Download Chemical Reactions

General and Physical Chemistry–Syllabus- one Semester
Sackler faculty of medicine
Tel-Aviv University-Israel
CONTENTS:
Chemistry and Measurement: Introduction to Chemistry, Matter: Physical
State and Chemical Constitution, Measurements, Units.
Atoms, Molecules, and Ions: The Structure of the Atom, Isotopes, Atomic
Weights, Periodic Table of the Elements, Chemical Substances,
Chemical Reactions: Equations.
Stoichiometry: Molecular Weight and Formula Weight, The Mole Concept,
Mass Percentages from the Formula, Elemental Analysis: Percentages of
Carbon, Hydrogen, and Oxygen. Determining Formulas, Molar Interpretation of
a Chemical Equation, Amounts of Substances in a Chemical Equation, Limiting
Reactant: Theoretical and Percentage Yields.
Chemical Reactions: Ionic Theory of Solutions, Molecular and Ionic
Equations, Precipitation Reactions, Acid–Base Reactions, Oxidation–Reduction
Reactions, Balancing Oxidation–Reduction Equations, Molar Concentration
Diluting Solutions, Titration.
Gases: Gas Pressure and Its Measurement, Empirical Gas Laws, The Ideal
Gas Law, Stoichiometric Relationships with Gases, Gas Mixtures; Law of Partial
Pressures, Kinetic Theory of Gases, Molecular Speeds; Diffusion and Effusion.
Thermochemistry: Energy and Its Units, First Law of Thermodynamics;
Work and Heat, Heat of Reaction; Enthalpy of Reaction, Thermochemical
Equations, Applying Stoichiometry to Heats of Reaction, Measuring Heats of
Reaction, Hess’s Law, Standard Enthalpies of Formation.
Atomic Structure: The Wave Nature of Light, Quantum Effects and Photons,
The Bohr Theory of the Hydrogen Atom, Quantum Mechanics, Quantum
Numbers and Atomic Orbitals, Electron Spin and the Pauli Exclusion Principle,
Building-Up Principle and the Periodic Table, Writing Electron Configurations
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Using the Periodic Table, Orbital Diagrams of Atoms; Hund’s Rule, Some
Periodic Properties.
Chemical Bond: Describing Ionic Bonds, Electron Configurations of Ions,
Ionic Radii, Describing Covalent Bonds, Polar Covalent Bonds;
Electronegativity, Writing Lewis Electron-Dot Formulas, Formal Charge and
Lewis Formulas, Delocalized Bonding: Resonance, Exceptions to the Octet Rule,
Bond Length and Bond Order, Bond Energy, The Valence-Shell Electron-Pair
Repulsion (VSEPR) Model, Dipole Moment and Molecular Geometry, Valence
Bond Theory, Description of Multiple Bonding, Principles of Molecular Orbital
Theory, Electron Configurations of Diatomic Molecules of the Second-Period
Elements, Molecular Orbitals and Delocalized Bonding.
Intermolecular Forces: Comparison of Gases, Liquids, and Solids, Phase
Transitions, Properties of Liquids: Surface Tension and Viscosity,
Intermolecular Forces; Explaining Liquid Properties, Classification of Solids by
Type of Attraction of Units.
Chemical kinetics: Definition of Reaction Rate, Experimental Determination
of Rate, Dependence of Rate on Concentration, Change of Concentration with
Time, Temperature and Rate; Collision and Transition-State Theories,
Arrhenius Equation, Reaction Mechanisms: Elementary Reactions, The Rate
Law and the Mechanism, Catalysis.
Chemical Equilibrium: Chemical Equilibrium—A Dynamic Equilibrium,
The Equilibrium Constant, Heterogeneous Equilibria; Solvents in Homogeneous
Equilibria, Qualitatively Interpreting the Equilibrium Constant, Predicting the
Direction of Reaction, Calculating Equilibrium Concentrations, Removing
Products or Adding Reactants, Changing the Pressure and Temperature, Effect
of a Catalyst.
Acids and Bases: Arrhenius Concept of Acids and Bases, Brønsted–Lowry
Concept of Acids and Bases, Lewis Concept of Acids and Bases, Relative
Strengths of Acids and Bases, Molecular Structure and Acid Strength,
Autoionization of Water, Solutions of a Strong Acid or Base, The pH of a
Solution, Acid-Ionization Equilibria, Polyprotic Acids, Base-Ionization
Equilibria, Acid–Base Properties of Salt Solutions, Common-Ion Effect, Buffers,
Acid–Base Titration Curves.
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Colligative Properties: Ways of Expressing Concentration, Vapor Pressure of
a Solution, Boiling-Point Elevation and Freezing-Point Depression, Osmosis,
Colligative Properties of Ionic Solutions.
Free Energy and Spontaneity: Entropy and the Second Law of
Thermodynamics, Standard Entropies and the Third Law of Thermodynamics,
Free Energy and Spontaneity, Change of Free Energy with Temperature,
RelatingG to the Equilibrium Constant, Interpretation of Free Energy.
Electrochemistry: Construction of Voltaic Cells, Notation for Voltaic Cells,
Cell Potential, Standard Cell Potentials and Standard Electrode Potentials,
Equilibrium Constants from Cell Potentials, Dependence of Cell Potentials on
Concentration, Some Commercial Voltaic Cells, Electrolysis, Stoichiometry of
Electrolysis.
Bibliography:
1. Chemistry , Steven S. Zumdahl , Susan A. Zumdahl.
2. General Chemistry: Principles and Modern, Ralph H. Petrucci , F. Geoffrey
Herring , Jeffry D. Madura , Carey Bissonnette.
3. General Chemistry, Darrell Ebbing , Steven D. Gammon.
4. Chemistry , John E. McMurry , Robert C. Fay , Jill Kirsten Robinson.
5. Principles of Chemistry: A Molecular Approach, Nivaldo J. Tro.
6. Chemistry: The Molecular Science ,John W. Moore, Conrad L. Stanitski.
7. Chemistry: The Central Science, Theodore E. Brown , H. Eugene LeMay ,
Bruce E. Bursten , Catherine Murphy, Patrick Woodward , Matthew E.
Stoltzfus.
8. Chemistry: Principles and Reactions, William L. Masterton , Cecile N. Hurley.
Dr. Haj Yahya Anan
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