Question 1

Give the coordination number for a body-centred cubic cell.

Accepted Answer

A)   4
B)   6
C)   8
D)   10
E)   12F) None of the above
G) All of the above

Question 2

Which of the following forms an ionic solid?

Accepted Answer

A)   Cr
B)   C4H9NH2
C)   Cs NO3
D)   N O4E) B) and C)
F) A) and C)

Question 3

How much energy is required to vaporize 98.6 g of ethanol (C2H5OH)  at its boiling point if its ΔvapH is 40.5 kJ mol-1?

Accepted Answer

A)   86.7 kJ
B)   11.5 kJ
C)   18.9 kJ
D)   52.8 kJ
E)   39.9 kJF) A) and C)
G) A) and E)

Question 4

Identify the type of solid for argon.

Accepted Answer

A)   metallic atomic solid
B)   ionic solid
C)   nonbonding atomic solid
D)   molecular solid
E)   networking atomic solidF) B) and C)
G) C) and D) C

Question 5

The enthalpy change for converting 1.00 mol of ice at -60.0°C to water at 80.0°C is -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > The specific heats of ice, water, and steam are -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > and -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > respectively. For -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > O, -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > = 6.01 kJ mol-1, and -1, and   . A)  9.77 B)  14.29 C)  8282 D)  13.17 E)  48.95" class="answers-bank-image d-inline" rel="preload" > .

Accepted Answer

A)   9.77
B)   14.29
C)   8282
D)   13.17
E)   48.95F) A) and B)
G) None of the above

Question 6

Describe the difference between the conduction band and the valence band.

Accepted Answer

The valence band is the group of highest...

Question 7

Choose the pair of substances that are most likely to form a homogeneous solution.

Accepted Answer

A)   CCl4 and SCl2
B)   NF3 and SO2
C)   CO and C6H6
D)   NH2CH3 and CH4
E)   None of the pairs above will form a homogeneous solution.F) A) and B)
G) A) and C)

Question 8

Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.

Accepted Answer

A)   SCl2
B)   C2H6
C)   CH3OH
D)   CH2F2
E)   None of the above compounds exhibit hydrogen bonding.F) D) and E)
G) A) and E)

Question 9

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l)  at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4) . The specific heat of CCl4(l)  is 4(l)  at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4) . The specific heat of CCl4(l)  is   its heat of fusion is   and its heat of vaporization is   A)  0.896 kJ B)  1.43 kJ C)  5.74 kJ D)  6.28 kJ" class="answers-bank-image d-inline" rel="preload" > its heat of fusion is 4(l)  at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4) . The specific heat of CCl4(l)  is   its heat of fusion is   and its heat of vaporization is   A)  0.896 kJ B)  1.43 kJ C)  5.74 kJ D)  6.28 kJ" class="answers-bank-image d-inline" rel="preload" > and its heat of vaporization is 4(l)  at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4) . The specific heat of CCl4(l)  is   its heat of fusion is   and its heat of vaporization is   A)  0.896 kJ B)  1.43 kJ C)  5.74 kJ D)  6.28 kJ" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   0.896 kJ
B)   1.43 kJ
C)   5.74 kJ
D)   6.28 kJE) A) and B)
F) A) and C)

Question 10

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 80.0 °C is ________ kJ. The specific heats of ice, water, and steam are -1, and   . A)  7.21 B)  6.16 C)  3870 D)  63.97 E)  26.46" class="answers-bank-image d-inline" rel="preload" > -1, and   . A)  7.21 B)  6.16 C)  3870 D)  63.97 E)  26.46" class="answers-bank-image d-inline" rel="preload" > and -1, and   . A)  7.21 B)  6.16 C)  3870 D)  63.97 E)  26.46" class="answers-bank-image d-inline" rel="preload" > respectively. For -1, and   . A)  7.21 B)  6.16 C)  3870 D)  63.97 E)  26.46" class="answers-bank-image d-inline" rel="preload" > O, -1, and   . A)  7.21 B)  6.16 C)  3870 D)  63.97 E)  26.46" class="answers-bank-image d-inline" rel="preload" > = 6.01 kJ mol-1, and -1, and   . A)  7.21 B)  6.16 C)  3870 D)  63.97 E)  26.46" class="answers-bank-image d-inline" rel="preload" > .

Accepted Answer

A)   7.21
B)   6.16
C)   3870
D)   63.97
E)   26.46F) B) and C)
G) C) and D)

Question 11

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

Accepted Answer

A)   capillary action
B)   viscosity
C)   surface tension
D)   densityE) All of the above
F) B) and C)

Question 12

Choose the substance with the lowest boiling point.

Accepted Answer

A)   H2S
B)   NBr3
C)   F2
D)   CF2H2
E)   H2O2F) A) and D)
G) A) and C)

Question 13

Choose the substance with the highest boiling point.

Accepted Answer

A)   CH4
B)   CH3CH3
C)   CH3CH2Cl
D)   CH3CH2CH2OH
E)   H2F) All of the above
G) A) and B)

Question 14

Which type of bonding does Sr form upon solidification?

Accepted Answer

A)   covalent network
B)   ionic
C)   metallic
D)   molecularE) A) and B)
F) None of the above

Question 15

Vanadium crystallizes in a body-centred cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium if the edge length of a bcc structure is 4r/ -3 B)  12.2 g cm-3 C)  6.11 g cm-3 D)  2.77 g cm-3 E)  8.46 g cm-3" class="answers-bank-image d-inline" rel="preload" > .

Accepted Answer

A)   3.06 g cm-3
B)   12.2 g cm-3
C)   6.11 g cm-3
D)   2.77 g cm-3
E)   8.46 g cm-3F) A) and D)
G) All of the above

Question 16

Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32  is ________ °C.

Accepted Answer

A)   10
B)   20
C)   30
D)   40
E)   0F) A) and E)
G) A) and B)

Question 17

Which of the following substances would you predict to have the highest ΔvapH?

Accepted Answer

A)   Xe
B)   C6H6
C)   SiF4
D)   Br2
E)   N2F) A) and C)
G) A) and E)

Question 18

Why is the ΔvapH higher than ΔfusH for a given compound?

Accepted Answer

Vaporizing a substance requires the complete "breaking" of all intermolecular attractions, whereas the melting of a substance only requires the breaking of a portion of the intermolecular attractions.

Question 19

What type of intermolecular force causes the dissolution of CH3CH2OH in water?

Accepted Answer

A)   hydrogen bonding
B)   dipole-dipole forces
C)   ion-dipole forces
D)   dispersion forces
E)   none of the aboveF) A) and B)
G) A) and C)

Question 20

Determine the vapour pressure (in mbar)  of a substance at 36 °C whose normal boiling point is 84 °C and has a ΔvapH of 22.1 kJ mol-1.

Accepted Answer

A)   319 mbar
B)   31.8 mbar
C)   41.8 mbar
D)   147 mbar
E)   98 mbarF) A) and E)
G) C) and D) A

Exam 11: Liquids, Solids, and Intermolecular Forces

Give the coordination number for a body-centred cubic cell.

Correct AnswerverifiedShow Answer

Which of the following forms an ionic solid?

Correct AnswerverifiedShow Answer

How much energy is required to vaporize 98.6 g of ethanol (C2H5OH) at its boiling point if its ΔvapH is 40.5 kJ mol-1?

Correct AnswerverifiedShow Answer

Identify the type of solid for argon.

Correct AnswerverifiedC

The enthalpy change for converting 1.00 mol of ice at -60.0°C to water at 80.0°C is The specific heats of ice, water, and steam are and respectively. For O, = 6.01 kJ mol-1, and .

Correct AnswerverifiedShow Answer

Describe the difference between the conduction band and the valence band.

Correct AnswerverifiedThe valence band is the group of highest...View AnswerShow Answer

Choose the pair of substances that are most likely to form a homogeneous solution.

Correct AnswerverifiedShow Answer

Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.

Correct AnswerverifiedShow Answer

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4) . The specific heat of CCl4(l) is its heat of fusion is and its heat of vaporization is

Correct AnswerverifiedShow Answer

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 80.0 °C is ________ kJ. The specific heats of ice, water, and steam are and respectively. For O, = 6.01 kJ mol-1, and .

Correct AnswerverifiedShow Answer

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

Correct AnswerverifiedShow Answer

Choose the substance with the lowest boiling point.

Correct AnswerverifiedShow Answer

Choose the substance with the highest boiling point.

Correct AnswerverifiedShow Answer

Which type of bonding does Sr form upon solidification?

Correct AnswerverifiedShow Answer

Vanadium crystallizes in a body-centred cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium if the edge length of a bcc structure is 4r/ .

Correct AnswerverifiedShow Answer

Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 is ________ °C.

Correct AnswerverifiedShow Answer

Which of the following substances would you predict to have the highest ΔvapH?

Correct AnswerverifiedShow Answer

Why is the ΔvapH higher than ΔfusH for a given compound?

Correct AnswerverifiedVaporizing a substance requires the complete "breaking" of all intermolecular attractions, whereas the melting of a substance only requires the breaking of a portion of the intermolecular attractions.

What type of intermolecular force causes the dissolution of CH3CH2OH in water?

Correct AnswerverifiedShow Answer

Determine the vapour pressure (in mbar) of a substance at 36 °C whose normal boiling point is 84 °C and has a ΔvapH of 22.1 kJ mol-1.

Correct AnswerverifiedA

Correct Answer
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Correct Answer
verified

How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH) at its boiling point if its Δ_vapH is 40.5 kJ mol^-1?

Correct Answer
verified

Correct Answer
verified
C

The enthalpy change for converting 1.00 mol of ice at -60.0°C to water at 80.0°C is The specific heats of ice, water, and steam are and respectively. For O, = 6.01 kJ mol^-1, and .

Correct Answer
verified

Correct Answer
verified
The valence band is the group of highest...
View Answer

Correct Answer
verified

Correct Answer
verified

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl₄(l) at 35.0 °C to gaseous CCl₄ at 76.8 °C (the normal boiling point for CCl₄) . The specific heat of CCl₄(l) is its heat of fusion is and its heat of vaporization is

Correct Answer
verified

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 80.0 °C is ________ kJ. The specific heats of ice, water, and steam are and respectively. For O, = 6.01 kJ mol^-1, and .

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Which of the following substances would you predict to have the highest Δ_vapH?

Correct Answer
verified

Why is the Δ_vapH higher than Δ_fusHfor a given compound?

Correct Answer
verified
Vaporizing a substance requires the complete "breaking" of all intermolecular attractions, whereas the melting of a substance only requires the breaking of a portion of the intermolecular attractions.

What type of intermolecular force causes the dissolution of CH₃CH₂OH in water?

Correct Answer
verified

Determine the vapour pressure (in mbar) of a substance at 36 °C whose normal boiling point is 84 °C and has a Δ_vapHof 22.1 kJ mol^-1.

Correct Answer
verified
A