Question 1

Nickel crystallizes in a face-centered cubic lattice. The density of the nickel is 8.91 g/cm3. What is the volume of a single unit cell?

Accepted Answer

A)  $4.3755313942 \times 10 ^ { - 23 }$ cm3 
B)  $3.4736512388 \times 10 ^ { - 21 }$ cm3 
C)  ?? $1.2701419732 \times 10 ^ { - 26 }$ cm3 
D)  $1.0938828486 \times 10^{ - 23}$ cm3 
E)  ?? $8.684128097 \times 10 ^ { - 22 }$ cm3 
A)  $4.3755313942 \times 10 ^ { - 23 }$ cm3 
B)  $3.4736512388 \times 10 ^ { - 21 }$ cm3 
C)  ?? $1.2701419732 \times 10 ^ { - 26 }$ cm3 
D)  $1.0938828486 \times 10^{ - 23}$ cm3 
E)  ?? $8.684128097 \times 10 ^ { - 22 }$ cm3

Question 2

The lattice energy of NaBr is -752 kJ/mol. This energy corresponds to which of the following reactions?

Accepted Answer

A)  Na(s) + 1/2 Br2(g) → NaBr(s) 
B)  Na(g) + Br(g) → NaBr(s).. 
C)  Na(g) + Br(g) → NaBr(s) 
D)  Na+(g) + Br-(g) → NaBr(s) 
E)  Na+(aq) + Br-(aq) → NaBr(s). 
A)  Na(s) + 1/2 Br2(g) → NaBr(s) 
B)  Na(g) + Br(g) → NaBr(s).. 
C)  Na(g) + Br(g) → NaBr(s) 
D)  Na+(g) + Br-(g) → NaBr(s) 
E)  Na+(aq) + Br-(aq) → NaBr(s).

Question 3

Cesium bromide crystallizes in a primitive cubic unit cell with bromide ions at the lattice points. The cesium ions occupy cubic holes. How many bromide ions surround each cesium ion in cesium bromide?

Accepted Answer

A)  1 
B)  2 
C)  4 
D)  8 
E)  12 
A)  1 
B)  2 
C)  4 
D)  8 
E)  12

Question 4

Which one of the following elements is a semiconductor?

Accepted Answer

A)  Li 
B)  Fe 
C)  Cl 
D)  Ni 
E)  Si 
A)  Li 
B)  Fe 
C)  Cl 
D)  Ni 
E)  Si

Question 5

If a metal crystallizes in a body-centered cubic lattice, each metal atom has _____ "nearest neighbors."

Accepted Answer

A)  3 
B)  4 
C)  6 
D)  8 
E)  12 
A)  3 
B)  4 
C)  6 
D)  8 
E)  12

Question 6

Sodium chloride crystallizes in a(n) _____ cubic unit cell with chloride ions occupying the lattice points. The sodium ions occupy interstitial regions, with each cation in contact with six chloride ions.

Accepted Answer

The answer of Sodium chloride crystallizes in a(n) _____ cubic...

Question 7

A salt with a 1:1 ratio of anions to cations may pack in a face-centered cubic unit cell with the anions at the lattice points and the cations occupying one-half of the _____ holes. Zinc sulfide is an example of this structure.

Accepted Answer

The answer of A salt with a 1:1 ratio of...

Question 8

Which of the following ionic compounds is expected to have the lowest enthalpy of fusion?

Accepted Answer

A)  NaI 
B)  NaCl 
C)  NaBr 
D)  NaF 
E)  None of these 
A)  NaI 
B)  NaCl 
C)  NaBr 
D)  NaF 
E)  None of these

Question 9

Copper crystallizes in a face-centered cubic lattice. The radius of a copper atom is 128 pm. What is the edge length of the unit cell?

Accepted Answer

A)  362 pm 
B)  256 pm 
C)  512 pm 
D)  272 pm 
E)  128 pm 
A)  362 pm 
B)  256 pm 
C)  512 pm 
D)  272 pm 
E)  128 pm

Question 10

Lithium chloride crystallizes in a face-centered cubic unit cell with chloride ions occupying the lattice points and lithium ions occupying octahedral holes. How many chloride ions surround each lithium ion in LiCl?

Accepted Answer

A)  1 
B)  4 
C)  6 
D)  8 
E)  12 
A)  1 
B)  4 
C)  6 
D)  8 
E)  12

Question 11

The energy of formation of one mole of solid crystalline ionic compound when ions in the gas phase combine is referred to as _____.

Accepted Answer

A)  lattice energy 
B)  degenerate energy 
C)  ionization energy 
D)  dissociation energy 
E)  elastic energy 
A)  lattice energy 
B)  degenerate energy 
C)  ionization energy 
D)  dissociation energy 
E)  elastic energy

Question 12

Magnesium sulfide (molar mass 56.37 g/mol) has a face-centered cubic unit cell with magnesium ions in octahedral holes. The ionic radii of magnesium ions and sulfide ions are 79 pm and 184 pm, respectively. What is the density of MgS (in g/cm3)?

Accepted Answer

A)  1.29 g/cm3 
B)  2.57 g/cm3 
C)  3.64 g/cm3 
D)  5.15 g/cm3 
E)  7.28 g/cm3 
A)  1.29 g/cm3 
B)  2.57 g/cm3 
C)  3.64 g/cm3 
D)  5.15 g/cm3 
E)  7.28 g/cm3

Question 13

Which two of the following materials are most likely to be amorphous solids: ice, nylon, glass, potassium nitrate?

Accepted Answer

A)  water and glass 
B)  nylon and aspirin 
C)  water and nylon 
D)  water and aspirin 
E)  nylon and glass 
A)  water and glass 
B)  nylon and aspirin 
C)  water and nylon 
D)  water and aspirin 
E)  nylon and glass

Question 14

If an ionic compound with the formula MX forms a primitive cubic unit cell with the anions (Xn-) at the lattice points, the cations (M2n+) will occupy:

Accepted Answer

A)  all of the tetrahedral holes in each unit cell. 
B)  half of the tetrahedral holes in each unit cell. 
C)  the cubic hole in the center of each unit cell. 
D)  the center of each face in each unit cell. 
E)  all of the octahedral holes in each unit cell. 
A)  all of the tetrahedral holes in each unit cell. 
B)  half of the tetrahedral holes in each unit cell. 
C)  the cubic hole in the center of each unit cell. 
D)  the center of each face in each unit cell. 
E)  all of the octahedral holes in each unit cell.

Question 15

Which one of the following substances is incorrectly matched with the kind of solid it forms? Substance/Kind of Solid

Accepted Answer

A)  sulfur dioxide/molecular 
B)  graphite/covalent 
C)  calcium bromide/ionic 
D)  iron/ionic 
E)  methane/molecular 
A)  sulfur dioxide/molecular 
B)  graphite/covalent 
C)  calcium bromide/ionic 
D)  iron/ionic 
E)  methane/molecular

Question 16

The metal sodium crystallizes in a body-centered cubic lattice. If the density of sodium is 0.968 g/cm3, what is the unit cell edge length?

Accepted Answer

A)  429 pm 
B)  51.9 pm 
C)  151​​ pm 
D)  41.2 pm 
E)  340​​ pm 
A)  429 pm 
B)  51.9 pm 
C)  151​​ pm 
D)  41.2 pm 
E)  340​​ pm

Question 17

Which process requires the greatest endothermic change in enthalpy for water?

Accepted Answer

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

Question 18

A low-melting solid readily dissolves in water to produce a nonconducting solution. The solid is most likely a(n) _____.

Accepted Answer

A)  molecular solid 
B)  ionic solid 
C)  covalent network solid 
D)  weak base 
E)  metallic solid 
A)  molecular solid 
B)  ionic solid 
C)  covalent network solid 
D)  weak base 
E)  metallic solid

Question 19

Using the following data to calculate the lattice energy of NaBr(s). ?IE and ?EA are enthalpy of ionization and electron attachment enthalpy, respectively. $$\begin{array} { l l } 
\mathrm { Na } ( \mathrm { s } ) \rightarrow \mathrm { Na } ( \mathrm { g } ) & \Delta _f H ^ { \circ } = + 107 \mathrm {~kJ} \
\mathrm { Na } ( \mathrm { g } ) \rightarrow \mathrm { Na } ^ { + } ( \mathrm { g } ) + \mathrm { e } ^ { - } & \Delta I E = + 496 \mathrm {~kJ} \
1 / 2 \mathrm { Br } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { Br } ( \mathrm { g } ) & \Delta_f H ^ { \circ } = + 112 \mathrm {~kJ} \
\mathrm { Br } ( \mathrm { g } ) + \mathrm { e } ^ { - } \rightarrow \mathrm { Br } ^ { - } ( \mathrm { g } ) & \Delta E A = - 325 \mathrm {~kJ} \
\mathrm { Na } ( \mathrm { s } ) + 1 / 2 \mathrm { Br } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { NaBr } ( \mathrm { s } ) & \Delta_f H ^ { \circ } = - 361 \mathrm {~kJ}
\end{array}$$

Accepted Answer

A)  -1401 kJ 
B)  -751 kJ 
C)  -241 kJ 
D)  +241 kJ 
E)  +751 kJ 
A)  -1401 kJ 
B)  -751 kJ 
C)  -241 kJ 
D)  +241 kJ 
E)  +751 kJ

Question 20

On the phase diagram below, which point corresponds to conditions where only the gas phase exists?

Accepted Answer

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

Exam 13: The Solid State

Nickel crystallizes in a face-centered cubic lattice. The density of the nickel is 8.91 g/cm3. What is the volume of a single unit cell?

The lattice energy of NaBr is -752 kJ/mol. This energy corresponds to which of the following reactions?

Cesium bromide crystallizes in a primitive cubic unit cell with bromide ions at the lattice points. The cesium ions occupy cubic holes. How many bromide ions surround each cesium ion in cesium bromide?

Which one of the following elements is a semiconductor?

If a metal crystallizes in a body-centered cubic lattice, each metal atom has _____ "nearest neighbors."

Sodium chloride crystallizes in a(n) _____ cubic unit cell with chloride ions occupying the lattice points. The sodium ions occupy interstitial regions, with each cation in contact with six chloride ions.

A salt with a 1:1 ratio of anions to cations may pack in a face-centered cubic unit cell with the anions at the lattice points and the cations occupying one-half of the _____ holes. Zinc sulfide is an example of this structure.

Which of the following ionic compounds is expected to have the lowest enthalpy of fusion?

Copper crystallizes in a face-centered cubic lattice. The radius of a copper atom is 128 pm. What is the edge length of the unit cell?

Lithium chloride crystallizes in a face-centered cubic unit cell with chloride ions occupying the lattice points and lithium ions occupying octahedral holes. How many chloride ions surround each lithium ion in LiCl?

The energy of formation of one mole of solid crystalline ionic compound when ions in the gas phase combine is referred to as _____.

Magnesium sulfide (molar mass 56.37 g/mol) has a face-centered cubic unit cell with magnesium ions in octahedral holes. The ionic radii of magnesium ions and sulfide ions are 79 pm and 184 pm, respectively. What is the density of MgS (in g/cm3)?

Which two of the following materials are most likely to be amorphous solids: ice, nylon, glass, potassium nitrate?

If an ionic compound with the formula MX forms a primitive cubic unit cell with the anions (Xn-) at the lattice points, the cations (M2n+) will occupy:

Which one of the following substances is incorrectly matched with the kind of solid it forms? Substance/Kind of Solid

The metal sodium crystallizes in a body-centered cubic lattice. If the density of sodium is 0.968 g/cm3, what is the unit cell edge length?

Which process requires the greatest endothermic change in enthalpy for water?

A low-melting solid readily dissolves in water to produce a nonconducting solution. The solid is most likely a(n) _____.

Using the following data to calculate the lattice energy of NaBr(s). ?IE and ?EA are enthalpy of ionization and electron attachment enthalpy, respectively. ()\rightarrow() =+107 ()\rightarrow()+ \DeltaIE=+496 1/2()\rightarrow() =+112 ()+\rightarrow() \DeltaEA=-325 ()+1/2()\rightarrow() =-361

On the phase diagram below, which point corresponds to conditions where only the gas phase exists?

Basic Concepts of Chemistry

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Principles of Chemical Reactivity: Entropy and Free Energy

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Carbon: Not Just Another Element

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Magnesium sulfide (molar mass 56.37 g/mol) has a face-centered cubic unit cell with magnesium ions in octahedral holes. The ionic radii of magnesium ions and sulfide ions are 79 pm and 184 pm, respectively. What is the density of MgS (in g/cm³)?

If an ionic compound with the formula MX forms a primitive cubic unit cell with the anions (Xn^-) at the lattice points, the cations (M²ⁿ⁺) will occupy:

The metal sodium crystallizes in a body-centered cubic lattice. If the density of sodium is 0.968 g/cm³, what is the unit cell edge length?