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Key Topics to Review
1. Fundamentals of Chemistry Matter and Measurement: o States of matter (solid, liquid, gas). o Physical vs. chemical properties. o Units of measurement (SI units, metric conversions). o Significant figures and scientific notation. Atomic Structure: o Subatomic particles (protons, neutrons, electrons). o Atomic number, mass number, isotopes. o Periodic table organization (groups, periods, trends). 2. Stoichiometry Chemical Equations: o Balancing chemical equations. o Types of reactions (combustion, synthesis, decomposition, single- replacement, double-replacement). Mole Concept: o Molar mass and conversions between moles, grams, and particles (Avogadro’s number). Stoichiometric Calculations: o Limiting and excess reactants. o Percent yield and theoretical yield. 3. Chemical Bonding
Types of Bonds: o Ionic vs. covalent bonding. o Polar vs. nonpolar bonds. Lewis Structures: o Drawing structures for molecules. o Octet rule exceptions. Molecular Geometry: o VSEPR theory (shapes: linear, trigonal planar, tetrahedral, etc.). Intermolecular Forces: o Hydrogen bonding, dipole-dipole, London dispersion forces.
4. Thermochemistry Energy and Heat: o Endothermic vs. exothermic reactions. o Heat capacity, specific heat, calorimetry. Enthalpy: o Standard enthalpy of formation (ΔHf0\Delta H_f^0ΔHf0). o Hess’s Law and enthalpy calculations. 5. Gases Gas Laws: o Ideal Gas Law: PV=nRTPV = nRTPV=nRT. o Boyle’s, Charles’s, and Avogadro’s laws. Kinetic Molecular Theory:
Equilibrium Constant (KKK): o Expression for KcK_cKc and KpK_pKp. o Relationship between QQQ and KKK (reaction quotient). Le Châtelier’s Principle: o How systems at equilibrium respond to changes in concentration, pressure, and temperature.
9. Thermodynamics Laws of Thermodynamics: o First law (energy conservation). o Second law (entropy increases in spontaneous processes). Gibbs Free Energy (ΔG\Delta GΔG): o ΔG=ΔH −TΔS\Delta G = \Delta H - T \Delta SΔG=ΔH −TΔS. o Relationship to spontaneity (ΔG<0\Delta G < 0ΔG<0). 10. Kinetics Reaction Rates: o Rate laws (Rate=k[A]m[B]n\text{Rate} = k[A]^m[B]^nRate=k[A]m[B]n). o Determining rate constants and reaction orders. Mechanisms: o Elementary steps and rate-determining step. Catalysts: o Role in lowering activation energy.
11. Lab Skills Measurements and Techniques: o Proper use of balances, pipettes, and burettes. o Reading lab instruments accurately. Error Analysis: o Percent error, precision, and accuracy. Safety Rules: o Handling chemicals and glassware properly. Study Tips 1. Understand Concepts, Not Just Formulas: o Focus on why reactions happen, not just how to calculate results. 2. Practice Problems: o Work through sample problems, especially in stoichiometry, gas laws, and equilibrium. 3. Use Flashcards: o Memorize key formulas, periodic table trends, and definitions. 4. Review Class Notes and Past Exams: o Identify common question types and focus on weak areas. 5. Utilize Online Resources: o Watch tutorials for topics like titrations or VSEPR theory. 6. Group Study: o Explaining concepts to peers can reinforce your understanding.
