CH 11 Chemistry – Flashcards

Liquids have a definite volume. Liquids have much higher densities in comparison to gases. Liquids have an indefinite shape and assume the shape of their container. Liquids are not easily compressed

Solids have much higher densities in comparison to gases. Solids have a definite volume. Solids are not easily compressed. Solids have a definite shape and do not assume the shape of their container. Solids may be crystalline (ordered) or amorphous (disordered).

A liquid can be converted to a solid by cooling. A solid can be converted to a liquid by heating.

A gas can be converted into a liquid by increasing the pressure of a gas sample. A gas can be converted into a liquid by cooling. A liquid can be converted to a gas by heating.

melting point, boiling point, viscosity, and surface tension increase vapor pressure decreases

Dispersion forces-the positive end of one instantaneous dipole attracting the negative end of another

True

In all molecules that are polar.

F,O, and N

Hydrogen bonds; they do not occur between individual atoms but between molecules

When an ionic compound is mixed with a polar compound; only occurs in mixtures of two compounds; strongest intermolecular force

The energy required to increase the surface area by a unit amount

The resistance of a liquid to flow; increases in longer molecules that can interact over a greater area; nearly all liquids become less viscous as temperature increases

The ability of a liquid to flow against gravity up a narrow tube

Cohesive- the attraction between molecules in a liquid Adhesive-the attractions between the molecules and the surface of the tube

The process by which thermal energy can overcome intermolecular forces and produce a state change from liquid to gas

condensation

non-volatile

Endothermic because it takes energy to vaporize the molecules in a liquid

Exothermic because heat is released when gas condenses to a liquid

The amount of heat required to vaporize one mole of a liquid to gas; increases with increasing intermolecular forces

When the rate of condensation and the rate of vaporization become equal

The pressure of gas in dynamic equilibrium with its liquid

the temperature at which the liquid's vapor pressure equals the external pressure

The temperature at which its vapor pressure equals 1 atm

the transition directly from the solid to the gas phase

a map of the state or phase of a substance as a function of pressure

the unique set of conditions at which the three states are equally stable and in equillibrium

The temperature and pressure above which a supercritical fluid exists

fusion curve-crossing this curve requires the complete transition from solid to liquid sublimation curve-transition from solid to gas vaporization curve-transition from liquid to gas

solids whose composite units are molecules;low melting points

composite units are ions; high melting points

composite units are individual atoms; three types

held together by relatively weak dispersion forces; only noble gases in solid form; low melting points

held together by metallic bonds; variable melting points

held together by covalent bonds; high melting points

A homogeneous mixture of two or more substances or components

the majority component in a solution

the minority component in a solution

The amount of the substance that will dissolve in a given amount of solvent

a measure of energy randomization or energy dispersal in a system

exothermic, positive

endothermic, negative

A solution in which the dissolved solute is in dynamic equilibrium with the solid solute

A solution containing less than the equilibrium amount of solute

one containing more than the equilibrium amount of solute

decreases

The flow of a solvent from a solution of a lower solute concentration to one of a higher solute concentration; concentrated solutions draw solvent from more dilute solutions because of nature's tendency to mix