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Chapter 10: Liquids, Solids, and Phase Changes

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Self Quiz 2

Self Quiz 2

This activity contains 20 questions.

	In which bond would the dipole moment be drawn to show electron displacement from the first atom to the second atom of the bond?   O-S O-N C-Si Cl-F Cl-C

	Which molecule does not have a dipole moment?   BF3 ClF3 OF2 NF3 BrF5

	Which is not a characteristic of dipole-dipole forces?   The energies of the dipole-dipole forces are generally weak. They include repulsive forces. The forces increase with increasing dipole moment. They include attractive forces. The forces are significant at any distance.

	Which molecule is not correctly matched to the strongest intermolecular force experienced by that molecule?   CH3CH2NH2, hydrogen bonding F2C=CF2, dipole-dipole force SO3, dispersion force NF3, dipole-dipole force I2, dispersion force

	Which statement concerning hydrogen bonding is true?   In the bond between oxygen and hydrogen, the hydrogen has a partial negative charge. The hydrogen can approach the other atom closely, since it is well shielded by its inner electrons. A hydrogen bond is as strong as a covalent bond. The size of the hydrogen atoms allows it to be closely approached by other atoms. Hydrogen bonding occurs between molecules of PH3.

	As the temperature of a liquid is lowered, its viscosity __________ and its surface tension __________.   decreases, decreases increases, decreases is unchanged, is unchanged increases, increases decreases, increases

	Which term is not correctly matched to the corresponding phase change?   deposition, gas ---> liquid fusion, solid ---> liquid sublimation, solid ---> gas vaporization, liquid ---> gas freezing, liquid ---> solid

	What is the boiling point (in °C) of methanol if the change in enthalpy is 37.5 kJ/mol and the change in entropy is 111 J/K for the process CH3OH(l) ---> CH3OH(g)?   37.4 °C 611 °C 0.34 °C 338 °C 65 °C

	How much energy (in kilojoules) is absorbed when 10.0 g of liquid water at 75.0 °C is converted to water vapor at 150.0 °C? (The enthalpy of vaporization of water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/K·mol for the liquid and 33.6 J/K·mol) for the vapor.)   25.0 kJ 28.5 kJ 24.5 kJ 2.00 x 103 kJ 4.42 x 102 kJ

	Which statement concerning vapor pressure is true?   As the temperature is increased, the number of gas molecules in equilibrium remains constant, since the extra energy also causes more molecules to enter the liquid phase. The pressure above a liquid in an open container is the vapor pressure of a liquid. As the temperature is increased, the number of gas molecules in equilibrium remains constant, but an increase in their kinetic energy results in a higher vapor pressure. The total number of molecules in the liquid phase remains constant once equilibrium has been reached. The individual molecules in a given phase remain in that phase once equilibrium has been reached.

	What is the enthalpy of vaporization of boron tribromide (in kJ/mol) if the vapor pressure is 67.0 mm of mercury at 25 °C, and the normal boiling point is 91 °C?   33.2 kJ/mol 76.4 kJ/mol 89.4 kJ/mol 3.32 x 104 kJ/mol 0.696 kJ/mol

	Which is not a typical characteristic of crystalline solids?   Nonconducting is not a typical characteristic of crystalline solids. Flat faces is not a typical characteristic of crystalline solids. Ordered arrangement of particles is not a typical characteristic of crystalline solids. Distinct angles is not a typical characteristic of crystalline solids. No long-range structure is not a typical characteristic of crystalline solids.

	Which group of solids is matched incorrectly with the appropriate type of crystalline solid?   CaO : ionic solids KrF2 : ionic solids Ir : metallic solids PCl3 : molecular solids C9H8O4 : molecular solids

	Which statement offers an explanation for why X-rays are used in crystallography?   X-rays are diffracted by crystalline solids. X-rays are absorbed by the solid particles. The X-rays are always reflected in-phase from the surface of a crystal. The wavelength of the X-rays is larger than the diameters of atoms. X-rays are scattered in random directions by a crystalline solid.

	The packing of spheres in order of increasing percentage of empty space is   body-centered cubic, simple cubic, and cubic closest-packed. body-centered cubic, cubic closest-packed, and simple cubic. simple cubic, cubic closest-packed, and body-centered cubic. cubic closest-packed, body-centered cubic, and simple cubic. simple cubic, body-centered cubic, and cubic closest-packed.

	The radius of a copper atom (in picometers) that crystallizes in a face-centered cubic unit cell having an edge length of 3.62 x 10-8 cm is   171 pm. 181 pm. 512 pm. 128 pm. 90.5 pm.

	The correct hybridization and molecular geometry of silicon in SiO2 is   sp : linear. sp3 : tetrahedral. sp3 : bent. sp3 : trigonal planar. sp2 : trigonal planar.

	Which statement gives the correct relationship between temperature, pressure, and the states of matter on a phase diagram?   A solid occurs at high temperatures and low pressures. A gas occurs at low temperatures and high pressures. A solid occurs at low temperatures and high pressures. A liquid occurs at low temperatures and low pressures. A gas occurs at moderate temperatures and high pressures.

	The phase change sequence that shows all of the phase changes that occur when the temperature is lowered from just below the critical-point temperature while maintaining the critical-point pressure is   solid ---> liquid. gas ---> liquid ---> solid. liquid ---> solid. liquid ---> gas ---> solid. gas ---> solid.

	Which statement is not true according to the phase diagram for a normal substance?   If a liquid is at a temperature and pressure above the triple point, the liquid will freeze as the temperature is decreased while the pressure remains constant. Above the critical temperature the normal liquid cannot exist, regardless of pressure. The melting point increases as the pressure increases. The boiling point decreases as the pressure decreases. If a solid is at a temperature and pressure below the triple point, the solid will melt as the temperature is increased while the pressure remains constant.

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