hold the nuclei together

b)

they form triple bonds

c)

low melting point

d)

high luster

172.

Why do metals have high melting points?

a)

Metallic bonds are weak and metals have a simple structure

b)

Metallic bonds are strong and metals have a lattice structure

c)

Metallic bonds are strong and metals have a simple structure

173.

What is the name for the electrostatic force of attraction between the particles shown in the image?

a)

covalent bond

b)

dative covalent bond

c)

metallic bond

d)

ionic bond

174.

A temporary electrical charge imbalance that causes molecules to attract is called...

a)

Hydrogen Bond

b)

London Dispersion Force

c)

Dipole-Dipole Forces

d)

Covalent Bond

175.

What type of force is labeled as "1" in the following picture? (choose the best answer)

a)

London Dispersion

b)

Dipole-Dipole

c)

Hydrogen Bond

d)

Ion-Dipole

176.

True or False: Intermolecular forces are weaker than intramolecular forces

a)

True

b)

False

177.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, hydrogen bonding

b)

hydrogen bonding, london dispersion

c)

ion-dipole, london dispersion

178.

 Which of these has ONLY London forces?

a)

I2 (nonpolar)

b)

NH3 (polar)

c)

OCl2 (polar)

d)

HCl (polar)

179.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

180.

Intermolecular forces for: NH3

a)

dispersion forces only

b)

dispersion forces and hydrogen bonding

c)

dispersion forces, dipole-dipole forces, and hydrogen bonding

d)

hydrogen bonding only

181.

Intermolecular force(s) present in HCl?

a)

dispersion forces and dipole-dipole forces

b)

dispersion forces only

c)

hydrogen bonding only

d)

dispersion forces, dipole-dipole forces, and hydrogen bonding

182.

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

183.

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

a)

higher

b)

lower

184.

Intermolecular forces for: CO2

a)

Dispersion Force only

b)

dispersion forces and dipole-dipole forces

c)

dipole-dipole forces only

d)

dispersion forces, dipole-dipole forces and hydrogen bonding

185.

Intermolecular force due to the formation of temporary dipole moments in molecules.

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

186.

Intermolecular force resulting from the attraction of partial positive and negative charges on polar molecules.

a)

dispersion force

b)

dipole-dipole force

c)

hydrogen bonding

187.

Intermolecular force resulting from the interaction of a large partial positive charge on a hydrogen that is attached to a N, O, or F atom with a lone pair of electrons on a nearby N, O, F atom.

a)

dispersion force

b)

dipole-dipole force

c)

hydrogen bonding

188.
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.
189.

Which inter-molecular force of attraction is responsible for the chemical bonding formed by AlCl3?

a)

Dispersion force

b)

Ion-dipole

c)

Hydrogen bonding

d)

Metallic bonding

190.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
191.

Define electronegativity.

a)

Ability of atom,ion or molecules to attract electron

b)

Ability of atom,ion or molecule to donate electron

192.

What could make London Dispersion Forces stronger?

a)

Heating up the molecules

b)

Heavier molecules

c)

Molecules with more electrons

193.

Which of these forces is always the strongest?

a)

Hydrogen bonds

b)

Dipole Dipole force

c)

London Dispersion force

d)

Ionic bonds

194.
The bond formed between atoms of the same element:
a)
nonpolar covalent
b)
polar covalent
c)
ionic bond
d)
hydrogen bond
195.

What type of bond only conducts electricity when dissolved in water?

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Hydrogen Bond

196.

What type of bond conducts electricity as a solid?

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Hydrogen Bond

197.

What type of bond does not conduct electricity as a solid or when dissolved in water?

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Hydrogen Bond

198.

What type of bond conducts electricity as a solid?

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Hydrogen Bond

199.

What type of bond only conducts electricity when dissolved in water?

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Hydrogen Bond

200.

What type of bond does not conduct electricity as a solid or when dissolved in water?

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Hydrogen Bond

201.

The image shows what type of compound?

a)

Ionic compound due to the alternating positive and negative ions in a crystalline structure

b)

Metallic compound due to the sea of electrons

c)

Covalent Compound due to the alternating positive and negatively charged ions

202.

The image shows what type of compound?

a)

Ionic compound due to the alternating positive and negative ions in a crystalline structure

b)

Metallic compound due to the sea of electrons

c)

Covalent Compound due to the alternating positive and negatively charged ions

203.

Which of the images shows a mixture?

a)

Left

b)

Middle

c)

Right

204.

The image shows which of the following

a)

Mixture

b)

Pure Substance

c)

Compound

205.

The image shows which of the following?

a)

Pure Substance

b)

Compound

c)

Mixture

206.

If two elements have similar electronegativities they bond will be ________

a)

Ionic

b)

Metallic

c)

Nonpolar Covalent

d)

Polar Covalent

207.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

208.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

209.

The more electrons present, the stronger the london dispersion forces

a)

True

b)

False

210.

Which has stronger london dispersion forces?

a)

F2F_2

b)

Cl2Cl_2

211.

When changing states between solid, liquid, and gas molecules break apart into their respective elements

a)

True

b)

False

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