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Chapter 11: Liquids, Solids, Intermolecular Forces

Self-Quiz

Self-Quiz

This activity contains 15 questions.

	Which of the following is NOT a property of solids?   Solids have a high density in comparison to gases. Solids have a definite shape. Solids have an indefinite volume, not easily compressed. Solids have relatively strong intermolecular forces. Solids may be crystalline or amorphous.

	Which of the following statements is false about the changes occurring when ice is heated in an open beaker from –10.0 °C to water vapor at 110.0 °C?   The energy of the water molecules increases. The H2O molecules have an increased velocity. The increase in temperature causes the H2O molecules to split into H2 and O2. The space between H2O molecules becomes larger. The volume occupied by the H2O molecules increases.

	Which of the following is a false statement about dispersion forces?   Dispersion forces are the result of fluctuations in the electron distribution within molecules or atoms. Dispersion forces are present in all atoms and molecules. Dispersion forces result from the formation of instantaneous dipoles in a molecule or atom. Dispersion forces always have a greater magnitude in molecules with a greater molar mass. Dispersion force magnitude depends on the amount of surface area available for interactions.

	In order for a molecule to exhibit dipole–dipole forces, __________ must be present in the molecule.   oxygen a double bond a permanent dipole a C–H bond a functional group

	The ability for liquids to mix without separating into two phases is called _________.   polarizability viscosity dynamic equilibrium miscibility compressibility

	Which of the following molecules will have the highest melting point?   (i) (ii) (iii) cannot be determined all the same

	Which of the following is true?   All molecules have the same thermal energy. Some molecules in an open beaker will have enough kinetic energy to vaporize from the surface of the liquid. Increasing temperature decreases the rate of vaporization. A decreased surface area will increase the rate of vaporization. The stronger the intermolecular forces, the faster the rate of vaporization.

	Calculate the volume (mL) of acetone (density = 0.786 g/mL) that can be vaporized at its normal boiling point with 345 kJ of heat. ΔHvap for acetone is 29.1 kJ/mol.   15.1 151 541 689 876

	Determine the vapor pressure (atm) of rubbing alcohol (isopropanol) at 20.0 °C. The normal boiling point of isopropanol is 82.3 °C and the heat of vaporization (ΔHvap) is 39.9 kJ/mol.   1.35 × 10-3 5.67 × 10-2 9.97 × 10-1 17.6 740.

	Calculate the amount of heat (in J) required to heat 2.00 grams of ice from –12.0 °C to 88.0 °C.   50.2 418 668 786 1450

	Which processes occur at the triple point?   melting and freezing only melting, freezing, vaporization, and condensation melting, freezing, sublimation, and deposition vaporization, condensation, sublimation, and deposition melting, freezing, vaporization, condensation, sublimation, and deposition

	Calculate the edge-length (in pm) of the polonium unit cell, which has a body-centered crystal lattice and an atomic radius of 190 pm.   95 190 380 439 537

	Determine the atomic radius (in pm) of gold if it crystallizes in a face-centered lattice and has a density of 19.4 g/cm3.   646 407 228 144 107

	Which of the following is a false statement about atomic solids?   Atomic solids are a type of crystalline solids. The composite units of atomic solids are atoms. Atomic solids can be nonbonding, metallic, or network covalent. All atomic solids have high melting points. Atomic solids are held together by dispersion forces, metallic bonds, and covalent bonds.

	The energy gap that exists between the valence band and conduction band in semiconductors and insulators is called a(n) _________.   conductor band gap p-n junction diode electric field

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