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Transcript
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