Download AP Chemistry

AP Chemistry
Fall Semester Review
Unit 1 Intro to Chem Ch 1 & 2
Writing formulas, etc.
Book info
Naming, writing formulas
Polyatomic ions
Metric conversions
Dimensional analysis
Sig figs
Uncertainty
Accuracy vs precision
Systematic/random error
Family/group names
Atom models
Subatomic particles
Unit 2 Stoichiometry Ch 3
Stoichiometry
Mole calculations
grams to mole to mc, fu, atom
Aversge molar mass (beanium)
% composition, mass percent
EF/MF
Stoichiometry, solutions & solids
Limiting reactant
Percent yield
Balancing equations
Molarity
Unit 3 Reactions Ch 4
Solubility rules
Ionic formulas
Types of reactions
Balancing Equations
Unit 4 Gases Ch 5
Barometer/manometer
Boyles, Charles, Avogadro’s
Ideal gas Law
Gas Stoich
Dalton’s law
KMT
Root mean square velocity
Graham’s Law
Van der Waals equation
Non-ideal conditions
Mole fractions
Unit 5 Thermo Ch 6
Heat
Temperature
Energy
State function
System vs surroundings
Work
Driving force
∆E = q + w(P∆V)
laws
enthalpy, H
endothermic
exothermic
calorimetry
Standard enthalpy of formations
Bond energy calculation (9.10)
Unit 6 ∆G, ∆S, ∆H Ch 16
entropy, S
Gibbs free energy, G
Spontaneity
∆Ssurr
∆Ssystem
∆Suniverse
Hess’s Law
∆E = Eproducts – Ereactants
equilibrium, Keq
∆G at other conditions
Potential energy
Kinetic energy
System vs surroundings
Unit 7 Quantum Chem Ch 7
Atomic structure & periodicity
EM radiation
Visible spectrum
, , c
E of visible spectrum
Quantized energy, E = mc2
Photons, E=hv
Dual nature of light
Continuous spectra
Bright line spectra
Bohr model of atom
Ground vs Excited state
Spectral series
Orbital
Heisenberg uncertainty princ.
(Unit 7 continued)
Quantum #’s: n, l, ml, ms
Pauli exclusion principle
Periodic table
Aufbau, Hund’s rule
Valence vs. Core electrons
Electron configurations
Diagonal rule, exceptions Cr, Cu
Trends: IE, electron affinity
Atomic radius, valence electrons
Unit 8 Bonding Ch 8 & 9
Bond energy,
bond length
Types of bonds
Electronegativity
Ionic radius
trend
Lattice energy
% ionic character
Lewis structures
Valence electrons
Octet rule
Resonance
Formal charge
VSEPR model
Bond angles
Hybridization
,  bonds
Unit 9 Liquids & Solids Ch 10
Intermolecular forces
Dipole-dipole forces
Hydrogen bonding
London dispersion forces
Van der Waal forces
Surface tension
Capillary action
Viscosity
Crystalline solids
Lattice unit cell
Ionic solids
Atomic solids (metallic, network, Group 18)
Molecular solids
Malleable
Ductile
Band model
Alloys: substitutional, interstitial
Diamonds vs graphite
** Fall semester final is 60 questions. It
is designed to take you 90 minutes, very
much like the first half of the AP exam.
You will be pressed for time to finish. I
will not allow you extra time to finish.
Good luck and happy studying. The final
will be worth 200 points.
Nuclear Packet Ch 21
Radiation (ionizing vs non)
Alpha decay
Beta decay
Gamma radiation
Half-life
Radioisotopes
Carbon dating
E=mc2
Fission
Fussion
Nuclear waste
Silica, silicates
Amorphous solids
Glass
Semiconductors
∆Hvaporiation
Vapor pressure
Evaporation
Sublimation
Changes of state
∆Hfusion
Melting, boiling point
Supercooled, super heated
Phase diagram
Triple point
Critical temp.
pressure
point