Chemistry chp 12 Flashcards
describes the behavior of gases in terms of particles in motion; makes several assumptions about size, motion, and energy of gas particles
kinetic-molecular theory
collision in which no kinetic energy is lost; kinetic energy can be transferred between the colliding particles, but the total kinetic energy of the two particles remains the same
elastic collision
a measure of the average kinetic energy of the two particles in a sample of matter
temperature
the movement of one material through another from an area of higher concentration to an area of lower concentration
diffusion
states that the rate of effusion for a gas is inversely proportional to the source root of its molar mass
graham’s law of effusion
force applied per unit area
pressure
an instrument that is used to measure atmospheric pressure
barometer
the SI unit of pressure; one pascal (Pa) is equal to a force of one newton per square meter
pascal
the unit that is often used to report air pressure
atmosphere
states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture
Dalton’s law of partial pressure
the weak forces resulting from temporary shifts in the density of electrons in electron clouds
dispersion forces
the attractions between oppositely charged regions of polar molecules
dipole-dipole forces
a strong dipole-dipole attraction between molecules that contain a hydrogen atom bonded to a small, highly electronegative atom
hydrogen bond
a measure of the resistance of a liquid to flow, which is affected by the size and shape of particles, and generally increases as the temperature decreases and as intermolecular forces increases
viscosity
the energy required to increase the surface area of a liquid by a given amount; results from uneven distribution of attractive forces
surface tension
a compound, such as soap, that lowers the surface tension of water by disrupting hydrogen bonds between water molecules; also called a surface active agent
surfactant
a solid whose atoms, ions, or molecules are arranged in an orderly, geometric, three dimensional structure
crystalline solid
the smallest arrangement of atoms in a crystal lattice that has the same symmetry as the whole crystal; a small representative part of a larger whole
unit cell
one of two or more forms of an element with different structures and properties when they are in the same state- solid, liquid, or gas
allotrope
a solid in which particles are not arranged in a regular, repeating pattern, that often is formed when molten material cools too quickly to form crystals
amorphous
for a crystalline solid, the temperature a which the forces holding a crystal lattice together are broken and it becomes a liquid
melting point
the energy requiring process by which a liquid changes to a gas or vapor
vaporization
the pressure in which vaporization occurs only at the surface of a liquid
evaporation
the pressure exerted by a vapor over a liquid
vapor pressure
the temperature at when liquids vapor pressure is equal to the external or atmospheric pressure
boiling pressure
the temperature at which a liquids vapor pressure is equal to the external or atmospheric pressure
boiling pressure
the temperature at which a liquid is converted into a a crystalline solid
freezing point
the energy releasing process by which a gas or vapor becomes a liquid
condensation
the energy releasing process by which a substance changes from a gas or vapor to a solid without changing into a liquid
decomposition
a graph of pressure versus temperature that sows which phase a substance exists in under different conditions of temperature and pressures
phase diagram
the point on a phase diagram representing the temperature and pressure at which the three phases of a substance (solid, liquid, and gas) can coexist
triple point
