Question 1

Which of the following best describes calcium hydride (CaH2)at room temperature and pressure?

Accepted Answer

A) nonpolar molecular gas 
B) metallic solid 
C) ionic solid 
D) polar molecular gas 
E) covalent network solid 
A) nonpolar molecular gas 
B) metallic solid 
C) ionic solid 
D) polar molecular gas 
E) covalent network solid

Question 2

The metal sodium crystallizes in a body-centered cubic lattice.If the density of sodium is 0.968 g/cm3,what is the atomic volume of sodium?​

Accepted Answer

A) ​4.76 × 104 pm3 
B) ​2.38 × 104 pm3 
C) ​1.34 × 107 pm3 
D) ​1.17 × 106 pm3 
E) ​2.68 × 107 pm3 
A) ​4.76 × 104 pm3 
B) ​2.38 × 104 pm3 
C) ​1.34 × 107 pm3 
D) ​1.17 × 106 pm3 
E) ​2.68 × 107 pm3

Question 3

Which of the following pure substances has the highest normal melting point?

Accepted Answer

A) KF 
B) KI 
C) NaF 
D) NaCl 
E) NaI 
A) KF 
B) KI 
C) NaF 
D) NaCl 
E) NaI

Question 4

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

Accepted Answer

A) ​   cm3 
B) ​   cm3 
C) ​   cm3 
D) ​   cm3 
E)    ​​ cm3 
A) ​   cm3 
B) ​   cm3 
C) ​   cm3 
D) ​   cm3 
E)    ​​ cm3

Question 5

If the diameter of a spherical water droplet is 100.0 μm,how much energy is required to increase the diameter of the water droplet by 5.0 μm? The surface tension of water is 1.0 × 10-3 J/m2.

Accepted Answer

A) 3.1 × 10-11 J 
B) 3 × 10-12 J 
C) 7.9 × 10-14 J 
D) 1 × 10-11 J 
E) 4 × 10-11 J 
A) 3.1 × 10-11 J 
B) 3 × 10-12 J 
C) 7.9 × 10-14 J 
D) 1 × 10-11 J 
E) 4 × 10-11 J

Question 6

Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides?

Accepted Answer

A) The H-F bond in hydrogen fluoride is very strong. 
B) Hydrogen fluoride has very strong London dispersion forces. 
C) Hydrogen fluoride is capable of forming hydrogen bonds. 
D) Hydrogen fluoride is ionic. 
E) Hydrogen fluoride is covalent. 
A) The H-F bond in hydrogen fluoride is very strong. 
B) Hydrogen fluoride has very strong London dispersion forces. 
C) Hydrogen fluoride is capable of forming hydrogen bonds. 
D) Hydrogen fluoride is ionic. 
E) Hydrogen fluoride is covalent.

Question 7

What is the value of q when 8.29 g of water vaporizes at 373 K? The enthalpy of condensation of water at 373 K is -40.7 kJ/mol.

Accepted Answer

A) -337 kJ 
B) -18.7 kJ 
C) 18.7 kJ 
D) 337 kJ 
E) 0.203 kJ 
A) -337 kJ 
B) -18.7 kJ 
C) 18.7 kJ 
D) 337 kJ 
E) 0.203 kJ

Question 8

Identify the van der Waals equation.

Accepted Answer

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

Question 9

Platinum crystallizes with a face-centered cubic unit cell.If the edge length of the unit cell is 393 pm,what is the radius of a platinum atom in picometers?

Accepted Answer

A) 139 pm 
B) 556 pm 
C) 1110 pm 
D) 321 pm 
E) 49.1 pm 
A) 139 pm 
B) 556 pm 
C) 1110 pm 
D) 321 pm 
E) 49.1 pm

Question 10

Which of the following processes is exothermic?

Accepted Answer

A) condensation of water 
B) fusion of ethanol 
C) vaporization of water 
D) evaporation of ammonia 
E) sublimation of carbon dioxide 
A) condensation of water 
B) fusion of ethanol 
C) vaporization of water 
D) evaporation of ammonia 
E) sublimation of carbon dioxide

Question 11

The vapor pressure of a liquid increases with increasing temperature.Which of the following statements best explains this relationship?

Accepted Answer

A) All the molecules have greater kinetic energies. 
B) The number of gaseous molecules above the liquid remains constant,but these molecules have greater average kinetic energy. 
C) The faster-moving molecules in the liquid exert a greater pressure. 
D) The intermolecular forces between the molecules decrease at higher temperatures. 
E) The average kinetic energy of molecules is greater; thus more molecules can enter the gaseous state. 
A) All the molecules have greater kinetic energies. 
B) The number of gaseous molecules above the liquid remains constant,but these molecules have greater average kinetic energy. 
C) The faster-moving molecules in the liquid exert a greater pressure. 
D) The intermolecular forces between the molecules decrease at higher temperatures. 
E) The average kinetic energy of molecules is greater; thus more molecules can enter the gaseous state.

Question 12

Each atom in a body-centered lattice has a coordination number of _____.

Accepted Answer

A) ​12 
B) ​8 
C) ​15 
D) ​6 
E) ​20 
A) ​12 
B) ​8 
C) ​15 
D) ​6 
E) ​20

Question 13

Which of the following pure substances has the highest normal melting point?

Accepted Answer

A) P4O10 
B) P4O6 
C) CO2 
D) CaO 
E) Na2O 
A) P4O10 
B) P4O6 
C) CO2 
D) CaO 
E) Na2O

Question 14

Rank the following in order of increasing normal boiling point: N2,O2,Br2,Xe.

Accepted Answer

A) N2 2 2 
B) O2 2 2 
C) Br2 2 2 
D) N2 2 2 2 2 2 
A) N2 2 2 
B) O2 2 2 
C) Br2 2 2 
D) N2 2 2 2 2 2

Question 15

When a solid undergoes a phase change to a gas,the process is called

Accepted Answer

A) fusion. 
B) condensation. 
C) melting. 
D) vaporization. 
E) sublimation. 
A) fusion. 
B) condensation. 
C) melting. 
D) vaporization. 
E) sublimation.

Question 16

Which of the following statements concerning the determination of crystal structure by x-ray diffraction is incorrect?

Accepted Answer

A) X-rays are reflected from the repeating planes of an ordered crystal lattice. 
B) A diffraction pattern reveals the locations of the electrons in a crystal. 
C) Analysis of a diffraction pattern reveals the structure of a crystal. 
D) X-rays undergo constructive and destructive interference upon reflection in a crystal lattice. 
E) A diffraction pattern from a crystal depends on the incident angle of the x-rays. 
A) X-rays are reflected from the repeating planes of an ordered crystal lattice. 
B) A diffraction pattern reveals the locations of the electrons in a crystal. 
C) Analysis of a diffraction pattern reveals the structure of a crystal. 
D) X-rays undergo constructive and destructive interference upon reflection in a crystal lattice. 
E) A diffraction pattern from a crystal depends on the incident angle of the x-rays.

Question 17

The strongest intermolecular forces present in a sample of pure I2 are

Accepted Answer

A) London forces. 
B) dipole-dipole forces. 
C) metallic bonds. 
D) covalent network bonds. 
E) covalent bonds. 
A) London forces. 
B) dipole-dipole forces. 
C) metallic bonds. 
D) covalent network bonds. 
E) covalent bonds.

Question 18

A solid has a very high melting point,is hard,and in the molten state is a non-conductor.The solid is most likely

Accepted Answer

A) a covalent network solid. 
B) a metallic solid. 
C) an amorphous solid. 
D) a molecular solid. 
E) an ionic solid. 
A) a covalent network solid. 
B) a metallic solid. 
C) an amorphous solid. 
D) a molecular solid. 
E) an ionic solid.

Question 19

Choose the correct statement about the diagram below.

Accepted Answer

A) The diagram shows the triple point above 1 atm pressure. 
B) The diagram is qualitatively correct for water. 
C) The diagram shows that the melting point of the solid increases with increasing pressure. 
D) The diagram could represent the phase diagram of CO2. 
E) None of the above statements is correct. 
A) The diagram shows the triple point above 1 atm pressure. 
B) The diagram is qualitatively correct for water. 
C) The diagram shows that the melting point of the solid increases with increasing pressure. 
D) The diagram could represent the phase diagram of CO2. 
E) None of the above statements is correct.

Question 20

The unit cell in a certain lattice consists of a cube formed by an anion at each corner,an anion in the center,and a cation at the center of each face.The unit cell contains a net:

Accepted Answer

A) 2 anions and 3 cations. 
B) 2 anions and 2 cations. 
C) 5 anions and 3 cations. 
D) 3 anions and 4 cations. 
E) 5 anions and 6 cations. 
A) 2 anions and 3 cations. 
B) 2 anions and 2 cations. 
C) 5 anions and 3 cations. 
D) 3 anions and 4 cations. 
E) 5 anions and 6 cations.

Exam 11: States of Matter; Liquids and Solids

Which of the following best describes calcium hydride (CaH2)at room temperature and pressure?

The metal sodium crystallizes in a body-centered cubic lattice.If the density of sodium is 0.968 g/cm3,what is the atomic volume of sodium?​

Which of the following pure substances has the highest normal melting point?

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

If the diameter of a spherical water droplet is 100.0 μm,how much energy is required to increase the diameter of the water droplet by 5.0 μm? The surface tension of water is 1.0 × 10-3 J/m2.

Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides?

What is the value of q when 8.29 g of water vaporizes at 373 K? The enthalpy of condensation of water at 373 K is -40.7 kJ/mol.

Identify the van der Waals equation.

Platinum crystallizes with a face-centered cubic unit cell.If the edge length of the unit cell is 393 pm,what is the radius of a platinum atom in picometers?

Which of the following processes is exothermic?

The vapor pressure of a liquid increases with increasing temperature.Which of the following statements best explains this relationship?

Each atom in a body-centered lattice has a coordination number of _____.

Which of the following pure substances has the highest normal melting point?

Rank the following in order of increasing normal boiling point: N2,O2,Br2,Xe.

When a solid undergoes a phase change to a gas,the process is called

Which of the following statements concerning the determination of crystal structure by x-ray diffraction is incorrect?

The strongest intermolecular forces present in a sample of pure I2 are

A solid has a very high melting point,is hard,and in the molten state is a non-conductor.The solid is most likely

Choose the correct statement about the diagram below.

The unit cell in a certain lattice consists of a cube formed by an anion at each corner,an anion in the center,and a cation at the center of each face.The unit cell contains a net:

Chemistry and Measurement

Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

Solutions

Rates of Reaction

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

Organic Chemistry

Polymer Materials: Synthetic and Biological

Filters

Which of the following best describes calcium hydride (CaH₂)at room temperature and pressure?

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

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

If the diameter of a spherical water droplet is 100.0 μm,how much energy is required to increase the diameter of the water droplet by 5.0 μm? The surface tension of water is 1.0 × 10^-3 J/m².

Rank the following in order of increasing normal boiling point: N₂,O₂,Br₂,Xe.

The strongest intermolecular forces present in a sample of pure I₂ are