Question 1

The molar volume of a certain form of solid lead is 18 cmS1U1P13S1S1P0/mol. Assuming cubic closest-packed structure, determine the following.
-The number of Pb atoms per unit cell

Accepted Answer

A)  3 
B)  4 
C)  10 
D)  12 
E)  14 
A)  3 
B)  4 
C)  10 
D)  12 
E)  14

Question 2

Which of the following chemical species has the highest boiling point?

Accepted Answer

A)  H2 
B)  He 
C)  C2H6 
D)  NO 
E)  N2 
A)  H2 
B)  He 
C)  C2H6 
D)  NO 
E)  N2

Question 3

You are given the following boiling-point data:   Which one of these liquids would you expect to have the highest vapor pressure at room temperature?

Accepted Answer

A)  diethyl ether, CH3OH2-O-CH2CH3 
B)  ethanol, CH3CH2OH 
C)  ethylene glycol, HO-CH2-CH2-OH 
D)  methanol, CH3OH 
E)  water, H2O 
A)  diethyl ether, CH3OH2-O-CH2CH3 
B)  ethanol, CH3CH2OH 
C)  ethylene glycol, HO-CH2-CH2-OH 
D)  methanol, CH3OH 
E)  water, H2O

Question 4

Aluminum metal crystallizes in a face-centered cubic structure. What is the relationship between the radius of an Al atom (r) and the length of an edge of the unit cell (E)?

Accepted Answer

A)    
B)    
C)  r = 2E 
D)  r = 4E 
E)  r = E/2 
A)    
B)    
C)  r = 2E 
D)  r = 4E 
E)  r = E/2

Question 5

On the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature?

Accepted Answer

A)  CH4 
B)  H2O 
C)  Cl2 
D)  SO2 
E)  NaBr 
A)  CH4 
B)  H2O 
C)  Cl2 
D)  SO2 
E)  NaBr

Question 6

Which of the compounds below is an example of a network solid?

Accepted Answer

A)  NaCl(s) 
B)  S8(s) 
C)  MgO(s) 
D)  SiO2(s) 
E)  C25H52(s) 
A)  NaCl(s) 
B)  S8(s) 
C)  MgO(s) 
D)  SiO2(s) 
E)  C25H52(s)

Question 7

A certain substance has the phase diagram shown below. At which of the following values of T and P is the substance a pure liquid?

Accepted Answer

A)  T = 70°C, P = 1.2 atm 
B)  T = 10°C, P = 1 atm 
C)  T = 8°C, P = 1 atm 
D)  T = 10°C, P = 0.5 atm 
E)  T = 80°C, P = 1 atm 
A)  T = 70°C, P = 1.2 atm 
B)  T = 10°C, P = 1 atm 
C)  T = 8°C, P = 1 atm 
D)  T = 10°C, P = 0.5 atm 
E)  T = 80°C, P = 1 atm

Question 8

The structure for CaF2 can be described as a face-centered array of Ca2+ ions with F- ions in the tetrahedral holes. The edge length of the unit cell is 5.45 × 10-8 cm.A. What fraction of the tetrahedral holes must be occupied by F- ions?
B. Calculate the density of CaF2.C. If the ionic radius of F- is 1.36 × 10-8 cm, estimate the ionic radius of Ca2+. Tetrahedral holes are located along the body diagonals of each unit cell so that 1/4 (body diagonal) = rCa2+ + rF-.

Accepted Answer

A. All tetrahedral holes are f

Question 9

Which of the following statements is incorrect?

Accepted Answer

A)  Ionic solids have high melting points. 
B)  The binding forces in a molecular solid include London dispersion forces. 
C)  Ionic solids are insulators. 
D)  Molecular solids have high melting points. 
E)  All of these statements are correct. 
A)  Ionic solids have high melting points. 
B)  The binding forces in a molecular solid include London dispersion forces. 
C)  Ionic solids are insulators. 
D)  Molecular solids have high melting points. 
E)  All of these statements are correct.

Question 10

Sodium oxide (Na2O) crystallizes in a structure in which the O2- ions are in a face-centered cubic lattice and the Na+ ions are in tetrahedral holes. What is the number of Na+ ions in the unit cell?

Accepted Answer

A)  8 
B)  2 
C)  4 
D)  6 
E)  none of these 
A)  8 
B)  2 
C)  4 
D)  6 
E)  none of these

Question 11

Based on intermolecular forces, which of the following will have the highest boiling point?

Accepted Answer

A)  SF4 
B)  AsF5 
C)  PF5 
D)  More information is needed to answer the question 
A)  SF4 
B)  AsF5 
C)  PF5 
D)  More information is needed to answer the question

Question 12

Which substance can be described as cations bonded together by mobile electrons?

Accepted Answer

A)  S8(s) 
B)  Ag(s) 
C)  Kr(l) 
D)  HCl(l) 
E)  KCl(s) 
A)  S8(s) 
B)  Ag(s) 
C)  Kr(l) 
D)  HCl(l) 
E)  KCl(s)

Question 13

A p-type semiconductor

Accepted Answer

A)  is made by doping host atoms with atoms having more valence electrons than the host. 
B)  has electrons that lie close in energy to the conduction bands. 
C)  is made by doping host atoms with atoms having fewer valence electrons than the host. 
D)  two of these 
E)  none of these 
A)  is made by doping host atoms with atoms having more valence electrons than the host. 
B)  has electrons that lie close in energy to the conduction bands. 
C)  is made by doping host atoms with atoms having fewer valence electrons than the host. 
D)  two of these 
E)  none of these

Question 14

Identify the major attractive force in Ne.

Accepted Answer

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

Question 15

The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net

Accepted Answer

A)  2 anions and 3 cations. 
B)  2 anions and 2 cations. 
C)  5 anions and 3 cations. 
D)  3 anions and 4 cations. 
E)  5 anions and 6 cations. 
A)  2 anions and 3 cations. 
B)  2 anions and 2 cations. 
C)  5 anions and 3 cations. 
D)  3 anions and 4 cations. 
E)  5 anions and 6 cations.

Question 16

A sample consisting of CO2(g) and CO2(s) at equilibrium at -78°C and 1 atm pressure is heated to -30°C, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen?

Accepted Answer

A)  At equilibrium, only CO2(g) will be present. 
B)  The melting point of the CO2(s) will decrease. 
C)  At equilibrium, CO2(g) and CO2(l) will be present. 
D)  All the CO2 will be converted to CO2(l). 
E)  none of these 
A)  At equilibrium, only CO2(g) will be present. 
B)  The melting point of the CO2(s) will decrease. 
C)  At equilibrium, CO2(g) and CO2(l) will be present. 
D)  All the CO2 will be converted to CO2(l). 
E)  none of these

Question 17

A sample of Co crystallizes in the hexagonal closest-packed (hcp) structure. Each atom in a layer is surrounded by and touches 6 other Co atoms. If the distance between Co atom centers within each layer is 2.0 × 102 pm, what is the distance between centers of nearest neighbors in adjacent layers?

Accepted Answer

A)  1.5 × 102 pm 
B)  4.0 × 102 pm 
C)  2.3 × 102 pm 
D)  2.0 × 102 pm 
E)  none of these 
A)  1.5 × 102 pm 
B)  4.0 × 102 pm 
C)  2.3 × 102 pm 
D)  2.0 × 102 pm 
E)  none of these

Question 18

When 1.00 mol of a pure liquid is vaporized at a constant pressure of 1.06 atm and at its boiling point of 332.6 K, 32.16 kJ of energy (heat) is absorbed and the volume change is 27.44 L. What is ΔH for this process? (1 L-atm = 101.3 J)

Accepted Answer

A)  -35.11 kJ 
B)  35.11 kJ 
C)  29.21 kJ 
D)  -29.21 kJ 
E)  32.16 kJ 
A)  -35.11 kJ 
B)  35.11 kJ 
C)  29.21 kJ 
D)  -29.21 kJ 
E)  32.16 kJ

Question 19

A certain metal fluoride crystallizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal atoms occupy the body centers of half the cubes. What is the formula for the metal fluoride?

Accepted Answer

A)  MF 
B)  M2F 
C)  MF8 
D)  MF2 
E)  none of these 
A)  MF 
B)  M2F 
C)  MF8 
D)  MF2 
E)  none of these

Question 20

In the unit cell of sphalerite, Zn2+ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S2- ions. What is the number of formula units of ZnS in the unit cell?

Accepted Answer

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

The molar volume of a certain form of solid lead is 18 cm³/mol. Assuming cubic closest-packed structure, determine the following. -The number of Pb atoms per unit cell

Which of the following chemical species has the highest boiling point?

You are given the following boiling-point data: Which one of these liquids would you expect to have the highest vapor pressure at room temperature?

Aluminum metal crystallizes in a face-centered cubic structure. What is the relationship between the radius of an Al atom (r) and the length of an edge of the unit cell (E)?

On the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature?

Which of the compounds below is an example of a network solid?

A certain substance has the phase diagram shown below. At which of the following values of T and P is the substance a pure liquid?

Which of the following statements is incorrect?

Sodium oxide (Na₂O) crystallizes in a structure in which the O^2- ions are in a face-centered cubic lattice and the Na⁺ ions are in tetrahedral holes. What is the number of Na⁺ ions in the unit cell?

Based on intermolecular forces, which of the following will have the highest boiling point?

Which substance can be described as cations bonded together by mobile electrons?

A p-type semiconductor

Identify the major attractive force in Ne.

The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net

A sample consisting of CO₂(g) and CO₂(s) at equilibrium at -78°C and 1 atm pressure is heated to -30°C, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen?

A sample of Co crystallizes in the hexagonal closest-packed (hcp) structure. Each atom in a layer is surrounded by and touches 6 other Co atoms. If the distance between Co atom centers within each layer is 2.0 × 10² pm, what is the distance between centers of nearest neighbors in adjacent layers?

When 1.00 mol of a pure liquid is vaporized at a constant pressure of 1.06 atm and at its boiling point of 332.6 K, 32.16 kJ of energy (heat) is absorbed and the volume change is 27.44 L. What is ΔH for this process? (1 L-atm = 101.3 J)

A certain metal fluoride crystallizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal atoms occupy the body centers of half the cubes. What is the formula for the metal fluoride?

In the unit cell of sphalerite, Zn²⁺ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S^2- ions. What is the number of formula units of ZnS in the unit cell?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

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Exam 16: Liquids and Solids

The molar volume of a certain form of solid lead is 18 cm3/mol. Assuming cubic closest-packed structure, determine the following. -The number of Pb atoms per unit cell

Which of the following chemical species has the highest boiling point?

You are given the following boiling-point data: Which one of these liquids would you expect to have the highest vapor pressure at room temperature?

Aluminum metal crystallizes in a face-centered cubic structure. What is the relationship between the radius of an Al atom (r) and the length of an edge of the unit cell (E)?

On the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature?

Which of the compounds below is an example of a network solid?

A certain substance has the phase diagram shown below. At which of the following values of T and P is the substance a pure liquid?

Which of the following statements is incorrect?

Sodium oxide (Na2O) crystallizes in a structure in which the O2- ions are in a face-centered cubic lattice and the Na+ ions are in tetrahedral holes. What is the number of Na+ ions in the unit cell?

Based on intermolecular forces, which of the following will have the highest boiling point?

Which substance can be described as cations bonded together by mobile electrons?

A p-type semiconductor

Identify the major attractive force in Ne.

The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net

A sample consisting of CO2(g) and CO2(s) at equilibrium at -78°C and 1 atm pressure is heated to -30°C, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen?

A sample of Co crystallizes in the hexagonal closest-packed (hcp) structure. Each atom in a layer is surrounded by and touches 6 other Co atoms. If the distance between Co atom centers within each layer is 2.0 × 102 pm, what is the distance between centers of nearest neighbors in adjacent layers?

When 1.00 mol of a pure liquid is vaporized at a constant pressure of 1.06 atm and at its boiling point of 332.6 K, 32.16 kJ of energy (heat) is absorbed and the volume change is 27.44 L. What is ΔH for this process? (1 L-atm = 101.3 J)

A certain metal fluoride crystallizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal atoms occupy the body centers of half the cubes. What is the formula for the metal fluoride?

In the unit cell of sphalerite, Zn2+ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S2- ions. What is the number of formula units of ZnS in the unit cell?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

The molar volume of a certain form of solid lead is 18 cm³/mol. Assuming cubic closest-packed structure, determine the following. -The number of Pb atoms per unit cell

Sodium oxide (Na₂O) crystallizes in a structure in which the O^2- ions are in a face-centered cubic lattice and the Na⁺ ions are in tetrahedral holes. What is the number of Na⁺ ions in the unit cell?

A sample consisting of CO₂(g) and CO₂(s) at equilibrium at -78°C and 1 atm pressure is heated to -30°C, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen?

A sample of Co crystallizes in the hexagonal closest-packed (hcp) structure. Each atom in a layer is surrounded by and touches 6 other Co atoms. If the distance between Co atom centers within each layer is 2.0 × 10² pm, what is the distance between centers of nearest neighbors in adjacent layers?

In the unit cell of sphalerite, Zn²⁺ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S^2- ions. What is the number of formula units of ZnS in the unit cell?