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Chemistry by Mind Map: Chemistry

1. Grade 9

1.1. Bohr-Rutherford Atomic Model

1.1.1. Nucleus Containing proton and neutron Electrons orbiting in energy levels

1.2. Elements

1.2.1. Compounds Ionic Covalent (Molecules)

1.3. Physical vs. Chemical Properties

1.4. Periodic Table

1.4.1. Element Symbols and Names

1.4.2. Simple Compound Formulas and Names

2. Grade 10

2.1. Chemical Reactions

2.1.1. Compounds

2.1.2. Products

2.1.3. Reactants

2.1.4. Types Synthesis Decomposition Single Displacement Double Displacement

2.1.5. Word Equations

2.1.6. Balanced Chemical Equations Law of Conservation of Mass

2.2. Simple Molecular Models

2.3. Chemical Changes

2.3.1. Evidence of

2.4. Physical Changes

2.5. Acids & Bases

2.5.1. Neutralization

2.5.2. pH Scale

3. Grade 11

3.1. Matter, Chemical Trends, and Chemical Bonding

3.1.1. Periodic Trends

3.1.2. Isotopes vs. Radioisotopes

3.1.3. Formation of Ionic vs. Covalent Bonds Lewis Structures Molecular Models with single & multiple bonds

3.1.4. Physical Properties of Ionic vs. Molecular Compounds

3.1.5. Activity Series of Elements

3.1.6. Polyatomic Compounds

3.1.7. Multivalent Compounds

3.2. Chemical Reactions

3.2.1. Types Synthesis Decomp Single Displacement Double Displacement Combustion Incomplete Complete Neutralization

3.2.2. Balanced Chemical Equations for all Types

3.3. Quantities in Chemical Reactions

3.3.1. Moles Avogadro's Number Molar Mass

3.3.2. Stoichiometry Percentage Yield Limiting Reagent Percentage Composition Empirical vs. Molecular Formula

3.4. Solutions & Solubility

3.4.1. Concentration Stoichiometry Dilution

3.4.2. Precipitates

3.4.3. Ionization Dissociation Net Ionic Equations

3.4.4. Solution Solute Solvent Dilute/Concentrated

3.4.5. Properties of Water Polarity Hydrogen Bonding Universal Solvent

3.4.6. Polar vs. Non-Polar

3.4.7. Solubility Factors Temperature Pressure

3.4.8. Arrhenius Theory of Acids and Bases

3.4.9. Strong vs. Weak Acids/Bases

3.5. Gases & Atmospheric Chemistry

3.5.1. Earth's Atmosphere

3.5.2. States of Matter in terms of Forces Kinetic Molecular Theory

3.5.3. Ideal Gases PV = nRT Dalton's Law Boyle's Law Charles' Law Gay-Lussac's Law Combined Gas Law

3.5.4. Avogadro's Hypothesis

3.5.5. Stoichiometry

4. Grade 12

4.1. Organic Chemistry

4.1.1. Classes of Org. Compounds Hydrocarbons Alcohols Aldehydes Ketones Carboxylic Acids Esters Ethers Amines Amides

4.1.2. Organic Chemical Reactions Substitution Addition Elimination Oxidation Esterification Hydrolysis

4.1.3. Polymers Addition Reaction Condensation Reaction

4.1.4. Isomerism

4.1.5. IUPAC Nomenclature

4.2. Structure and Properties of Matter

4.2.1. Electron Configurations s, p, d, f orbitals Pauli Exclusion Principle Hund's Rule Aufbau Principle

4.2.2. Forces Intramolecular Ionic Bonding Covalent Bonding Intermolecular Van der Waals Forces Hydrogen Bonding Metallic Bonding Physical Properties dependent on type of forces present

4.2.3. Atomic and Molecular Theory VSEPR emission spectrum photons

4.3. Energy Changes and Rates of Reaction

4.3.1. Enthalpy Endothermic Exothermic Specific Heat Capacity Q=mcdeltaT

4.3.2. Energy Changes Physical Change Chemical Reaction Nuclear Reaction Bonds Formed/Broken Hess's Law

4.3.3. Rate of Chem Rxn Factors Affecting Rate Catalysts

4.3.4. Potential Energy Diagrams Activation Energy

4.3.5. Reaction Mechanisms Elementary Steps Rate Determining Step

4.4. Chemical Systems and Equilibrium

4.4.1. Le Chatelier's Principle

4.4.2. Equilibrium Constants

4.4.3. Bronsted-Lowry Theory of Acids and Bases Properties of Acids/Bases based on Dynamic Equilibrium Acid-Base Titration

4.4.4. Buffers

4.5. Electrochemistry

4.5.1. Redox Reactions Oxidation Number Balanced Chemical Equations for Redox Reactions Reducing Agent Oxidizing Agent Half-Reaction

4.5.2. Galvanic Cells Voltage Overall Cell Potential Half Cells

4.5.3. Industrial Processes

4.5.4. Corrosion of Metals