1. Unit#2 - Chemical Reactions
1.1. Activity Series
1.1.1. Non-Metal Activity Series
1.1.2. Metal Activity Series
1.2. Types of chemical reactions
1.2.1. Decomposition Reaction
1.2.1.1. AB ---> A + B
1.2.2. Double Replacement Reaction
1.2.2.1. AB+CD => AD+BC
1.2.3. Single Displacement Reaction
1.2.3.1. Type A
1.2.3.1.1. A(metal) + B(metal)C ---> B + AC
1.2.3.2. Type B
1.2.3.2.1. A(non-metal) + Bnon-(metal)C ---> C + BA
1.2.4. Combustion Reactions
1.2.4.1. Complete Combustion Reactions
1.2.4.1.1. contains extra oxygen gas
1.2.4.2. Incomplete Combustion Reactions
1.2.4.2.1. contains limited oxygen gas
1.2.5. Neutralization Reaction
1.2.5.1. Acid+Base=> Water+Salt
1.2.6. Synthesis Reaction
1.2.6.1. A+B=> AB
1.2.7. Oxidation Reactions
1.2.7.1. Non-Metal Oxide
1.2.7.2. Metal Oxide
1.3. Balanced Equations
1.4. Skeleton Equations
1.5. Word Equations
1.6. Chemical Equations
2. Unit#4 - Solutions & Solubility
2.1. Concetration Calculations
2.1.1. Molar Concetration
2.1.1.1. nsolute/Vsolution
2.1.2. CIVI=CFVF
2.1.3. % Concetration (m/V)
2.1.3.1. % C (m/V) = msolute/Vsolution
2.1.4. % Concentration (m/m)
2.1.4.1. % C (m/m) = msolute/msolution
2.1.5. % Concentration (V/V)
2.1.5.1. % C (V/V) =Vsolute/Vsolution
2.1.6. Parts Per Million
2.1.6.1. ppm=solute/solution x 10^6
2.1.7. Parts Per Billion
2.1.7.1. ppb=solute/solution x 10^9
2.1.8. Parts Per Trillion
2.1.8.1. ppt=solute/solution x 10^12
2.2. Aqueous Solution
2.3. Concentrated Solution
2.4. Dilute Solution
2.5. Like dissolves like
2.5.1. Polar
2.5.2. Non Polar
2.6. Stoichiometry of solutions
2.6.1. moles:moles
2.6.2. Limiting Reactant
2.6.3. Excess Reactant
2.7. Acids & Bases
2.7.1. Acids Have H+
2.7.2. Bases Have OH-
2.8. dissociation
2.8.1. ionic
2.9. Titration
2.9.1. Neutralization of an acid or base
2.10. Solubility
2.10.1. Saturated
2.10.2. Supersaturated
2.10.3. Unsaturated
2.10.4. Solubility Curve
2.11. Solution
2.12. Disolve
2.13. Solvent
2.14. Solute
3. Unit#1 - Matter, Chemical Trends & Chemical Bonding
3.1. Isotopes
3.1.1. Isotopic Abundance
3.2. Periodic Table Trends
3.2.1. Electronegatvity
3.2.1.1. Ionic
3.2.1.1.1. EN is bigger than 1.7
3.2.1.2. Covalent
3.2.1.2.1. EN is smaller than 1.7
3.2.2. Atomic Radius
3.2.2.1. decreases across a period
3.2.2.2. increases down a group
3.2.3. Electron Affinity
3.2.4. Shielding Levels
3.2.5. Ionization Energy
3.2.5.1. increases across a period
3.2.5.2. decreases down a group
3.2.6. Nuclear Charge
3.2.7. Valence Electrons
3.3. Group Types
3.3.1. Alkali Metal
3.3.1.1. Group 1
3.3.2. Alkaline Earth Metal
3.3.2.1. Group 2
3.3.3. Halogens
3.3.3.1. Group 17
3.3.4. Noble Gases
3.3.4.1. Group 18
3.4. Bohr-Rutherford Diagrams
3.5. Lewis Diagrams
3.5.1. Lewis Dot Diagrams
3.5.2. Lewis Line Diagrams
3.6. Bond Polarity
3.6.1. Non-Polar Bond
3.6.1.1. EN < 0.4
3.6.2. Polar Bond
3.6.2.1. EN >= 1.7
3.6.3. Covalent Bond
3.6.3.1. EN>=0.4
3.7. Nomenclature
3.7.1. Ionic Compounds
3.7.2. Covalent Compunds
3.7.3. The Strong Acids
3.7.4. The Diatomic Gases
3.8. Chemical Bonds
3.8.1. Metallic Bonds
3.8.2. Covalent Bonds
3.8.3. Ionic Bonds
4. Unit#3 - Quantities in Chemical Reactions
4.1. Stoichiometry
4.1.1. mole:mole ratio
4.1.2. chemical equations
4.1.3. Limiting Reactants
4.1.4. Excess Reactants
4.2. % yield of product
4.2.1. actual yield/theoretical yield x 100%
4.2.2. theoretical yield
4.2.3. experimental yield
4.2.4. percentage yield
4.3. Empirical Formula
4.4. Molecular Formula
4.5. Moles
4.5.1. Avogadro's Number
4.5.1.1. 6.02 x 10^23
4.6. Molar Mass
4.6.1. M=m/n
4.7. Calculations
4.7.1. n=m/M
4.7.2. M=m/n
4.7.3. m=nxM
4.8. Accuracy
4.9. Precision
4.10. Law Of Definite Proportions
4.10.1. % element = (mass of element / total mass) x 100%
4.10.2. % element = (atomic mass of element / molar mass of substance) x 100%