Ap Chemistry (Thermochemistry)

Front 1

enthalpy

Back 1

heat content (H) of a substance.

Front 2

Calorimetry

Back 2

calculating the change in enthalpy.

Front 3

Heat Capacity

Back 3

way a particular substance responds to E (release/absorb)

Front 4

Standard Enthalpy of Formation

Back 4

Enthalpy change associated with the formation of one mole of a substance from its elements.

Front 5

Hess's Law

Back 5

calculates the change in entalpy of reactions. The enthalpy change of reaction depends only on the nature of the reactants and products and independant of route taken.

Front 6

entropy

Back 6

chaos/driving force of spontinaity.
measurement of disorder and arrangements.

Front 7

first law of thermodynamics

Back 7

energy of the universe is constant (systems and surroudings)

Front 8

second law of thermodynamics

Back 8

entropy or disorder in universe is increasing.

Front 9

Gibb's Free Energy

Back 9

One must consider the effects of enthalpy change and entropy change to predict a reaction's spontinaity.

Front 10

Tipping Factor

Back 10

Temperature makes it spontanious or not.

Front 11

the change in enthalpy of reaction can be calculated (5 ways)

Back 11

1. Hess's Law
2. Change of H of formation
3. Calorimetry (experiment)
4. Gibb's free energy law.
5. Bond enthalpy

Front 12

Gibb's free energy (spontinuity)

Back 12

change in G is negative = spontanious
Change in G is positive = nonspontanious

Front 13

Bond Enthalpy

Back 13

Change in enthalpy is the sum of all bond energies.

Front 14

Method of calculation of Enthalpy of formation of ionic solids

Back 14

Born-Haber cycle

Front 15

Atomization

Back 15

evaporating metal

Front 16

sublimation

Back 16

vaporizing metal.

Front 17

ionization energy

Back 17

ionizing a metal gas

Front 18

dissociation energy

Back 18

splitting diatomic atoms

Front 19

Electron affinigy

Back 19

ionizing a diatomic gas atom.

Front 20

Lattice formation

Back 20

the final creation of the lattice structure.

Front 21

Chemical Kinetics

Back 21

Looking into rates of reactions

Front 22

Collision theory

Back 22

reaction will only take place if:
1. contact of reactants
2. collisions have sufficient minimum energy
3. collision geometry/angle/orientation is correct.

Front 23

Maxwell Boltzman graph

Back 23

graphing energy against number of particles to see what portion of the particles have the energy neccessary to react.