Question 1

Give an example of an ionic crystal and a metallic crystal which contain an element common to each.

Accepted Answer

NaCl = ion

Question 2

Octane is a component of fuel used in internal combustion engines.The dominant intermolecular forces in octane are

Accepted Answer

A) dipole-dipole forces. 
B) London dispersion forces. 
C) hydrogen bonding. 
D) covalent bonds. 
E) carbon-hydrogen bonds. 
A) dipole-dipole forces. 
B) London dispersion forces. 
C) hydrogen bonding. 
D) covalent bonds. 
E) carbon-hydrogen bonds.

Question 3

___________ is the attraction of unlike molecules involved in capillary action.

Accepted Answer

The answer of ___________ is the attraction of unlike molecules...

Question 4

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
Specific heat of water 4.18 J/g • °C
Specific heat of steam 1.84 J/g • °C
Molar heat of fusion 6.02 kJ/mol
Molar heat of vaporization 40.7 kJ/mol

Accepted Answer

A) 12.0 kJ 
B) 23.0 kJ 
C) 46.4 kJ 
D) 158 kJ 
E) 2.30 ×104 kJ 
A) 12.0 kJ 
B) 23.0 kJ 
C) 46.4 kJ 
D) 158 kJ 
E) 2.30 ×104 kJ

Question 5

If liquid bromine is cooled to form a solid,which type of solid does it form?

Accepted Answer

A) atomic 
B) metallic 
C) molecular 
D) ionic 
E) covalent 
A) atomic 
B) metallic 
C) molecular 
D) ionic 
E) covalent

Question 6

What is the intermolecular force that exists between a magnesium ion and hydrogen sulfide?

Accepted Answer

A) dipole-dipole forces 
B) London dispersion forces 
C) ionic bonding 
D) ion-dipole forces 
E) ion-ion forces 
A) dipole-dipole forces 
B) London dispersion forces 
C) ionic bonding 
D) ion-dipole forces 
E) ion-ion forces

Question 7

Ice is less dense than water due to the formation of hydrogen bonds.

Accepted Answer

A) True 
 B)False

Question 8

Which is the correct equation for the molar heat of sublimation?

Accepted Answer

A) ΔHsub = ΔHfus - ΔHvapVliq 
B) ΔHsub = ΔHdep + ΔHfus 
C) ΔUsub= ΔUfus + ΔUvap 
D) ΔHsub = ΔHfus - ΔHvap 
E) ΔHsub = ΔHfus + ΔHvap 
A) ΔHsub = ΔHfus - ΔHvapVliq 
B) ΔHsub = ΔHdep + ΔHfus 
C) ΔUsub= ΔUfus + ΔUvap 
D) ΔHsub = ΔHfus - ΔHvap 
E) ΔHsub = ΔHfus + ΔHvap

Question 9

At what temperature does ethanol boil on a day in the mountains when the barometric pressure is 547 mmHg? The heat of vaporization of ethanol is 39.3 kJ/mol and its normal boiling point is 78.3°C.(R = 8.314 J/K • mol)

Accepted Answer

A) 76.5°C 
B) 69.9°C 
C) 10.0°C 
D) 77.9°C 
E) 74.6°C 
A) 76.5°C 
B) 69.9°C 
C) 10.0°C 
D) 77.9°C 
E) 74.6°C

Question 10

Ionic crystals are composed of charged spheres that are held together by covalent bonds.

Accepted Answer

A) True 
 B)False

Question 11

Octane has a vapor pressure of 40.torr at 45.1°C and 400.torr at 104.0°C.What is its heat of vaporization? (R = 8.314 J/K • mol)

Accepted Answer

A) 39.1 kJ/mol 
B) 46.0 kJ/mol 
C) 590 kJ/mol 
D) 710 kJ/mol 
E) None of these choices is correct. 
A) 39.1 kJ/mol 
B) 46.0 kJ/mol 
C) 590 kJ/mol 
D) 710 kJ/mol 
E) None of these choices is correct.

Question 12

What is the name given for the attraction between unlike molecules involved in capillary action?

Accepted Answer

A) Adhesion 
B) Ionization 
C) Cohesion 
D) Surface tension 
E) Viscosity 
A) Adhesion 
B) Ionization 
C) Cohesion 
D) Surface tension 
E) Viscosity

Question 13

A face-centered crystal lattice has one atom in the center of the unit cell.

Accepted Answer

A) True 
 B)False

Question 14

Polyethylene plastic consists of long chains of carbon atoms,each of which is also bonded to hydrogens as shown below:   Water forms beads when placed on a polyethylene surface.Why?

Accepted Answer

Water is highly polar and poly

Question 15

Which statement is true about phase diagrams?

Accepted Answer

A) Every phase diagram has only one triple point. 
B) The slope of the liquid-solid phase boundary line is typically negative. 
C) The triple point temperature is the lowest temperature where a liquid can exist. 
D) The critical temperature is lower than the triple point temperature. 
E) The critical temperature is lower than the normal boiling point. 
A) Every phase diagram has only one triple point. 
B) The slope of the liquid-solid phase boundary line is typically negative. 
C) The triple point temperature is the lowest temperature where a liquid can exist. 
D) The critical temperature is lower than the triple point temperature. 
E) The critical temperature is lower than the normal boiling point.

Question 16

Which arrow represents the process of vaporization?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 17

Platinum has a face-centered cubic crystal structure and a density of 21.5 g/cm3.What is the radius of a platinum atom?

Accepted Answer

A) 69 pm 
B) 98 pm 
C) 139 pm 
D) 196 pm 
E) 277 pm 
A) 69 pm 
B) 98 pm 
C) 139 pm 
D) 196 pm 
E) 277 pm

Question 18

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 19

Which of the following pure substances has the strongest dispersion forces?

Accepted Answer

A) C4H10 
B) C5H12 
C) C6H14 
D) C7H16 
E) C8H18 
A) C4H10 
B) C5H12 
C) C6H14 
D) C7H16 
E) C8H18

Question 20

What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?

Accepted Answer

A) Surface tension 
B) Adhesion 
C) Polarity 
D) Viscosity 
E) Cohesion 
A) Surface tension 
B) Adhesion 
C) Polarity 
D) Viscosity 
E) Cohesion

Exam 11: Intermolecular Forces and the Physical Properties of Liquids and Solids

Give an example of an ionic crystal and a metallic crystal which contain an element common to each.

Octane is a component of fuel used in internal combustion engines.The dominant intermolecular forces in octane are

___________ is the attraction of unlike molecules involved in capillary action.

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 Specific heat of water 4.18 J/g • °C Specific heat of steam 1.84 J/g • °C Molar heat of fusion 6.02 kJ/mol Molar heat of vaporization 40.7 kJ/mol

If liquid bromine is cooled to form a solid,which type of solid does it form?

What is the intermolecular force that exists between a magnesium ion and hydrogen sulfide?

Ice is less dense than water due to the formation of hydrogen bonds.

Which is the correct equation for the molar heat of sublimation?

At what temperature does ethanol boil on a day in the mountains when the barometric pressure is 547 mmHg? The heat of vaporization of ethanol is 39.3 kJ/mol and its normal boiling point is 78.3°C.(R = 8.314 J/K • mol)

Ionic crystals are composed of charged spheres that are held together by covalent bonds.

Octane has a vapor pressure of 40.torr at 45.1°C and 400.torr at 104.0°C.What is its heat of vaporization? (R = 8.314 J/K • mol)

What is the name given for the attraction between unlike molecules involved in capillary action?

A face-centered crystal lattice has one atom in the center of the unit cell.

Polyethylene plastic consists of long chains of carbon atoms,each of which is also bonded to hydrogens as shown below: Water forms beads when placed on a polyethylene surface.Why?

Which statement is true about phase diagrams?

Which arrow represents the process of vaporization?

Platinum has a face-centered cubic crystal structure and a density of 21.5 g/cm3.What is the radius of a platinum atom?

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

Which of the following pure substances has the strongest dispersion forces?

What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters