Course Aim

  • Prepare students for challenges in professional medical programs involving Biochemistry, Physiology, Pharmacology, and Medicinal Chemistry.

Course Outline

  • Key topics: Chemical bonding, Acid-Base Equilibria, Electrochemistry, Chemical Equilibrium, Chemical Kinetics, Solubility.

Course Objectives

  • Understand chemical bonding, acids and bases, electrochemistry, and chemical thermodynamics/equilibrium concepts.

Key Concepts in Chemical Bonding

  • Types of bonding: Intramolecular (ionic, covalent, metallic) and Intermolecular (dipole-dipole, hydrogen bonding, London forces).

Ionic Bonding

  • Electrostatic force between cations and anions, Lattice energy calculation:
    ΔH<em>f=ΔH</em>1+ΔH<em>2+ΔH</em>3−ΔH<em>4−ΔH</em>5\Delta H<em>f = \Delta H</em>1 + \Delta H<em>2 + \Delta H</em>3 - \Delta H<em>4 - \Delta H</em>5
  • Example: formation of NaCl.

Covalent Bonding

  • Characterized by shared electron pairs, forming sigma (σ) bonds and potentially pi (π) bonds in multiple bond scenarios.
  • Importance of electronegativity and bond polarity.

Molecular Shape

  • VSEPR theory to determine molecular shapes and angles based on electron pair repulsion.
  • Different configurations: Linear (AX2), Trigonal planar (AX3), Tetrahedral (AX4), Trigonal pyramidal, Bent.

Hybridization

  • Types: sp3, sp2, sp, sp3d, sp3d2, relevant for molecular geometry and bonding characteristics.

Intermolecular Forces

  • Types: Dipole-Dipole, Hydrogen bonding, London dispersion forces, affecting physical properties of substances.

Acids and Bases

  • Definitions: Arrhenius (producing H+ or OH-), Bronsted-Lowry (proton donors/acceptors), Lewis (electron pair acceptors/donors).
  • Strength classification: Strong vs. weak acids/bases based on ionization in solution.

Concepts of Acid/Base Equilibria

  • Key expressions: Dissociation Constants (Ka, Kb), pH, pOH, Kw, and their significance.
  • Calculations of pH from concentrations and relation to hydroxide ions.

Redox Reactions in Electrochemistry

  • Explanation of oxidation/reduction processes in terms of oxygen, hydrogen, electrons, and oxidation numbers.
  • Electrolysis principles and applications: purification, electroplating, and Faraday's laws of electrolysis.

Chemical Equilibrium

  • Concepts of equilibrium, factors affecting it including temperature, concentration, and pressure changes (Le Chatelier's Principle).
  • Equilibrium expression formulation and calculations using concentrations and partial pressures.

Summary of Important Formulas

  • pH = −log[H+]-log[H+]
  • Kc and Kp relationships, Law of mass action, and effects of temperature on equilibrium constants.