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Chemistry 6th Edition McMurry Fay Test Bank

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Chemistry 6th Edition McMurry Fay Test Bank

ISBN-13: 978-0321704955

ISBN-10: 0321704959

 

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Chemistry 6th Edition McMurry Fay Test Bank

ISBN-13: 978-0321704955

ISBN-10: 0321704959

 

 

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Chemistry, 6e (McMurry/Fay)

Chapter 10   Liquids, Solids, and Phase Changes

 

10.1   Multiple-Choice Questions

 

1) The bonds in the polyatomic ion CO32– are classified as

  1. A) ionic
  2. B) metallic
  3. C) nonpolar covalent
  4. D) polar covalent

Answer:  D

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

2) Which covalent bond is the most polar?

  1. A) NF
  2. B) CF
  3. C) ClF
  4. D) FF

Answer:  B

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

3) Which has a dipole moment?

  1. A) CO2
  2. B) CO32–
  3. C) SO2
  4. D) SO42–

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

4) Which of the following molecules does not have a dipole moment?

  1. A) CH2=CH2
  2. B) NH3
  3. C) CH3NH2
  4. D) HCl

Answer:  A

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

5) Which of the following should have the largest dipole moment?

  1. A) H2(g)
  2. B) CO2(g)
  3. C) KCl(g)
  4. D) CH3F(g)

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

 

6) The dipole moment of ClF is 0.88 D, and its bond length is 163 pm. What is the percent ionic character of the ClF bond?

  1. A) 0.54%
  2. B) 7.8%
  3. C) 11%
  4. D) 25%

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

7) The dipole moment of BrF is 1.29 D, and its bond length is 178 pm. What is the percent ionic character of the BrF bond?

  1. A) 3.9%
  2. B) 8.5%
  3. C) 15%
  4. D) 33%

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

8) AgCl is found to have 78.1% ionic character, and its gas phase dipole moment is 11.5 D. What is the distance between the Ag and Cl atoms in gaseous AgCl?

  1. A) 9.19 x 10-10pm
  2. B) 14.7 pm
  3. C) 307 pm
  4. D) 903 pm

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

9) Which compound, shown with its dipole moment, is expected to exhibit the smallest percent ionic character?

  1. A) HCl, 1.11 D
  2. B) HF, 1.83 D
  3. C) LiH,6.00 D
  4. D) LiF, 6.28 D

Answer:  A

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

10) The HI bond has a length of 161 pm and 4.92% ionic character. What is the experimental dipole moment of HI?

  1. A) 0.380 D
  2. B) 0.772 D
  3. C) 3.80 D
  4. D) 7.72 D

Answer:  A

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

 

11) Which compound below could have a zero dipole moment?

  1. A) CCl2F2(tetrahedral)
  2. B) CuCl2F2(tetrahedral)
  3. C) PtCl2F2(square planar)
  4. D) SCl2F2(see-saw)

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

12) Which has the smallest dipole-dipole forces?

  1. A) CH3F
  2. B) HCl
  3. C) N2
  4. D) CO

Answer:  C

Topic:  Section 10.2 Intermolecular Forces

 

13) Which of the following compounds exhibits hydrogen bonding?

  1. A) CH3Cl
  2. B) HI
  3. C) H3C-O-CH3
  4. D) NH3

Answer:  D

Topic:  Section 10.2 Intermolecular Forces

 

14) Which of the following exhibits ion-dipole forces?

  1. A) NaCl(s)
  2. B) NaCl(aq)
  3. C) Na(s)
  4. D) Cl2(g)

Answer:  B

Topic:  Section 10.2 Intermolecular Forces

15) Which is expected to have the largest dispersion forces?

  1. A) C2H6
  2. B) C8H18
  3. C) N2
  4. D) CO2

Answer:  B

Topic:  Section 10.2 Intermolecular Forces

 

 

16) Which substance in each of the following pairs is expected to have the larger dispersion forces?

 

 

  1. A) Br2in set I and n-butane in set II
  2. B) Br2in set I and isobutane in set II
  3. C) I2in set I and n-butane in set II
  4. D) I2in set I and isobutane in set II

Answer:  C

Topic:  Section 10.2 Intermolecular Forces

 

17) Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?

  1. A) N2
  2. B) HBr
  3. C) CO2
  4. D) H2O

Answer:  B

Topic:  Section 10.2 Intermolecular Forces

18) In liquid methanol, CH3OH, which intermolecular forces are present?

  1. A) Dispersion, hydrogen bonding and dipole-dipole forces are present.
  2. B) Only dipole-dipole and ion-dipole forces are present.
  3. C) Only dispersion and dipole-dipole forces are present.
  4. D) Only hydrogen bonding forces are present.

Answer:  A

Topic:  Section 10.2 Intermolecular Forces

 

19) When a narrow diameter glass tube is inserted into a body of water, water rises in the tube and its surface inside is concave upwards. Which statement, concerning the strength of the intermolecular forces between glass and water molecules compared to those between water molecules, is accurate?

  1. A) The forces of attraction between the glass and water are weaker than those in water.
  2. B) The forces of attraction between the glass and water are stronger than those in water.
  3. C) The forces of attraction between the glass and water are the same as those in water.
  4. D) Intermolecular forces are irrelevant to this situation.

Answer:  B

Topic:  Section 10.3 Some Properties of Liquids

 

 

20) Which of the intermolecular forces is the most important contributor to the high surface tension shown by water?

  1. A) dipole-dipole forces
  2. B) dispersion forces
  3. C) hydrogen bonding
  4. D) ion-dipole forces

Answer:  C

Topic:  Section 10.3 Some Properties of Liquids

 

21) The property of a liquid that measure the liquid’s resistance to flow is

  1. A) boiling point.
  2. B) heat of vaporization.
  3. C) surface tension.
  4. D) viscosity.

Answer:  D

Topic:  Section 10.3 Some Properties of Liquids

 

22) Which of the following is most likely to have the highest viscosity at 25°C?

  1. A) C4H10
  2. B) HOCH2CH2OH
  3. C) C8H18
  4. D) C2H5NH2

Answer:  B

Topic:  Section 10.3 Some Properties of Liquids

23) Which is expected to have the highest surface tension at 25°?

  1. A) C5H12
  2. B) C6H6
  3. C) C2H5OH
  4. D) C3H5(OH)3

Answer:  D

Topic:  Section 10.3 Some Properties of Liquids

 

24) The magnitude of the heats of vaporization, fusion and sublimation of a substance reflect the

  1. A) density of the substance.
  2. B) magnitudes of the boiling and melting points of the substance.
  3. C) strength of the covalent bonds between atoms in each molecule of the substance.
  4. D) strength of the intermolecular forces of the substance.

Answer:  D

Topic:  Section 10.4 Phase Changes

 

25) For a particular compound, which is expected to be the largest in general?

  1. A) the heat required to raise the temperature of one mole of the gas 10.0°C
  2. B) the heat required to raise the temperature of one mole of the liquid 10.0°C
  3. C) the molar heat of fusion at the normal melting point
  4. D) the molar heat of vaporization at the normal boiling point

Answer:  D

Topic:  Section 10.4 Phase Changes

 

26) Which of the following phase changes has a positive value for its entropy change?

  1. A) boiling water
  2. B) formation of raindrops from a cloud
  3. C) making dry ice from gaseous CO2
  4. D) making ice cubes from liquid water

Answer:  A

Topic:  Section 10.4 Phase Changes

 

27) For which of the following phase changes is the sign of ΔS negative?

  1. A) boiling of water
  2. B) formation of snow from water vapor in clouds
  3. C) melting of ice cream
  4. D) sublimation of I2

Answer:  B

Topic:  Section 10.4 Phase Changes

28) When a substance melts at its normal melting point, the sign of ΔH is ________ and the sign of ΔS of this phase change is ________.

  1. A) +, –
  2. B) -, +
  3. C) +, +
  4. D) -, –

Answer:  C

Topic:  Section 10.4 Phase Changes

 

29) Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes. The heat of vaporization is 26.4 kJ/mol. How much heat could be removed by 10.0 g of ethyl chloride?

  1. A) 4.09 kJ
  2. B) 170 kJ
  3. C) 264 kJ
  4. D) 1700 kJ

Answer:  A

Topic:  Section 10.4 Phase Changes

 

30) Bromine is one of only two elements that is a liquid at room temperature. Bromine has a heat of vaporization of 30.91 kJ/mol and its boiling point is 59°C. What is the entropy of vaporization for bromine?

  1. A) -301 J/(mol ∙ K)
  2. B) -93.1 J/(mol ∙ K)
  3. C) 10.7 J/(mol ∙ K)
  4. D) 93.1 J/(mol ∙ K)

Answer:  D

Topic:  Section 10.4 Phase Changes

 

 

31) CFC-11 (trichlorofluoromethane, CCl3F) has been used for many years as the working fluid in refrigerators. Given its heat of vaporization is 26.88 kJ/mol and its entropy of vaporization is 90.51 J/(mol ∙ K), what is the boiling point of CFC-11?

  1. A) -272.9°C
  2. B) 0.297°C
  3. C) 2.44°C
  4. D) 23.8°C

Answer:  D

Topic:  Section 10.4 Phase Changes

32) How much heat is released when 75.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).

  1. A) 54.8 kJ
  2. B) 195 kJ
  3. C) 228 kJ
  4. D) 248 kJ

Answer:  C

Topic:  Section 10.4 Phase Changes

 

33) For the process: HNO3(g) ⇌ HNO3(l)

ΔH° is -39.04 kJ/mol and ΔS° is -111.74 J/(mol ∙ K). What is the normal boiling point of pure HNO3?

  1. A) 2.86°C
  2. B) 76.2°C
  3. C) 270.3°C
  4. D) 349.4°C

Answer:  B

Topic:  Section 10.4 Phase Changes

 

34) When a liquid is heated at its boiling point, the

  1. A) covalent bonds are broken, allowing vaporization to occur.
  2. B) temperature of the liquid increases.
  3. C) temperature of the liquid remains the same as long as any liquid is present.
  4. D) temperature of the vapor phase increases.

Answer:  C

Topic:  Section 10.4 Phase Changes

 

35) As a liquid evaporates at a temperature below its boiling point, the temperature of the liquid

  1. A) decreases.
  2. B) decreases at low temperatures, but increases at high temperatures.
  3. C) increases.
  4. D) remains unchanged.

Answer:  A

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

 

36) Molecules of a liquid can pass into the vapor phase only if the

  1. A) liquid has little surface tension.
  2. B) molecules have sufficient kinetic energy to overcome the intermolecular forces in the liquid.
  3. C) temperature of the liquid is near its boiling point.
  4. D) vapor pressure of the liquid is high.

Answer:  B

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

37) The vapor pressure of a pure liquid increases as the

  1. A) average kinetic energy of the molecules in the liquid phase decreases.
  2. B) intermolecular attractive forces increase.
  3. C) temperature of the liquid phase decreases.
  4. D) temperature of the liquid phase increases.

Answer:  D

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

38) The normal boiling point occurs when the

  1. A) intermolecular forces within the liquid phase are broken.
  2. B) temperature of the pure liquid equals the external temperature.
  3. C) vapor pressure of a pure liquid equals an external pressure of one atmosphere.
  4. D) vapor pressure of the liquid equals the external pressure.

Answer:  C

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

39) Which of the following compounds has the highest boiling point?

  1. A) H2O
  2. B) HCl
  3. C) H2S
  4. D) NH3

Answer:  A

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

40) Which of the following substances has the highest boiling point?

  1. A) CH3-CH2-CH2-CH2-CH3
  2. B) Xe
  3. C) CH3-CH2-CH3
  4. D) (CH3)4C

Answer:  A

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

41) Which of the following compounds has the highest boiling point?

  1. A) CH3CH2OH
  2. B) HOCH2CH2OH
  3. C) H3C-O-CH3
  4. D) CH3CH2CH2CH3

Answer:  B

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

42) Arrange the following in order of increasing boiling point.

CH3CH2OH      CH3CH2CH3       H3C-O-CH3       CH3CH2NH2

I                          II                           III                         IV

  1. A) IV < III < II < I
  2. B) II < III < IV < I
  3. C) I < IV < III < II
  4. D) II < III < I < IV

Answer:  B

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

43) The normal boiling point for HBr is higher than the normal boiling point for HCl. This can be explained by

  1. A) larger dipole-dipole forces for HBr.
  2. B) larger dispersion forces for HBr.
  3. C) larger hydrogen-bond forces for HBr.
  4. D) larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for HBr.

Answer:  B

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

44) A kitchen pressure cooker operates at 1.50 atm. The ΔHvap of water is 40.7 kJ/mol. What is the boiling point of water in the pressure cooker?

  1. A) 362 K
  2. B) 373 K
  3. C) 385 K
  4. D) 410 K

Answer:  C

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

45) While mercury is very useful in barometers, mercury vapor is toxic. Given that mercury has a ΔHvap of 59.11 kJ/mol and its normal boiling point is 356.7°C, calculate the vapor pressure in mm Hg at room temperature, 25°C.

  1. A) 2.68 × 10-3mm Hg
  2. B) 2.99 mm Hg
  3. C) 372 mm Hg
  4. D) 753 mm Hg

Answer:  A

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

46) Hydroquinone is an antioxidant that is also used as a photographic reducer and developer. The normal boiling point of hydroquinone is 310°C. Calculate the pressure at which hydroquinone will boil at 200°C given that its ΔHvap is 73.38 kJ/mol.

  1. A) 1.210 × 10-4mm Hg
  2. B) 1.35 mm Hg
  3. C) 22.5 mm Hg
  4. D) 757 mm Hg

Answer:  C

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

47) The vapor pressure of liquid chloroform, CHCl3, is 400.0 torr at 24.1°C and 100.0 torr at -6.3°C. What is ΔHvap of chloroform?

  1. A) 15.3 kJ/mol
  2. B) 30.1 kJ/mol
  3. C) 57.6 kJ/mol
  4. D) 86.7 kJ/mol

Answer:  B

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

48) Solids having no ordered long-range structure are classified as

  1. A) amorphous
  2. B) crystalline
  3. C) metallic
  4. D) molecular

Answer:  A

Topic:  Section 10.6 Kinds of Solids

 

49) Which is classified as an amorphous solid?

  1. A) palladium(II) chloride
  2. B) phosphorus tetrachloride
  3. C) plastic
  4. D) platinum

Answer:  C

Topic:  Section 10.6 Kinds of Solids

 

50) Which of the following forms a molecular solid?

  1. A) CaO
  2. B) C10H22
  3. C) C(graphite)
  4. D) gold

Answer:  B

Topic:  Section 10.6 Kinds of Solids

51) Which of the following statements is not consistent with the properties of a molecular solid?

  1. A) a compound that conducts electricity when molten
  2. B) a low melting solid
  3. C) a solid formed by the combination of two nonmetallic elements
  4. D) a solid that is a nonconductor of electricity

Answer:  A

Topic:  Section 10.6 Kinds of Solids

 

52) Which of the following forms an ionic solid?

  1. A) Ag
  2. B) C7H15NH2
  3. C) RbI
  4. D) SO3

Answer:  C

Topic:  Section 10.6 Kinds of Solids

 

53) A crystalline solid of unknown origin forms an aqueous solution that conducts an electrical current. The solid has a high melting point and shatters when struck with a hammer. The solid is likely to be

  1. A) a covalent network solid.
  2. B) an ionic solid.
  3. C) a metallic solid.
  4. D) a molecular solid.

Answer:  B

Topic:  Section 10.6 Kinds of Solids

 

54) Which of the following compounds forms a covalent network solid?

  1. A) Li
  2. B) C (diamond)
  3. C) O2
  4. D) CO2

Answer:  B

Topic:  Section 10.6 Kinds of Solids

 

55) Which of the following compounds forms a covalent network solid?

  1. A) C8H18
  2. B) NO2
  3. C) SiO2
  4. D) SnCl4

Answer:  C

Topic:  Section 10.6 Kinds of Solids

56) Which type of bonding does Mg form upon solidification?

  1. A) covalent network
  2. B) ionic
  3. C) metallic
  4. D) molecular

Answer:  C

Topic:  Section 10.6 Kinds of Solids

 

57) The wavelength of light used to observe an object must be ________ than the object itself.

  1. A) larger
  2. B) smaller
  3. C) of higher energy
  4. D) of lower energy

Answer:  B

Topic:  Section 10.7 Probing the Structure of Solids: X-Ray Crystallography

 

 

58) The structure of a solid can be determined by diffraction of radiation in which region of the electromagnetic radiation spectrum?

  1. A) infrared
  2. B) microwave
  3. C) visible
  4. D) X-ray

Answer:  D

Topic:  Section 10.7 Probing the Structure of Solids: X-Ray Crystallography

 

59) How many atoms are in one face-centered cubic unit cell of a metal?

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 4

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

60) How many atoms are in one body-centered cubic unit cell of a metal?

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 4

Answer:  B

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

61) When cubic unit cells stack together, how many unit cells share a common corner?

  1. A) 2
  2. B) 4
  3. C) 6
  4. D) 8

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

62) How many unit cells share an atom that is on the face of a face-centered cubic unit cell?

  1. A) 1
  2. B) 2
  3. C) 4
  4. D) 8

Answer:  B

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

63) Which type of spherical packing has the most unused space?

  1. A) body-centered cubic
  2. B) cubic closest-packed
  3. C) cubic closest-packed and hexagonal closest-packed
  4. D) simple cubic

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

64) Iron crystallizes in a body-centered cubic cell having an edge length of 287 pm. What is the density of iron in g/cm3.

  1. A) 1.99
  2. B) 7.85
  3. C) 11.9
  4. D) 15.9

Answer:  B

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

65) What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 175 pm?

  1. A) 247 pm
  2. B) 495 pm
  3. C) 700 pm
  4. D) 1400 pm

Answer:  B

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

66) Rhodium has a face-centered cubic structure and has a density of 12.4 g/cm3. What is its atomic radius?

  1. A) 134 pm
  2. B) 268 pm
  3. C) 380 pm
  4. D) 1070 pm

Answer:  A

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

67) Silver crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of silver is 144 pm?

  1. A) 204 pm
  2. B) 288 pm
  3. C) 333 pm
  4. D) 407 pm

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

68) An element forms a body-centered cubic crystalline substance. The edge length of the unit cell is 287 pm and the density of the crystal is 7.92 g/cm3. Calculate the atomic weight of the substance.

  1. A) 45.0 amu
  2. B) 48.0 amu
  3. C) 56.4 amu
  4. D) 63.5 amu

Answer:  C

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

 

69) Cesium has a radius of 272 pm and crystallizes in a face-centered cubic unit cell. What is the edge length of the unit cell?

  1. A) 314 pm
  2. B) 385 pm
  3. C) 544 pm
  4. D) 769 pm

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

70) Manganese crystallizes in a body-centered cubic structure. What is the coordination number of each atom?

  1. A) 4
  2. B) 6
  3. C) 8
  4. D) 12

Answer:  C

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

71) Cubic closest-packing

  1. A) has a body-centered cubic unit cell.
  2. B) has a face-centered cubic unit cell.
  3. C) has a simple cubic unit cell.
  4. D) has the same unit cell as hexagonal closest-packing.

Answer:  B

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

72) The highest coordination number for spherical packing is found in the

  1. A) body-centered cubic structure.
  2. B) simple cubic structure.
  3. C) body-centered cubic and face-centered cubic.
  4. D) cubic closest-packing and hexagonal closest packing.

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

73) KCl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many K+ ions and Cl- ions are in each unit cell of KCl?

  1. A) 1 K+ion and 1 Cl-ion
  2. B) 2 K+ions and 2 Cl-ions
  3. C) 4 K+ions and 4 Cl-ions
  4. D) 8 K+ions and 8 Cl-ions

Answer:  C

Topic:  Section 10.9 Structures of Some Ionic Solids

 

 

74) An ionic compound crystallizes in a unit cell having a face-centered cubic array of anions, X–, and half of the tetrahedral holes filled with metal ions, Mn+ The empirical formula of this ionic compound is

  1. A) MX.
  2. B) MX2.
  3. C) M2
  4. D) M2X7.

Answer:  A

Topic:  Section 10.9 Structures of Some Ionic Solids

75) An ionic compound crystallizes in a unit cell having a face-centered cubic array of metal ions, Mn+, and all of the tetrahedral holes occupied by anions, X–. The empirical formula of this ionic compound is

  1. A) MX.
  2. B) MX2.
  3. C) M2
  4. D) M7X4.

Answer:  B

Topic:  Section 10.9 Structures of Some Ionic Solids

 

76) The edge length of a face-centered cubic lattice of NaCl is 564 pm. What is the density of NaCl in g/cm3?

  1. A) 0.720
  2. B) 1.08
  3. C) 2.16
  4. D) 4.32

Answer:  C

Topic:  Section 10.9 Structures of Some Ionic Solids

 

77) How many Cl- ions are around each K+ ion in KCl, which has a cubic unit cell with Cl- ions on each corner and each face?

  1. A) 1
  2. B) 4
  3. C) 6
  4. D) 8

Answer:  C

Topic:  Section 10.9 Structures of Some Ionic Solids

 

78) A binary ionic compound, MxAy, crystallizes in a cubic structure that contains eight anions (A) entirely within its unit cell and a cation (M) on each corner and on each face. What is the empirical formula of this compound?

  1. A) MA
  2. B) MA2
  3. C) M2A
  4. D) M4A8

Answer:  B

Topic:  Section 10.9 Structures of Some Ionic Solids

 

79) O2 and O3 are ________ of oxygen.

  1. A) allotropes
  2. B) isomers
  3. C) isotopes
  4. D) stereomers

Answer:  A

Topic:  Section 10.10 Structures of Some Covalent Network Solids

 

80) Which of the following is not an allotrope of carbon?

  1. A) coal
  2. B) diamond
  3. C) fullerene
  4. D) graphite

Answer:  A

Topic:  Section 10.10 Structures of Some Covalent Network Solids

 

81) The layers of graphite are held together by

  1. A) covalent bonds.
  2. B) dipole-dipole forces.
  3. C) London dispersion forces.
  4. D) All of these

Answer:  C

Topic:  Section 10.10 Structures of Some Covalent Network Solids

 

82) Diamond is held together by

  1. A) covalent bonds.
  2. B) dipole-dipole forces.
  3. C) London dispersion forces.
  4. D) All of these

Answer:  A

Topic:  Section 10.10 Structures of Some Covalent Network Solids

 

83) Pencil lead is actually

  1. A) fullerene.
  2. B) graphite.
  3. C) lead.
  4. D) silica.

Answer:  B

Topic:  Section 10.10 Structures of Some Covalent Network Solids

84) The critical temperature of a substance is the

  1. A) highest temperature at which the liquid phase can exist in equilibrium with the gas phase.
  2. B) temperature above which the compound decomposes.
  3. C) temperature at which all three phases can exist in equilibrium.
  4. D) temperature at which sublimation occurs.

Answer:  A

Topic:  Section 10.11 Phase Diagrams

 

 

85) Which transition could occur if a solid is heated at a pressure below the triple point pressure?

  1. A) condensation
  2. B) deposition
  3. C) melting
  4. D) sublimation

Answer:  D

Topic:  Section 10.11 Phase Diagrams

 

86) Which transition could occur if a solid is heated at a pressure above the triple point pressure?

  1. A) condensation
  2. B) deposition
  3. C) melting
  4. D) sublimation

Answer:  C

Topic:  Section 10.11 Phase Diagrams

 

87) A supercritical fluid refers to a substance

  1. A) above both its critical temperature and its critical pressure.
  2. B) at its triple point.
  3. C) that is in the liquid crystal state.
  4. D) with a viscosity of zero.

Answer:  A

Topic:  Section 10.11 Phase Diagrams

 

88) The liquid crystal state

  1. A) is a liquid in which the molecules tend to assume an overall orientation with respect to each other.
  2. B) occurs when a supercritical fluid is rapidly cooled below the critical point.
  3. C) occurs when an amorphous solid first begins to melt.
  4. D) occurs when the first crystals form in the liquid during freezing.

Answer:  A

Topic:  Chapter 10 Interlude – Ionic Liquids

 

 

89) In the drawing of acetaldehyde, CH3CHO, the largest partial positive charge (δ+) occurs on

  1. A) atom (a).
  2. B) atom (b).
  3. C) atom (c).
  4. D) atom (d).

Answer:  B

Topic:  Conceptual Problems

 

90) In the drawing of acetaldehyde, CH3CHO, the largest partial negative charge (δ -) occurs on

  1. A) atom (a).
  2. B) atom (b).
  3. C) atom (c).
  4. D) atom (d).

Answer:  C

Topic:  Conceptual Problems

 

 

 

91) In the drawing of acetic acid, CH3CO2H, a partial positive charge (δ+) occurs on

  1. A) only atom (a).
  2. B) only atom (b).
  3. C) atoms (a) and (c).
  4. D) atoms (b) and (d).

Answer:  D

Topic:  Conceptual Problems

92) In the drawing of acetic acid, CH3CO2H, a partial negative charge (δ-) occurs on

  1. A) only atom (a).
  2. B) only atom (b).
  3. C) atoms (a) and (c).
  4. D) atoms (b) and (d).

Answer:  C

Topic:  Conceptual Problems

 

 

93) Which drawing best accounts for the polarity of water, H2O, and the bond polarities that make a major contribution to the overall molecular polarity?

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  D

Topic:  Conceptual Problems

 

94) Which drawing best accounts for the polarity of methanol, CH3OH, and the bond polarities that make a major contribution to the overall molecular polarity?

 

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  B

Topic:  Conceptual Problems

 

95) Which drawing best shows the molecular polarity of methylamine, CH3NH2, and the bond polarities that make a major contribution to the overall molecular polarity?

 

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  A

Topic:  Conceptual Problems

 

96) Which drawing best shows the direction of the dipole moment in H2C=CCl2?

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  C

Topic:  Conceptual Problems

 

97) Which best indicates the direction of the dipole moment in formaldehyde, H2C=O?

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  C

Topic:  Conceptual Problems

 

98) Which best indicates the direction of the dipole moment in acetone, (CH3)2C=O?

 

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  B

Topic:  Conceptual Problems

 

99) Which drawing best represents hydrogen bonding?

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  C

Topic:  Conceptual Problems

 

100) Which drawing below best represents hydrogen bonding methanol, CH3OH?

 

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  C

Topic:  Conceptual Problems

 

101) Which drawing best represents hydrogen bonding in methylamine, CH3NH2?

 

  1. A) drawing (1)
  2. B) drawing (2)
  3. C) drawing (3)
  4. D) drawing (4)

Answer:  A

Topic:  Conceptual Problems

 

 

 

102) If figure (1) represents the vapor pressure of water at 25°C, which figure represents the vapor pressure of water at 45°C?

  1. A) figure (2)
  2. B) figure (3)
  3. C) figure (4)

Answer:  B

Topic:  Conceptual Problems

 

103) If figure (1) represents the vapor pressure of water at 25°C in a 1 liter container, which figure represents the vapor pressure of water at 25°C in a 2 liter container?

 

  1. A) figure (2)
  2. B) figure (3)
  3. C) figure (4)

Answer:  B

Topic:  Conceptual Problems

 

 

 

104) If figure (1) represents the vapor pressure of water at 25°C, which figure represents the vapor pressure of ethanol, CH3CH2OH at 25°C?

  1. A) figure (2)
  2. B) figure (3)
  3. C) figure (4)

Answer:  B

Topic:  Conceptual Problems

 

105) If figure (1) represents the vapor pressure of diethyl ether, CH3CH2OCH2CH3, at 25°C, which figure represents the vapor pressure of ethanol at 25°C?

  1. A) figure (2)
  2. B) figure (3)
  3. C) figure (4)

Answer:  C

Topic:  Conceptual Problems

 

106) If figure (1) represents the vapor pressure of water, at 25°C, which figure represents the vapor pressure of mercury at 25°C?

  1. A) figure (2)
  2. B) figure (3)
  3. C) figure (4)

Answer:  C

Topic:  Conceptual Problems

 

The plots below represent vapor pressure vs. temperature curves for diethyl ether, ethanol, mercury, and water, not necessarily in that order.

 

107) Based on the relative strengths of the intermolecular forces of attraction of each substance, which is the most likely vapor pressure vs. temperature curve for diethyl ether?

  1. A) curve (a)
  2. B) curve (b)
  3. C) curve (c)
  4. D) curve (d)

Answer:  A

Topic:  Conceptual Problems

 

108) Based on the relative strengths of the intermolecular forces of attraction of each substance, which is the most likely vapor pressure vs. temperature curve for ethanol?

  1. A) curve (a)
  2. B) curve (b)
  3. C) curve (c)
  4. D) curve (d)

Answer:  B

Topic:  Conceptual Problems

 

109) Based on the relative strengths of the intermolecular forces of attraction of each substance, which is the most likely vapor pressure vs. temperature curve for mercury?

  1. A) curve (a)
  2. B) curve (b)
  3. C) curve (c)
  4. D) curve (d)

Answer:  D

Topic:  Conceptual Problems

 

110) Based on the relative strengths of the intermolecular forces of attraction of each substance, which is the most likely vapor pressure vs. temperature curve for water?

  1. A) curve (a)
  2. B) curve (b)
  3. C) curve (c)
  4. D) curve (d)

Answer:  C

Topic:  Conceptual Problems

 

111) From the plot of vapor pressure as a function of temperature shown below, the normal boiling point for tert-butyl alcohol is approximately

 

 

  1. A) 0°C.
  2. B) 40°C.
  3. C) 85°C.
  4. D) 100°C.

Answer:  C

Topic:  Conceptual Problems

 

The picture shown below represents a two-dimensional lattice of atoms M and X.

 

 

112) Which of the areas designated A, B, and C are smallest repeating units, analogous to two-dimensional unit cells?

  1. A) only A
  2. B) only B
  3. C) only C
  4. D) A, B, or C

Answer:  D

Topic:  Conceptual Problems

 

113) What is the formula of the compound formed from M and X?

  1. A) MX
  2. B) MX2
  3. C) MX3
  4. D) MX4

Answer:  A

Topic:  Conceptual Problems

 

114) Identify the packing in the figure shown below.

 

 

  1. A) body-centered cubic
  2. B) cubic closest packed (face-centered cubic)
  3. C) hexagonal closest packed
  4. D) simple cubic

Answer:  B

Topic:  Conceptual Problems

 

115) Identify the packing in the figure shown below.

 

 

  1. A) body-centered cubic
  2. B) cubic closest packed (face-centered cubic)
  3. C) hexagonal closest packed
  4. D) simple cubic

Answer:  D

Topic:  Conceptual Problems

 

116) Identify the packing in the figure shown below.

 

 

  1. A) body-centered cubic
  2. B) cubic closest packed (face-centered cubic)
  3. C) hexagonal closest packed
  4. D) simple cubic

Answer:  C

Topic:  Conceptual Problems

 

117) Identify the packing in the figure shown below.

 

 

  1. A) body-centered cubic
  2. B) cubic closest packed (face-centered cubic)
  3. C) hexagonal closest packed
  4. D) simple cubic

Answer:  A

Topic:  Conceptual Problems

 

A certain mineral crystallizes in the cubic unit cell shown below.

 

 

118) What kind of packing do the anions adopt?

  1. A) body-centered cubic
  2. B) cubic closest packed (face-centered cubic)
  3. C) hexagonal closest packed
  4. D) simple cubic

Answer:  B

Topic:  Conceptual Problems

 

119) How many cations and how many anions are in the unit cell?

  1. A) 4 cations and 4 anions
  2. B) 4 cations and 8 anions
  3. C) 4 cations and 14 anions
  4. D) 8 cations and 4 anions

Answer:  A

Topic:  Conceptual Problems

 

120) A certain mineral crystallizes in the cubic unit cell shown below. M represents the cations and A represents the anions. What is the empirical formula of the mineral?

 

 

  1. A) MA
  2. B) MA2
  3. C) M2A
  4. D) M4A4

Answer:  A

Topic:  Conceptual Problems

 

A certain mineral, MxM’yAz, crystallizes in the cubic unit cell shown below. M and M’ represent cations and A represents the anions.

 

 

121) How many cations M are in the unit cell?

  1. A) 1
  2. B) 2
  3. C) 4
  4. D) 8

Answer:  A

Topic:  Conceptual Problems

 

122) How many anions are in the unit cell?

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 6

Answer:  C

Topic:  Conceptual Problems

 

123) What is the empirical formula of the mineral?

  1. A) MM’A
  2. B) MM’A3
  3. C) M2M’A3
  4. D) M8M’A6

Answer:  B

Topic:  Conceptual Problems

 

124) If cation M has a 2+ charge and anion A has a 2- charge, what is the oxidation state of cation M’?

  1. A) +1
  2. B) +2
  3. C) +3
  4. D) +4

Answer:  D

Topic:  Conceptual Problems

 

125) Consider a compound that undergoes sublimation at 125°C and a pressure of one atm. Which of the following could be a heating curve appropriate for heating the compound from 100°C to 150°C?

 

 

  1. A) graph a
  2. B) graph b
  3. C) graph c
  4. D) graph d

Answer:  B

Topic:  Conceptual Problems

 

Use the diagram below to answer the following questions.

 

 

126) According to the diagram, the solid phase of this substance

  1. A) has the same density as the liquid phase.
  2. B) is less dense than water.
  3. C) is less dense than the liquid phase.
  4. D) is more dense than the liquid phase.

Answer:  D

Topic:  Conceptual Problems

 

127) Melting occurs along the

  1. A) AC line.
  2. B) CB line.
  3. C) CD line.
  4. D) All of these

Answer:  B

Topic:  Conceptual Problems

 

128) The solid and liquid phases can exist in equilibrium along line

  1. A) AC.
  2. B) CB.
  3. C) CD.
  4. D) BD.

Answer:  B

Topic:  Conceptual Problems

129) The temperature and pressure at which all three phases can coexist in equilibrium is

  1. A) 0.25 atm and 110°C.
  2. B) 1.0 atm and 140°C.
  3. C) 1.25 atm and 300°C.
  4. D) 0.45 atm and 130°C.

Answer:  D

Topic:  Conceptual Problems

 

130) From the phase diagram above, the minimum pressure at which this substance can exist in the liquid phase is

  1. A) 0.25 atm.
  2. B) 0.45 atm.
  3. C) 1.0 atm.
  4. D) 1.2 atm.

Answer:  B

Topic:  Conceptual Problems

 

131) The normal boiling point of this substance is approximately

  1. A) 25°C.
  2. B) 140°C.
  3. C) 300°C.
  4. D) 350°C.

Answer:  C

Topic:  Conceptual Problems

 

132) What phases can be present at 200°C and 0.75 atm pressure?

  1. A) only the vapor phase
  2. B) only the liquid phase
  3. C) only the solid phase
  4. D) both the solid and vapor phases

Answer:  B

Topic:  Conceptual Problems

 

133) What phase changes occur when the temperature is held constant at 140°C and the pressure is increased from 0.25 atm to 1.4 atm?

  1. A) gas → liquid → solid
  2. B) gas → solid → liquid
  3. C) liquid → solid → gas
  4. D) solid → liquid → vapor

Answer:  A

Topic:  Conceptual Problems

134) What phase changes occur when the pressure is held constant at 0.25 atm and the temperature increases from 100°C to 300°C?

  1. A) liquid → gas
  2. B) solid → gas
  3. C) solid → liquid
  4. D) solid → liquid → gas

Answer:  B

Topic:  Conceptual Problems

 

 

The phase diagram of a substance is shown below.

 

 

135) The approximate normal boiling point of this substance is

  1. A) 180 K.
  2. B) 190 K.
  3. C) 300 K.
  4. D) 430 K.

Answer:  C

Topic:  Conceptual Problems

 

136) The approximate normal melting point of this substance is

  1. A) 100 K.
  2. B) 190 K.
  3. C) 300 K.
  4. D) 430 K.

Answer:  B

Topic:  Conceptual Problems

 

137) What is the physical phase of the substance at T = 100 K and P = 0.1 atm?

  1. A) gas
  2. B) liquid
  3. C) solid
  4. D) supercritical fluid

Answer:  C

Topic:  Conceptual Problems

138) What is the physical phase of the substance at T = 225 K and P = 1.1 atm?

  1. A) gas
  2. B) liquid
  3. C) solid
  4. D) supercritical fluid

Answer:  B

Topic:  Conceptual Problems

 

 

139) What is the physical phase of the substance at T = 400 K and P = 2.0 atm?

  1. A) gas
  2. B) liquid
  3. C) solid
  4. D) supercritical fluid

Answer:  A

Topic:  Conceptual Problems

 

10.2   Algorithmic Questions

 

1) Which covalent bond is the most polar?

  1. A) N- F
  2. B) C- F
  3. C) Cl- F
  4. D) F- F

Answer:  B

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

2) Which of the following should have the largest dipole moment?

  1. A) F2(g)
  2. B) BCl3(g)
  3. C) KBr(g)
  4. D) CH3I(g)

Answer:  C

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

3) Which of the following molecules does not have a dipole moment?

  1. A) C2H2
  2. B) H2O
  3. C) CH3CH2OH
  4. D) H I

Answer:  A

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

4) Which has the smallest dipole-dipole forces?

  1. A) CH3Cl
  2. B) HBr
  3. C) O2
  4. D) NO

Answer:  C

Topic:  Section 10.2 Intermolecular Forces

 

 

5) Which is expected to have the largest dispersion forces?

  1. A) C3H8
  2. B) C12H26
  3. C) F2
  4. D) Be Cl2

Answer:  B

Topic:  Section 10.2 Intermolecular Forces

 

6) Which of the following compounds exhibits hydrogen bonding?

  1. A) CH3Cl
  2. B) HI
  3. C) CH3OCH3
  4. D) NH3

Answer:  D

Topic:  Section 10.2 Intermolecular Forces

 

7) Which of the following compounds has the highest boiling point?

  1. A) H2O
  2. B) H Cl
  3. C) H2S
  4. D) N H3

Answer:  A

Topic:  Section 10.2 Intermolecular Forces

 

8) In liquid  propanol, CH3CH2CH2OH, which intermolecular forces are present?

  1. A) Dispersion, hydrogen bonding and dipole-dipole forces are present.
  2. B) Only dipole-dipole and ion-dipole forces are present.
  3. C) Only dispersion and dipole-dipole forces are present.
  4. D) Only hydrogen bonding forces are present.

Answer:  A

Topic:  Section 10.2 Intermolecular Forces

9) Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?

  1. A) H2
  2. B) HI
  3. C) CO2
  4. D) CH3NH2

Answer:  B

Topic:  Section 10.2 Intermolecular Forces

 

 

10) The normal boiling point for  H2Te  is higher than the normal boiling point for  H2Se . This can be explained by

  1. A) larger dipole-dipole forces for H2Te .
  2. B) larger dispersion forces for H2Te .
  3. C) larger hydrogen-bond forces for H2Te .
  4. D) larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for H2Te .

Answer:  B

Topic:  Section 10.2 Intermolecular Forces

 

11) Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol. How much heat could be removed by  20.0 g of ethyl chloride?

  1. A) 8.18 kJ
  2. B) 341 kJ
  3. C) 528 kJ
  4. D) 3410 kJ

Answer:  A

Topic:  Section 10.4 Phase Changes

 

12) How much heat is released when  105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).

  1. A) 54.8 kJ
  2. B) 273 kJ
  3. C) 319 kJ
  4. D) 347 kJ

Answer:  C

Topic:  Section 10.4 Phase Changes

13) Which of the following forms a molecular solid?

  1. A) NH4NO3
  2. B) C6H4Cl2
  3. C) SiO2
  4. D) copper

Answer:  B

Topic:  Section 10.6 Kinds of Solids

 

14) Which of the following forms an ionic solid?

  1. A) Ag
  2. B) C7H15NH2
  3. C) Rb I
  4. D) S O3

Answer:  C

Topic:  Section 10.6 Kinds of Solids

 

 

15) Which type of bonding does  Sr form upon solidification?

  1. A) covalent network
  2. B) ionic
  3. C) metallic
  4. D) molecular

Answer:  C

Topic:  Section 10.6 Kinds of Solids

 

16) What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of  128 pm?

  1. A) 181 pm
  2. B) 362 pm
  3. C) 512 pm
  4. D) 1020 pm

Answer:  B

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

17) Nickel has a face-centered cubic structure and has a density of  8.90 g/cm3. What is its atomic radius?

  1. A) 125 pm
  2. B) 249 pm
  3. C) 353 pm
  4. D) 997 pm

Answer:  A

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

18) A certain metal crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of the metal is  144 pm?

  1. A) 204 pm
  2. B) 288 pm
  3. C) 333 pm
  4. D) 407 pm

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

19) Cesium has a radius of  272 pm and crystallizes in a body-centered cubic structure. What is the edge length of the unit cell?

  1. A) 314 pm
  2. B) 385 pm
  3. C) 544 pm
  4. D) 628 pm

Answer:  D

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

 

20) Lithium crystallizes in a body-centered cubic structure. What is the coordination number of each atom?

  1. A) 4
  2. B) 6
  3. C) 8
  4. D) 12

Answer:  C

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

21) Na Cl crystallizes in a cubic unit cell with  Cl- ions on each corner and each face. How many  Na+ and  Cl- ions are in each unit cell of  Na Cl?

  1. A) 1 Na+ion and 1  Cl- ion
  2. B) 2 Na+ions and 2  Cl- ions
  3. C) 4 Na+ions and 4  Cl- ions
  4. D) 8 Na+ions and 8  Cl- ions

Answer:  C

Topic:  Section 10.9 Structures of Some Ionic Solids

22) How many  H- ions are around each  Na+ ion in  NaH, which has a cubic unit cell with  H- ions on each corner and each face?

  1. A) 1
  2. B) 4
  3. C) 6
  4. D) 8

Answer:  C

Topic:  Section 10.9 Structures of Some Ionic Solids

 

10.3   Short Answer Questions

 

1) The bonds in the polyatomic ion NO3– are classified as ________.

Answer:  polar covalent.

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

2) In the molecule BF3 there is a δ+ charge on the ________ atom and a δ– charge on the ________ atom.

Answer:  boron, fluorine

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

3) LiH has an experimental dipole moment, μ = 6.00 D. If LiH were 100% ionic, the distance between positive and negative charges would be 161 pm. What is the percent ionic character in the LiH bond?

Answer:  77.7%

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

4) The Br-Cl bond has 5.05% ionic character and a dipole moment of 0.518 D. What is the distance between atoms in BrCl?

Answer:  214 pm

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

5) The HBr bond has a length of 141 pm and 12.1% ionic character. What is the dipole moment of HBr?

Answer:  0.82 D

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

6) Pt(NH3)2Cl2 is square planar. The isomer of Pt(NH3)2Cl2 that has a non-zero dipole moment has a Cl-Pt-Cl bond angle of ________ degrees.

Answer:  90

Topic:  Section 10.1 Polar Covalent Bonds and Dipole Moments

 

7) The intermolecular forces formed when NaCl is dissolved in water are ________ forces.

Answer:  ion-dipole

Topic:  Section 10.2 Intermolecular Forces

8) The intermolecular forces responsible for CH3CH2OH being at liquid at 20°C are ________ bonds.

Answer:  hydrogen

Topic:  Section 10.2 Intermolecular Forces

 

9) Helium can be liquefied when He atoms are attracted to one another by intermolecular ________ forces.

Answer:  dispersion (or London dispersion)

Topic:  Section 10.2 Intermolecular Forces

 

10) The property of a liquid that is a measure of the liquid’s resistance to increase its surface area is ________.

Answer:  surface tension

Topic:  Section 10.3 Some Properties of Liquids

 

11) Of C2H5OH and C3H5(OH)3 the one expected to have the higher viscosity is ________, and the one expected to have the higher surface tension is ________.

Answer:  C3H5(OH)3, C3H5(OH)3

Topic:  Section 10.3 Some Properties of Liquids

 

12) The phase change H2(g) → H2(s) is called ________, and the enthalpy change, ΔH, for this phase change has a ________ sign.

Answer:  deposition, negative (–)

Topic:  Section 10.4 Phase Changes

 

13) Of C2H5OH and C3H5(OH)3 the one expected to have the higher vapor pressure is ________, and the one expected to have the higher boiling point is ________.

Answer:  C2H5OH, C3H5(OH)3

Topic:  Section 10.5 Evaporation, Vapor Pressure, and Boiling Point

 

14) The solids formed by K, K2O2, SiO2, and O2 are classified as ________, ________, ________, and ________, respectively.

Answer:  metallic, ionic, covalent network, molecular

Topic:  Section 10.6 Kinds of Solids

 

15) Rubber is classified as an ________ solid, whereas diamond is classified as a ________ solid.

Answer:  amorphous, covalent network

Topic:  Section 10.6 Kinds of Solids

 

16) A low-melting crystalline compound that does not conduct electricity in the solid or liquid state is classified as a ________ solid.

Answer:  molecular

Topic:  Section 10.6 Kinds of Solids

17) First-order diffraction of X-rays with d = 154.2 pm at an angle of 32.5° is caused by layers of atoms in a crystalline solid with a spacing of ________ pm.

Answer:  143

Topic:  Section 10.7 Probing the Structure of Solids: X-Ray Crystallography

 

18) Layers of atoms having a spacing of 105 pm will diffract X-rays with d = 154.2 pm at an angle of ________ degrees.

Answer:  47.2

Topic:  Section 10.7 Probing the Structure of Solids: X-Ray Crystallography

 

19) The cubic closest-packed arrangement of atoms is the same as which cubic unit cell?

Answer:  face-centered cubic

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

20) The two most efficiently packed unit cells have the hexagonal closest-packed and the ________ the atomic arrangements.

Answer:  cubic closest-packed

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

21) The coordination number of each atom in a simple cubic unit cell is ________.

Answer:  6

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

22) The cubic unit cell in which the radius of an atom is 31/2 d/4, where d is the unit cell edge length, is the ________ unit cell.

Answer:  body-centered cubic

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

23) A certain metal can exist in two different cubic cells, body-centered cubic and face-centered cubic. Which unit cell will have the greater density?

Answer:  face-centered

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

24) Ni has a face-centered unit cell. The number of Ni atoms in the unit cell is ________.

Answer:  four

Topic:  Section 10.8 Unit Cells & Packing of Spheres in Crystalline Solids

 

 

25) A compound having A ions on each corner and B ions on each face of a cubic unit cell has the empirical formula ________.

Answer:  AB3

Topic:  Section 10.9 Structures of Some Ionic Solids