Shorthand notation for galvanic/voltaic cells

1.1   VSEPR for 5 electron clouds (part 1)

1.2   Electronegativity and bonding

1.3   VSEPR for 3 electron clouds

1.4   VSEPR for 2 electron clouds

1.5   Steric number

1.6   sp hybridization

1.7   Ionic, covalent, and metallic bonds

1.8   More on the dot structure for sulfur dioxide

1.9   Worked examples: Finding the hybridization of atoms in organic molecules

1.10   sp³ hybridization

1.11   sp² hybridization

1.12   Electronegativity

1.13   Covalent networks, metallic crystals, and ionic crystals

1.14   VSEPR for 6 electron clouds

1.15   Resonance and dot structures

1.16   Formal charge and dot structures

1.17   VSEPR for 4 electron clouds

1.18   Drawing dot structures

1.19   Metallic nature

1.20   Electronegativity and bonding

1.21   VSEPR for 5 electron clouds (part 2)

2.1   The mole and Avogadro_s number

2.2   Common polyatomic ions

2.3   Atomic number, mass number, and isotopes

2.4   Elements and atoms

2.5   Atomic weight and atomic mass

2.6   Molecular mass and molecular weight

2.7   Empirical, molecular, and structural formulas

2.8   Atomic weight

2.9   Introduction to chemistry

2.10   Calculating atomic weight

2.11   Worked example: Identifying isotopes and ions

2.12   Introduction to ions

2.13   Naming ions and ionic compounds

2.14   Naming ionic compound with polyvalent ion

2.15   Worked example: Finding the formula of an ionic compound

3.1   Suspensions, colloids and solutions

3.2   Van der Waals forces

3.3   Phase diagrams

3.4   Specific heat and latent leat of fusion and vaporization

3.5   States of matter follow-up

3.6   Surface tension

3.7   Capillary action and why we see a meniscus

3.8   Vapor pressure

3.9   Chilling water problem

3.10   States of matter

3.11   Change of state example

3.12   Boiling point elevation and freezing point depression

3.13   Solubility and intermolecular forces

3.14   Specific heat, heat of fusion and vaporization example

4.1   Introduction to electrolysis

4.2   Worked example: Balancing a redox equation in acidic solution

4.3   Free energy and cell potential

4.4   Using reduction potentials

4.5   Introduction to galvanic/voltaic cells

4.6   Oxidation state trends in periodic table

4.7   Standard cell potential and the equilibrium constant

4.8   Oxidation and reduction

4.9   Redox titrations

4.10   Practice determining oxidation states

4.11   Introduction to redox reactions

4.12   Lead storage battery

4.13   Disproportionation

4.14   Electrolysis of molten sodium chloride

4.15   Quantitative electrolysis

4.16   Nernst equation

4.17   Unusual oxygen oxidation states

4.18   Oxidizing and reducing agents

4.19   Galvanic cells and changes in free energy

4.20   Worked example: Balancing a redox equation in basic solution

4.21   Using the Nernst equation

4.22   Calculating the equilibrium constant from the standard cell potential

4.23   Electrodes and voltage of Galvanic cell

4.24   Concentration cell

4.25   Redox reaction with iron

4.26   Standard reduction potentials

4.27   Spontaneity and redox reactions

4.28   Nickel-cadmium battery

4.29   Redox reaction from dissolving zinc in copper sulfate

4.31   Voltage as an intensive property

5.1   Types of decay

5.2   Half-life and carbon dating

5.3   Mass defect and binding energy

5.4   Exponential decay formula proof (can skip, involves calculus)

5.5   Introduction to exponential decay

5.6   More exponential decay examples

5.7   Half-life plot

5.8   Nuclear stability and nuclear equations

5.9   Writing nuclear equations for alpha, beta, and gamma decay

5.10   Exponential decay and semi-log plots