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Liquids and Theories of Covalent Bonding

Total questions: 126

Worksheet time: 42mins

Name
Class
Date
1.

What are the two main types of intermolecular forces?

a)

Ionic and covalent forces

b)

London dispersion forces and dipole-dipole forces

c)

Hydrogen bonding and adhesion

d)

Surface tension and viscosity

2.

Which type of intermolecular force is the weakest?

a)

Ionic forces

b)

Covalent forces

c)

London dispersion forces

d)

Hydrogen bonding

3.

What is the main factor that determines the phase of a substance?

a)

Density

b)

Viscosity

c)

Kinetic energy

d)

Surface tension

4.

Which substance is an example of a non-polar molecule?

a)

Water

b)

Carbon dioxide

c)

Hydrogen bromide

d)

Glycerol

5.

What is the effect of cohesion in liquids?

a)

Resistance to flow

b)

Capillary action

c)

Surface tension

d)

Viscosity

6.

Which type of intermolecular force is responsible for the unique properties of water?

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonding

d)

Adhesion

7.

What is the term for the attraction of molecules in a liquid to the container?

a)

Cohesion

b)

Viscosity

c)

Adhesion

d)

Surface tension

8.

What is the term for the resistance of a liquid to flow?

a)

Cohesion

b)

Viscosity

c)

Adhesion

d)

Surface tension

9.

What is the effect of surface tension in liquids?

a)

Resistance to flow

b)

Capillary action

c)

Viscosity

d)

Formation of a spherical shape

10.

Which substance is an example of a liquid at room temperature?

a)

Bromine

b)

Mercury

c)

Diamond

d)

Methane

11.

What is the effect of boiling point on intermolecular forces?

a)

The boiling point is inversely proportional to intermolecular forces.

b)

The boiling point increases with stronger intermolecular forces.

c)

The boiling point is not affected by intermolecular forces.

d)

The boiling point decreases with stronger intermolecular forces.

12.

Which type of intermolecular force is responsible for the high boiling point of water?

a)

Ionic bonding

b)

Hydrogen bonding

c)

London dispersion forces

d)

Dipole-dipole interactions

13.

What is the term for the process of a liquid turning into a gas?

a)

condensation

b)

sublimation

c)

melting

d)

evaporation

14.

Which substance is an example of a polar molecule?

a)

Methane

b)

Water

c)

Carbon dioxide

d)

Oxygen

15.

What is the term for the attraction of molecules in a liquid to each other?

a)

cohesion

b)

repulsion

c)

adhesion

d)

dispersion

16.

What do you mean by PROPERTIES of LIQUIDS?

a)

The attraction between water molecules at the surface of water

b)

The process in which a substance changes from its liquid to gas

c)

The measure of a fluid’s resistance to flow

d)

The ability of a substance to dissolve in a given amount of solvent at a specified temperature

17.

What do you mean by VAPORIZATION?

a)

The attraction between water molecules at the surface of water

b)

The process in which a substance changes from its liquid to gas

c)

The ability of a substance to dissolve in a given amount of solvent at a specified temperature

d)

The measure of a fluid’s resistance to flow

18.

Which will exert a higher vapor pressure? Why?

a)

Acetone - because it has a lower molar heat of vaporization

b)

Water - because it has a higher boiling point

c)

Acetone - because it has a higher molar heat of vaporization

d)

Water - because it has a lower boiling point

19.

What are the factors affecting the rate of vaporization?

a)

Viscosity and boiling point

b)

Surface tension and molar heat of vaporization

c)

Pressure and solubility

d)

Temperature and intermolecular forces

20.

What is the measure of how much energy it takes to make a liquid boil and turn into a gas?

a)

Vapor pressure

b)

Viscosity

c)

Molar heat of vaporization

d)

Surface tension

21.

What is the temperature at which a liquid turns into a gas?

a)

Boiling point

b)

Surface tension

c)

Molar heat of vaporization

d)

Viscosity

22.

What refers to the gas form of a substance that is usually a liquid or solid at room temperature?

a)

Vaporization

b)

Solubility

c)

Boiling point

d)

Vapor pressure

23.

What is the measure of a fluid’s resistance to flow?

a)

Surface tension

b)

Molar heat of vaporization

c)

Viscosity

d)

Vapor pressure

24.

What is the ability of a substance to dissolve in a given amount of solvent at a specified temperature?

a)

Miscibility

b)

Vaporization

c)

Boiling point

d)

Solubility

25.

What is the attraction between like molecules?

a)

Viscosity

b)

Adhesion

c)

Cohesion

d)

Surface tension

26.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-dipole interactions

c)

ion-ion attractions

d)

London dispersion forces

27.

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

28.

The weaker the intermolecular forces of a substance the (a)   the boiling point

29.

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

a)

intramolecular forces

b)

polar covalent bonds

c)

metallic bonds

d)

intermolecular forces

30.

Water and ammonia molecules are roughly the same size and the same mass but ammonia boils at -28°F and water boils at 212°F. What can we conclude about the intermolecular forces between water and ammonia?

a)

The intermolecular forces are the same strength

b)

Ammonia has stronger intermolecular forces

c)

Water has stronger intermolecular forces

d)

Not enough information is given

31.

This refers to the surface film on the surface of the liquid caused by the attraction of particles.

a)

Specific heat

b)

Surface tension

c)

Density

d)

Volatility

32.

Higher IMF means (a)   Viscosity.

33.

A substance with a high vapor pressure have _______ intermolecular forces?

a)

weak

b)

strong

34.

As the temperature of a liquid increases, the viscosity

a)

Increases

b)

Doesn't change

c)

Not enough information

d)

Decreases

35.

These are forces between liquid molecules and another substance.


a)

adhesive forces

b)

cohesive forces

c)

coercive forces

d)

adversive forces

36.

The ascension of liquids through slim tube, cylinder or permeable substance due to adhesive and cohesive forces interacting between the liquid and the surface is called_____.

a)

capillarity

b)

surface tension

c)

cohesion

d)

adhesion

37.

Which of the following will take the longest to evaporate?

a)

CH3CH2OH

b)

CH3OH

c)

CH3CH2CH2OH

38.

The temperature at which its vapor pressure equals atmospheric pressure.

a)

specific heat

b)

molar heat of fusion

c)

vapor pressure

d)

boiling point

39.

Which of the following would best remove Sharpie marker from your wall if this marker is known to be non-water soluble. 


a)

acetone (nail polish remover)

b)

salt water

c)

ammonia (nitrogen trihydride)

d)

distilled water

40.

Cohesive forces

a)

Are the attraction of molecules to the container walls

b)

Are only present when the liquid is exposed to glue

c)

Are the attraction of molecules within a liquid

d)

Are important for upward movement in capillary action

41.

the interactive force that exist between water molecules and sides of a graduated cylinder is______.

a)

adhesion

b)

capillarity

c)

cohesion

d)

IMF

42.

The temperature at which its vapor pressure equals atmospheric pressure.

a)

specific heat

b)

vapor pressure

c)

molar heat of fusion

d)

boiling point

43.

The ascension of liquids through slim tube, cylinder or permeable substance due to adhesive and cohesive forces interacting between the liquid and the surface is called_____.

a)

surface tension

b)

cohesion

c)

capillarity

d)

adhesion

44.

Cohesive forces

a)

Are the attraction of molecules within a liquid

b)

Are only present when the liquid is exposed to glue

c)

Are the attraction of molecules to the container walls

d)

Are important for upward movement in capillary action

45.

Capillary action is

a)

Caused by cohesive and adhesive forces

b)

Not observed in liquid mercury

c)

Allows some liquids to 'flow' vertically up a thin tube

d)

All of the above

46.

A substance with a high vapor pressure have _______ intermolecular forces?

a)

strong

b)

weak

47.

A substance with a high amount of intermolecular forces will have a ______ vapour pressure.

a)

high

b)

low

48.

Water droplets are mainly formed by what force?

a)

Viscosity

b)

Van der Waals forces

c)

Hydrogen Bonding

d)

Dipole-Dipole interactions

49.

As the temperature of a liquid increases, the viscosity

a)

Increases

b)

Decreases

c)

Doesn't change

d)

Not enough information

50.

Which of the following is NOT a property of a liquid

a)

surface tension

b)

capillary action

c)

viscosity

d)

polar

51.

Property of liquid to resist an external force and thus assume a lesser surface area.

a)

Surface Tension

b)

Viscosity

c)

Vapor Pressure

d)

Boiling Point

52.

The resistance of a liquid to flow. It is loosely referred to as the thickness or thinness of a liquid

a)

Surface Tension

b)

Viscosity

c)

Vapor Pressure

d)

Boiling Point

53.

Is the pressure exerted by its vapor when in equilibrium with its liquid or solid

a)

Surface Tension

b)

Viscosity

c)

Vapor Pressure

d)

Boiling Point

54.

Is the temperature at which its vapor pressure is equal to the external or atmospheric pressure

a)

Surface Tension

b)

Viscosity

c)

Vapor Pressure

d)

Boiling Point

55.

Is the amount of heat required to vaporize one mole of a substance at its boiling point.

a)

Heat of Vaporization

b)

Amorphous Solids

c)

Crystalline Solids

d)

Heat of Fusion

56.

The amount of heat needed for the solid-state change into liquid state.

a)

Heat of Vaporization

b)

Amorphous Solids

c)

Crystalline Solids

d)

Heat of Fusion

57.

Have considerable disorder in their structure

a)

Heat of Vaporization

b)

Amorphous Solids

c)

Crystalline Solids

d)

Heat of Fusion

58.

The type of solid that has a highly arrangement of particles.

a)

Heat of Vaporization

b)

Amorphous Solids

c)

Crystalline Solids

d)

Heat of Fusion

59.

The substance changes from liquid to solid

a)

Freezing

b)

Melting

c)

Condensation

d)

Vaporization

60.

The substance changes from solid to liquid

a)

Freezing

b)

Melting

c)

Condensation

d)

Vaporization

61.

The substance changes from a gas to a liquid

a)

Freezing

b)

Melting

c)

Condensation

d)

Vaporization

62.

It is a boiling point or the substance changes from a liquid to a gas

a)

Freezing

b)

Melting

c)

Condensation

d)

Vaporization

63.

The substance changes directly from a solid to a gas without going through the liquid phase

a)

Sublimation

b)

Deposition

c)

Equilibrium

d)

Critical Point

64.

The substance changes directly from a gas to a solid without going through the liquid phase

a)

Sublimation

b)

Deposition

c)

Equilibrium

d)

Critical Point

65.

Triple point

a)

Sublimation

b)

Deposition

c)

Equilibrium

d)

Critical Point

66.

When the gas can’t be liquified, some will be stay as gas

a)

Sublimation

b)

Deposition

c)

Equilibrium

d)

Critical Point

67.

Which type of bond forms when valence electrons are traded?

a)

ionic

b)

covalent

c)

metallic

68.

Which type of bond is described as a "sea of electrons" floating on the surface of the material?

a)

ionic

b)

covalent

c)

metallic

69.

Which type of elements tend to lose electrons when forming bonds?

a)

metalloids

b)

metals

c)

nonmetals

d)

noble gases

70.

Which type of elements is unlikely to form a bond of any kind?

a)

metalloids

b)

nonmetals

c)

metals

d)

noble gases

71.

Which type of compound dissolves easily in water?

a)

ionic compound

b)

covalent compound

c)

metallic compound

72.

Covalent bonds occur between....

a)

Metals

b)

Metalloids

c)

Non-metals

d)

Actinide

73.

Covalent bonds occur when.....

a)

Atoms share valence electrons

b)

Atoms transfer valence electrons

c)

Atoms lose electrons and become ions

d)

Atoms dance to the Macarena

74.

What type of covalent bond is characterized by an unequal sharing of electrons?

a)

Ionic Bond

b)

Polar Covalent Bond

c)

Non-Polar Covalent Bond

d)

Covalent Bond

75.

What type of covalent bond is characterized by an equal sharing of electrons

a)

Non-Polar Covalent Bond

b)

Covalent Bond

c)

Ionic Bond

d)

Polar Covalent Bond

76.
 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
77.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
78.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
79.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
80.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
81.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
82.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
83.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
84.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
85.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

86.
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
a)
True
b)
False
87.
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
88.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
89.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
90.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

91.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
92.

The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons, AB2E2

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

93.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
94.

AB3 is a symbol for molecular shape __________________

a)

Tetrahedral

b)

Linear

c)

Trigonal planar

d)

Trigonal pyramidal

95.

The general formula for TETRAHEDRAL shape is __________

a)

AB2

b)

AB3

c)

AB4

d)

AB

96.

s-s overlap is a _______

a)

undefined

b)

π Bond\pi\ Bond  

97.

px - px overlap (perpendicular to internuclear axis) is a _______

a)

undefined

b)

π Bond\pi\ Bond  

98.

Heitler and London introduced which theory?

a)

VSEPR Theory

b)

Valence Bond Theory

c)

Molecular Orbital Theory

d)

Covalent Theory

99.

s-s overlap is a _______

a)

undefined

b)

π Bond\pi\ Bond  

100.

A π (pi) bond is the result of the

a)

overlap of two s orbitals

b)

overlap of an s orbital and a p orbital

c)

overlap of two p orbitals along their axes

d)

sidewise overlap of two parallel p orbitals

e)

sidewise overlap of two s orbitals

101.

Sigma bonds are formed by

a)

side to side overlap of s orbitals

b)

end to end overlap of s orbitals

c)

side to side overlap of p orbitals

d)

end to end overlap of p orbitals

102.

Greater the overlap of the orbitals, _________________________

a)

lesser the bond strength

b)

greater the bond strength

c)

bond strength remains the same

d)

no bond formation

103.
How many sigma and pi bonds does this have? 
a)
3 sigma and 2 pi
b)
5 sigma and 5 pi
c)
5 sigma and 0 pi
d)
0 sigma and 5 pi
104.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

105.

What is the hybridization of this molecule shown above

a)

sp

b)

sp2

c)

sp3

d)

sp4

106.

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

107.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
108.

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

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

sp3d hybridization

109.
Nitrogen atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
110.

Which sub shell has more stability????

a)

3d

b)

4p

c)

5s

d)

4d

111.

Sigma bond is formed when overlapping takes place along (if z-axis is inter nuclear axis)

a)

x-axis

b)

y-axis

c)

z-axis

d)

All axis

112.

Which Quantum Number is used to describe Sub shell????

a)

n

b)

l

c)

m

d)

s

113.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

114.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
115.

Two atoms form a compound by the attraction between positive and negative charges.

a)

covalent compound

b)

ionic compound

c)

polymer

d)

organic compound

116.

True or False: An ionic bond forms when atoms of a non-metal give up electrons to atoms of a metal

a)

True

b)

False

117.

In all covalent bonds, valence electrons are

a)

lost

b)

gained

c)

shared equally

d)

shared

118.

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

119.

What type of compound is formed when atoms share electrons to have a complete octet?

a)

hydrocarbon

b)

covalent compound

c)

ionic compound

d)

inorganic compound

120.

What is the chemical formula for the ionic compound formed between magnesium and oxygen?

a)

MnO

b)

Mg2O

c)

MgO

d)

MnO2

121.

What is the chemical formula for sodium nitride?

a)

Na3N

b)

NaN3

c)

SN3

d)

S3N

122.

An example of a covalent compound is

a)

sodium floride

b)

calcium chloride

c)

carbon dioxide

d)

all of the above

123.

Identify the following compound as ionic or covalent: Na2SO4

a)

ionic

b)

covalent

124.

Identify the following compound as metallic, ionic or covalent: SO2

a)

ionic

b)

covalent

c)

metallic

125.

Identify the following compound as ionic or covalent: CO

a)

ionic

b)

covalent

126.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline

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