Chemistry

1. Groups of elements

1.1. Halogen

1.1.1. Diatomic molecule

1.2. Transition Metal

1.2.1. Heavy

1.2.2. Strong

1.2.3. Less Reactive

1.2.4. Used as a Catalyst

1.3. Alkaline Metal

1.3.1. More Reactive

1.3.2. Light

1.3.3. Soft

1.4. Noble Gas

1.4.1. No color

2. Atoms, Elements, compounds, and mixtures

2.1. Formulas given the name

2.2. Name given the formula

2.3. Ionic and covalent bonding

2.4. Atoms = single molecule

2.5. Compound = an molecule that has 2 same atoms

2.6. Elements = specific type of atom

2.7. Mixture = an molecule that has 2 different atom

3. Atomic Structure

3.1. Proton = Atomic number

3.2. Electron = Atomic number (changed based on the + or - in the molecule)

3.3. Neutron = Atomic mass - Proton

3.4. Electronic Structure: Structure of the molecule

3.5. Valence

4. Separating Techniques

4.1. Chromatography

4.1.1. Colors

4.2. Distillation

4.2.1. Liquids w/ diff. boiling point

4.3. Filtration

4.3.1. Insoluble solid particles and liquid

4.4. Decantation

4.4.1. Large insoluble solid particles and liquid

4.5. Evaporation

4.5.1. Soluble solid particles and liquid

4.6. Crystallization

4.6.1. Soluble solid particles and liquid

4.7. Separatory funnel

4.7.1. Immisible liquild

5. Particulate nature of matter

5.1. Solid -> Liquid = Melting

5.2. Liquid -> Gas = Evaporation

5.3. Gas -> Liquid = Condesation

5.4. Liquid -> Solid = Solidification

5.5. Solid -> Gas / Gas -> Solid = Sublimation

6. Acids and bases

6.1. Acid = Below pH 7

6.2. Alkali = Above pH 7

6.3. Neutral Solution = pH 7

6.4. Acid turns red litmus paper into blue

6.5. Alkaline turns blue litmus paper into red

7. Stoichiometry

7.1. Balance

7.2. Empirical and molecular formula

7.3. moles -> moles

7.4. Grams -> moles

7.5. Moles -> grams

7.6. Grams -> grams

7.7. Limiting and excess reagents