Unit 2978 Comprehensive Outline

1. Matter and its Properties

1.1 Definition of Matter

• What is matter?
• Importance of matter in chemistry

1.2 States of Matter

• Solid: characteristics and particle arrangement
• Liquid: characteristics and particle arrangement
• Gas: characteristics and particle arrangement

1.3 Physical and Chemical Properties

• Physical properties: color, density, melting point, boiling point, etc.
• Chemical properties: reactivity, flammability, acidity, etc.

1.4 Classification of Matter

• Pure substances vs. mixtures
• Elements, compounds, homogeneous and heterogeneous mixtures

2. Atomic Structure

2.1 Structure of the Atom

• Subatomic particles: protons, neutrons, electrons
• Atomic nucleus and electron cloud

2.2 Atomic Number and Mass Number

• Definitions and significance
• Isotopes and their properties

2.3 Organization of the Periodic Table

• Periods and groups
• Metals, nonmetals, metalloids

2.4 Electron Configurations

• Energy levels and orbitals
• Aufbau principle, Pauli Exclusion Principle, Hund’s rule
• Writing electron configurations

3. Chemical Bonding

3.1 Types of Chemical Bonds

• Ionic bonds: formation and properties
• Covalent bonds: single, double, triple bonds; polar and nonpolar
• Metallic bonds: electron sea model

3.2 Formation of Molecules and Compounds

• Octet rule
• Lewis structures
• Bond polarity and molecular geometry

4. Chemical Reactions

4.1 Types of Chemical Reactions

• Synthesis (Combination)
• Decomposition
• Single displacement (Replacement)
• Double displacement (Metathesis)
• Combustion

4.2 Balancing Chemical Equations

• Law of conservation of mass
• Step-by-step balancing techniques

4.3 Predicting Products

• General patterns
• Reactions of acids, bases, and salts

5. Acids and Bases

5.1 Properties of Acids and Bases

• Taste, pH scale, indicators

5.2 pH Scale and Indicators

• pH range and meaning
• Common indicators and their color changes

5.3 Neutralization Reactions

• Acid-base reactions producing salt and water

5.4 Acid-Base Theories

• Arrhenius theory
• Bronsted-Lowry theory
• Lewis theory

6. Stoichiometry

6.1 Mole Concept

• Avogadro’s number
• Molar mass

6.2 Mole Ratios in Chemical Equations

• Using balanced equations for calculations

6.3 Limiting Reactants

• Identifying limiting and excess reactants

6.4 Percent Yield

• Theoretical yield vs. actual yield
• Calculating percent yield

7. Gas Laws

7.1 Behavior of Gases

• Properties and assumptions of ideal gases

7.2 Boyle’s Law

• Relationship between pressure and volume

7.3 Charles’s Law

• Relationship between volume and temperature

7.4 Gay-Lussac’s Law

• Relationship between pressure and temperature

7.5 Ideal Gas Law

• PV = nRT
• Applications and problem-solving

8. Thermochemistry

8.1 Heat and Enthalpy

• Definition of enthalpy (ΔH)
• Exothermic and endothermic reactions

8.2 Calorimetry

• Measuring heat changes
• Specific heat capacity

8.3 Hess’s Law

• Using Hess’s law for enthalpy calculations

8.4 Calculating Heat Energy Changes

• q = mCΔT and other formulas

9. Organic Chemistry

9.1 Introduction to Carbon Compounds

• Importance of carbon in chemistry

9.2 Hydrocarbons

• Alkanes, alkenes, alkynes
• Saturated and unsaturated hydrocarbons

9.3 Functional Groups

• Alcohols, carboxylic acids, amines, etc.

9.4 Isomerism

• Structural isomers
• Geometric (cis-trans) isomers

9.5 Basic Organic Reactions

• Addition, substitution, elimination reactions

10. Nuclear Chemistry

10.1 Structure of Atomic Nuclei

• Protons and neutrons
• Nuclear notation

10.2 Types of Nuclear Reactions

• Radioactive decay: alpha, beta, gamma
• Nuclear fission and fusion

10.3 Radioactivity

• Properties and effects
• Half-life

10.4 Nuclear Stability

• Band of stability
• Factors affecting stability

10.5 Applications of Nuclear Chemistry

• Medical uses (radiotherapy, imaging)
• Industrial uses (power generation, sterilization)