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