wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

IMF Practice

Total questions: 95

Worksheet time: 57mins

Name
Class
Date
1.

List the strongest to weakest IMFs.

a)

Hydrogen Bond, London Dispersion, Dipole-dipole

b)

London Dispersion, Dipole-dipole,

Hydrogen Bond

c)

Hydrogen Bond, Dipole-dipole, London Dispersion

d)

Dipole-dipole, Hydrogen Bond, London Dispersion

2.

Hydrogen Bond is the strongest because

a)

it is temporary

b)

H only has 1 electron and when shared unequally creates extreme poles

c)

It is permanent

d)

Hydrogen has a very strong electronegativity and pulls on the electrons

3.

A strong IMF increases

a)

boiling point

b)

solubility

c)

flammability

d)

malleability

4.

A weak IMF will result in a

a)

high melting point

b)

high viscosity

c)

high surface tension

d)

low surface tension

5.

A hydrogen bond is a covalent bond. True or False

a)

True

b)

False, because it is ionic

c)

False because it has an intramolecular force

d)

False because it has an intermolecular force

6.

Soap has a polar head and a nonpolar tail.

a)

True

b)

False

7.

For something to be soluble

a)

the solvent IMF must be stronger than the solute IMF

b)

the solvent IMF must be weaker than the solute IMF

c)

both IMFs must be weak

d)

the solute and solvent IMFs must be close to the same strength

8.

The dissolving process is

a)

the IMF broken between the solute and solvent molecules, new IMF formed between solvent and solute, solvent carries solvent particles further apart

b)

the IMF is formed between the solute and solvent creating a new substance

c)

the solvent breaks the bonds of the solute and creates a new bond with the solvent

9.

Why do oil and water not mix?

a)

Water and oil have similar IMF

b)

Water and oil's IMFs are too different in strength.

10.

Why does water bead on a clean window?

a)

Water has a strong IMF ~ high surface tension and stick together and resist spreading out

b)

Water has a weak IMF ~ high surface tension and stick together and resist spreading out

c)

Water has a strong IMF ~ low surface tension and stick together and resist spreading out

d)

Water has a weak IMF ~ weak surface tension and stick together and resist spreading out

11.

How does soap work in cleaning oil?

a)

Soap is nonpolar and interacts with oil.

b)

Soap is polar and with the stronger IMF than oil will wash it away.

c)

The polar head dissolves in water and spreads out the soap surrounding the oil with the nonpolar tail which interacts with soap

d)

Soap is magical!

12.

Predict the substance with the highest melting point (based on IMF)

a)

CO2

b)

AlCl3

c)

C2H6

d)

CH3OH

13.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

14.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

15.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

16.
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
17.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)

HF

b)

Ne

c)

O2

d)

OCl2

18.
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
19.

Type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

20.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

21.

Intermolecular forces for: CO2

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

22.

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

a)

higher

b)

lower

23.

Which molecule: Br2, HCl, H2S, or NH3, will most likely have London dispersion forces as the MOST important IMF considered when determining melting/boiling points?

a)

Br2, it only has dispersion forces when interacting

b)

HCl, it can participate in dipole-dipole interactions and also dispersion forces

c)

H2S, it can participate in dipole-dipole interactions and also dispersion forces

d)

NH3, it can participate in hydrogen bonding and also dispersion forces

24.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

25.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
26.

Which of the following will have the lowest melting point?

a)
b)
c)
d)
27.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
28.

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

29.
Does HF have hydrogen bonding?
a)
yes
b)
no
30.
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
31.

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

32.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
33.

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

34.

Which model represents a LOWER Vapor Pressure?

a)

A

b)

B

35.
Liquids with weak intermolecular forces
a)
contain a lot of kinetic energy
b)
easily evaporate
c)
cannot diffuse
d)
freeze easily
36.

Which model represents STRONGER Intermolecular Forces?

a)

A

b)

B

37.

Which container has the greatest Vapor Pressure

a)

red

b)

yellow

c)

blue

38.

Which container has the greatest Intermolecular Force between Molecules?

a)

red

b)

yellow

c)

blue

39.

Molecules with strong attraction between themselves require __________ to separate than weakly attracted molecules.

a)

More energy

b)

Less energy

c)

No energy

d)

Nuclear energy

40.

Which compound has the strongest IMF

a)

HOH

b)

CH4

c)

C2H6

d)

CH3OH

41.

Which compound has the weakest IMF

a)

C3H8

b)

CH4

c)

C2H6

d)

C4H10

42.

In what situation does DIPOLE -DIPOLE FORCES are stronger?

a)

If two molecules are of comparable size and shape, dipole–dipole interactions will likely be the dominating force.

b)

If one molecule is much larger than another, dipole–dipole interactions will likely be the dominating force.

c)

If positive ends of polar molecules are oriented to negatively charged anions, dipole–dipole interactions will likely be the dominating force.

d)

If negative ends of polar molecules are oriented to positively charged cations, dipole–dipole interactions will likely be the dominating force.

43.

In which situation does DISPERSION FORCES are strongest?

a)

If two molecules are of comparable size and shape, dispersion forces will likely determine its physical properties.

b)

If one molecule is much larger than another, dispersion forces will likely determine its physical properties.

c)

If negative ends of polar molecules are oriented to positively charged cations, dispersion forces will likely determine its physical properties.

d)

If positive ends of polar molecules are oriented to negatively charged anions, dispersion forces will likely determine its physical properties.

44.

Sodium chloride is completely soluble in water. What is responsible

for its solubility in water?

a)

Na+ and Cl- ions are favorable sites for H-bonding to form.

b)

The ions in NaCl participate in ion-induced dipole attractions with

water.

c)

The presence of charged ends in NaCl enables dipole-dipole

interaction with water.

d)

London dispersion forces in NaCl predominate leading to strong

dipole interactions with water.

45.

Xenon has a greater atomic weight than neon. Xe has 131.3 amu while

Ne has 20.2 amu. The boiling points are 166.1K and 27.3K, respectively.

How do intermolecular forces account for the difference?

a)

Dipole- dipole interaction is greater in Xe than Ne so more

energy is needed to break the bonds.

b)

H-bonding is greater for substances with higher atomic weight

so greater energy is needed to change Xe to vapour.

c)

Atomic weight increases the chance of lesser dispersion forces

so greater energy is needed to separate Xe atoms to change to

vapour

d)

London dispersion forces are greater in substances with

heavier atomic weight so greater energy is needed to separate

the atoms of Xe than Ne.

46.

Which statement explains why Br2 is a liquid at STP and I2 is a solid at STP?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar

b)

Molecules of Br2 are nonpolar, and molecules of I2 are polar

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

47.

The force beween MOLECULES of HCl which contains two polar molecules woudl be

a)

dipole-dipole

b)

hydrogen bonding

c)

Van der Waals

d)

Ionic bond

48.

The force between molecules of F2 which is a nonpolar molecule (electrons are shared) would be:

a)

Dipole-Dipole

b)

Hydrogen bonding

c)

Van der Waals

d)

Ionic bond

49.

Identify the IMF exist in CH4

a)

dipole-dipole forces

b)

Van der Waals

c)

ion-dipole forces

d)

hydrogen bonding

50.

Identify the IMF exist in NH3

a)

Van der Waals

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

51.

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

52.

Hydrogen bonding is a special case of __________.

a)

Van der Waals

b)

ion-dipole

c)

dipole-dipole

53.

Which of the following has the lowest boiling point?

a)

PH3

b)

H2O

c)

SiH4

d)

NH3

54.

Does NH3 or PH3 have a higher boiling point?

(Hint: identify the types of IMF's present for each)

a)

NH3 because it has the strongest IMF's

b)

PH3 because it has the strongest IMF's

c)

NH3 because it has the weakest IMF's

d)

PH3 because it has the weakest IMF's

55.

________________ an intermolecular force of attraction that occurs when a

temporary dipole of one atom induces polarity in a neighboring atom. They form due to random fluctuations in the density of the electron cloud surrounding the nucleus. The weakest type of intermolecular force.

a)

Van der Waals

b)

Hydrogen Bonding

c)

Dipole-Dipole

d)

Ionic

56.

Which molecule will have ion-dipole as its strongest type of intermolecular force?

a)
b)
c)
d)
57.

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

58.
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
59.

Does a sample of H2S have hydrogen bonding with another molecule of H2S?

a)

yes

b)

no

60.

How will the following molecule bond with another identical molecule?

a)

London

b)

Dipole-Dipole

c)

Hydrogen bonds

61.
Is the following molecule polar or nonpolar?
a)
Nonpolar
b)
Polar
62.

What intermolecular force is present between two molecules of HCl?

a)

Dipole-Dipole

b)

London

c)

Hydrogen bonds

d)

Ionic

63.

What type of intermolecular force is present between two molecules of HF?

a)

Dipole-Dipole

b)

London

c)

Hydrogen bonds

d)

ionic

64.

Rank these in order of strength (from strongest to weakest):

London forces

hydrogen bond

dipole-dipole attraction

a)

dipole-dipole>hydrogen bond>London

b)

London>dipole-dipole>hydrogen bond

c)

hydrogen bond>dipole-dipole>London

d)

London>hydrogen bond>dipole-dipole

65.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

66.
Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
Cl2
d)
I2
67.

Dipole-dipole forces get stronger as...

a)

the molecule is more polar

b)

the molecule is less polar

c)

the LDF increases

d)

the distance between the molecules increases

68.

Boiling point and melting point _________ as IMFs increase

a)

increase

b)

decrease

c)

do not change

d)

have no connection

69.

Which of these are true for ionic solids?

a)

high melting points

b)

not conductive as a solid

c)

conduct as a liquid or (aq)

d)

conductive as a solid

e)

low melting points

70.

What interaction is occurring in the picture?

a)

Ion-dipole

b)

dipole-dipole

c)

hydrogen bonding

d)

London Dispersion

71.

Which molecule has the highest boiling point (Strongest IMF)

a)
b)
c)
d)

All have same boiling point

72.

Which molecule that has London Dispersion Force has the strongest bond?

a)
b)
c)
d)
73.

Which molecule would have the highest surface tension?

(Think strongest intermolecular force)

a)

CH4CH_4

b)

HBr

c)

HF

d)

NH3NH_3

74.

Which molecule has the strongest London Dispersion Force?

a)
b)
c)
d)

They all have the same force

75.

Why do straighter molecules have higher boiling points?

a)

They don't

b)

They have more places to interact

c)

They are smaller

d)

They can stretch out

76.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

77.

If fluorine is more electronegative then carbon, what charge will the fluorine receive?

a)

negative

b)

slight negative

c)

positive

d)

slight positive

78.

Hydrocarbons such as the one pictured will have which type of intermolecular forces?

a)

Dispersion

b)

dipole

c)

hydrogen bonds

79.

Strongest intermolecular force present in HF.

a)

dipole dipole

b)

dispersion

c)

H-bond

d)

ionic

80.

Strongest intermolecular force in H2S?

a)

dipole dipole

b)

dispersion

c)

H-bond

d)

ionic

81.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
82.

Strongest intermolecular force present in HCl?

a)

dipole dipole

b)

dispersion

c)

H-bond

d)

ionic

83.
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.
84.
Does HCl have hydrogen bonding?
a)
yes
b)
no
85.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
86.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

87.

What is the strongest IMF's that would occur in between molecules of Carbon Tetrachloride?

a)

London Dispersion Force (LDF)

b)

Dipole-Dipole

c)

Hydrogen Bond

d)

Ion-Dipole

88.

What IMF would exist between molecules of BrF5?

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

LDF and Dipole-Dipole Forces

d)

None

89.

Determine the VSEPR shape and intermolecular forces of the given structure.

a)

T-Shape; LDF

b)

T-Shape; LDF and Dipole-Dipole

c)

See Saw; LDF and Dipole-Dipole

d)

See Saw; LDF

90.

Identify the hybridization and IMF of the given structure.

a)

sp3d; LDF

b)

sp3d; LDF and Dipole-Dipole

c)

sp3d2; LDF

d)

sp3d2; LDF and Dipole-Dipole

91.

Determine the VSEPR shape and intermolecular forces that exist between molecules of the given structure.

a)

Square Pyramidal; LDF

b)

Square Pyramidal; LDF and Dipole-Dipole

c)

Octahedral; LDF

d)

Octahedral; LDF and Dipole-Dipole

92.

Which of the following linear molecules would be considered polar?

a)
b)
c)
d)
93.

Which of the following would experience dipole-dipole forces of attraction between molecules?

a)
b)
c)
d)
94.

For which of the following would hydrogen bonding occur between molecules?

a)
b)
c)
d)
95.

Which of the following has T-shape molecular geometry?

a)
b)
c)
d)

Similar Resources on Wayground

100 câu hóa

100 questions

100 câu hóa

quiz

Worksheet

•

11th Grade

HC07 Balancing Reactions

98 questions

HC07 Balancing Reactions

quiz

Worksheet

•

10th Grade

Part C Physical Science EOC Review

100 questions

Part C Physical Science EOC Review

quiz

Worksheet

•

9th - 12th Grade

AP Chemistry Unit 4 Review

100 questions

AP Chemistry Unit 4 Review

quiz

Worksheet

•

11th Grade

PreAP Chem Fall Review

92 questions

PreAP Chem Fall Review

quiz

Worksheet

•

10th - 12th Grade

ALKANE - TỔNG HỢP

100 questions

ALKANE - TỔNG HỢP

quiz

Worksheet

•

11th Grade

Semester 1 Review

100 questions

Semester 1 Review

quiz

Worksheet

•

10th - 12th Grade

Chemistry Final Review

100 questions

Chemistry Final Review

quiz

Worksheet

•

10th Grade