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Fundamentals of Chemistry

This course covers the basic principles of chemistry, including atomic structure, bonding, chemical reactions, and thermochemistry. Students will develop a strong understanding of the foundational concepts that are essential for more advanced chemical engineering studies. The outcome is the ability to apply chemical principles to engineering problems.


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  • The Atomic Theory
  • Electrons and Other Discoveries in Atomic Physics
  • The Nuclear Atom
  • Chemical Elements
  • Atomic Mass
  • Introduction to the Periodic Table
  • The Concept of the Mole and the Avogadro Constant
  • Using the Mole Concept in Calculations
  • The Periodic Law and the Periodic Table
  • Metals and Nonmetals
  • Sizes of Atoms and Ions
  • Ionization Energy
  • Electron Affinity
  • Magnetic Properties
  • Polarizability
  • Chemical Reactions and Equations
  • Stoichiometry
  • Chemical Reactions in Solution
  • Determining the Limiting Reactant
  • Other Practical Matters in Reaction Stoichiometry
  • The Extent of Reaction
  • The Nature of Aqueous Solutions
  • Precipitation Reactions
  • Acid-Base Reactions
  • Oxidation-Reduction Reactions
  • Balancing Oxidation-Reduction Reactions Equations
  • Oxidizing and Reducing Agents
  • Titrations
  • Properties of Gases
  • The Simple Gas Laws
  • Ideal Gas Equation and Its Application
  • Gases in Chemical Reactions
  • Mixtures of Gases
  • Kinetic-Molecular Theory yg Gases
  • Nonideal (Real) Gases

  • Terminology in Thermochemistry
  • Heat, Heats of Reaction, and Calorimetry
  • Work
  • The Frist Law of Thermodynamics
  • Application of The First Law to Chemical and Physical Changes
  • Hess's Law
  • Standar Enthalpies of Formation
  • Fuels as Sources of Energy
  • The Nature of the Equilibrium State
  • Equilibrium Constant Expression
  • Relationships Involving Equilibrium Constants
  • The Magnitude of an Equilibrium Constants
  • Predicting the Direction of Net Chemical Change
  • Le Chatelier's Principle
  • Equilibrium Calculations

  • Acids, Bases, and Conjugate Acid-Base Pairs
  • Self-Ionization of Water and the pH Scale
  • Ionization of Acids and Bases in Water
  • Strong Acids and Strong Bases
  • Weak Acids and Weak Bases
  • Polyprotic Acids
  • Simultaneous Acid-Base Reactions
  • Ions as Acids and Bases
  • Lewis Acids and Bases
  • Ion Effect in Acid-Base Equilibria
  • Buffer Solutions
  • Acid-Base Indicators
  • Neutralization Reactions and Titration Curves
  • Acid-Base Equilibrium Calculations
  • Solubility Product Constant
  • Relationship Between Solubility and Ksp
  • Ion Effect in Solubility Equilibria
  • Limitations of the Ksp Concept
  • Criteria for Precipitation and Its Completeness
  • Fractional Precipitation
  • Solubility and pH
  • Equilibria Involving Complex Ions
  • Electrode Potentials and Their Measurement
  • Standard Electrode Potentials
  • Electrode Potentials as a Function of Concentrations
  • Batteries and Corrosion
  • Industrial Electrolysis Processes
  • Rate of a Chemical Reaction
  • Measuring Reaction Rates
  • Effect of Concentration on Reaction Rules
  • Zero-Order, First-Order, and Second-Order Reaction
  • Reaction Kinetics
  • Theoretical Models for Chemical Kinetics
  • The Effect of Temperature on Reaction Rates
  • Reaction Mechanism
  • Catalysis

References:

Petrucci, R. H., Herring, F. G., Madura, J. D., & Bissonnette, C. (2017). General Chemistry: Principles and Modern Applications (11th ed.). Pearson.