Question 1

Researchers at the University of Texas at Austin prepared a linear allotrope of carbon in 1998. What is the hybridization of its atomic orbitals?

Accepted Answer

A)  sp 
B)  sp2 
C)  sp3 
D)  dsp3 
E)  Cannot be determined from the information provided. 
A)  sp 
B)  sp2 
C)  sp3 
D)  dsp3 
E)  Cannot be determined from the information provided.

Question 2

Which two of the following elements are found as a covalent network solid?
I.beryllium
II.carbon
III.phosphorus
IV.sulfur

Accepted Answer

A)  I and II 
B)  I and III 
C)  II and III 
D)  II and IV 
E)  III and IV 
A)  I and II 
B)  I and III 
C)  II and III 
D)  II and IV 
E)  III and IV

Question 3

In addition to carbon and iron, stainless steel contains ________

Accepted Answer

A)  Teflon and polyethylene. 
B)  gold and silver. 
C)  copper and nickel. 
D)  chromium and nickel. 
E)  platinum. 
A)  Teflon and polyethylene. 
B)  gold and silver. 
C)  copper and nickel. 
D)  chromium and nickel. 
E)  platinum.

Question 4

In the Bragg equation, $\theta$refers to the angle of ________ or ________and 2$\theta$ refers to the angle of ________.

Accepted Answer

incidence;

Question 5

Polonium crystallizes in a simple cubic pattern. How many polonium atoms are in each unit cell?

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

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

In the sodium chloride unit cell, the chloride ions form a cube in which each side is arranged like the following figure. The circles represent the positions of the chloride ions on one square face of the cube. All the other faces are the same. What is the name of this unit cell?

Accepted Answer

A)  simple cubic 
B)  chloride-centered cubic 
C)  face-centered cubic 
D)  x-face cubic 
E)  body-centered cubic 
A)  simple cubic 
B)  chloride-centered cubic 
C)  face-centered cubic 
D)  x-face cubic 
E)  body-centered cubic

Question 8

Electrical and thermal conductivity in metals ________

Accepted Answer

A)  is explained by a dipolar coupling model. 
B)  is explained by band theory. 
C)  is explained by matrix isolation techniques. 
D)  is explained by temporary ionization. 
E)  is a function of the level of contamination by excess electrons. 
A)  is explained by a dipolar coupling model. 
B)  is explained by band theory. 
C)  is explained by matrix isolation techniques. 
D)  is explained by temporary ionization. 
E)  is a function of the level of contamination by excess electrons.

Question 9

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

A)  equal number of tennis balls and basketballs 
B)  twice as many tennis balls as basketballs 
C)  three times as many tennis balls as basketballs 
D)  four times as many tennis balls as basketballs 
E)  five times as many tennis balls as basketballs 
A)  equal number of tennis balls and basketballs 
B)  twice as many tennis balls as basketballs 
C)  three times as many tennis balls as basketballs 
D)  four times as many tennis balls as basketballs 
E)  five times as many tennis balls as basketballs

Question 10

The molecular orbital description for metal bonding is different from that for diatomic molecules in that ________

Accepted Answer

A)  there are no antibonding orbitals in the metal bonding description. 
B)  quantum theory no longer applies as the orbitals are continuous. 
C)  the orbitals are so close in energy that they are referred to as bands. 
D)  the increased number of electrons results in each bond being stronger. 
E)  All of the above are true. 
A)  there are no antibonding orbitals in the metal bonding description. 
B)  quantum theory no longer applies as the orbitals are continuous. 
C)  the orbitals are so close in energy that they are referred to as bands. 
D)  the increased number of electrons results in each bond being stronger. 
E)  All of the above are true.

Question 11

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 12

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 13

In antifluorite structures, ________

Accepted Answer

A)  cations are smaller than the anions, and there are two cations for every anion. 
B)  anions are smaller than the cations, and there are two anions for every cation. 
C)  cations are smaller than the anions, and there are two anions for every cation. 
D)  anions are smaller than the cations, and there are two cations for every anion. 
E)  anions and cations are the same size. 
A)  cations are smaller than the anions, and there are two cations for every anion. 
B)  anions are smaller than the cations, and there are two anions for every cation. 
C)  cations are smaller than the anions, and there are two anions for every cation. 
D)  anions are smaller than the cations, and there are two cations for every anion. 
E)  anions and cations are the same size.

Question 14

Which two of the following elements are not found as a covalent network solid?
I.beryllium
II.carbon
III.phosphorus
IV.sulfur

Accepted Answer

A)  I and III 
B)  I and II 
C)  I and IV 
D)  II and III 
E)  II and IV 
A)  I and III 
B)  I and II 
C)  I and IV 
D)  II and III 
E)  II and IV

Question 15

Glass is a term used to describe any solid that is ________

Accepted Answer

A)  crystalline. 
B)  amorphous. 
C)  a liquid crystal. 
D)  a crystalline liquid. 
E)  transparent. 
A)  crystalline. 
B)  amorphous. 
C)  a liquid crystal. 
D)  a crystalline liquid. 
E)  transparent.

Question 16

In a two-component alloy the more abundant metal can be thought of as the solvent while the less abundant metal can be thought of as the solute. Which of the following would not change the position of atoms in the solvent's unit cell?
I.a solute with the same atomic radius as the solvent
II.a solute that was sufficiently small to fit into holes in the solvent's unit cell
III.a solvent that was sufficiently small to fit into holes in the solute's unit cell

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I or II 
E)  I, II, or III 
A)  I only 
B)  II only 
C)  III only 
D)  I or II 
E)  I, II, or III

Question 17

Aluminum (Al) has a density of 2.70 g/cm3 and crystallizes in a face-centered cubic structure. What is the unit cell edge length in picometers?

Accepted Answer

Question 18

Which of the following is true regarding the attractive force that holds sodium chloride in the solid state?
I.It is electrostatic.
II.It is termed ionic bonding.
III.It depends on the distance between the sodium and chloride.
IV.It only operates between adjacent sodium and chloride.

Accepted Answer

A)  I and II only 
B)  II and III only 
C)  I, II, and III only 
D)  II and IV only 
E)  I-IV are all true statements. 
A)  I and II only 
B)  II and III only 
C)  I, II, and III only 
D)  II and IV only 
E)  I-IV are all true statements.

Question 19

Molecular orbital theory can be applied ________

Accepted Answer

A)  only to two adjacent metal atoms. 
B)  only to a few metal atoms that are very close to each other. 
C)  to any number of metal atoms. 
D)  to nonmetals only, not to metals. 
E)  to nonmetals and ionic bonds only, not to metals. 
A)  only to two adjacent metal atoms. 
B)  only to a few metal atoms that are very close to each other. 
C)  to any number of metal atoms. 
D)  to nonmetals only, not to metals. 
E)  to nonmetals and ionic bonds only, not to metals.

Question 20

In fluorite, ________

Accepted Answer

A)  cations are smaller than the anions, and there are two cations for every anion. 
B)  anions are smaller than the cations, and there are two anions for every cation. 
C)  cations are smaller than the anions, and there are two anions for every cation. 
D)  anions are smaller than the cations, and there are two cations for every anion. 
E)  anions and cations are the same size. 
A)  cations are smaller than the anions, and there are two cations for every anion. 
B)  anions are smaller than the cations, and there are two anions for every cation. 
C)  cations are smaller than the anions, and there are two anions for every cation. 
D)  anions are smaller than the cations, and there are two cations for every anion. 
E)  anions and cations are the same size.

Exam 12: Solids: Structures and Applications

Researchers at the University of Texas at Austin prepared a linear allotrope of carbon in 1998. What is the hybridization of its atomic orbitals?

Which two of the following elements are found as a covalent network solid? I.beryllium II.carbon III.phosphorus IV.sulfur

In addition to carbon and iron, stainless steel contains ________

In the Bragg equation, θ\thetaθ refers to the angle of ________ or ________and 2 θ\thetaθ refers to the angle of ________.

Polonium crystallizes in a simple cubic pattern. How many polonium atoms are in each unit cell?

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.

In the sodium chloride unit cell, the chloride ions form a cube in which each side is arranged like the following figure. The circles represent the positions of the chloride ions on one square face of the cube. All the other faces are the same. What is the name of this unit cell?

Electrical and thermal conductivity in metals ________

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.

The molecular orbital description for metal bonding is different from that for diatomic molecules in that ________

Pure solid metals ________

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

In antifluorite structures, ________

Which two of the following elements are not found as a covalent network solid? I.beryllium II.carbon III.phosphorus IV.sulfur

Glass is a term used to describe any solid that is ________

Aluminum (Al) has a density of 2.70 g/cm3 and crystallizes in a face-centered cubic structure. What is the unit cell edge length in picometers?

Which of the following is true regarding the attractive force that holds sodium chloride in the solid state? I.It is electrostatic. II.It is termed ionic bonding. III.It depends on the distance between the sodium and chloride. IV.It only operates between adjacent sodium and chloride.

Molecular orbital theory can be applied ________

In fluorite, ________

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

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

In the Bragg equation, $\theta$ refers to the angle of or and 2 $\theta$ refers to the angle of .

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.

Aluminum (Al) has a density of 2.70 g/cm³ and crystallizes in a face-centered cubic structure. What is the unit cell edge length in picometers?