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General chemistry is an introductory level chemistry course usually taken by students during their first year of college or university. It covers the basic principles of chemistry, including atomic structure, chemical bonding, chemical reactions, and the properties of matter. General chemistry is a prerequisite for many other chemistry courses, such as organic chemistry, inorganic chemistry, and physical chemistry. It is also a valuable foundation for students who plan to pursue careers in science, engineering, medicine, or other fields that require a fundamental understanding of chemistry.
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Chapter 1
1.1 What is Chemistry and Why it is Important?
1.2 Measurements
1.4 Matter
Chapter 2
2.1 Atomic Theory
2.2 Periodic Table
2.3 Isotopes
2.4 Molecular and Ionic Compounds
• Chemical bonds • Molecular formula • Empirical formula
2.5 Nomenclature of Ionic and Molecular Compounds
Chapter 3
3.1 Understanding and Balancing Chemical Equations
3.2 Mass Relationships in Chemistry
• Atomic mass • Average atomic mass • Avogadro's number • Moles • Molar mass • Molecular mass
3.3 Percent of Composition by Mass
• % of composition by mass of each element in a compound • Determination of the empirical and molecular formula from % of composition • Predicting the molar mass from experimental data
3.4 Stoichiometry
Chapter 4
4.1 Concepts for understanding Reactions in Aqueous Solutions
• Solution, solvent, solute • Electrolytes • Hydration • Solubility rules for ionic compounds
4.2 Precipitation Reactions
• Predicting the products • Molecular equation • Ionic equation • Net ionic equation
4.3 Concentration and Preparation of Solutions
• Molarity • Preparation of solutions from solids and dilutions
4.4 Acid-Base Reactions
• Acids and bases • Neutralization reaction • Stoichiometry involving concentration • pH of solutions • Titration
Chapter 5
• What is a gas? • Why is it important to study gases? • Characteristics of gases • Gases on the periodic table • Molecular gases • Comparison of gases, liquids, and solids
5.2 Gas Laws
• Combined gas law • Pressure • Atmospheric pressure • Standard temperature and pressure (STP) • Ideal gas law • Density of gases • Molar mass of gases
Chapter 6
• Quantifying heat added to matter • Quantifying the energy transfer • System and surrounding
• Endothermic and exothermic processes • Methods to estimate the enthalpy change of reactions • Enthalpy of phase changes • Stoichiometry involving enthalpy change • Hess's Law • What is a state function?
Chapter 7
7.2 Electron Configuration
• Different representation of electronic configuration • Filling the electron configuration • Order of atomic sub-shells • Relationship between quantum numbers and electron configuration • Calculating the maximum number of electrons in a shell • Pauli exclusion principle • Hund’s rule
Chapter 8
• Atoms size • Ions size • 1st and 2nd ionization energies • Electronegativity
Chapter 9
• What is a bond? - Ionic bond • Covalent bond • Non-polar covalent bond • Polar covalent bond • Bond length and strength • Dipole moment • Formal charge
9.2 Lewis Structure Theory
• Lewis dot structure • Octet rule • Exceptions to the octet rule • Resonance
9.3 Valence Bond Theory
Chapter 10
• Valence-shell electron-pair repulsion theory • Molecular polarity
Chapter 11
• Importance of intermolecular forces • Intra-molecularforces vs. intermolecular forces • Types of intermolecular forces • Coulomb's Law
11.2 Intermolecular Forces in Action
• Physical properties that depend on intermolecular forces • Surface tension • Viscosity • Capillary action • Volatility • Freezing point • Vapor pressure
11.3 Heating Curves, Phase Diagrams, and Vapor Pressure
• Phase changes • Calculating heat from heating curves • Understanding phase diagrams • Dynamic equilibrium • Calculating vapor pressure
Chapter 12
• Components of a solution • Solubility • Saturated solution • Unsaturated solution • Super saturated solution • Effect of intermolecular forces in a solution • Enthalpy change of solution formation • Heat of hydration • Factors affecting the solubility of gases in water • Quantifying the solubility of gases (Henry's Law)
12.2 Methods for expressing concentration
• Molarity • Molality • Percent by mass • Part per million • Part per billion • Mole fraction • Mole percent
12.3 Colligative Properties
• Properties of pure solvents vs solutions • Vapor pressure of solutions • Effect of a solute on the properties of solutions • Colligative properties and calculations
