Question 1

Indicate all the types of intermolecular forces of attraction in C2H6(g).

Accepted Answer

Question 2

Octane, C8H18, boils at 125°C as compared to water, which boils at 100°C. This information suggests that the dispersion forces in nonpolar octane molecules are stronger than dispersion forces and hydrogen bonding in water.

Accepted Answer

A) True 
 B)False

Question 3

Which is expected to have a higher boiling point, C5H12 or C(CH3)4?

Accepted Answer

Question 4

Ethanol (C2H5 - OH)will have a greater viscosity than ethylene glycol (HO - CH2CH2 - OH)at the same temperature.

Accepted Answer

A) True 
 B)False

Question 5

Each of the following substances is a liquid at -50°C. Place these liquids in order of increasing vapor pressure: dimethyl ether (CH3OCH3), propane (C3H8), and ethanol (CH3CH2OH).

Accepted Answer

A) ethanol < propane < dimethyl ether 
B) ethanol < dimethyl ether < propane 
C) propane < dimethyl ether < ethanol 
D) dimethyl ether < ethanol < propane 
E) propane < ethanol < dimethyl ether 
A) ethanol < propane < dimethyl ether 
B) ethanol < dimethyl ether < propane 
C) propane < dimethyl ether < ethanol 
D) dimethyl ether < ethanol < propane 
E) propane < ethanol < dimethyl ether

Question 6

Which of the following is not true with regard to water?

Accepted Answer

A) Water has a high heat capacity. 
B) Water has an unusually high boiling point. 
C) Water can form hydrogen bonds. 
D) Ice is more dense than liquid water. 
E) Water is a polar molecule. 
A) Water has a high heat capacity. 
B) Water has an unusually high boiling point. 
C) Water can form hydrogen bonds. 
D) Ice is more dense than liquid water. 
E) Water is a polar molecule.

Question 7

How much energy (heat)is required to convert 52.0 g of ice at -10.0°C to steam at 100°C? specific heat of ice: 2.09 J/g·°C $\Delta$Hfus = 6.02 kJ/mol
Specific heat of water: 4.18 J/g·°C $\Delta$Hvap = 40.7 kJ/mol
Specific heat of steam: 1.84 J/g·°C

Accepted Answer

A) 2,570 kJ 
B) 1,086 kJ 
C) 157.8 kJ 
D) 40.2 kJ 
E) 22,957 kJ 
A) 2,570 kJ 
B) 1,086 kJ 
C) 157.8 kJ 
D) 40.2 kJ 
E) 22,957 kJ

Question 8

What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 105 J of heat from your body? H2O(l)$\rarr$ H2O(g)$\Delta$Hvap = 40.7 kJ/mol

Accepted Answer

A) 7.52 * 104 g 
B) 418 g 
C) 75.2 g 
D) 58.4 g 
E) 6.92 * 106 g 
A) 7.52 * 104 g 
B) 418 g 
C) 75.2 g 
D) 58.4 g 
E) 6.92 * 106 g

Question 9

Of the given pair of compounds, which would have the higher boiling point?
H2Se or H2O

Accepted Answer

Question 10

Which one of the following substances is expected to have the highest boiling point?

Accepted Answer

A) HBr 
B) HCl 
C) HF 
D) HI 
A) HBr 
B) HCl 
C) HF 
D) HI

Question 11

Suppose the atoms in a two-dimensional crystal have the following arrangement:   How many atoms are in one unit cell?

Accepted Answer

one (each corner of

Question 12

The number of atoms in a body-centered cubic unit cell is

Accepted Answer

A) 1. 
B) 2. 
C) 3. 
D) 4. 
E) 8. 
A) 1. 
B) 2. 
C) 3. 
D) 4. 
E) 8.

Question 13

Indicate all the types of intermolecular forces of attraction in SO2(l).

Accepted Answer

dipole-dip

Question 14

Which one of the following substances is expected to have the lowest melting point?

Accepted Answer

A) BrI 
B) CsI 
C) LiI 
D) NaI 
E) RbI 
A) BrI 
B) CsI 
C) LiI 
D) NaI 
E) RbI

Question 15

Identify the dominant (strongest)type of intermolecular force present in NH3(l).

Accepted Answer

Question 16

What phase exists at the point labeled b?

Accepted Answer

The answer of What phase exists at the point labeled...

Question 17

Of the pair of compounds given, which would have the stronger intermolecular forces of attraction?
HF or HCl

Accepted Answer

The answer of Of the pair of compounds given, which...

Question 18

Each of the following substances is a gas at 25°C and 1 atmosphere pressure. Which one will liquefy most easily when compressed at a constant temperature?

Accepted Answer

A) F2 
B) H2 
C) HF 
D) SiH4 
E) Ar 
A) F2 
B) H2 
C) HF 
D) SiH4 
E) Ar

Question 19

Given that the heat of vaporization of mercury is 59.0 kJ/mol and the vapor pressure of mercury is 0.0017 torr at 25°C, calculate the normal boiling point of mercury.

Accepted Answer

380°C (the

Question 20

An example of a covalent network solid is

Accepted Answer

A) diamond. 
B) potassium. 
C) iodine. 
D) sodium chloride. 
E) None of these. 
A) diamond. 
B) potassium. 
C) iodine. 
D) sodium chloride. 
E) None of these.

Exam 12: Intermolecular Forces and Liquids and Solids

Indicate all the types of intermolecular forces of attraction in C2H6(g).

Octane, C8H18, boils at 125°C as compared to water, which boils at 100°C. This information suggests that the dispersion forces in nonpolar octane molecules are stronger than dispersion forces and hydrogen bonding in water.

Which is expected to have a higher boiling point, C5H12 or C(CH3)4?

Ethanol (C2H5 - OH)will have a greater viscosity than ethylene glycol (HO - CH2CH2 - OH)at the same temperature.

Each of the following substances is a liquid at -50°C. Place these liquids in order of increasing vapor pressure: dimethyl ether (CH3OCH3), propane (C3H8), and ethanol (CH3CH2OH).

Which of the following is not true with regard to water?

How much energy (heat)is required to convert 52.0 g of ice at -10.0°C to steam at 100°C? specific heat of ice: 2.09 J/g·°C Δ\DeltaΔ Hfus = 6.02 kJ/mol Specific heat of water: 4.18 J/g·°C Δ\DeltaΔ Hvap = 40.7 kJ/mol Specific heat of steam: 1.84 J/g·°C

What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 105 J of heat from your body? H2O(l) →\rarr→ H2O(g) Δ\DeltaΔ Hvap = 40.7 kJ/mol

Of the given pair of compounds, which would have the higher boiling point? H2Se or H2O

Which one of the following substances is expected to have the highest boiling point?

Suppose the atoms in a two-dimensional crystal have the following arrangement: How many atoms are in one unit cell?

The number of atoms in a body-centered cubic unit cell is

Indicate all the types of intermolecular forces of attraction in SO2(l).

Which one of the following substances is expected to have the lowest melting point?

Identify the dominant (strongest)type of intermolecular force present in NH3(l).

What phase exists at the point labeled b?

Of the pair of compounds given, which would have the stronger intermolecular forces of attraction? HF or HCl

Each of the following substances is a gas at 25°C and 1 atmosphere pressure. Which one will liquefy most easily when compressed at a constant temperature?

Given that the heat of vaporization of mercury is 59.0 kJ/mol and the vapor pressure of mercury is 0.0017 torr at 25°C, calculate the normal boiling point of mercury.

An example of a covalent network solid is

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Indicate all the types of intermolecular forces of attraction in C₂H₆(g).

Octane, C₈H₁₈, boils at 125°C as compared to water, which boils at 100°C. This information suggests that the dispersion forces in nonpolar octane molecules are stronger than dispersion forces and hydrogen bonding in water.

Which is expected to have a higher boiling point, C₅H₁₂ or C(CH₃)₄?

Ethanol (C₂H₅ - OH)will have a greater viscosity than ethylene glycol (HO - CH₂CH₂ - OH)at the same temperature.

Each of the following substances is a liquid at -50°C. Place these liquids in order of increasing vapor pressure: dimethyl ether (CH₃OCH₃), propane (C₃H₈), and ethanol (CH₃CH₂OH)_.

How much energy (heat)is required to convert 52.0 g of ice at -10.0°C to steam at 100°C? specific heat of ice: 2.09 J/g·°C $\Delta$ H_fus = 6.02 kJ/mol Specific heat of water: 4.18 J/g·°C $\Delta$ H_vap = 40.7 kJ/mol Specific heat of steam: 1.84 J/g·°C

What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 10⁵ J of heat from your body? H₂O(l) $\rarr$ H₂O(g) $\Delta$ H_vap = 40.7 kJ/mol

Of the given pair of compounds, which would have the higher boiling point? H₂Se or H₂O

Indicate all the types of intermolecular forces of attraction in SO₂(l).

Identify the dominant (strongest)type of intermolecular force present in NH₃(l).