Chemistry 10-12

Front 1

condensed states

Back 1

liquid or solid

Front 2

intermolecular forces

Back 2

forces between molecules

Front 3

dipole-dipole attraction

Back 3

molecules that orient themselves to maximize + and - attractions

Front 4

hydrogen bonding

Back 4

unusually strong dipole dipole attraction, where a hydrogen atom is bound to a N, O, or F

Front 5

london forces

Back 5

forces that exist between noble gases and nonpolar molecules

Front 6

surface tension

Back 6

resistance of a liquid to increase its surface area

Front 7

capillary action

Back 7

spontaneous rising of a liquid in a tube

Front 8

viscosity

Back 8

liquid's resistance to flow

Front 9

heat of vaporization

Back 9

energy required to vaporize one mole of a liquid at one atm

Front 10

equilibrium vapor pressure

Back 10

pressure present at equilibrium

Front 11

heating curve

Back 11

plot of temperature vs time for a process where energy is added at a constant rate

Front 12

enthalpy of fusion

Back 12

enthalpy change that occurs at the melting point when a solid melts

Front 13

normal melting point

Back 13

temperature at which the solid and liquid states have the same vapor pressure under conditions where the total pressure is one atm

Front 14

normal boiling point

Back 14

the temperature at which the vapor pressure of the liquid is exactly one atm

Front 15

supercooled

Back 15

can be cooled below 0 celsius and 1 atm and remain a liquid

Front 16

superheated

Back 16

raised to a temperature above its boiling point and remain a liquid

Front 17

phase diagram

Back 17

way to represent the phases of a substance as a function of temperature and pressure

Front 18

triple point

Back 18

when the solid and liquid have identical vapor pressures

Front 19

critical temperature

Back 19

the temperature above which the vapor cannot be liquified no matter what pressure is applied

Front 20

critical pressure

Back 20

the pressure required to produce liqufication at the critical temperature

Front 21

critical point

Back 21

critical pressure + critical temperature

Front 22

molarity

Back 22

number of moles of solute per liter of solution

Front 23

mass percent

Back 23

percent by mass of the solute in the solution

Front 24

mole fraction

Back 24

the ratio of the number of moles of a given component to the total number of moles of the two components

Front 25

molality

Back 25

number of moles of solute per kilogram of solvent

Front 26

normality

Back 26

number of equivalents per liter of solution

Front 27

enthalpy of solution

Back 27

the sum of the energies used un expanding both solvent and solute and the energy of solvent-solute interaction

Front 28

enthalpy of hydration

Back 28

enthalpy change associated with the dispersal of a gaseous solute in water

Front 29

henry's law

Back 29

amount of gas dissolved in a solution is directly proportional th the pressure of the gas above the solution

Front 30

raoult's law

Back 30

P solution = x solvent * P solvent