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Chem Exam '12

People of Chemistry on my Exam and Constants

Lewis atoms want to get stable electron configuration of a noble gas (octet rule) Lewis dot structure
Boyle's PV=PV
Gibbs' said if a reaction loses/gives off energy, it will be spontaneous but the reaction can give off energy in 2 forms: heat or work. gibbs free energy tells you whether or not a reaction will be spontaneous.
Bohr model most recent model said there are only certain allowable distances that electrons can orbit and can't orbit in between
Henry's Law as gas pressure increases, solubility goes up
Gay Lussac's principle P/T=P/T
Celsius (F-32)*(5/9)= °C
Fahrenheit °F = (9/5 x °C) + 32
Charles's V/T=V/T
Kelvin Celcius + 273= K
Torricelli invented the barometer a unit of pressure, one mm of mercury 1 Torr= 160mmHg
Le Chatelier's if you put stress on a system that's in equilibrium ir will adjust to relieve the stress
Hund's rule when filling a sublevel, one electron goes into each orbital b4 a second goes into any.
Pauli exclusion principle an atomic orbital can hold at most 2 electrons
Van Der Waal 1.dispersion forces 2.dipole interractions 3. hydrogen bonds (strongest)
Hess's` the enthalpy change for a reaction that is carried out in a series of steps is equal to the sum of the enthalpy changes for the individual steps
K(sub a) acid equilibrium constant
K(sub w) ion product constant [H+] times [OH-] = 1.0 * 10^-14
K(sub b) boiling point elevation constant
Created by: paulina.knoblock



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