Chem+II+Final+Review

Chapter 11: gases kinetic molecular theory assumptions of gases pressure is from constant molecular collisions pressure units pressure unit conversion Boyle's Law, Charle's Law, Gay-Lusac Combined gas law ideal gas law: value of R, units of R Avogadro's Law: volume and moles molar mas Dalton's law of partial pressures molar volume of a gas at stp: X L /mole, it's a conversion factor

Chapter 12: intermolecular forces thermal energy properties of liquids, solids, gases, surface tension, viscosity evaporation and condensation boiling boiling point energetics of vaporization adn condensation heat of vaporization melting point freezing and sublimation heat of fusion Types of intermolecular forces dispersion force instanteous dipole dipole-dipole hydrogen bonding types of solid: molecular solids, ionic solids, atomic solids

Chapter 13: homogeneous, hetergeneous aqueous solutions solubility saturated, unsaturated, super saturated eletrolytes, non electrolytes and conductivity solubility vs temperature for solids and gases mass percent mass percent in calculations concentration: Molarity! moles/liter solution dilution m1v1=m2v2 solution stoich: use mL and molarity to reach moles, then use mole map boiling point elevation calculate new boiling point freezing point depression calculate new freezing point osmosis

Chapter 14 Acids and Bases acid properties sulfuric acid, nitric acid, acetic acid, carboylic acid bases properties Arrehenius definition of acids and bases hydronium (H3O+) Bronsted-lowry definition of acids and bases conjugate acids and conjugate bases acid base reaction, neutralization, similar to double displacement reaction acids with metals titrations indicators strong acids weak cacids strong base weak base Water is amphoteric, acts like an acid and a base pH scale calculating pH from [H3O+] pOH scale calculating pOH from {OH-] buffers

Chapter 15 equilibrium collision theory concentration and temperature as dials dynamic equilibrium reversible reactions equilibrium constant (Keq) writing equilibrium equations Keq bigger than 1, smaller than 1 what to do with pure solids and pure liquids Isolating concentration using Keq Le Chatelier's Principle concentration changes on Keq pressure changes on Keq temperature chagnes on Keq: endo vs exothermic rxns volume changes on Keq Solubility product constant : Ksp Ksp -> molar solubility aka concentraction aka molarity Activation Energy Activation Energy vs reaction rate role of catalysts role of enzymes

Chapter 16 Redox LeoGer reducing agent oxidizing agent oxidation number, 2 pages of rules in notes balancing redox half reactions balancing redox reactions in acid or in base activity series batteries electrical current anode cathode half cell electrochemical cell salt bridge volatege Lead Acid Batteris Fuel Cells Electrolysis splitting water into hydrogen and oxygen

Chapter 18 Organic- alkanes, alkenes, alkynes saturated vs unsatured isomers nomenclature Hydrocarbon reactions with Cl2 Benzene naming benzene molecules: ortho, meta, para, aka 1,2 or 1,3 or 1,4 substitution functional grouops: alcohols, ethers, aldehydes, ketones, carboxyilic acids, esters, amines nomenclautre for each functional group

Chapter 17 nuclear chemistry rontgen henri bequerel marie curie radioactivity alpha, beta, gamma, positron atomic symbols using molecular mass and atomic number mass of a proton, neutron, electron half life decay series carbon dating atomic fission atomic bombs chain reactions