Chemical Reactions and Stoichiometry
Chemical reactions create new substances by breaking and forming bonds, unlike physical changes that just break IMFs. When writing ionic equations, remember to separate aqueous compounds into ions while keeping solids, liquids, and gases intact.
There are three ways to write chemical equations:
- Molecular equations show the complete formulas
- Complete ionic equations separate aqueous compounds into ions
- Net ionic equations eliminate spectator ions that don't participate in the reaction
Stoichiometry is your tool for calculating quantities in chemical reactions. The limiting reactant determines the theoretical yield because it's completely consumed first. Calculate percent yield by dividing actual yield by theoretical yield and multiplying by 100.
🧪 In acid-base reactions, acids donate H⁺ ions while bases accept them. When an acid reacts, it forms its conjugate base; when a base reacts, it forms its conjugate acid.
Redox reactions involve the transfer of electrons, with oxidation (losing electrons) and reduction (gaining electrons) occurring simultaneously. To identify what's being oxidized or reduced, track oxidation numbers using these rules:
- Free elements = 0
- Group 1 elements = +1 in compounds
- Group 2 elements = +2 in compounds
- Fluorine = -1 in compounds
- Hydrogen = +1 with non-metals, -1 with metals
- Oxygen usually = -2
Remember those diatomic molecules (Br₂, I₂, N₂, Cl₂, H₂, O₂, F₂) and polyatomic ions like sulfate (SO₄²⁻), nitrate (NO₃⁻), and ammonium (NH₄⁺) for writing correct formulas in reactions.