Mole

Limiting Reagents

Percent composition of compounds

Determining formulas of composition

Stoichiometric calculations

Molarity vs Molality

Water is the Universal Solvent

Electrolytes

Dilutions

Acid Base Definitions

Hydronium Ions

Conjugate Acids

PH and POH

Cations and Anions

·         Cations: Positively charged
·         Anions:Negatively charged

Precipitation Reactions

·         2 aqueous solutions form a precipitate and another aqueous solution

Writing Precipitation Reactions

·         Molecular
·         Ionic
·         Net ionic (only counting ions that lead to the solid precipitate)

Troy ounce

·         I troy ounce weighs 31.1 grams

Redox reactions

·         Reduction: gains electrons
·         Oxidation: loses electrons

Oxidation numbers

·         The oxidation number for any element by itself is 0
·         Oxidation number of a monatomic ion = charge of the ion
·         Oxygen when not in hydrogen peroxide has on oxidation state of -2
·         Hydrogen = +1
·         Fluorine = -1
·         All halogens have an oxidation state of -1 unless bound to hydrogen or fluorine

Naming Ionic compounds

·         Cation, Anion
 
 
 
 
 

The Ideal Gas Laws

·         Boyle’s law; p*v = k
·         Jacques Charles; v/t = b
·         Amadeo Avogadro; volume/amount of moles = constant
·         Ideal gas Law; PV = nRT

The ideal gas law explained

·         Pressure is measured in pascals [newton’s/area in meters2] or in atmospheres
·         1ATM is equal to 101325 pascals or 100 kilopascals
·         N = amount of moles
·         R = universal gas constant [8.3145 lkpa/kmol]
·         T = degrees in kelvin

Gas jargon

·         STP = 0 degrees Celsius and 100 kilopascals of pressure
·         1 mol of any ideal gas takes up 22.4 liters of space at STP
·         Absolute zero; 0 kelivins or -273.15 Celsius
 
 

Vander walls Equation

·         (P+n2a/v2)(v-nb) = nRT
·         b= mass taken by each gass
·         a= attraction constant

Rule of partial pressures

·         so long as the gases don’t chemically react the total pressure of 2 gases in a container is equal to the sum of the pressure of the 2 gasses

Kinetic Energy

·         Ek = ½ mv2
·         V = square root of 2 * Ek/m

Effusion

·         r = v/t
·         ra/rb = sqare root of ma / square root of mb

Change in Energy

·         change in energy = q + E
·         exothermic = - value of delta E
·         endothermic = + value of delta E

Enthalpy

·         H = E + PV
·         Change in enthalpy = change in heat
·         Delta H = q

Standard formations

·         T=25 degrees Celsius
·         C=278.15 k
·         P=1atm

Hess’s law

·         Change in enthalpy = sum of the standard enthalpies of the formation of the products – the sum of the standard enthalpies of the reactants
·         Delta H = the sum of the number of moles of products time the standard enthalpies of the products – the number of moles of reactants times the sum of the reactants

Calorimetry

·         Delta H = the specific heat capacity of the substance times it’s total mass time the change in temperature
·         Mass is represented as grams
·         Temperature is represented as kelvin

Entropy

·         Change in entropy = the sum of the standard entropies of formations of the products time the moles of products – the sum of the standard entropies of formations of the reactants time the moles of reactants

Gibbs free energy

·         Delta g = delta h – t time delta entropy

The Speed of Light

·         C = wavelength * frequency
·         C = 3*108 m/s
·         High frequency beams will eject an electron
�����&�i=