Kinetic-Molar Theory of Matter
Define "diffusion"
Spontaneous mixing of the particles of two substances is caused by their random motion.
Define "fluid"
A substance that can flow and therefore take the shape of its container.
Define "unit cell"
The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice.
Define "sublimation"
The change of state from a solid directly to a gas.
The type of bond that holds together a water molecule
Covalent bond
Define "real gas"
A gas that doesn't behave completely according to the assumptions of the kinetic-molar theory.
Define "evaporation"
The process by which particles escape from the surface of a nonboiling liquid and enter a gas state.
Define "crystal structure"
The total three-dimensional arrangement of particles of a crystal.
Define "equilibrium"
A dynamic condition in which two opposing changes occur at equal rates in a closed system.
Can both easily be dissolved by water
Polar molecules and ionic substances
Define "ideal gas"
A hypothetical gas that perfectly fits all the assumptions of the kinetic-molar theory.
Define "vaporization"
The process by which a liquid or solid changes to a gas.
Define "amorphous solid"
A solid in which the particles are arranged randomly.
Define "volatile liquid"
Liquids that evaporate readily, have relatively weak forces of attraction between their particles.
Under the pressure of 1atm water...
water boils at 100oC
Define "kinetic-molar theory"
The idea that particles of matter are always in motion.
Define "surface tension"
A force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size.
Define "crystalline solid"
A solid that consists of crystals.
Define "critical temperature"
The temperature above which the substance cannot exist in the liquid state.
The angle between the two hydrogen-oxygen bonds
About 105o
A collision in which there is no net loss of total kinetic energy.
Define "capillary action"
The attraction of the surface of a liquid to the surface of a solid, a property closely related to surface tension.
Define "supercooled liquid"
A substance that retains certain liquid properties even at temperatures at which they appear to be solid.
Define "normal freezing point"
The temperature at which the solid and liquid are at equilibrium at 1 atm (760 torr/101.3 kPa) pressure.
The molar enthalpy of fusion of ice
6.009 kJ/mol