thermodynamics-
enthalpy - endothermic vs exothermic describe energy changes associated with reactions
entropy – disorder predict and describe change in entropy
equilibrium and reversible reactions- describe changes in rates of reaction over time
- at equilibrium- rate of forward reaction equal rate of reverse and conditions remain constant
vapor pressure equilibrium
solubility of ionic compounds in aqueous solutions and Ksp
calculating Keq
using collisions and rates to predict direction of shift
using Le Chatelier’s Principle to predict direction of shift
rates of reactions- factors affecting the rates- Explain using collisions
temperature / surface area / concentration / agitation
bonding-
metallic (m w/ m)- loose sea of electrons shared by all of the atoms
electronegativity and bonding (difference in EN allows you to determine extent of sharing)
diff in EN 0.0 – 0.5 (nonpolar) 0.5 – 1.9 (polar) above 1.9 (ionic)
ionic ions held together due to their opposite charges
covalent electrons shared in pairs between two atoms- in discrete orbitals
polar covalent vs nonpolar covalent
intermolecular attractions- attraction between molecules special example- hydrogen bonding
polar molecules- oppos. charged ends attracted - dipole-dipole attractions
nonpolar molecules
no oppos. charged ends so little attraction between - induced dipole-induced dipole att.
ions dissociate and are attracted to polar water molecules - ion-dipole attractions
stable octet and bonding- drawing Lewis structures
reactions- complete analysis be able to describe particles, bonds and changes
sythesis and decomposition
double replacement- formation of precipitates, acid/base neutralization
single replacement and activity series
redox reactions- oxidation and reduction- be able to write half-reactions
combustion combine w/ O2- specifically of hydrocarbons to form water and CO2
nomenclature naming ionic compounds including acids and covalent molecules
conductivity- require movement of charged particles
metals conduct as solids- since the electrons (charged particles) are free to move
ionic compounds conduct as liquids and in solution - since the ions (charged particles) are free to move
solutionspolarity predicts solubility- like dissolves like
ionic compounds - dissociate in solution -
ions separated and surrounded by water molecules (ion-dipole attractions)
varying degrees of solubility- as defined by Ksp (equilibrium)
mole calculations- stoichiometry
predicting quantities using the balanced equation
calculate moles given grams, volume of gas or volume of solution with molarity
identifying the limiting reactant
development of atomic models- Democritus, Dalton, Thomson, Rutherford, Bohr
electromagnetic radiation- radio waves, infrared, ROYGBIV, ultraviolet, x-rays, gamma rays
relate and calculate wavelength, frequency and energy
excited atoms and the emission spectrum
electron configuration and quantum mechanicsand patterns on periodic table e- config relates to reactivity
gas laws andrelating pressure, volume, temperature and moles and calculations using ideal gas law (PV=nRT)
acid/base chemistry – weak vs strong acids and titration calculations and pH