Chapter 10 Liquids and Solids
Chapter 10 Key Terms
force of attraction between molecules of different chemical identities
(also, noncrystalline solid) solid in which the particles lack an ordered internal structure
temperature at which the vapor pressure of a liquid equals the pressure of the gas above it
flow of liquid within a porous material due to the attraction of the liquid molecules to the surface of the material and to other liquid molecules
mathematical relationship between the temperature, vapor pressure, and enthalpy of vaporization for a substance
force of attraction between identical molecules
change from a gaseous to a liquid state
solid whose particles are held together by covalent bonds
temperature and pressure above which a gas cannot be condensed into a liquid
solid in which the particles are arranged in a definite repeating pattern
change from a gaseous state directly to a solid state
intermolecular attraction between two permanent dipoles
(also, London dispersion force) attraction between two rapidly fluctuating, temporary dipoles; significant only when particles are very close together
state of a system in which reciprocal processes are occurring at equal rates
change from a liquid state to a solid state
temperature at which the solid and liquid phases of a substance are in equilibrium; see also melting point
occurs when exceptionally strong dipoles attract; bonding that exists when hydrogen is bonded to one of the three most electronegative elements: F, O, or N
temporary dipole formed when the electrons of an atom or molecule are distorted by the instantaneous dipole of a neighboring atom or molecule
temporary dipole that occurs for a brief moment in time when the electrons of an atom or molecule are distributed asymmetrically
noncovalent attractive force between atoms, molecules, and/or ions
spaces between the regular particle positions in any array of atoms or ions
solid composed of positive and negative ions held together by strong electrostatic attractions
change from a solid state to a liquid state
temperature at which the solid and liquid phases of a substance are in equilibrium; see also freezing point
solid composed of metal atoms
solid composed of neutral molecules held together by intermolecular forces of attraction
temperature at which a liquid’s vapor pressure equals 1 atm (760 torr)
pressure-temperature graph summarizing conditions under which the phases of a substance can exist
measure of the ability of a charge to distort a molecule’s charge distribution (electron cloud)
change from solid state directly to gaseous state
substance at a temperature and pressure higher than its critical point; exhibits properties intermediate between those of gaseous and liquid states
energy required to increase the area, or length, of a liquid surface by a given amount
temperature and pressure at which three phases of a substance are in equilibrium
defect that occurs when a position that should contain an atom or ion is vacant
attractive or repulsive force between molecules, including dipole-dipole, dipole-induced dipole, and London dispersion forces; does not include forces due to covalent or ionic bonding, or the attraction between ions and molecules
(also, equilibrium vapor pressure) pressure exerted by a vapor in equilibrium with a solid or a liquid at a given temperature
change from liquid state to gaseous state
measure of a liquid’s resistance to flow