Question 1

The two types of closest-packed lattices are ________

Accepted Answer

A) cubic closest-packed and face-centered cubic. 
B) cubic closest-packed and hexagonal closest-packed. 
C) cubic closest-packed and random closest-packed. 
D) cubic closest-packed and pyramidal closest-packed. 
E) simple cubic and hexagonal closest-packed. 
A) cubic closest-packed and face-centered cubic. 
B) cubic closest-packed and hexagonal closest-packed. 
C) cubic closest-packed and random closest-packed. 
D) cubic closest-packed and pyramidal closest-packed. 
E) simple cubic and hexagonal closest-packed.

Question 2

Iron (Fe) crystallizes as a body-centered unit cell and has an atomic radius of 126 pm. What is the edge length for the unit cell of iron?

Accepted Answer

A) 55 pm 
B) 63 pm 
C) 252 pm 
D) 291 pm 
E) 356 pm 
A) 55 pm 
B) 63 pm 
C) 252 pm 
D) 291 pm 
E) 356 pm

Question 3

Which of the following monomers is used in making the polymer illustrated below?

Accepted Answer

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

Question 4

An approximately spherical allotrope of carbon containing 60 or 70 atoms is ________

Accepted Answer

A) spherohexadecalene and spheroheptadecalene. 
B) spheralene-60 and spheralene-70. 
C) fullerene. 
D) graphitolene. 
E) soccerene. 
A) spherohexadecalene and spheroheptadecalene. 
B) spheralene-60 and spheralene-70. 
C) fullerene. 
D) graphitolene. 
E) soccerene.

Question 5

Consider the three unit cells below for ionic solids. In each unit cell, one of the ions is arranged in one of the standard unit cell structures while the other is found between these sites. What are the names of the minerals associated with each of these structures? I ________; II ________;
III ________.

Accepted Answer

rock salt

Question 6

Graphite and diamond are examples of ________ solids; sulfur and white phosphorus are examples of ________ solids; and sodium chloride and zinc sulfide are examples of ________ solids.

Accepted Answer

network co

Question 7

A face-centered cubic unit cell contains ________ octahedral holes.

Accepted Answer

A) 1 
B) 4 
C) 8 
D) 12 
E) 13 
A) 1 
B) 4 
C) 8 
D) 12 
E) 13

Question 8

Copper crystallizes in a face-centered cubic pattern. How many copper atoms are in each unit cell?

Accepted Answer

A) 2 
B) 4 
C) 8 
D) 12 
E) 14 
A) 2 
B) 4 
C) 8 
D) 12 
E) 14

Question 9

What type of packing best describes the layering pattern shown below?

Accepted Answer

A) body-centered closest-packed 
B) hexagonal closest-packed 
C) random-packed 
D) cubic closest-packed 
E) cubic packing 
A) body-centered closest-packed 
B) hexagonal closest-packed 
C) random-packed 
D) cubic closest-packed 
E) cubic packing

Question 10

Nylon is a ________

Accepted Answer

A) polyester. 
B) polyamide. 
C) polyaminoacid. 
D) polyaromatic. 
E) polyether. 
A) polyester. 
B) polyamide. 
C) polyaminoacid. 
D) polyaromatic. 
E) polyether.

Question 11

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

Accepted Answer

A) tetrahedral hole 
B) octahedral hole 
C) Atom 
D) square planar hole 
E) cubic hole 
A) tetrahedral hole 
B) octahedral hole 
C) Atom 
D) square planar hole 
E) cubic hole

Question 12

Ionic solids have ________ melting points, and are ________.

Accepted Answer

A) high; malleable 
B) high; brittle 
C) low; malleable 
D) low; brittle 
E) high; soft 
A) high; malleable 
B) high; brittle 
C) low; malleable 
D) low; brittle 
E) high; soft

Question 13

In ionic solids, one ion often occupies a hole in the unit cell defined by the other ion. In a body-centered cubic cell, what are the types and numbers of each hole?

Accepted Answer

type: octa

Question 14

How many nearest neighbor atoms are there around each atom in a body-centered cubic unit cell?

Accepted Answer

A) 4 
B) 6 
C) 8 
D) 10 
E) 12 
A) 4 
B) 6 
C) 8 
D) 10 
E) 12

Question 15

The alpha form of polonium (Po) has a density of 9.196 g/cm3 and crystallizes in a simple cubic structure. What is the atomic radius of polonium?

Accepted Answer

A) 119 pm 
B) 168 pm 
C) 266 pm 
D) 335 pm 
E) 419 pm 
A) 119 pm 
B) 168 pm 
C) 266 pm 
D) 335 pm 
E) 419 pm

Question 16

Pure solid metals ________

Accepted Answer

A) do not crystallize. 
B) are amorphous. 
C) often crystallize in closest-packed structures. 
D) often crystallize in very complex unit cells. 
E) are like liquids with the nuclei flowing through a sea of electrons. 
A) do not crystallize. 
B) are amorphous. 
C) often crystallize in closest-packed structures. 
D) often crystallize in very complex unit cells. 
E) are like liquids with the nuclei flowing through a sea of electrons.

Question 17

Which type of solid is held together by relatively weak dispersion forces?

Accepted Answer

A) ionic solid 
B) metal 
C) molecular solid 
D) ceramic 
E) semiconductor 
A) ionic solid 
B) metal 
C) molecular solid 
D) ceramic 
E) semiconductor

Question 18

Which of the following unit cells has the lowest packing efficiency?

Accepted Answer

A) simple cubic 
B) face-centered cubic 
C) body-centered cubic 
D) both face-centered and body-centered cubic 
E) Simple, face-centered, and body-centered cubic all have the same packing efficiency. 
A) simple cubic 
B) face-centered cubic 
C) body-centered cubic 
D) both face-centered and body-centered cubic 
E) Simple, face-centered, and body-centered cubic all have the same packing efficiency.

Question 19

The alpha form of polonium (Po) has a density of 9.196 g/cm3 and crystallizes in a simple cubic structure. What is the atomic radius of polonium in picometers?

Accepted Answer

Question 20

In interstitial alloys, a small ( F1F1F1S1F1F1F10 0.3) atomic radius ratio would indicate an atom would fit in what type of hole(s)?

Accepted Answer

A) tetrahedral hole 
B) octahedral hole 
C) cubic hole 
D) both an octahedral and tetrahedral hole 
E) both an octahedral and cubic hole 
A) tetrahedral hole 
B) octahedral hole 
C) cubic hole 
D) both an octahedral and tetrahedral hole 
E) both an octahedral and cubic hole

Exam 12: Solids: Crystals, Alloys, and Polymers

The two types of closest-packed lattices are ________

Iron (Fe) crystallizes as a body-centered unit cell and has an atomic radius of 126 pm. What is the edge length for the unit cell of iron?

Which of the following monomers is used in making the polymer illustrated below?

An approximately spherical allotrope of carbon containing 60 or 70 atoms is ________

Graphite and diamond are examples of ________ solids; sulfur and white phosphorus are examples of ________ solids; and sodium chloride and zinc sulfide are examples of ________ solids.

A face-centered cubic unit cell contains ________ octahedral holes.

Copper crystallizes in a face-centered cubic pattern. How many copper atoms are in each unit cell?

What type of packing best describes the layering pattern shown below?

Nylon is a ________

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

Ionic solids have ________ melting points, and are ________.

In ionic solids, one ion often occupies a hole in the unit cell defined by the other ion. In a body-centered cubic cell, what are the types and numbers of each hole?

How many nearest neighbor atoms are there around each atom in a body-centered cubic unit cell?

The alpha form of polonium (Po) has a density of 9.196 g/cm3 and crystallizes in a simple cubic structure. What is the atomic radius of polonium?

Pure solid metals ________

Which type of solid is held together by relatively weak dispersion forces?

Which of the following unit cells has the lowest packing efficiency?

The alpha form of polonium (Po) has a density of 9.196 g/cm3 and crystallizes in a simple cubic structure. What is the atomic radius of polonium in picometers?

In interstitial alloys, a small (  0.3) atomic radius ratio would indicate an atom would fit in what type of hole(s)?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Graphite and diamond are examples of solids; sulfur and white phosphorus are examples of solids; and sodium chloride and zinc sulfide are examples of solids.

Ionic solids have melting points, and are .

The alpha form of polonium (Po) has a density of 9.196 g/cm³ and crystallizes in a simple cubic structure. What is the atomic radius of polonium?

The alpha form of polonium (Po) has a density of 9.196 g/cm³ and crystallizes in a simple cubic structure. What is the atomic radius of polonium in picometers?