AP  Chemistry  2013  Outline   1. Structure  of  Matter  (Chapters  1,2,3,7,8  electron  configuration   packet)   o Atoms  and  elements    Combinations  of  atoms  and  elements    Number  of  atoms  in  a  substance    Moles   o Atomic  structure    Protons,  neutrons,  electrons    Electron  configuration   o Periodicity    Trends  based  on  electrons    Quantum  mechanical  model   o Atomic  models    Models  are  theoretical  and  can  change    All  atoms  of  one  element  aren’t  the  same    Electromagnetic  waves  help  describe  atoms   o Atoms  are  conserved    Chemical  equations    Stoichiometry   2. Bonding  &  Intermolecular  Forces  (9,  10,  11,  12,  gas  laws  packet)   o Physical  Properties    Properties  of  solids  and  liquids  by  stucture    Gasses    Solutions   o Forces  of  Attraction    London  Dispersion  Forces    Dipole  Forces/Electronegativity    Intermolecular  forces  help  determine  properties   o Electrostatic  force  –  aka  chemical  bond    Covalent/Shared  bonding    Ionic  bonding    Metallic  Bonding    Molecular  geometry  (VSEPR  and  Lewis)   o Solid  State  Bonding    Properties  of  ionic  solids    Properties  of  metallic  solids    Properties  of  covalent  network  solids    Properties  of  molecular  solids  with  low  molecular  weight   3. Reactions  (Chapter  4,  19,  reactions  packet)   o Chemical  Equations    Molecular  vs  Ionic  vs  Net  ionic  equations    Stoichiometry   o Classifying  types  of  Chemical  Equations    Synthesis  and  Decomposition    Acid  Base  Neutralization   o Chemical/Physical  transformations  involve  changes  in  energy    Production  of  precipitates  and  gasses    Endo/Exothermic      Electrochemistry/Redox  Reactions  

AP  Chemistry   Semester  1  

 

4. Kinetics  (Chapter  13)   o Rates  found  by  measuring  changes  in  concentration    Factors  affecting  rate  of  reactions    Rate  Law    Rate  constant   o Formation  of  products    Elementary  reactions:  unimolecular  or  multiple   molecules    Activation  energy    Arrhenius  equation   o Elementary  Reactions    Multisteps  are  made  of  many  elementary  steps    Rate  limiting  step    Reaction  intermediates   o Catalysts    Role  of  catalysts  with  activation  energy    Classes  of  catalysts   5. Thermodynamics  (Chapter  6,  18)   o Heat  transfer    Temperature    Movement  of  heat  energy   o Conservation  of  energy    Energy  transfer  does  work    Energy  in  =  energy  out    3  Processes  to  change  energy    Calorimetry   o Bonds  and  energy    Potential  energy  associated  with  bond  geometry    Net  changes  in  energy   o Electostatic  Forces    Attractive  forces    Chemical  bonds  vs.  intermolecular  interactions    Biological  and  polymer  systems   o Spontaneous  Reactions    Entropy    Enthalpy    Gibbs  Free  energy    External  soures  and  Gibbs  free  energy    Kinetics  and  thermodynamics   6. Equilibrium  (Chapters  14,15,16)   o Chemical  equilibrium  is  dynamic    Forward  and  reverse  reaction    Reaction  quotient    Equilibrium  means  large  variables  will  not  change   o Equilibrium  is  impacted  by  external  changes    Le  Chatelier’s  Principle    Q  and  K   o Chemical  equilibrium  and  acid  base  reactions  and  solubility    pH  and  pOH    pH  and  pKa    Ksp   o Equilibrium  and  Gibbs  free  energy    Equilibrium,  Gibbs  energy  and  thermal  energy  

AP  Chemistry   Semester  2