Question 1

You have a solid that it characterized by high melting and boiling points, is NOT conductive, and does NOT dissolve in water. Bonding is most likely

Accepted Answer

A)  metallic. 
B)  covalent. 
C)  molecular covalent. 
D)  ionic. 
E)  polar covalent. 
A)  metallic. 
B)  covalent. 
C)  molecular covalent. 
D)  ionic. 
E)  polar covalent. C

Question 2

Acetone CH3COCH3 boils at a significantly higher temperature than 2-methylpropane isobutene

Accepted Answer

A)  because dipole-dipole forces are always greater than dispersion forces. 
B)  because the molecular mass of acetone is slightly less than that of 2-methylpropane. 
C)  because the density of acetone is greater than that of 2-methylpropane. 
D)  because the attractive dispersion forces in 2-methylpropane are weaker than those in acetone. 
E)  because the attractive dispersion forces in 2-methylpropane are weaker than the dipole forces in acetone. 
A)  because dipole-dipole forces are always greater than dispersion forces. 
B)  because the molecular mass of acetone is slightly less than that of 2-methylpropane. 
C)  because the density of acetone is greater than that of 2-methylpropane. 
D)  because the attractive dispersion forces in 2-methylpropane are weaker than those in acetone. 
E)  because the attractive dispersion forces in 2-methylpropane are weaker than the dipole forces in acetone. E

Question 3

Understand amorphous and crystalline solids at the molecular level.

Accepted Answer

Solid materials may be crystalline or amorphous. The unit cell is the building block of crystalline solids. One way to discuss ionic structures is to identify a crystal lattice for one set of ions and then describe how the other ions pack within the lattice of the first set. Crystalline defects can profoundly alter the properties of a solid.

Question 4

How much energy is required when 23 grams of ice at -4?C are melted in a 240 ml glass of pop? ?H?vap = 40.7 kJ/mol, ?H?fus = 6.0 kJ/mol, Cice = 37.8 J/mol?C, Cwater = 75.3 J/mol?C

Accepted Answer

Includes energy to warm ice to

Question 5

Use the following equation for questions 
  
-The relative size of the Van der Waals constant,$\alpha$, correlates well with boiling point; that is, the larger$\alpha$is, the higher the boiling point. The reason for this correlation is

Accepted Answer

A)  the $\alpha$constant is a measure of molecular size. 
B)  the boiling point is directly proportional to $\alpha$. 
C)  the $\alpha$ constant varies with temperature. 
D)  the $\alpha$ constant is a measure of intermolecular force strength. 
E)  the $\alpha$constant varies with vapour pressure. 
A)  the $\alpha$constant is a measure of molecular size. 
B)  the boiling point is directly proportional to $\alpha$. 
C)  the $\alpha$ constant varies with temperature. 
D)  the $\alpha$ constant is a measure of intermolecular force strength. 
E)  the $\alpha$constant varies with vapour pressure.

Question 6

List at least two different physical properties between network and molecular solids.

Accepted Answer

1. Network solids have much higher melti

Question 7

What is the main difference between an amorphous solid and a crystalline solid?

Accepted Answer

The main difference is that th

Question 8

Your solid is non-conductive and melts at relatively low temperature. Based on this information, one can conclude that bonding in the solid is most likely

Accepted Answer

A)  metallic. 
B)  covalent. 
C)  molecular covalent. 
D)  ionic. 
E)  polar covalent. 
A)  metallic. 
B)  covalent. 
C)  molecular covalent. 
D)  ionic. 
E)  polar covalent.

Question 9

What are the differences in interparticle forces for network and metallic solids?

Accepted Answer

Network solids are held togeth

Question 10

Understand the effects of intermolecular forces on condensation, vapourization, and melting and boiling points.

Accepted Answer

Attractive intermolecular forc

Question 11

Which of the following will have the lowest viscosity?

Accepted Answer

A)  nonane 
B)  octane 
C)  pentane 
D)  heptane 
E)  hexane 
A)  nonane 
B)  octane 
C)  pentane 
D)  heptane 
E)  hexane

Question 12

What feature makes the phase diagram of water unusual?

Accepted Answer

A)  The boiling point is high. 
B)  The positive slope of the liquid-gas equilibrium line. 
C)  The positive slope of the solid-liquid equilibrium line. 
D)  The negative slope of the liquid-gas equilibrium line. 
E)  The negative slope of the solid-liquid equilibrium line. 
A)  The boiling point is high. 
B)  The positive slope of the liquid-gas equilibrium line. 
C)  The positive slope of the solid-liquid equilibrium line. 
D)  The negative slope of the liquid-gas equilibrium line. 
E)  The negative slope of the solid-liquid equilibrium line.

Question 13

Which is the expected order of increasing boiling point for the following molecules?

Accepted Answer

A)  1, 2, 3 
B)  1, 3, 2 
C)  3, 2, 1 
D)  2, 1, 3 
E)  2, 3, 1 
A)  1, 2, 3 
B)  1, 3, 2 
C)  3, 2, 1 
D)  2, 1, 3 
E)  2, 3, 1

Question 14

Ruby is a crystalline compound that contains aluminum, oxygen and chromium. The structure of ruby is best described as having

Accepted Answer

A)  amorphous structure. 
B)  interstitial defects. 
C)  substitutional defects. 
D)  a and c 
E)  a and b 
A)  amorphous structure. 
B)  interstitial defects. 
C)  substitutional defects. 
D)  a and c 
E)  a and b

Question 15

To melt or vapourize a substance, a certain amount of energy needs to be supplied. These are referred to as the heat of fusion and heat of vapourization. Which is typically a lot larger and why?

Accepted Answer

The heat of vapourization is a lot large

Question 16

Sketch the phase diagram for benzene identifying the solid, liquid, and gas phases given the following: normal boiling point (80.1˚C), triple point (5.5˚C, 35.8 mm Hg), critical point (288.5˚C and 47.7 atm)

Accepted Answer

The answer of Sketch the phase diagram for benzene identifying...

Question 17

Arrange the following in order of decreasing surface tension at room temperature:
1) H2O,
2) Hg,
3) benzene,
4) n-hexane

Accepted Answer

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

Question 18

Explain trends in surface tension, capillary action, viscosity, and vapour pressure in terms of intermolecular forces.

Accepted Answer

Substances with higher intermo

Question 19

The order of increasing melting point for several simple molecular compounds is: H2, F2, O2, N2, Ar, while for these same compounds boiling point increases as H2, N2, F2, Ar, O2. Explain why the trends for boiling point and melting point are different.

Accepted Answer

On boiling, intermolecular for

Question 20

Which of the following is the expected order of boiling points for H2, He, F2 and Ne?

Accepted Answer

A)  H2 2 2 2 2 2 
D)  He 2 2 2 2 
A)  H2 2 2 2 2 2 
D)  He 2 2 2 2

You have a solid that it characterized by high melting and boiling points, is NOT conductive, and does NOT dissolve in water. Bonding is most likely

Acetone CH₃COCH₃boils at a significantly higher temperature than 2-methylpropane isobutene

Understand amorphous and crystalline solids at the molecular level.

How much energy is required when 23 grams of ice at -4?C are melted in a 240 ml glass of pop? ?H?_vap = 40.7 kJ/mol, ?H?_fus = 6.0 kJ/mol, C_ice = 37.8 J/mol?C, C_water = 75.3 J/mol?C

List at least two different physical properties between network and molecular solids.

What is the main difference between an amorphous solid and a crystalline solid?

Your solid is non-conductive and melts at relatively low temperature. Based on this information, one can conclude that bonding in the solid is most likely

What are the differences in interparticle forces for network and metallic solids?

Understand the effects of intermolecular forces on condensation, vapourization, and melting and boiling points.

Which of the following will have the lowest viscosity?

What feature makes the phase diagram of water unusual?

Which is the expected order of increasing boiling point for the following molecules?

Ruby is a crystalline compound that contains aluminum, oxygen and chromium. The structure of ruby is best described as having

To melt or vapourize a substance, a certain amount of energy needs to be supplied. These are referred to as the heat of fusion and heat of vapourization. Which is typically a lot larger and why?

Sketch the phase diagram for benzene identifying the solid, liquid, and gas phases given the following: normal boiling point (80.1˚C), triple point (5.5˚C, 35.8 mm Hg), critical point (288.5˚C and 47.7 atm)

Arrange the following in order of decreasing surface tension at room temperature: 1) H₂O, 2) Hg, 3) benzene, 4) n-hexane

Explain trends in surface tension, capillary action, viscosity, and vapour pressure in terms of intermolecular forces.

The order of increasing melting point for several simple molecular compounds is: H₂, F₂, O₂, N₂, Ar, while for these same compounds boiling point increases as H₂, N₂, F₂, Ar, O₂. Explain why the trends for boiling point and melting point are different.

Which of the following is the expected order of boiling points for H₂, He, F₂ and Ne?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Exam 8: Effects of Intermolecular Forces

You have a solid that it characterized by high melting and boiling points, is NOT conductive, and does NOT dissolve in water. Bonding is most likely

Acetone CH3COCH3 boils at a significantly higher temperature than 2-methylpropane isobutene

Understand amorphous and crystalline solids at the molecular level.

How much energy is required when 23 grams of ice at -4?C are melted in a 240 ml glass of pop? ?H?vap = 40.7 kJ/mol, ?H?fus = 6.0 kJ/mol, Cice = 37.8 J/mol?C, Cwater = 75.3 J/mol?C

Use the following equation for questions -The relative size of the Van der Waals constant, α\alphaα , correlates well with boiling point; that is, the larger α\alphaα is, the higher the boiling point. The reason for this correlation is

List at least two different physical properties between network and molecular solids.

What is the main difference between an amorphous solid and a crystalline solid?

Your solid is non-conductive and melts at relatively low temperature. Based on this information, one can conclude that bonding in the solid is most likely

What are the differences in interparticle forces for network and metallic solids?

Understand the effects of intermolecular forces on condensation, vapourization, and melting and boiling points.

Which of the following will have the lowest viscosity?

What feature makes the phase diagram of water unusual?

Which is the expected order of increasing boiling point for the following molecules?

Ruby is a crystalline compound that contains aluminum, oxygen and chromium. The structure of ruby is best described as having

To melt or vapourize a substance, a certain amount of energy needs to be supplied. These are referred to as the heat of fusion and heat of vapourization. Which is typically a lot larger and why?

Sketch the phase diagram for benzene identifying the solid, liquid, and gas phases given the following: normal boiling point (80.1˚C), triple point (5.5˚C, 35.8 mm Hg), critical point (288.5˚C and 47.7 atm)

Arrange the following in order of decreasing surface tension at room temperature: 1) H2O, 2) Hg, 3) benzene, 4) n-hexane

Explain trends in surface tension, capillary action, viscosity, and vapour pressure in terms of intermolecular forces.

The order of increasing melting point for several simple molecular compounds is: H2, F2, O2, N2, Ar, while for these same compounds boiling point increases as H2, N2, F2, Ar, O2. Explain why the trends for boiling point and melting point are different.

Which of the following is the expected order of boiling points for H2, He, F2 and Ne?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Acetone CH₃COCH₃boils at a significantly higher temperature than 2-methylpropane isobutene

How much energy is required when 23 grams of ice at -4?C are melted in a 240 ml glass of pop? ?H?_vap = 40.7 kJ/mol, ?H?_fus = 6.0 kJ/mol, C_ice = 37.8 J/mol?C, C_water = 75.3 J/mol?C

Arrange the following in order of decreasing surface tension at room temperature: 1) H₂O, 2) Hg, 3) benzene, 4) n-hexane

The order of increasing melting point for several simple molecular compounds is: H₂, F₂, O₂, N₂, Ar, while for these same compounds boiling point increases as H₂, N₂, F₂, Ar, O₂. Explain why the trends for boiling point and melting point are different.

Which of the following is the expected order of boiling points for H₂, He, F₂ and Ne?