Chemistry

1. Chemical Quantities

1.1. The Mole: Measurement of matter

1.2. Mole mass and Mole volume relationships

1.2.1. mol = representative particles/avagadros number

1.2.2. mol = mass/ molar mass

1.2.3. mol = volume/ molar volume

1.3. Percent composition and chemical forumlas

2. Acids and Bases

2.1. describing acids and bases

2.2. hydrogen ions and acidicity

2.3. acid base theories; Arrhenius Model & Bronsted-Lowry Model

2.4. strenghts of acids and bases

2.5. pH = - log [H+]

2.6. pOH = - log [OH-]

2.7. pH + pOH = 14

2.7.1. [H+][OH-] = 10E-14 at 25C

2.8. Titration

2.9. Buffer Solutions

3. Equilibrium

3.1. chemical equilibruim

3.2. equilibruim position

3.3. Le chatelier Principle; Changes to Concentration, Volume & Temperature

3.4. Reaction Rate

4. Redox Reactions - Oxidation & Reduction Reactions

4.1. meaning of oxidation and reduction (OIL RIG )

4.2. Oxidation numbers

4.3. balancing redox equations

4.4. Identifying Half-Reactions

4.5. Reactions Occurring in Acidic vs Basic Solutions

5. Thermodynamics

5.1. First Law of Thermodynamics - Law of conservation of Energy

5.2. Specific heat

5.3. Internal Energy (E)

5.4. delta E = q + w

5.5. Enthalpy (H) - State Change

5.6. delta H = Change in internal energy @constant pressure

5.7. Entropy (S)

6. Chemical Bonding

6.1. Covalent, Ionic & Polar Bonds

6.2. Electronegativity

6.3. Lewis Structures

6.4. Octect Rule

6.5. Molecular Structures - VSEPR Model

7. Gas Laws

7.1. Boyle's law, Charles Law, Avogardo's Law

7.2. Ideal Gas Law pv = nRT

7.3. Dalton's law of partial pressure

8. Solutions

8.1. Solubility of Ionic & Polar Substances

8.2. Molarity

8.3. Moles = Molarity x Volume

8.4. Normality

8.5. Boiling & Freezing Points