Chemistry 121 Spring Quarter 2014 - Review

1. Chemistry 121Spring Quarter 2014 - Review Online HW for 9 (due 5/30) & 10 (due 6/3/2014, Tues) Last Wet Lab: Attend 2nd half this week (12 noon for me) Final Exam: Tuesday, 6/10/2014, 1:00-3:00 pm Based on Points, the Final Exam is about: ~ 35 % Quantitative ~ 65 % Qualitative

2. Chapter 1- Intro & Measurements Divisions of Chemistry Scientific Method Matter Categories Precision & Accuracy Physical & Chemical Properties Significant Figures Measurements - Length, Volume, Mass, Density, Temperature Problem Solving - Equations & Conversion Factor Separations: Filtration, Distillation, Chromatography Equations: d=m/v, oF=(1.8xoC)+32, K=oC+273 Eng. Syst: ft, in, yd, mi, lb, oz, ton, qt, cup, gal, sec, min, hr SI: k,c,m,μ,n,p; 1 mL = 1 cm3 Cv. Fact.: 1lb=454g, 1L=1.06qt, 1in=2.54cm, d of H2O=1g/mL 12 %

3. Chapter 2 - Atoms, Molecules, Ions Atomic Structure: # P, N, e- & general positions within atom History Periodic Table & General Trends Formulas Ionic Bonding Nomenclature: Ionic, Ionic & Transition Metals, Molecular Polyatomic Ions: Names & Charges for all given in L. notes Mass Spectrometer Balancing Chemical Equations Isotopes Metals & Nonmetals Acids – Definitions, Strengths, Rxns with bases 13 %

4. Chapter 3 - Stoichiometry Moles - #s - grams: 1mol = FW in g = 6.02x1023 # Avogadro’s Number Percent Composition: W/W% = (g part / g total) x 100% Empirical Formulas: Defn; get from % or from g Molecular Formulas: Get from EF & MW Regular Stoichiometric Problems Limiting Reagent Problems Left Over Reagent Problems % Yield 17 %

5. Chapter 4 - Reactions Electrolytes Solubility Rules (from lecture notes) Molecular (ME), Complete Ionic (CIE), Net Ionic Equations (NIE) Rxn Types - Precipitation, Neutralization, Redox & Nonredox Predicting Products: 1) formation of gas - 6 gas eqns; 2) ppt - solubility rules; 3) H2O formation - acid-base rxn. Oxidation Numbers (Know Rules) Oxidation & Reduction: Definitions, Identify, half reactions Molarity, MM = moles/L Dilution Problems: M1V1 = M2V2 Gravimetric & Volumetric Problems (get moles from MxL) Titrations – Rxns, calculations, indicators, terminology 20 %

6. Chapter 7 - Atomic Theory History EMR – Types, Excitation, Calculations: λ, ν, or E EMR Equations: E = hv = hC/λ; v = C/λ Speed of Light, C = 3.00x108 m/s Quantum Numbers & Quantum Model of Atom Principal n = 1,2,3,…n; Subshelll = 0,1,2,3,4,5…n-1 (s,p,d,f,g); # Subshellml = -l,…-1,0,+1…+l; Spin Levels ms = ± 1/2 Orbital Shapes for s & p Electron Configurations for Atoms & Ions (Continued )

7. Chapter 8 - Electron Configurations Stable Electron Configurations: closest inert gas rule (octet) Exceptions to octet rule: 1) H stable with 2 valence e-2) Al & B somewhat stable with 6 Valence e-3) n≥3 elements use d orbitals & have 8, 10, or 12 e- involved in bonding. Trends: Size; Ionization Energy; Electronegativity Periodic Chart & electron configurations Magnetism – Magnetic & Nonmagnetic Elements 16 % for Chapters 7 & 8

8. Chapter 9 - Ionic & Covalent Bonding Ionic Bonds Covalent Bonds Nonbonding Valence Electrons Bond & Molecule Polarity Lewis Structures (know rules for Lewis Structures) Exceptions to Octet Rule: 1) B, Al & 2) use of d orbitals Multiple Bonds – Double & Triple Resonance Formal Charge: FC = VE - 1/2 BE - n Bond Energy & Bond Energy Problems IR Spectrophotometer (Continued )

9. Chapter 10 - Molecular Geometry and Bonding Valence Bond Theory Electron Geometry - for up to 4 “things” attached Molecular Geometry - for up to 4 “things” attached Bond & Molecular Polarity Hybrid Atomic Orbitals (HAO): sp, sp2, sp3, sp3d & sp3d2 Molecular Orbital (MO) Theory - General Sigma and Pi Bonds Definition of “things” (pairs of nbve & atom/s attached) 22 % for Chapters 9 &10

10. Study for the Final – Even if you are content with your present grade or else you may end up like these miserable felines.