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Review States (IMFs & Solutions)

Total questions: 65

Worksheet time: 11hrs 50mins

Name
Class
Date
1.

Which state of matter have the weakest intermolecular forces (attraction between the different particles)?

a)

solid

b)

liquid

c)

gas

2.

What statement best 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.
3.

All molecules have London forces between them, but some molecules can have additional types of intermolecular forces.  Which of these molecules has ONLY London dispersion forces?

a)

I2

b)
NH3
c)
OCl2
d)
SH2
4.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

5.

What is the strongest intermolecular force for NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

6.

What would be the strongest IMF between 2 of these molecules?

a)

London Dispersion

b)
Dipole
c)
Hydrogen bond
7.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
8.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)

London Dispersion

d)
metallic
9.

H2S has what kind of intermolecular force as its strongest IMF?

a)
dipole dipole
b)

London dispersion

c)
H-bond
d)
ionic
10.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
11.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
12.
Which of the following will take the longest to evaporate?
a)
CH3CH2OH
b)
CH3OH
c)
CH3CH3
13.

Which substance will have the highest vapor pressure?

(HINT High vapor pressure means the substance evaporates easily - like a volatile liquid.)

a)

CH3CH2CH2CH2CH3

b)

H2O

c)

CH4

d)

CH3F

14.

What is the strongest IMF between molecules of this substance?

a)
dispersion forces
b)
dipoles
c)
hydrogen bonding
15.

The strongest intermolecular force for CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

16.

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

17.
Which of the following liquids experiences dipole-dipole intermolecular forces?
a)
H2 (l)
b)
CF4 (l)
c)
SO2 (l)
d)
CCl4 (l)
18.
Which of the following molecules is least soluble in water?
a)
CH2F2
b)
CH3OH
c)
CH2O
d)
CH3CH3
19.
At room temperature, chlorine, Cl2, is a gas.  Which of the following provides a characteristic of chlorine with a correct explanation?
a)

chlorine has a lower boiling point than bromine (which is a liquid at room temperature) because chlorine has fewer polarizable electrons than bromine

b)
chlorine has a lower first ionization energy than argon (an atomic element that is also a gas at room temperature) because elemental chlorine forms molecules whereas elemental argon does not.
c)
chlorine is a not a good conductor of electricity because it has lone pairs of electrons.
d)
chlorine is soluble in water because chlorine is polar.
20.
Based on the information in the table, which liquid has a higher vapor pressure at 25oC and why?
a)
CBr4 (l), because it has weaker intermolecular forces
b)
CBr4 (l), because it has stronger intermolecular forces
c)
CHBr3 (l), because it has weaker intermolecular forces
d)
CHBr3 (l), because it has stronger intermolecular forces
21.

Which of the following would have ion-dipole attractions?

a)
Cl2(aq)
b)
H2O(s)
c)
NaCl(aq)
d)
CaBr2(s)
22.
Which of the following geometries could be nonpolar?
a)
bent
b)
tetrahedral
c)
trigonal pyrimidal
d)
none of the above
23.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
24.

Which of the following liquids experiences dipole-dipole intermolecular forces?

a)

O2(l)

b)

CCl4(l)

c)

SO3(l)

d)

CF2Cl2

25.

Which of the following answer best describes the solubility of pyridine and benzene in water?

a)

Pyridine, a polar molecule, can form strong dipole-dipole interactions with water, another polar molecule. Benzene, a non-polar molecule, cannot form strong intermolecular interactions with water. Therefore, pyridine is soluble in water while benzene is not.

b)

Pyridine, a non-polar molecule, cannot form strong intermolecular interactions with water. Benzene, a polar molecule, can form strong dipole-dipole interactions with water, another polar molecule. Therefore, benzene is soluble in water while pyridine is not.

c)

Pyridine, a non-polar molecule, cannot form strong intermolecular interactions with water. Benzene, a non-polar molecule, cannot form strong intermolecular interactions with water. Therefore, neither pyridine nor benzene are soluble in water.

d)

Pyridine, a polar molecule, can form strong dipole-dipole interactions with water, another polar molecule. Benzene, a polar molecule, can form strong dipole-dipole interactions with water, another polar molecule. Therefore, both pyridine and benzene are soluble in water.

26.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
27.

Which of the following will have the lowest melting point?

a)
b)
c)
d)
28.

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

29.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

The number of electrons shared in the bond

30.

Which of the following molecules would dissolve in oil?

a)

CHCl3

b)

NH3

c)

CCl4

d)

HBr

31.
If a liquid has high viscosity, it probably has:
a)
strong IMF
b)
weak IMF
32.

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

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.

What type of IMF's would occur in between molecules of Carbon Tetrachloride? You can choose more than one answer.

a)

London Dispersion Force (LDF)

b)

Dipole-Dipole

c)

Hydrogen Bond

d)

Ion-Dipole

35.

What type of IMF's would occur in between molecules of Sulfur Dioxide? You can choose more than one answer.

a)

London Dispersion Force (LDF)

b)

Dipole-Dipole

c)

Hydrogen Bond

d)

Ion-Dipole

36.

Which type of IMF's are present between molecules of butanol? Check all that apply

a)

London Dispersion Force (LDF)

b)

Dipole-Dipole

c)

Hydrogen Bonding

d)

Ion Dipole

37.

What type of IMF's are in-between molecules of ethyl acetate? Check all that are correct

a)

London Dispersion Forces (LDF)

b)

Dipole-Dipole

c)

Hydrogen Bonding

d)

Ion Dipole

38.

Which numbered arrow in the image above points to a hydrogen bond?

a)

1

b)

2

c)

3

d)

4

39.

Propane is a gas at room temperature, while bromine is a liquid at room temperature. 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

40.

At 30'C, which substance has the lowest solubility?

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

41.

At which temperature do KBr and KNO3 have the same solubility?

a)

60

b)

55

c)

50

d)

Never

42.

Determine the solubility for the substances at 55'C and arrange them in order from lowest to highest solubility.

a)

NaCl, NH4Cl, KBr, NaNO3

b)

NaCl, NH4Cl, NaNO3, KBr

c)

NH4Cl, NaCl, NaNO3, KBr

d)

NaNO3, KBr, NH4Cl, NaCl

43.

At 10'C, the solubility of NaNO3 is 80 g/100 g of H2O. Based on this information, what would the solubility be in 50 g of H2O.

a)

40

b)

80

c)

160

d)

16

44.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

45.

Identify a method to decrease the dissolving rate of a solution:

a)

decrease the temperature

b)

add KE

c)

stir the solution

d)

increase the temperature

46.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
47.
How many more grams of KNO3 dissolve at 50 ⁰C compared to 0 ⁰C?
a)
85 g
b)
15 g
c)
70 g
d)
100 g
48.

What is the concentration of nitrate ions in a 2.00 M Al(NO3)3 solution?

a)

2.00 M NO3-1

b)

4.00 M NO3-1

c)

6.00 M NO3-1

d)

8.00 M NO3-1

49.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility of the solute in the solvent?

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

50.

What is the molarity of a 0.500L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

51.

What is the molarity of a solution that contains 125 g NaCl in 4.00 L of solution?

a)
0.535 M NaCl
b)
2.14 M NaCl
c)
8.56 M NaCl
d)
31.3 M NaCl
52.

If 400 mL of a 8.0 M solution is diluted to a molarity of 5.3M, about how much solvent volume was added?

a)

200 mL

b)

600 mL

c)

400 mL

d)

180 mL

53.

Ethanol is a polar solvent. Which of the following statements is true?

a)

Water will dissolve into ethanol because water is polar too.

b)

Water will dissolve into ethanol because water is nonpolar.

c)

Oil will dissolve into ethanol because oil is polar too.

d)

Oil will dissolve into ethanol because oil is nonpolar.

54.

Table salt (NaCl) dissolves into water because...

a)

table salt is polar and water is polar too.

b)

table salt is ionic and water is polar.

c)

table salt is nonpolar and water is nonpolar too.

d)

table salt is ionic and water is nonpolar.

55.
chromatography separates the mixture of dyes on the basis of their ----------------------------
a)
density
b)
solubility
c)
gravity
d)
boiling point
56.
The diagram below shows a chromatogram obtained when a sample X was analysed together with four other known dyes P, Q, R and S. Dye Q was known to cause cancer. Which of the following dye(s) is/are safe for use?
a)
P only
b)
S only
c)
P and S
d)
P and X
57.
A student extracts the colour from some green smarties and uses paper chromatography to separate components colours. She finds blue has a Rf =0.38 and yellow Rf =0.75 this suggests 
a)
the yellow is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
b)
the yellow is more strongly adsorbed onto the stationary phase and is more soluble in the mobile phase.
c)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
d)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
58.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
59.
The Rf value  for the red component is 
a)
0.3
b)
0.7
c)
10
d)
7
60.

In paper chromatography, the LEAST soluble solute ____.

a)

does not move from the start point

b)

stays closest to the start point

c)

travels furthest away from the start point

d)

can be found in the middle of the chromatogram

61.

The diagram above represents a particle in aqueous solution. Which of the following statements about the particle is correct? 

a)

The particle must be a cation because the negative end of each water molecule is pointed toward it.

b)

The particle must be an anion because the positive end of each water molecule is pointed toward it. 

c)

The charge of the particle cannot be determined because water molecules  have no net charge.

d)

The charge of the particle cannot be determined because the water molecules are arranged symmetrically and their partial charges cancel. 

62.

A student obtains a mixture of the liquids hexane and octane, which are miscible in all proportions. Which of the following techniques would be best for separating the two components of the mixture, and why?

a)

Filtration, because the different densities of the liquids would allow one to pass through the filter paper while the other would not. 

b)

Paper chromatography, because the liquids would move along the stationary phase at different rates owing to the difference in polarity of their molecules. 

c)

Column chromatography, because the higher molar mass of octane would cause it to move down   the column faster than hexane. 

d)

 Distillation, because the liquids would boil  at different temperatures owing to the difference in strength of their intermolecular forces. 

63.

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

a)

50 ml

b)

1.3 ml

c)

30 ml

d)

130 ml

64.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
65.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M

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