Question 1

Lattice enthalpy may be calculated from thermodynamic data using _____.

Accepted Answer

A)  the Clausius-Clapeyron equation 
B)  the Born-Haber cycle 
C)  the dynamic equilibrium expression 
D)  Avogadro's hypothesis 
E)  cubic cell enthalpy of formation equation 
A)  the Clausius-Clapeyron equation 
B)  the Born-Haber cycle 
C)  the dynamic equilibrium expression 
D)  Avogadro's hypothesis 
E)  cubic cell enthalpy of formation equation B

Question 2

Rubidium iodide (molar mass 212.4 g/mol) has a face-centered cubic unit cell with rubidium ions in octahedral holes. If the radius of iodide ion is 219 pm and the density of RbI is 3.55 g/cm3, what is the radius of the rubidium ion (in pm)?

Accepted Answer

A)  112 pm 
B)  149 pm 
C)  181 pm 
D)  297 pm 
E)  419 pm 
A)  112 pm 
B)  149 pm 
C)  181 pm 
D)  297 pm 
E)  419 pm B

Question 3

Which of the following is expected to have the most negative lattice enthalpy?

Accepted Answer

A)  LiCl 
B)  NaCl 
C)  KCl 
D)  RbCl 
E)  CsCl 
A)  LiCl 
B)  NaCl 
C)  KCl 
D)  RbCl 
E)  CsCl A

Question 4

Palladium crystallizes in a face-centered cubic lattice with an edge length of 388.8 pm. What is the density of palladium?

Accepted Answer

A)  0.752 g/cm3 
B)  3.01 g/cm3 
C)  1.50 g/cm3 
D)  6.01 g/cm3 
E)  12.0 g/cm3 
A)  0.752 g/cm3 
B)  3.01 g/cm3 
C)  1.50 g/cm3 
D)  6.01 g/cm3 
E)  12.0 g/cm3

Question 5

The lattice energy of NaCl(s) is -786 kJmol. Use this value and the following thermochemical data to determine the electron attachment enthalpy of Cl(g). ?IE is the enthalpy of ionization. $$\begin{array} { l l } 
\mathrm { Na } ( \mathrm { s } ) \rightarrow \mathrm { Na } ( \mathrm { g } ) & \Delta _ { f } H ^ { \circ } = + 107 \mathrm {~kJ} / \mathrm { mol } \
\mathrm { Na } ( \mathrm { g } ) \rightarrow \mathrm { Na } ^ { + } ( \mathrm { g } ) + \mathrm { e } ^ { - } & \Delta I E = + 496 \mathrm {~kJ} / \mathrm { mol } \
1 / 2 \mathrm { Cl } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { Cl } ( \mathrm { g } ) & \Delta _ { f } H ^ { \circ } = + 121 \mathrm {~kJ} / \mathrm { mol } \
\mathrm { Na } ( \mathrm { s } ) + 1 / 2 \mathrm { Cl } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { NaCl } ( \mathrm { s } ) & \Delta _ { f } H ^ { \circ } = - 411 \mathrm {~kJ} / \mathrm { mol }
\end{array}$$

Accepted Answer

A)  -1921 kJ/mol 
B)  -473 kJ/mol 
C)  -349 kJ/mol 
D)  +349 kJ/mol 
E)  +473 kJ/mol 
A)  -1921 kJ/mol 
B)  -473 kJ/mol 
C)  -349 kJ/mol 
D)  +349 kJ/mol 
E)  +473 kJ/mol

Question 6

Gold (atomic mass 197 g/mol), with an atomic radius of 144.2 pm, crystallizes in a face-centered cubic lattice. What is the density of gold?

Accepted Answer

A)  19.3 g/cm3 
B)  1.21 g/cm3 
C)  4.82 g/cm3 
D)  2.41 g/cm3 
E)  9.65 g/cm3 
A)  19.3 g/cm3 
B)  1.21 g/cm3 
C)  4.82 g/cm3 
D)  2.41 g/cm3 
E)  9.65 g/cm3

Question 7

Arrange the three common cubic unit cells in order from least dense to most dense packing.

Accepted Answer

A)  Face-centered cubic < body-centered cubic < primitive cubic 
B)  Primitive cubic < body-centered cubic < face-centered cubic 
C)  Primitive cubic < face-centered cubic < body-centered cubic 
D)  Body-centered cubic < primitive cubic < face-centered cubic 
E)  Body-centered cubic < face-centered cubic < primitive cubic 
A)  Face-centered cubic < body-centered cubic < primitive cubic 
B)  Primitive cubic < body-centered cubic < face-centered cubic 
C)  Primitive cubic < face-centered cubic < body-centered cubic 
D)  Body-centered cubic < primitive cubic < face-centered cubic 
E)  Body-centered cubic < face-centered cubic < primitive cubic

Question 8

Which of the following compounds is expected to have the strongest ionic bonds?

Accepted Answer

A)  RbI 
B)  KCl 
C)  NaBr 
D)  CsF 
E)  LiF 
A)  RbI 
B)  KCl 
C)  NaBr 
D)  CsF 
E)  LiF

Question 9

Elements that have their highest energy electrons in a filled band of molecular orbitals, separated from the lowest empty band by an energy difference much too large for electrons to jump between bands, are called _____.

Accepted Answer

A)  semiconductors 
B)  metals 
C)  conductors 
D)  insulators 
E)  isomorphs 
A)  semiconductors 
B)  metals 
C)  conductors 
D)  insulators 
E)  isomorphs

Question 10

What process occurs when the temperature of a substance at Point A is increased (at constant pressure) until the substance is at Point B?

Accepted Answer

A)  Condensation 
B)  Vaporization 
C)  Sublimation 
D)  Melting 
E)  Freezing 
A)  Condensation 
B)  Vaporization 
C)  Sublimation 
D)  Melting 
E)  Freezing

Question 11

The space-filling representation provided below is an example of a _____ unit cell, which contains _____ atom(s).

Accepted Answer

A)  face centered cubic, 4 atoms 
B)  primitive cubic, 1 atom 
C)  body centered cubic, 2 atoms 
D)  face centered cubic, 13 atoms 
E)  primitive cubic, 7 atoms 
A)  face centered cubic, 4 atoms 
B)  primitive cubic, 1 atom 
C)  body centered cubic, 2 atoms 
D)  face centered cubic, 13 atoms 
E)  primitive cubic, 7 atoms

Question 12

The metal vanadium crystallizes in a body-centered cubic lattice. If the density of vanadium is 6.11 g/cm3, what is the unit cell volume?

Accepted Answer

A)  5.44 × 105 pm3 
B)  1.99 × 105 pm3 
C)  2.77 × 107 pm3 
D)  1.38 × 107 pm3 
E)  3.98 × 105 pm3 
A)  5.44 × 105 pm3 
B)  1.99 × 105 pm3 
C)  2.77 × 107 pm3 
D)  1.38 × 107 pm3 
E)  3.98 × 105 pm3

Question 13

An unknown white solid was found to have a melting point of 150oC. It is soluble in water, but it is a poor conductor of electricity in an aqueous solution. The white solid most likely is _____.

Accepted Answer

A)  C6H12O6 (glucose) 
B)  KCl 
C)  Rb 
D)  C (diamond) 
E)  Si 
A)  C6H12O6 (glucose) 
B)  KCl 
C)  Rb 
D)  C (diamond) 
E)  Si

Question 14

For a metal that crystallizes in a body-centered cubic unit cell, what percentage of the space in the cell is occupied by the metal atoms?

Accepted Answer

A)  47% 
B)  62.4% 
C)  68% 
D)  77% 
E)  87% 
A)  47% 
B)  62.4% 
C)  68% 
D)  77% 
E)  87%

Question 15

Using the thermodynamic data below and a value of -717 kJ/mole for the lattice enthalpy for KCl, calculate the ionization energy of K. $$\begin{array} { l l } 
\text { Enthalpy of atomization of } \mathrm { K } & + 89 \mathrm {~kJ} / \mathrm { mol } \
\text { Enthalpy of formation of } \mathrm { KCl } ( \mathrm { s } ) & - 437 \mathrm {~kJ} / \mathrm { mol } \
\text { Enthalpy of formation of } \mathrm { Cl } ( \mathrm { g } ) & + 121 \mathrm {~kJ} / \mathrm { mol } \
\text { Electron attachment enthalpy of } \mathrm { Cl } ( \mathrm { g } ) & - 349 \mathrm {~kJ} / \mathrm { mol }
\end{array}$$

Accepted Answer

A)  -576 kJ/mol 
B)  +141 kJ/mol 
C)  +419 kJ/mol 
D)  +576 kJ/mol 
E)  +597 kJ/mol 
A)  -576 kJ/mol 
B)  +141 kJ/mol 
C)  +419 kJ/mol 
D)  +576 kJ/mol 
E)  +597 kJ/mol

Question 16

Strontium oxide has a face-centered cubic unit cell of oxide ions with the strontium in octahedral holes. If the radius of Sr2+ is 127 pm and the density of SrO is 4.7 g/cm3, what is the radius of the oxide ion? (100 cm = 1 × 1012 pm)

Accepted Answer

A)  176 pm 
B)  132 pm 
C)  127 pm 
D)  137 pm 
E)  273 pm 
A)  176 pm 
B)  132 pm 
C)  127 pm 
D)  137 pm 
E)  273 pm

Question 17

The metal vanadium crystallizes in a body-centered cubic lattice. If the density of vanadium is 6.11 g/cm3, what is the atomic radius of vanadium?

Accepted Answer

A)  25.3 pm 
B)  104 pm 
C)  35.3 pm 
D)  31.9 pm 
E)  131 pm 
A)  25.3 pm 
B)  104 pm 
C)  35.3 pm 
D)  31.9 pm 
E)  131 pm

Question 18

Chromium (atomic mass 52.00 g/mol) crystallizes in a body-centered cubic unit cell. If the length of an edge of the unit cell is 289 pm, what is the density (in g/cm3) of chromium?

Accepted Answer

A)  3.58 g/cm3 
B)  7.15 g/cm3 
C)  13.7 g/cm3 
D)  14.3 g/cm3 
E)  21.3 g/cm3 
A)  3.58 g/cm3 
B)  7.15 g/cm3 
C)  13.7 g/cm3 
D)  14.3 g/cm3 
E)  21.3 g/cm3

Question 19

Calcium sulfide has a face-centered cubic unit cell with calcium ions in octahedral holes. How many ions of each element are contained in each unit cell?

Accepted Answer

A)  1 calcium ion; 1 sulfide ion 
B)  2 calcium ions; 2 sulfide ions 
C)  2 calcium ions; 4 sulfide ions 
D)  4 calcium ions; 2 sulfide ions 
E)  4 calcium ions; 4 sulfide ions 
A)  1 calcium ion; 1 sulfide ion 
B)  2 calcium ions; 2 sulfide ions 
C)  2 calcium ions; 4 sulfide ions 
D)  4 calcium ions; 2 sulfide ions 
E)  4 calcium ions; 4 sulfide ions

Question 20

Given the accompanying phase diagram, under what conditions will liquid be found in equilibrium with either solid or gas?

Accepted Answer

A)  Anywhere along curve AB 
B)  Anywhere along curve AC 
C)  Anywhere along curve AD 
D)  Anywhere along curve AB and AC 
E)  Anywhere along curve AB and AD 
A)  Anywhere along curve AB 
B)  Anywhere along curve AC 
C)  Anywhere along curve AD 
D)  Anywhere along curve AB and AC 
E)  Anywhere along curve AB and AD

Exam 13: The Solid State

Lattice enthalpy may be calculated from thermodynamic data using _____.

Rubidium iodide (molar mass 212.4 g/mol) has a face-centered cubic unit cell with rubidium ions in octahedral holes. If the radius of iodide ion is 219 pm and the density of RbI is 3.55 g/cm3, what is the radius of the rubidium ion (in pm)?

Which of the following is expected to have the most negative lattice enthalpy?

Palladium crystallizes in a face-centered cubic lattice with an edge length of 388.8 pm. What is the density of palladium?

The lattice energy of NaCl(s) is -786 kJmol. Use this value and the following thermochemical data to determine the electron attachment enthalpy of Cl(g). ?IE is the enthalpy of ionization. ()\rightarrow() =+107/ ()\rightarrow()+ \DeltaIE=+496/ 1/2()\rightarrow() =+121/ ()+1/2()\rightarrow() =-411/

Gold (atomic mass 197 g/mol), with an atomic radius of 144.2 pm, crystallizes in a face-centered cubic lattice. What is the density of gold?

Arrange the three common cubic unit cells in order from least dense to most dense packing.

Which of the following compounds is expected to have the strongest ionic bonds?

Elements that have their highest energy electrons in a filled band of molecular orbitals, separated from the lowest empty band by an energy difference much too large for electrons to jump between bands, are called _____.

What process occurs when the temperature of a substance at Point A is increased (at constant pressure) until the substance is at Point B?

The space-filling representation provided below is an example of a _____ unit cell, which contains _____ atom(s).

The metal vanadium crystallizes in a body-centered cubic lattice. If the density of vanadium is 6.11 g/cm3, what is the unit cell volume?

An unknown white solid was found to have a melting point of 150oC. It is soluble in water, but it is a poor conductor of electricity in an aqueous solution. The white solid most likely is _____.

For a metal that crystallizes in a body-centered cubic unit cell, what percentage of the space in the cell is occupied by the metal atoms?

Using the thermodynamic data below and a value of -717 kJ/mole for the lattice enthalpy for KCl, calculate the ionization energy of K. Enthalpy of atomization of +89/ Enthalpy of formation of () -437/ Enthalpy of formation of () +121/ Electron attachment enthalpy of () -349/

Strontium oxide has a face-centered cubic unit cell of oxide ions with the strontium in octahedral holes. If the radius of Sr2+ is 127 pm and the density of SrO is 4.7 g/cm3, what is the radius of the oxide ion? (100 cm = 1 × 1012 pm)

The metal vanadium crystallizes in a body-centered cubic lattice. If the density of vanadium is 6.11 g/cm3, what is the atomic radius of vanadium?

Chromium (atomic mass 52.00 g/mol) crystallizes in a body-centered cubic unit cell. If the length of an edge of the unit cell is 289 pm, what is the density (in g/cm3) of chromium?

Calcium sulfide has a face-centered cubic unit cell with calcium ions in octahedral holes. How many ions of each element are contained in each unit cell?

Given the accompanying phase diagram, under what conditions will liquid be found in equilibrium with either solid or gas?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Rubidium iodide (molar mass 212.4 g/mol) has a face-centered cubic unit cell with rubidium ions in octahedral holes. If the radius of iodide ion is 219 pm and the density of RbI is 3.55 g/cm³, what is the radius of the rubidium ion (in pm)?

The space-filling representation provided below is an example of a _ unit cell, which contains _ atom(s).

The metal vanadium crystallizes in a body-centered cubic lattice. If the density of vanadium is 6.11 g/cm³, what is the unit cell volume?

Strontium oxide has a face-centered cubic unit cell of oxide ions with the strontium in octahedral holes. If the radius of Sr²⁺ is 127 pm and the density of SrO is 4.7 g/cm³, what is the radius of the oxide ion? (100 cm = 1 × 10¹² pm)

The metal vanadium crystallizes in a body-centered cubic lattice. If the density of vanadium is 6.11 g/cm³, what is the atomic radius of vanadium?

Chromium (atomic mass 52.00 g/mol) crystallizes in a body-centered cubic unit cell. If the length of an edge of the unit cell is 289 pm, what is the density (in g/cm³) of chromium?