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Chem II > Ch 12 > Flashcards

Ch 12 Flashcards

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1
Q

Using the following data to calculate the lattice energy of NaBr(s). ΔIE and ΔEA are enthalpy of ionization and electron attachment enthalpy, respectively.

–1401 kJ
–751 kJ
–241 kJ
+241 kJ
+751 kJ

A

b

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2
Q

Which one of the following elements is a semiconductor?
Li
Fe
Cl
Ni
Si

A

e.

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3
Q

A phase diagram of a pure compound has a triple point at 22.0 °C and 32 mm Hg, a normal melting point at 22.8 °C, and a normal boiling point at 107 °C. Which of the following statements regarding this compound is/are correct?

1. The density of the liquid is greater than that of the solid.
2. Sublimation occurs at a constant temperature of 25 °C if the pressure is decreased until a phase change occurs.
3. Condensation occurs if the temperature is decreased from 122 °C to 75 °C at a constant pressure of 1.00 atm

A

3 only

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4
Q

A sketch of a phase diagram is given below.

Which statement about this diagram is not true?

Increasing pressure at constant temperature can melt the solid.

Increasing temperature at constant pressure can cause the solid to sublime.

Increasing temperature at constant pressure can cause the liquid to vaporize.

Increasing pressure at constant temperature can cause deposition of solid from gas.

Increasing pressure at constant temperature can cause liquid to freeze.

A

e.

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5
Q

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?
5.44 × 10^5 pm^3
1.99 × 10^5 pm^3
2.77 × 10^7 pm^3
1.38 × 10^7 pm^3
3.98 × 10^5 pm^3

A

c.

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6
Q

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?
19.3 g/cm^3
1.21 g/cm^3
4.82 g/cm^3
2.41 g/cm^3
9.65 g/cm^3

A

a.

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7
Q

Iron crystallizes in a body-centered cubic lattice. If the radius of iron is 126 pm, what is the unit cell edge length?
291 pm
252 pm
168 pm
126 pm
54.6 pm

A

a.

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8
Q

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?
429 pm
51.9 pm
151​​ pm
41.2 pm
340​​ pm

A

a.

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9
Q

Palladium crystallizes in a face-centered cubic lattice with an edge length of 388.8 pm. What is the density of palladium?
0.752 g/cm3
3.01 g/cm3
1.50 g/cm3
6.01 g/cm3
12.0 g/cm3

A

e.

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10
Q

Using the thermodynamic data below and a value of –717 kJ/mole for the lattice enthalpy for KCl, calculate the ionization energy of K.
–576 kJ/mol
+141 kJ/mol
+419 kJ/mol
+576 kJ/mol
+597 kJ/mol

A

c.

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11
Q

What is the length of the diagonal (in atomic radii) along the face of a face-centered cubic unit cell?

A

c.

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12
Q

If an ionic compound with the formula MX2 forms a face-centered cubic unit cell with the cations (M2n+) at the lattice points, the anions (Xn–) will occupy:

all of the tetrahedral holes in each unit cell.

half of the tetrahedral holes in each unit cell.

all of the octahedral holes in each unit cell.

the center of each face in each unit cell.

the cubic hole in the center of each unit cell.

A

a.

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13
Q

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?
362 pm
256 pm
512 pm
272 pm
128 pm

A

a.

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14
Q

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)
176 pm
132 pm
127 pm
137 pm
273 pm

A

d.

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15
Q

Iron(II) sulfide has a primitive cubic unit cell with sulfide ions at the lattice points. The ionic radii of iron(II) ions and sulfide ions are 88 pm and 184 pm, respectively. What is the density of FeS (in g/cm3)?
2.56 g/cm3
4.71 g/cm3
5.25 g/cm3
6.66 g/cm3
8.97 g/cm3

A

b.

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16
Q

Which of the following statements is/are correct for the 2-D lattice provided below is/are correct?
1. One possible unit cell contains a single Α and a single ∙.
2. More than one unit cell which reproduces this lattice is possible.
3. One possible unit cell contains four Α’s and four ∙’s.

A

1 and 2

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17
Q

Cesium crystallizes in the body-centered cubic system. If the edge of the unit cell is 612 pm, what is the radius of a cesium atom in picometers?
265 pm
1060 pm
1410 pm
1220 pm
115 pm

A

a.

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18
Q

The bandgap of ZnTe is 218 kJ/mol. What is the maximum wavelength of light that can excite an electron transition across the band gap? (h = 6.626 × 10–34 J·s; c = 3.000 × 108 m/s)
551 nm
549.0 nm
7298 nm
873.7 nm
517 nm

A

b.

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19
Q

What is the distance, in atomic radii, along any edge of a body-centered cubic unit cell?

A

a.

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20
Q

Polonium (atomic mass 209.0 g/mol) crystallizes in a primitive cubic unit cell. If the density of polonium is 9.15 g/cm3, what is the radius of a polonium atom (in pm)?
168 pm
238 pm
336 pm
475 pm
672 pm

A

a.

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21
Q

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?
25.3 pm
104 pm
35.3 pm
31.9 pm
131 pm

A

e.

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22
Q

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?
3.58 g/cm3
7.15 g/cm3
13.7 g/cm3
14.3 g/cm3
21.3 g/cm3

A

b.

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23
Q

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 _____.
C6H12O6 (glucose)
KCl
Rb
C (diamond)
Si

A

a.

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24
Q

Which of the following statements concerning the cubic unit cell is/are correct?
1. Within cubic unit cells, three cell symmetries occur: primitive cubic, face-centered cubic, and body-centered cubic.
2. The cell edges of a cubic unit cell are all equal in length.
3. The corner angles of a cubic cell are 90°.

A

1,2, and 3

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25
Q

The lattice energy of NaBr is –752 kJ/mol. This energy corresponds to which of the following reactions?
Na(s) + 1/2 Br2(g) → NaBr(s)
Na(g) + Br(g) → NaBr(s)
Na(g) + Br(g) → NaBr(s)
Na+(g) + Br–(g) → NaBr(s)
Na+(aq) + Br–(aq) → NaBr(s)

A

d.

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26
Q

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)?
1.29 g/cm3
2.57 g/cm3
3.64 g/cm3
5.15 g/cm3
7.28 g/cm3

A

b.

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27
Q

Which of the statements concerning the phase diagram is/are correct?
1. Only the solid phase exists at point A.
2. At point C, the solid and liquid phases are in equilibrium.
3. At point D, the critical point, the substance exists as a supercritical fluid.

A

1 only

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28
Q

Which of the following is expected to have the most negative lattice enthalpy?
LiCl
NaCl
KCl
RbCl
CsCl

A

a.

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29
Q

Lattice enthalpy may be calculated from thermodynamic data using _____.
the Clausius-Clapeyron equation

the Born-Haber cycle

the dynamic equilibrium expression

Avogadro’s hypothesis

cubic cell enthalpy of formation equation

A

b.

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30
Q

Which of the following statements is true about semiconductors?

Pure silicon and germanium are called intrinsic semiconductors.

In extrinsic semiconductors, the number of electrons in the conduction band is determined by the temperature and the magnitude of the band gap.

Dopants are present in intrinsic semiconductors.

The conductivity of intrinsic semiconductors is controlled by adding small numbers of different atoms.

The types of intrinsic semiconductors include p-type and n-type semiconductors.

A

a.

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31
Q

Which equation represents the number of atoms in a body-centered cubic unit cell?

A

c.

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32
Q

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

sulfur dioxide/molecular
graphite/covalent
calcium bromide/ionic
iron/ionic
methane/molecular

A

d.

33
Q

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

A

c.

34
Q

The space-filling representation provided below is an example of a _____ unit cell, which contains _____ atom(s).
face centered cubic, 4 atoms
primitive cubic, 1 atom
body centered cubic, 2 atoms
face centered cubic, 13 atoms
primitive cubic, 7 atoms

A

a.

35
Q

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

A

a.

36
Q

Palladium crystallizes in a face-centered cubic unit cell. If the edge length of the unit cell is 387 pm, what is the radius of a palladium atom in picometers?
137 pm
548 pm
1100 pm
316 pm
48.4 pm

A

a.

37
Q

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

MgO
KBr
NaI
BaO
SrS

A

a.

38
Q

Which of the following statements is/are correct?
1. A unit cell is the smallest repeating unit that has all of the symmetry characteristics of the arrangement of atoms, ions, or molecules in a solid.
2. Transition metals with high densities, especially those in period 6, preferentially crystallize with a primitive cubic cell structure.
3. The preferred crystal structure of the Group 1A metals is face-centered cubic.

A

not c or d or e

39
Q

Which of the following elements might be used as a dopant in a silicon host to create a p-type semiconductor?
Group of answer choices
Al
P
As
S
Ge

A

a.

40
Q

Strontium oxide has a face centered cubic unit cell of oxide ions with the strontium ions in octahedral holes. If the radius of Sr2+ is 127 pm and the radius of O2– is 135 pm, what is the density of strontium ions oxide? (100 cm = 1 × 1012 pm)
0.209 g/cm3
1.20 g/cm3
2.39 g/cm3
4 g/cm3
4.78 g/cm3

A

e.

41
Q

If a metal crystallizes in a body-centered cubic lattice, each metal atom has _____ “nearest neighbors.”
Group of answer choices
3
4
6
8
12

A

d.

42
Q

Which of the following compounds is expected to have the strongest ionic bonds?
Group of answer choices
RbI
KCl
NaBr
CsF
LiF

A

e.

43
Q

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)?
Group of answer choices
112 pm
149 pm
181 pm
297 pm
419 pm

A

b.

44
Q

A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 214 pm and the density of the element is 2.63 g/cm3. What is the identity of the metal?
Group of answer choices
Ni
Yb
Cu
Ca
Sr

A

e.

45
Q

In metals, there are not enough electrons to fill all of the electronic energy levels. At 0 K, the highest energy level filled is referred to as the ________.
Group of answer choices
valence band
conduction band
triple point
Fermi level
band gap

A

d.

46
Q

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

Anywhere along curve AB
Anywhere along curve AC
Anywhere along curve AD
Anywhere along curve AB and AC
Anywhere along curve AB and AD

A

d.

47
Q

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). ΔIE is the enthalpy of ionization.

–1921 kJ/mol
–473 kJ/mol
–349 kJ/mol
+349 kJ/mol
+473 kJ/mol

A

c.

48
Q

Which of the following statements concerning a metal crystallized in a face-centered cubic cell is/are correct?
1. One metal atom is located on each face of the unit cell, where it is shared equally between four unit cells.
2. One metal atom is located at the center of the unit cell.
3. A metal atom is located at each of the eight lattice points, where it is shared equally between eight unit cells.

A

3 only

49
Q

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?
1
2
4
8
12

A

d.

50
Q

Nickel has a face-centered cubic cell, and its density is 8.90 g/cm3. What is the radius (in pm) of a nickel atom? (The molar mass of nickel is 58.69 g/mol)
62.3 pm
88.1 pm
125 pm
249 pm
535 pm

A

c.

51
Q

Which process requires the greatest endothermic change in enthalpy for water?
Freezing
Condensation
Sublimation
Melting
Vaporization

A

c.

52
Q

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:

all of the tetrahedral holes in each unit cell.

half of the tetrahedral holes in each unit cell.

the cubic hole in the center of each unit cell.

the center of each face in each unit cell.

all of the octahedral holes in each unit cell.

A

c.

53
Q

Point D on the phase diagram is referred to as the _____ point.

triple
normal boiling
critical
normal freezing
divergent

A

a.

54
Q

If an ionic solid has a face-centered cubic lattice of anions (Xn−) and all the octahedral holes are occupied by metal cations (Mm+), what is the formula for the compound?
M2X
MX
MX2
M2X3
M3X2

A

b.

55
Q

The phase diagram for CO2 has a triple point at –56.6 °C and 5.19 atm, and a critical point at 31.0 °C and 73 atm. The solid and gas phases are in equilibrium at –78.7 °C and 1.00 atm. Which of the following statements regarding CO2 is/are correct?
1. Sublimation occurs if the temperature of the solid phase is increased from –79.0 °C to 0.0 °C at a constant pressure of 2.5 atm.
2. CO2 is a supercritical fluid at 55 °C and 75 atm.
3. At pressures greater than its critical pressure (73 atm), CO2 will not exist as a solid at any temperature.

A

d.

56
Q

Silver chloride adopts the sodium chloride (rock salt) structure. The length of a unit cell edge is 555 pm. What is the density of AgCl?
5.57 g/cm3
4.19 g/cm3
2.79 g/cm3
2.10 g/cm3
1.39 g/cm3

A

not c. or d. or e.

57
Q

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?
cm3
cm3
​​ cm3
cm3
​​ cm3

A

a.

58
Q

Which of the following ionic compounds is expected to have the lowest enthalpy of fusion?
NaI
NaCl
NaBr
NaF
None of these

A

a.

59
Q

A metal crystallizes in a face-centered cubic lattice. The atomic radius of the metal is 198 pm and the density of the metal is 6.57 g/cm3. What is the volume of the unit cell?
3.25 × 107 pm3
1.52 × 109 pm3
1.76 × 108 pm3
7.76 × 106 pm3
1.3 × 108 pm3

A

not a. or b.

60
Q

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?
Group of answer choices
47%
62.4%
68%
77%
87%

A

c.

61
Q

Which one of the following statements is incorrect?
Group of answer choices

Polonium is the only metal that has a primitive cubic lattice.

The lattice structure of the alkali metals is body-centered cubic.

Many metals can crystallize in more than one type of crystal lattice.

Metals with a body-centered cubic lattice contain a net of four metal atoms per unit cell.

A hexagonal close packed structure is not an example of a cubic unit cell.

A

not a. or b. or c.

62
Q

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

A

not b. or c. or d.

63
Q

Which of the following statements is/are correct? If an ionic compound with the formula MX forms a face-centered cubic unit cell with the anions (Xn–) at the lattice points, the cations (Mn+) may occupy
1. one fourth of the tetrahedral holes in each unit cell.
2. all the octahedral holes in each unit cell.
3. the center of each face in each unit cell.

A

not c. or e. or a

64
Q

Which of the compounds below is not an example of a molecular solid?
Group of answer choices
I2(s)
SiO2(s)
CO2(s)
H2O(s)
C25H52(s)

A

b.

65
Q

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 _____.
Group of answer choices
semiconductors
metals
conductors
insulators
isomorphs

A

d.

66
Q

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

Face-centered cubic < body-centered cubic < primitive cubic

Primitive cubic < body-centered cubic < face-centered cubic

Primitive cubic < face-centered cubic < body-centered cubic

Body-centered cubic < primitive cubic < face-centered cubic

Body-centered cubic < face-centered cubic < primitive cubic

A

b.

67
Q

Above a substance’s _____ temperature, it is not possible to compress the substance into the liquid phase. If enough pressure is applied the substance will become a supercritical fluid.

A

critical

68
Q

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

face-centered

69
Q

Which of the following statements concerning semiconductors is/are correct?
1. The conduction of electricity in p-type semiconductors occurs by the movement of electrons in the conduction band.
2. Doping an intrinsic semiconductor, such as silicon, with a Group 3A element will produce a p-type semiconductor.
3. An n-type semiconductor uses the movement of positive holes in the valence band to conduct electricity.

A

2 only

70
Q

In what type of unit cell are the “A” atoms arranged in the given unit cell? 2

primitive cubic

body-centered cubic

face-centered cubic

A

b.

71
Q

According to the below phase diagram, what process occurs if a pure substance begins at point C and the pressure on the substance is increased until point B is reached?
Fusion
Vaporization
Condensation
Sublimation
None of these

A

c.

72
Q

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?

A

c.

73
Q

Which of the following is/are physical properties of amorphous solids?
1. Amorphous solids have well-defined melting points.
2. At the particulate level, amorphous solids do not have long-not d. range order.
3. Polymeric materials never form amorphous solids.

A

not d.or e.

74
Q

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?
Group of answer choices

1 calcium ion; 1 sulfide ion

2 calcium ions; 2 sulfide ions

2 calcium ions; 4 sulfide ions

4 calcium ions; 2 sulfide ions

4 calcium ions; 4 sulfide ions

A

e.

75
Q

What process occurs when the temperature of a substance at Point A is increased (at constant pressure) until the substance is at Point B?
Group of answer choices
Condensation
Vaporization
Sublimation
Melting
Freezing

A

d.

76
Q

In any cubic lattice, an atom lying at the face of a unit cell is shared equally by how many number of unit cells?

A

a.

77
Q

What is the simplest formula of the compound represented by the unit cell provided below?
Group of answer choices
AB
AB2
AB3
A2B3
A2B4

A

a.

78
Q

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.

A

maybe tetrahedral

79
Q

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

molecular solid

ionic solid

covalent network solid

weak base

metallic solid

A

not b.

Chem II (13 decks)

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