CHEM 130 Final Review Chapter Chp 1 Chemistry Define Introduction Scientific approach Describe Theory, natural law Distinguish between theory & law Chp 2 Scientific notation Conversions between standard and SN forms Measure- Metric prefixes Must know kilo, centi & milli ments & Uncertainty, Counting, rounding, determining SF s Calculations significant figures Dimensional analysis, conversion factor, equivalence statement Unit conversions Fahrenheit, Celsius & T K = T + 273.15 o Temperature conversions C Kelvin scales T = 1.80 o F ( To C) + 32 Density D calc s, determining m, V from D Chp 3 Matter & Energy Physical & properties & changes Mixtures & pure substances Heterogeneous & homogeneous mixtures Energy, temperature, exo- & endothermic States of matter D = m V 1 cal = 4.184 J Q = S x m x ΔT Identifying, distinguish Identifying, distinguish Find T i, T f, S or Q Define gas, liquid, solid Indicate properties of each phase -making/breaking intramolec. bonds. Physicalmaking/breaking intermolec. bonds
Chp 4 Elements Atoms & Ions Chp 5 Nomenclature Chp 6 Reactions Elemcnts & symbols Dalton s atomic theory Proton, neutron, electron, isotope, cation, anion, ionic compound Compounds & formulas Diatomic molecules Metals, nonmetals, noble gases, transition metals, inner transition metals, alkalai metals, alkaline earth metals Metal-nonmetal binary compounds Non-metal non-metal binary compounds Polyatomic ions and their compounds Acids Reaction evidence Writing reactions, reactants, products Conservation of matter A Z X Identify element from symbol Identify symbol of element Identify ideas Identify isotopes Interpret or write isotopic symbols Write formulas based on ion charges to achieve zero net charge Locate on periodic table Identify classification of element from location on periodic table Identifying change Define Balancing reactions Must memorize Remembering when to use diatomic formula Remembering to use Roman numeral if metal has more than 1 charge Use prefixes Memorize polyatomic ions Learn prefixes, suffixes -ate polyatomic ions becomes ic acid -ite ion becomes ous acid Know nomenclature! Remember physical states
Chp 7 Reactions in Aqueous Solution Chp 15.1-5 Acids & Bases Chp. 17.1-2 Redox Reactions Molecular, total ionic Write them out & net ionic equations, Convert between types spectator ions Precipitation reactions, Define, recognize, write equations Know how to use solubility guidelines solubility Acid-base reactions Define, recognize, write equations Remember strong acids Use H 3 O + NOT H +! Redox reactions, Define, recognize, write equations Combustion always includes O 2 and oxidation, reduction often H 2 O & CO 2 Combustion, synthesis & decomposition rxns Conjugate acids & Define, identify bases, conjugate pairs Acid ionization & dissociation Autoionization of [H 3 O + ][OH - water, K w ]=1.0x10-14 ph, poh, pk w px=-log(x) Calculate ph, poh Low ph = high [H 3 O + ] & low [OH - ] Oxidation states Identify OS in a reaction Chp 8 Composition Amu Mole 6.022x10 23 Molar mass % composition Empirical & molecular formula mole MM = m n % = part whole x100 Convert between atoms & moles Calculate, use to convert between mass & moles Calculate Determine EF & MF Just a relative weight
Chp 9 Quantities Stoichiometry, limiting reactant, excess reactant Theoretical, actual & % yield % yield = actual theoretical x100 Define, calculate Calculate theoretical or % yield MUST use mole/mole ratio from balanced reaction Watch for LR problems! Chp 10 Modern Atomic Theory Chp 11 Bonding Electromagnetic radiation, wavelength, frequency Photons, quantized energy, emission & absorption spectra Principle energy levels & sublevels, orbitals Pauli exclusion principle, hund s rule Electron configurations, shorthand configurations, orbital diagrams Ionization energy, electron affinity, atomic & ionic size Covalent, polar covalent and ionic bonds c=λ ν explanations Writing electron configurations & orbital diagrams Predicting and explaining periodic trends Determine bond type Electronegativity Define, explain Know periodic trend Bond polarity, dipole moment Indicate bond polarity, predict molecular dipole Lewis structures 6N+2 Draw Lewis structures from formula N is number of atoms NOT including H! VSEPR, molecular geometry Predict geometry
Chp 12 Gases Pressure, barometer, 1 atm=760 mm Hg= Describe, explain, convert units manometer, units 760 torr Ideal gas law PV=nRT Calculate one of the variables Use ONLY on gases, R=0.08206 L Use when missing 1 variable atm/mol K Combined gas law P 1 V 1 = P V Calculate one of the variables Use when conditions have been changed 2 2 n 1 T 1 n 2 T 2 Dalton s Law of partial P total =P 1 + P 2 + Calculate partial or total pressure pressure STP, molar volume 22.4 L Define ONLY at STP! mol Gas stoichiometry Calculate Rearrange ideal gas law for n Chp 13 Liquids & Solids Phase diagrams, energy requirements for phase changes Specific heat, heat of fusion, heat of vaporization Intermolecular forces, dipole-dipole, hydrogen bonding, dispersion forces Vapor pressure Crystalline solids, ionic, molecular, atomic Electron sea model Q=m S ΔT Q=m ΔH Sketch phase diagram Calulate energy requirements for temperature and phase changes Define, identify Define, use to indicate relative strength of intermolecular forces Define, give examples Amorphous solid, substitutional and interstitial alloys Define, give example
Chp 14 Solutions Solute, solvent, saturated, unsaturated, supersaturated Mass percent mass solute mass solution x100 Define Calculate Chp 16 Equilibrium Molarity M = n solute V solution Dilution M 1 V 1 = M 2 V 2 Calculate new [ ] or volume needed Must use ONLY on dilution, never on stoichiometry problem Stoichiometry Use molarity to calculate n used in Watch for LR Neutralization reaction, titration, standard, indicator Activation energy, catalyst, equilibrium, eq. constant, eq. conditions Le Chatelier s principle K = [C]c [D] d [A] a [B] b stoich problems etc Define, calculate Define, write eq. expression, calculate K from [ ], calculate [ ] from K Predict eq. positions changes Just another stoichiometry problem Equilibrium expression does not include s or pure l Solubility equilibria K sp = [M + ] m [X " ] x Calculate K sp or [ ]