Deck 14: Liquids and Solids

Question 1

When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction?

A) a hydrogen from one molecule and a hydrogen from the other molecule
B) a hydrogen from one molecule and an oxygen from the other molecule
C) an oxygen from one molecule and an oxygen from the other molecule
D) two hydrogens from one molecule and one oxygen from the other molecule
E) two hydrogens from one molecule and one hydrogen from the other molecule

Answer 1

a hydrogen from one molecule and an oxygen from the other molecule

Question 2

The bonding forces that hold the atoms of a molecule together are called intermolecular forces, whereas the forces that occur among molecules that cause them to aggregate to form a solid or a liquid are called intramolecular forces.

Answer 2

False

Question 3

The normal freezing point of water is

A) 0°F
B) 273 K
C) 32°C
D) 373°C
E) none of these

Answer 3

273 K

Question 4

The bonds between hydrogen and oxygen in a water molecule can be characterized as

A) hydrogen bonds.
B) London forces.
C) intermolecular forces.
D) intramolecular forces.
E) dispersion forces.

Question 5

At 1 atm of pressure and a temperature of 0°C, which phase(s) of H₂O can exist?

A) ice and water
B) ice and water vapor
C) water only
D) water vapor only
E) ice only

Question 6

Which of the following has the lowest vapor pressure?

A) H₂O
B) NaCl
C) NH₃
D) O₂
E) CH₄

Question 7

The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 14.7 g of water.

A) 6.02 kJ
B) 4.91 kJ
C) 88.5 kJ
D) 44.0 kJ
E) none of these

Question 8

At 1 atm pressure, liquid water always changes to gaseous water at 100^oC.

Question 9

The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 44.3 g of water.

A) kJ
B) 267 kJ
C) 2.46 kJ
D) 133 kJ
E) 14.8 kJ

Question 10

The molar heats of fusion of water and iodine are 6.02 kJ/mol and 16.7 kJ/mol, respectively. It will take more energy to melt a gram of ice than to melt a gram of solid iodine.

Question 11

Calculate the quantity of energy required to change 7.72 mol of liquid water to steam at 100^oC. The molar heat of vaporization of water is 40.6 kJ/mol.

A) 5.26 kJ
B) 40.6 kJ
C) 313 kJ
D) 77.2 kJ
E) 48.3 kJ

Question 12

The specific heat capacity of liquid water is 4.18 J/g ^oC. Calculate the quantity of energy required to heat 10.4 g of water from 26.5^oC to 83.7^oC.

A) J
B) J
C) 23.9 J
D) J
E) none of these

Question 13

The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 3.13 mol of ice.

A) 1.92 kJ
B) 6.02 kJ
C) 18.8 kJ
D) 339 kJ
E) none of these

Question 14

The specific heat capacity of liquid water is 4.18 J/g ^oC. Calculate the quantity of energy required to heat 1.46 g of water from 26.5^oC to 83.7^oC. (Ignore significant figures for this problem.)

A) 349 J
B) 511 J
C) 162 J
D) 83.5 J
E) 673 J

Question 15

The normal boiling point of water is

A) 0°F
B) 32°F
C) 273 K
D) 373 K
E) none of these

Question 16

Calculate the quantity of energy required to change 22.8 g of liquid water to steam at 100^oC. The molar heat of vaporization of water is 40.6 kJ/mol.

A) 10.1 kJ
B) 51.4 kJ
C) 0.562 kJ
D) 32.1 kJ
E) kJ

Question 17

The freezing point of helium is approximately -270°C. The freezing point of xenon is -112°C. Both of these are in the noble gas family. Which of the following statements is supported by these data?

A) Helium and xenon form highly polar molecules.
B) As the molar mass of the noble gas increases, the freezing point decreases.
C) The London forces between the helium molecules are greater than the London forces between the xenon molecules.
D) The London forces between the helium molecules are less than the London forces between the xenon molecules.
E) none of these

Question 18

More than two-thirds of the earth's surface is covered by water.

Question 19

Choose the state of water in which the water molecules are farthest apart on average.

A) steam (vapor)
B) liquid
C) ice (solid)
D) all the same

Question 20

Which of the following should have the lowest boiling point?

A) CH₄
B) C₂H₆
C) C₃H₈
D) C₄H₁₀
E) C₅H₁₂

Question 21

What is the major attractive force in CO?

A) dipole-dipole
B) London dispersion
C) ionic
D) hydrogen bonding
E) none of these

Question 22

Of the following substances, choose the one with the greatest vapor pressure.

A) He(l)
B) Ne(l)
C) Ar(l)
D) Xe(l)
E) Rn(l)

Question 23

What is the major attractive force in O₂?

A) dipole-dipole
B) London dispersion
C) ionic
D) hydrogen bonding
E) none of these

Question 24

The normal boiling point of liquid W is lower than that of X, which is lower than that of Y. Which of the following is the correct order of increasing vapor pressure of the thee liquids at STP?

A) Y, X, W
B) X, W, Y
C) W, Y, X
D) W, X, Y
E) X, Y, W

Question 25

As the temperature of a liquid increases, the vapor pressure of the liquid generally

A) increases
B) decreases
C) stays the same
D) depends on the type of intermolecular forces

Question 26

What is the major attractive force in K₂O?

A) dipole-dipole
B) London dispersion
C) ionic
D) hydrogen bonding
E) none of these

Question 27

Which of the following is true for ionic solids dissolved in water?

A) The solution will conduct electricity.
B) The solid will dissolve into neutral molecules.
C) The solution will not conduct electricity.
D) The ions in solution will form a large crystal.
E) none of these

Question 28

An alloy has metallic properties.

Question 29

Name the type of crystalline solid formed by sodium chloride.

A) ionic solid
B) molecular solid
C) atomic solid
D) amorphous solid
E) none of these

Question 30

Which of the following has the highest melting temperature?

A) H₂O
B) CO₂
C) S₈
D) MgF₂
E) P₄

Question 31

Rank the following compounds from lowest to highest boiling point. CH₃OH CH₄ H₂O C₂H₆

A) H₂O < CH₃OH < C₂H₆ < CH₄
B) C₂H₆ < CH₄ < CH₃OH < H₂O
C) CH₄ < C₂H₆ < CH₃OH < H₂O
D) CH₄ < C₂H₆ < H₂O < CH₃OH
E) CH₄ < CH₃OH < C₂H₆ < H₂O

Question 32

Consider the following compounds: CO NH₃ CO₂ CH₄ H₂
Which compound has the highest boiling point?

A) CO
B) NH₃
C) CO₂
D) CH₄
E) At least two of the above compounds have equally high boiling points.

Question 33

The P_vap for water at 100.0°C is

A) 85 torr
B) 760 torr
C) 175 torr
D) 1 torr
E) More information is needed.

Question 34

What is the major attractive force in CH₄?

A) dipole-dipole
B) London dispersion
C) ionic
D) hydrogen bonding
E) none of these

Question 35

Name the type of crystalline solid formed by argon.

A) atomic solid
B) molecular solid
C) ionic solid
D) amorphous solid
E) none of these

Question 36

Consider the following compounds: CO NH₃ CO₂ CH₄ H₂
How many of the compounds above exhibit London dispersion forces?

A) 1
B) 2
C) 3
D) 4
E) 5

Question 37

Select the two compounds that are more likely to be a gas at room temperature (as opposed to a liquid).
a.
CH₃OH
b.
CH₄
c.
H₂O
d.
C₂H₆

Question 38

Name the type of crystalline solid formed by SiO₂.

A) molecular solid
B) atomic solid
C) ionic solid
D) amorphous solid
E) none of these

Question 39

Select the two compounds that are more likely to be a liquid at room temperature (as opposed to a gas).
a.
CH₃OH
b.
CH₄
c.
H₂O
d.
C₂H₆