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Unit 4- Chemical Bonding Unit Review

Total questions: 187

Worksheet time: 3hrs 18mins

Name
Class
Date
1.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

2.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

3.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

4.

Which of these is incorrect?

a)
b)
5.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

6.

What are the elements (Be, Mg, Ca,...) in Group 2 called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble Gases

7.

Elements that have atoms with full valence shells in the ground state are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

8.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
9.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
10.

This could be the dot diagram of an element with the atomic number

a)

8

b)

31

c)

19

d)

36

11.
How do positive ions form?
a)
by gaining electrons
b)
getting compliments
c)
by losing electrons
d)
gaining more protons
12.

Which of these is correct?

a)
b)
c)
13.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
14.

Valence electrons are the

a)

outer most electrons in an atom

b)

total electrons in an atom

15.

The _____ the element is in determines the number of valence electrons it has.

a)

period/row

b)

group/column

16.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

17.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

18.

How many valence electrons does Hydrogen have?

a)

4

b)

1

c)

8

d)

2

19.

How many valence electrons should Magnesium have in its electron dot diagram?

a)

1

b)

2

c)

3

d)

4

20.

How many valence electrons does potassium have?

a)

19

b)

6

c)

39

d)

1

21.

How many valence electrons does Carbon have?

a)

4

b)

6

c)

14

d)

12

22.

What is the "magic number" of valence electrons for atoms to be stable?

a)

1

b)

2

c)

8

d)

18

23.

Neon is a noble gas because it is stable, nonreactive, and has ___ valence electrons.

a)

1

b)

8

c)

10

d)

4

24.

Two objects that are similarly charged will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

25.

A positively charged object and a neutral object will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

26.

A negatively charged object and a neutral object will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

27.

An object becomes positively charged by...

a)

gaining negative charges.

b)

losing negative charges.

c)

gaining positive charges.

d)

losing positive charged.

28.

An object becomes negatively charged by...

a)

gaining negative charges.

b)

losing negative charges.

c)

gaining positive charges.

d)

losing positive charged.

29.

Metal atoms are most likely to form...

a)

positively charged cations.

b)

negatively charged anions.

c)

neutral molecules.

d)

bations.

30.

Non-Metal atoms are most likely to form...

a)

positively charged cations.

b)

negatively charged anions.

c)

neutral molecules.

d)

bations.

31.

Atoms from group 2 on the Periodic Table are likely to form ions of what charge?

a)

+1

b)

+2

c)

0

d)

−1

e)

−2

32.

The Lewis Dot structure for aluminum would have ______ electrons.

a)

13

b)

3

c)

8

d)

27

33.

Valence electrons are those that are

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

in the outermost energy level of the atom.

d)

unable to become involved in chemical bonding.

34.

Which of the following is not a way that ions can form?

a)

gaining electrons

b)

gaining protons

c)

losing electrons

d)

All of the above are ways that ions can form.

35.

Oxygen has six valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

36.

Which of the following best describes the correct arrangement of the electrons in a Lewis dot structure for phosphorus?

a)

five single electrons

b)

two pairs of electrons and one single electron

c)

three pairs of electrons and one single electron

d)

three single electrons and one pair of electrons

37.

Atoms and ions that are isoelectronic have

a)

the same charge.

b)

the same number of electrons.

c)

the same number of protons.

d)

no charge since the number of protons and electrons is equal.

38.

Atoms and ions that are isoelectronic have

a)

the same charge.

b)

the same number of electrons.

c)

the same number of protons.

d)

no charge since the number of protons and electrons is equal.

39.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

40.

Atoms that have gained electrons form

a)

cations.

b)

anions.

c)

negions.

d)

positrons.

41.

Most elements are most stable when their outermost energy levels contain ________ electrons.

a)

2

b)

6

c)

8

d)

18

42.

Look at the Periodic table. Which of the following elements would you expect to form an ion that has the same charge as the oxide ion?

a)

calcium

b)

boron

c)

sulfur

d)

chlorine

43.

Which of the following pairs of atoms and/or ions is isoelectronic?

a)

Na and K

b)

Cl and Cl-1

c)

Ne and Na+1

d)

O-2 and S-2

44.

Which of the following elements is an exception to the octet rule?

a)

helium

b)

oxygen

c)

chlorine

d)

magnesium

45.

Which of the following tend to gain electrons when forming ions?

a)

metalloids

b)

metals

c)

nonmetals

d)

cations

46.

Anions have

a)

gained electrons.

b)

lost electrons.

c)

gained protons.

d)

lost protons.

47.

Which of the following groups on the Periodic Table will only form ions with positive charges?

a)

Group 2

b)

Group 15

c)

Group 17

d)

Group 18

48.
Name the following compound; ScCl2
a)
sulfur dichloride
b)
scandium chloride
c)
scandium (II) chloride
d)
scandium dichloride
49.
Which formula correctly represents aluminum phosphate?
a)
AlPO4
b)
AlSO4
c)
AlP
d)
AlPO3
50.
Gallium sulfate has which of the following formulas?
a)
Ga2S3
b)
Ga3(SO4)2
c)
Ge2(SO4)3
d)
Ga2(SO4)3
51.
Which of the following is the metallic ion in copper (II) chloride?
a)
Cu2+
b)
Cu2-
c)
Co2-
d)
Cl2+
52.
What is the name of the following compound; FeCrO4?
a)
iron chromate
b)
iron dichromate
c)
iron (II) chromate
d)
Iron (II) dichromate
53.
CaCO3 is represented best by which name?
a)
calcium bicarbonate
b)
carbonic acid
c)
calcium carbon trioxide
d)
calcium carbonate
54.
NiSO4 is known as-
a)
nickel (II) sulfate
b)
nickel (II) sulfite
c)
nickel (II) sulfide
d)
nickel sodium tetraoxide
55.
The correct chemical name for water is-
a)
dihydrogen monoxide
b)
hydrogen hydroxide
c)
hydrogen peroxide
d)
H2O
56.
What is the formula for Tin (IV) carbide?
a)
S2C
b)
S4C2
c)
TiC
d)
SnC
57.
What is the name of the compound with the formula; Ba(NO3)2?
a)
Barium nitrate
b)
Barium nitrite
c)
Barium nitride
d)
barium dinitrate
58.
What is the NAME of....
Na2S
a)
sodium (II) sulfide
b)
sodium sulfide
c)
disodium sulfide
d)
sodium sulfur
59.
What is the NAME of....
Mg3N2
a)
magnesium (III) nitride
b)
magnesium (II) nitride
c)
magnesium (II) nitrogen
d)
magnesium nitride
60.
What is the NAME of...
CrN
a)
chromium (II) nitride
b)
chromium (III) nitride
c)
chromium nitride
d)
chromium (I) nitride
61.
What is the NAME of...
PtO2
a)
platinum (II) oxide
b)
platinum (IV) oxide
c)
platinum oxide
d)
platinum (I) oxide
62.
What is the NAME of...
FeP
a)
Iron (II) phosphide
b)
Iron phosphide
c)
Iron (III) phosphide
d)
Iron (III) phosphorus
63.
What is the FORMULA for...
calcium arsenide
a)
Ca3As2
b)
CaAs2
c)
Ca3As
d)
Ca3Ar2
64.
What is the FORMULA for....
beryllium iodide
a)
Be2I
b)
BeI
c)
BeI2
d)
BI2
65.
The name of the compound NH4F is
a)
Nitrogen hydrogen fluorine
b)
Ammonium Fluoride
c)
Ammonia Fluoride
d)
Nitrogen tetrahydride fluoride
66.
The name of Al₂(SO₄)₃ is
a)
aluminum sulfur oxide
b)
aluminum sulfate
c)
aluminum trisulfate
d)
aluminum (III) sulfate
67.
The name of Ca₃(PO₄)₂ is
a)
calcium phosphide oxide
b)
calcium phosphate
c)
tricalcium diphosphate
d)
carbon phosphate
68.
The name of Fe(OH)₂ is
a)
iron oxide
b)
iron hydroxide
c)
iron (II) hydroxide
d)
iron dihydroxide
69.
The chemical formula of sodium sulfate is
a)
S₂SO₄
b)
NaSO₂
c)
NaSO₄
d)
Na₂SO₄
70.
What is the formula for tin (II) nitride?
a)
Sn3N2
b)
SnN2
c)
Sn3N
d)
SnN
71.
What is the formula for Magnesium Carbonate?
a)
MgCO3
b)
Mg(CO3)2
c)
Mg2CO6
d)
Mg2CO3
72.
What is the chemical name for Fe(NO3)3?
a)
Iron (III) Nitrate
b)
Iron (III) Nitride
c)
Iron (II) Nitrate
d)
Iron (III) Nitride
73.
Which of the following combination is incorrect?
a)
phosphate  PO43-                 

b)
sulfite  SO32-                 
c)
nitrite    NO3-   
d)
iron(II)    Fe2+                   
74.
The charge on a barium ion in its ionic compounds is
a)
1+
b)
2+
c)
3+
d)
4+
75.
The polyatomic ion:  SO42- has the name
a)
Phosphate
b)
Sulfate
c)
Sulfite
d)
Sulfur tetra oxide
76.
Fe+3 combines with S-2 to form 
a)
Fe+4(S)=3
b)
Fe2S4
c)
Fe2S3
d)
Fe3S2
77.
What formula results when Fe+3 and CO3-2 ions bond?
a)
FeCO3
b)
Fe2CO3
c)
Fe2(CO3)3
d)
Fe3(CO3)2
78.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
79.
A covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
80.

tetra

a)

six

b)

Four

c)

Five

d)

seven

81.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
82.
What is the name of the molecular geometry for this Lewis Structure?
a)
trigonal planar
b)
trigonal pyramidal
c)
tetrahedral
d)
bent
83.
How would you describe this structure?
a)
nonpolar and London forces
b)
polar and dipole-dipole forces
c)
polar and hydrogen bonding forces
d)
nonpolar and hydrogen bonding forces
84.
What is the name of this Lewis Structure?
a)
linear
b)
bent
c)
tetrahedral
d)
planar
85.
How would you describe this picture
a)
polar and London forces
b)
nonpolar and dipole-dipole
c)
nonpolar and London Forces
d)
polar and Hydrogen bonding
86.

How many electrons can be used in the Lewis Structure for : NO3 -

a)

23

b)

20

c)

18

d)

24

87.

Which compound would have a high melting point?

a)

CaCl2

b)

CO2

c)

PI3

d)

SO3

88.
Which substance would be a poor conductor?
a)
NaCl (s)
b)
CO
c)
Both CO and NaCl(s)
d)
NaCl(aq)
89.
Which substance would be polar?
a)
O2
b)
HCl
c)
CO2
d)
CH4
90.
Which substance is nonpolar?
a)
water
b)
N2
c)
NH3
d)
HCl
91.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal pyramidal
92.
What is the shape of this molecule?
a)
Linear
b)
bent
c)
tetrahedral
d)
trigonal planar
93.
What is the shape of this molecule?
a)
linear
b)
bent
c)
triognal planar
d)
tetrahedral
94.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
tetrahedral
d)
Trigonal Pyramidal
95.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
96.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Planar
97.

Which of the following is the correct Lewis diagram for the fluorine molecule, F2?

a)
b)
c)
d)
98.

Which of the following is the correct Lewis diagram for ammonia, NH3?

a)
b)
c)
d)
99.

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

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

100.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

101.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

102.
How do you determine the number of valence electrons an element has?
a)
Look at its period
b)
Look at its group
c)
Look at its atomic number
d)
Look at its atomic mass
103.

Classify the following molecule.

a)

polar

b)

nonpolar

104.

Classify the following molecule.

a)

polar

b)

nonpolar

105.

Classify the following molecule.

a)

polar

b)

nonpolar

106.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

107.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

108.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

109.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

110.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

111.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

112.

Classify the following molecule.

a)

polar

b)

nonpolar

113.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

114.
HCl
a)
Polar 
b)
Nonpolar 
115.
F2
a)
Polar 
b)
Nonpolar 
116.
H2O
a)
Polar 
b)
Nonpolar 
117.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
118.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
119.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
120.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
121.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
122.
What is Sulfur Trichloride?
a)
SCl3
b)
SiCl3
c)
SCl4
d)
Si3Cl
123.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
124.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
125.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
126.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
127.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
128.
A covalent compound made of one sulfur and two oxygen atoms would be named
a)
sulfur dioxide.
b)
sulfur oxide.
c)
disulfur oxide.
d)
sulfide oxygen.
129.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
130.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
131.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
132.
Bromine monofluoride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
133.

What is the name of the compound H2SH_2S  ?

(a)  

134.

What is the name of the compound SF6SF_6  ?

(a)  

135.

What is the name of the compound H2CO3H_2CO_3  ?

(a)  

136.

What is the name of the compound (NH4)2SO4\left(NH_4\right)_2SO_4  ?

(a)  

137.

What is the chemical formula of calcium carbide?

a)

CaCCaC  

b)

CaC2CaC_2  

c)

Ca2CCa_2C  

d)

Ca2C4Ca_2C_4  

138.

What is the correct formula for the compound Tin (IV) oxide?

a)

SnO2SnO_2  

b)

SnOSnO  

c)

SnO4SnO_4  

d)

Sn2OSn_2O  

139.

What is the chemical formula of Tetraphosphorous nonasulfide?

a)

P4S8P_4S_8  

b)

P4S7P_4S_7  

c)

P4S10P_4S_{10}  

d)

P4S9P_4S_9  

140.

When metals bond with non-metals they form what type of bonds

a)

covalent

b)

ionic

141.

Which of the following anions is polyatomic?

a)

Hydride

b)

Fluoride

c)

Cyanide

d)

Iodide

142.

What is the charge of copper in the compound: CuBr2CuBr_2  ?

a)

+1

b)

-1

c)

+2

d)

-2

143.

What is the charge of barium in the compound: BaCrO4BaCrO_4  ?

a)

+1

b)

+2

c)

+3

d)

+4

144.

When naming compounds that contain a nonmetal bonded to a nonmetal, _____ must be used.

a)

ionic charges

b)

Parentheses

c)

Lewis structure

d)

Greek prefixes

145.

For monoatomic anions, the name of the element is modified by the suffix ____

a)

-ide

b)

-ic

c)

-ite

d)

-ate

146.

The net charge of an ionic compound must be _____

a)

1

b)

0

c)

3

d)

2

147.
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.
148.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
149.
Does H2O have hydrogen bonding?
a)
yes
b)
no
150.
Does HF have hydrogen bonding?
a)
yes
b)
no
151.
Does HCl have hydrogen bonding?
a)
yes
b)
no
152.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
153.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
154.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
155.
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
156.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

157.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

158.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

159.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

160.
Determine the type of intermolecular force present in SiO2.
a)
dipole dipole
b)
dispersion
c)
ionic
d)
covalent network
161.
Which is the strongest intermolecular force below"
a)
Ionic
b)
Dispersion
c)
Hydrogen
d)
Metallic
162.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
163.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
164.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
165.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
166.
Which of the following molecules contains only London dispersion forces?
a)
CF4
b)
HCl
c)
H2O
d)
MgO(aq)
167.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
168.
Which of the following molecules would have the lowest boiling point?
a)
CH4
b)
C2H6
c)
C3H8
d)
C4H10
169.
Propane is a gas at STP, while bromine is a liquid at STP. Which statement correctly explains these observations?
a)
Bromine has weaker intermolecular forces than propane does
b)
Bromine has greater molecular polarity than propane does
c)
Bromine has weaker molecular polarity than propane does
d)
Bromine has stronger intermolecular forces than propane does
170.
Which of the following molecules has hydrogen bonding?
a)
HCl
b)
HI
c)
HF
d)
HBr
171.
Which of the following statements correctly compares the behavior of a mixture of ethanol and water at STP?
a)
Water will evaporate first, because it has weaker intermolecular forces
b)
Ethanol will evaporate first, because it has weaker intermolecular forces
c)
Ethanol and water will evaporate simultaneously
d)
The aqueous solution will evaporate partially at a temperature between the boiling points of water and of ethanol
172.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
173.
HCl and F2 both have a molecular mass of approximately 36 g/mol. Based on IMF, which will have a lower boiling point?
a)
HCl
b)
F2
174.
Hydrogen bonds are a form of bonding.
a)
True 
b)
False
175.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
176.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
177.
If a liquid has high viscosity, it probably has:
a)
strong IMF
b)
weak IMF
178.
The strength of temporary dipoles:
a)
increases with the size of molecules
b)
is greater than intremolecular forces
c)
is the strongest intermolecular force
179.
The force of attraction between nonpolar molecules:
a)
Hydrogen Bonding
b)
Dipole - Dipole Forces
c)
LDF
d)
Ionic Forces
180.

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

181.

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

182.

Which state of matter has a high density and an indefinite shape?

a)

solids

b)

liquids

c)

gases

d)

both solids and liquids

183.

The tendency of a liquid to minimize its surface area is called:

a)

capillary action.

b)

viscosity.

c)

surface tension.

d)

vaporization.

184.

The measure of the resistance to the flow of a liquid is called:

a)

vapor pressure.

b)

sublimation.

c)

viscosity.

d)

condensation.

185.

Which intermolecular force is present in all molecules and atoms?

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

186.

Select all the physical properties true for ionic compounds.

a)

high melting and boiling points

b)

low melting and boiling points

c)

can dissolve in water

d)

cannot dissolve in water

e)

can dissolve in organic solvents

187.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)

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