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Comprehensive Study Guide for Chemistry: Key Concepts and Problem-Solving Strategies

This study guide covers essential chemistry topics from introductory concepts to advanced theories. It provides systematic approaches to studying, such as reviewing exams and homework, identifying problem areas, and understanding fundamental principles. Key chapters include dimensional analysis, atomic theory, stoichiometry, reactions in aqueous solutions, gas laws, energy relationships, electronic structure, periodic trends, bonding theories, molecular geometry, intermolecular forces, kinetics, and thermodynamics. This guide emphasizes active problem-solving and foundational understanding to facilitate learning and retention.

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Comprehensive Study Guide for Chemistry: Key Concepts and Problem-Solving Strategies

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  1. How I would study: • Look over exams • Look over review sheets • Difficulties? Work HW problems, examples from the text • Start early: where are your problem spots?

  2. Chapter 1: Introduction • Dimensional analysis • Change among units (eg. feet vs. meters) • Prefixes (1 kilogram/1000 grams) • Density (d = m/v) • Scientific notation • Don’t worry about sig. figs

  3. Chapter 2: Atomic Theory • Chemical formulas • Molecular formula vs. empirical formula • Naming compounds • Ionic (Table 2.3) vs. molecular • Atomic number

  4. Table 2.3

  5. Chapter 3: Stoichiometry • Atomic mass, molecular mass • Molar mass • Percent composition/determining empirical formulas • Chemical equations • What do coefficients tell you?

  6. Chapter 3: Stoichiometry • Limiting reagents • Assume each reagent is limiting, calculate theoretical yields. Lower result? • Actual, theoretical, percent yields

  7. Chapter 4: Reactions in aqueous solutions • Electrolytes • Precipitation reactions • Solubility • Molecular/ionic/net ionic equations • Acid/base reactions • Oxidation-reduction reactions • Writing half-reactions • Oxidation numbers

  8. Table 4.2

  9. Chapter 4: Reactions in aqueous solutions • Molarity • Gravimetric analysis • Essentially limiting reagent problems • Acid-base titrations • #mol acid = #mol base

  10. Chapter 5: Gases • Ideal gas equation (PV = nRT) • Partial pressures • eg. if a gas is collected “over water,” the total pressure comes from the gas and water’s vapor pressure • Mole fraction Px = nxPT

  11. Chapter 6: Energy relationships in chemical reactions • Endothermic vs exothermic • DE = q + w • q = heat (thermal energy) • w = work (w = -PDV) • Enthalpy/thermochemical equations • DH = H9products) – H(reactants) • DH of formation • Indirect vs. direct methods

  12. Chapter 6: Energy relationships in chemical reactions • Calorimetry: find the energy change in a reaction (or process) qcal + qrxn = 0 qrxn = -qcal q = msDt = CDt

  13. Ch 7: Electronic structure of atoms • Atomic orbitals • s, p • Electron configurations • Quantum numbers • 1s2 2s2 2p6 … • Pauli exclusion principle • Hund’s rule

  14. Fig. 7.21

  15. Ch 8: The Periodic Table • Isoelectronic • Effective nuclear charge • Atomic/ionic radius • Ionization energy • Electron affinity

  16. Ch 9: The Covalent Bond • Lewis structures • Formal charge • Resonance • Electronegativities • Covalent/polar covalent/ionic • Bond energies DH = BE(reactants) – BE(products)

  17. Ch 10: Molecular Geometry & Hybridization of Atomic Orbitals • Geometries (VSEPR model) • Hybridization • Sigma (s) vs. pi (p) bonds

  18. Table 10.1 No lone pairs

  19. Table 10.2 With one pairs

  20. Table 10.4 Hybridization

  21. Ch 12: Intermolecular forces • Boiling, melting points • Dipole: molecule must be polar • Electronegativity AND geometry • Ionic • Ion/dipole • Dipole/dipole • Hydrogen bond • Induced dipole • Dispersion

  22. Ch 14: Chemical Kinetics • Rate of reaction • Decrease of reactant/increase of product • Depends on coefficients • Rate laws Rate = k[A]x[B]y • Half-life (first order) • Rate vs. temperature • Collision frequency • Activation energy • Arrhenius equation

  23. Ch 15: Chemical Equilibrium • Equilibrium constant • Direction of a reaction • Q vs. Kc • Le Châtlier • Concentration (adding reactant or product) • Pressure • Temperature

  24. Ch 16: Acids and Bases Ch 17: Buffers • Conjugate acid/base pairs • Water: both an acid and a base • Kw = 10-14 • Strong vs. weak acids • Ka & Kb • Calculate pH, given pKa and concentration of a weak acid • Calculate concentration of a weak acid to give a pH (given pKa)

  25. Ch 18: Thermodynamics • Entropy (S): disorder • Increased S (more disorder) favorable • Decreased H (less thermal energy) favorable DG = DH - TDS

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