Question 1

In antifluorite structures,________

Accepted Answer

The answer of In antifluorite structures,________
...

Question 2

If a salt has a face-centered cubic (fcc)unit cell and a 1:2 cation: anion stoichiometry with cations occupying the fcc positions,then the anions fill all the ________ holes.

Accepted Answer

In an fcc unit cell, there are four tetrahedral holes for every one cubic hole. The cations occupy the cubic holes, leaving the anions to fill the tetrahedral sites. Therefore, the anions in this salt fill all the tetrahedral holes.

Question 3

Which of the following contribute to the arrangement of ions in the unit cells of an ionic solid? 
I.The empirical formula
II.The relative radii of the ions
III.The shape of polyatomic ions

Accepted Answer

The answer of Which of the following contribute to the...

Question 4

In the cubic closest-packed structure of sodium chloride,which ions are touching or nearly touching? 
I.Sodium ions and sodium ions
II.Chloride ions and chloride ions
III.Sodium ions and chloride ions

Accepted Answer

In the cubic closest-packed structure of sodium chloride, the sodium and chloride ions are arranged in a face-centered cubic lattice. In this lattice, each sodium ion is surrounded by six chloride ions, and each chloride ion is surrounded by six sodium ions. Therefore, the ions that are touching or nearly touching are the sodium and chloride ions, making choices II and III correct. However, sodium ions do not touch each other in this structure, so choice I is incorrect. Therefore, the best choice is D, which includes only choices II and III.

Question 5

A tetrahedral hole in a crystal lattice is defined as ________

Accepted Answer

A tetrahedral hole is the space between a cluster of four adjacent atoms arranged in a tetrahedron.

Question 6

In bismuth(III)iodide,iodide ions are arranged in an hcp lattice.Assuming the ionic radii of bismuth and iodine in this compound are 117 and 206 pm,respectively,which of the following statements is correct?

Accepted Answer

The answer of In bismuth(III)iodide,iodide ions are arranged in an...

Question 7

In fluorite,________

Accepted Answer

Fluorite has a CaF2 composition where the cation (Ca2+) is smaller than the anion (F-), and there are two anions for every cation. Therefore, the correct choice is C.

Question 8

Cesium chloride adopts a simple cubic lattice where the eight Cl^- ions lie at the corners of the cubic unit cell and the Cs⁺ ion lies in the center of the cube.If the edge length of the unit cell is approximately 412.3 pm and the ionic radius of Cl^- is about 181 pm,calculate an estimate of the ionic radius of Cs⁺.

Accepted Answer

The Cs ion is located at the center of the cube, so the distance from one Cs ion to its nearest Cl ion in the cube can be calculated as follows:
Cs-Cl distance = (edge length of the unit cell)/2 - ionic radius of Cl
= 412.3 pm/2 - 181 pm
= 25.15 pm
Therefore, the Cs ion radius can be calculated by subtracting this distance from the edge length of the unit cell:
Cs ion radius = (edge length of the unit cell)/2 - Cs-Cl distance
= 412.3 pm/2 - 25.15 pm
= 176.0 pm
Therefore, the best choice is D) 176 pm.

Question 9

An ionic compound of iron and sulfur has a crystal structure in which sulfide ions create an fcc lattice and iron ions occupy half of the available tetrahedral holes.What is the empirical formula of the compound?

Accepted Answer

The compound consists of iron and sulfur ions, with iron ions occupying half of the tetrahedral holes in an fcc lattice of sulfide ions. This is consistent with the empirical formula FeS, which represents a 1:1 ratio of iron to sulfur ions. None of the other answer choices represent a plausible empirical formula for the described crystal structure.

Question 10

What is the likely unit cell for ionic compounds of 1:1 stoichiometry in which the difference in the radii is only about 25% or less?

Accepted Answer

Rock salt structure is typical for ionic compounds with a 1:1 stoichiometry and a relatively small difference in ionic radii.

Question 11

How many tennis balls will fit within the interstitial holes between a truckload of basketballs perfectly placed in a closest-packed arrangement? Assume that the tennis balls have a radius that is 20% that of a basketball.

Accepted Answer

The answer of How many tennis balls will fit within...

Question 12

A salt with the formula AB has a ratio of its ions' radii A/B = 0.28.Which structure is it likely to adopt?

Accepted Answer

The answer of A salt with the formula AB has...

Question 13

A face-centered cubic unit cell has a(n)________ in its center.

Accepted Answer

The answer of A face-centered cubic unit cell has a(n)________...

Question 14

Compare the packing efficiency of face-centered cubic gold and face-centered cubic sodium chloride.

Accepted Answer

The packing efficiency in a face-centered cubic (FCC) structure is calculated by assuming that the atoms are spheres and that they touch one another along the diagonals of a face of the unit cell. For gold, which is a metallic element, the packing efficiency can be calculated as:

Packing efficiency of FCC gold = (number of atoms) × (volume of each atom) / (volume of unit cell)
= 4 × (4/3πr^3) / (a^3/4), where r is the radius of a gold atom and a is the length of the edge of the unit cell.

For sodium chloride, which is an ionic compound, the packing efficiency can be calculated as:

Packing efficiency of FCC NaCl = (number of ions) × (volume of each ion) / (volume of unit cell)
= 4 × (4/3πr^3) / (a^3/4), where r is the radius of a chloride ion.

Since both FCC gold and FCC sodium chloride have the same number of atoms/ions per unit cell and also have the same crystal structure, their packing efficiencies are the same. However, the size of the ions/atoms differ, so the efficiency of packing in the sodium chloride unit cell is higher.

Question 15

If half of the tetrahedral holes in a face-centered cubic unit cell are filled,what must be the stoichiometry of the ionic compound,written as nonhole sites: hole sites in lowest terms?

Accepted Answer

The answer of If half of the tetrahedral holes in...

Question 16

Magnesium oxide adopts a rock salt structure with a density of approximately 3.58 g/cm³.Based on this information,calculate an estimate of the unit cell edge length in picometers.

Accepted Answer

The rock salt structure is face-centered cubic (FCC), and the formula for density is ρ = (Z * M) / (a^3 * N_A), where Z is the number of formula units per unit cell (4 for FCC), M is the molar mass, a is the edge length, and N_A is Avogadro's number. Solving for a using the given density and molar mass of MgO (40.3 g/mol) gives approximately 421 pm.

Question 17

In the unit cell of sphalerite,________

Accepted Answer

In the sphalerite structure, half of the tetrahedral holes are filled with cations, while the other half remain empty. This arrangement is characteristic of the zinc sulfide (ZnS) crystal structure, where zinc atoms occupy half of the tetrahedral sites in the cubic close-packed (ccp) array of sulfur atoms.

Question 18

A rock salt structure has smaller ions in ________

Accepted Answer

In a rock salt structure, the smaller ions occupy the octahedral holes between the larger ions.

Question 19

In an ionic compound of cobalt and fluorine,fluoride ions adopt a closest-packed structure with cobalt ions in one half of the octahedral holes.What is the empirical formula of the compound?

Accepted Answer

The empirical formula for the compound can be determined by the ratio of cobalt ions to fluoride ions. Since each cobalt ion occupies one-half of an octahedral hole and each hole is surrounded by six fluoride ions, the ratio of cobalt to fluoride ions is 1:6. Therefore, the empirical formula of the compound is CoF6. Option C represents this empirical formula.

Question 20

In the solid-state structure of sodium chloride,the closest distance between the centers of ions is observed ________

Accepted Answer

In the solid-state structure of sodium chloride (NaCl), each sodium ion is surrounded by six chloride ions and each chloride ion is surrounded by six sodium ions in an octahedral geometry. This arrangement is consistent throughout the crystal, meaning the closest distance between the centers of ions is observed between all adjacent sodium and chloride ions, reflecting the highly symmetrical and uniform nature of the NaCl crystal structure.

Quiz 18: The Solid State-A Particulate View

In antifluorite structures,________

If a salt has a face-centered cubic (fcc) unit cell and a 1:2 cation: anion stoichiometry with cations occupying the fcc positions,then the anions fill all the ________ holes.

Which of the following contribute to the arrangement of ions in the unit cells of an ionic solid? I.The empirical formula II.The relative radii of the ions III.The shape of polyatomic ions

In the cubic closest-packed structure of sodium chloride,which ions are touching or nearly touching? I.Sodium ions and sodium ions II.Chloride ions and chloride ions III.Sodium ions and chloride ions

A tetrahedral hole in a crystal lattice is defined as ________

In bismuth(III) iodide,iodide ions are arranged in an hcp lattice.Assuming the ionic radii of bismuth and iodine in this compound are 117 and 206 pm,respectively,which of the following statements is correct?

In fluorite,________

An ionic compound of iron and sulfur has a crystal structure in which sulfide ions create an fcc lattice and iron ions occupy half of the available tetrahedral holes.What is the empirical formula of the compound?

What is the likely unit cell for ionic compounds of 1:1 stoichiometry in which the difference in the radii is only about 25% or less?

How many tennis balls will fit within the interstitial holes between a truckload of basketballs perfectly placed in a closest-packed arrangement? Assume that the tennis balls have a radius that is 20% that of a basketball.

A salt with the formula AB has a ratio of its ions' radii A/B = 0.28.Which structure is it likely to adopt?

A face-centered cubic unit cell has a(n) ________ in its center.

Compare the packing efficiency of face-centered cubic gold and face-centered cubic sodium chloride.

If half of the tetrahedral holes in a face-centered cubic unit cell are filled,what must be the stoichiometry of the ionic compound,written as nonhole sites: hole sites in lowest terms?

Magnesium oxide adopts a rock salt structure with a density of approximately 3.58 g/cm³.Based on this information,calculate an estimate of the unit cell edge length in picometers.

In the unit cell of sphalerite,________

A rock salt structure has smaller ions in ________

In an ionic compound of cobalt and fluorine,fluoride ions adopt a closest-packed structure with cobalt ions in one half of the octahedral holes.What is the empirical formula of the compound?

In the solid-state structure of sodium chloride,the closest distance between the centers of ions is observed ________

Quiz 18: The Solid State-A Particulate View

In antifluorite structures,________

If a salt has a face-centered cubic (fcc) unit cell and a 1:2 cation: anion stoichiometry with cations occupying the fcc positions,then the anions fill all the ________ holes.

Which of the following contribute to the arrangement of ions in the unit cells of an ionic solid? I.The empirical formula II.The relative radii of the ions III.The shape of polyatomic ions

In the cubic closest-packed structure of sodium chloride,which ions are touching or nearly touching? I.Sodium ions and sodium ions II.Chloride ions and chloride ions III.Sodium ions and chloride ions

A tetrahedral hole in a crystal lattice is defined as ________

In bismuth(III) iodide,iodide ions are arranged in an hcp lattice.Assuming the ionic radii of bismuth and iodine in this compound are 117 and 206 pm,respectively,which of the following statements is correct?

In fluorite,________

An ionic compound of iron and sulfur has a crystal structure in which sulfide ions create an fcc lattice and iron ions occupy half of the available tetrahedral holes.What is the empirical formula of the compound?

What is the likely unit cell for ionic compounds of 1:1 stoichiometry in which the difference in the radii is only about 25% or less?

How many tennis balls will fit within the interstitial holes between a truckload of basketballs perfectly placed in a closest-packed arrangement? Assume that the tennis balls have a radius that is 20% that of a basketball.

A salt with the formula AB has a ratio of its ions' radii A/B = 0.28.Which structure is it likely to adopt?

A face-centered cubic unit cell has a(n) ________ in its center.

Compare the packing efficiency of face-centered cubic gold and face-centered cubic sodium chloride.

If half of the tetrahedral holes in a face-centered cubic unit cell are filled,what must be the stoichiometry of the ionic compound,written as nonhole sites: hole sites in lowest terms?

Magnesium oxide adopts a rock salt structure with a density of approximately 3.58 g/cm3.Based on this information,calculate an estimate of the unit cell edge length in picometers.

In the unit cell of sphalerite,________

A rock salt structure has smaller ions in ________

In an ionic compound of cobalt and fluorine,fluoride ions adopt a closest-packed structure with cobalt ions in one half of the octahedral holes.What is the empirical formula of the compound?

In the solid-state structure of sodium chloride,the closest distance between the centers of ions is observed ________

Magnesium oxide adopts a rock salt structure with a density of approximately 3.58 g/cm³.Based on this information,calculate an estimate of the unit cell edge length in picometers.