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Study Guide and Practice questions for final paper.
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American Chemical Society (A.C.S) General Chemistry Exam 70 multiple choice questions, 110 minute Bring a Scantron, calculator and pencil(s)
Preview for ACS-Standardized final Exam
Percentile Rank
Grade Recorded
Score
Percentile Rank
Grade Recorded
Score
Percentile Rank
Grade Recorded 10 0% 15 33 31% 75 52 90% 100 17 2% 20 34 34% 75 53 92% 100 (17.5 should be the statistically average score of a monkey guessing!)
20 4% 35 National Average is 38.3 58 97% 100 21 5% 40 39 53% 80 59 98% 100 22 6% 45 40 56% 80 60 98% 100 23 7% 50 41 60% 85 61 98% 100 24 9% 55 42 64% 85 62 99% 100 25 10% 55 43 67% 85 63 99% 100 26 12% 60 44 71% 90 64 99% 100 27 14% 60 45 74% 90 65 99% 100 28 16% 65 46 77% 90 66 100% 100 29 19% 65 47 80% 90 67 100% 100 30 22% 70 48 82% 95 68 100% 100 31 24% 70 49 84% 95 69 100% 100 32 28% 70 50 87% 95 70 100% 100 51 89% 95
I. States of matter Ideal Gas Law: pV=nRT, pM=dRT, deviations from ideal (high P, low T) Ionic solids: simple cubic, face centered cubic, body centered cubic Phase diagrams: Pressure versus temperature Intermolecular Forces: ion-diope, hydrogen bonding, etc. II. Stoichiometry and Thermochemistry Hess’s Law and Enthalpy: “standard states” have ΔHf^0 = 0 Percent composition: %C, %H, etc. Combustion analysis Limiting Reactants Stoichiometry III. Atomic Structure and periodicity Oxidation states of “main group” elements (Li, Be, B, etc) Oxidation numbers Electron configurations and relation to groups on periodic table (ns^2 np^5 =halogens) Periodic trends: Electronegativity, atomic radii Nuclear chemistry: Mass number, atomic number IV. Molecular Structure Modes of bonding: ionic, covalent (both polar and non-polar) Lewis Dot, VSEPR, polarity, bond angles, resonance structures V. Solutions Molarity: mol solute/L solution; also dilution (M 1 V 1 =M 2 V 2 ) Net ionic equations Percent dissociation in water (electrolyte strength) Molality: mol solute/kg solvent Freezing point depression/boiling point elevation ΔTf=Kfm VI. Acids, Bases and Ionic Equilibria Know the “spectator” ions in acid/base reaction: Na+, K+, Cl-, NO 3 -^ etc. Know general reactions for acid base (strong acid+ strong base, SA + WB, WA+SB) Equivalence point, finding unknown concentrations Buffers: What makes a buffer, what a buffer is, etc. pH: calculate pH of weak acids or reactions prior to the end point (strong acid+ strong base, SA + WB, WA+SB) VII. Chemical Equilibrium – Molecular General equilibrium expressions: know how to find K LeChatlier’s principle: effect of heat upon endothermic/exothermic reactions Precipitation reactions VIII. Kinetics Rate of disappearance, rate of formation Effect of catalysis Rate laws and ahlf life from experimental data Energy of activation IX. Thermodynamics Enthalpy, entropy, free energy Relation of free energy to equilibrium constant and Eo