Metal Reactivity Series

Study Notes

The reactivity series is a list of metals in order of their reactivity, from most reactive to least reactive
The series helps predict the outcome of single displacement reactions
Metals high in the series will displace metals lower in the series from their salts
Examples:
- Potassium (high in the series) will displace sodium (lower in the series) from its salt
- Copper (lower in the series) will not displace zinc (higher in the series) from its salt

Formed from the reaction between a metal and a non-metal
Metal loses electrons to form a cation, non-metal gains electrons to form an anion
Electrostatic attraction between oppositely charged ions holds the compound together
Examples:
- Sodium (metal) + Chlorine (non-metal) → Sodium Chloride (NaCl)
- Calcium (metal) + Oxygen (non-metal) → Calcium Oxide (CaO)

Oxidation: loss of one or more electrons by an atom, molecule, or ion
Reduction: gain of one or more electrons by an atom, molecule, or ion
Oxidation and reduction occur simultaneously in a redox reaction
Examples:
- 2Na (s) + Cl2 (g) → 2NaCl (s) (oxidation of sodium, reduction of chlorine)
- Zn (s) + CuSO4 (aq) → ZnSO4 (aq) + Cu (s) (oxidation of zinc, reduction of copper)

Acid: a species that donates a proton (H+)
Base: a species that accepts a proton (H+)
Neutralization reaction: acid + base → salt + water
Examples:
- HCl (acid) + NaOH (base) → NaCl (salt) + H2O
- Ca(OH)2 (base) + HNO3 (acid) → Ca(NO3)2 (salt) + H2O

Guidelines for predicting whether an ionic compound is soluble or insoluble in water
Rules:
- All sodium, potassium, and ammonium salts are soluble
- All nitrates and acetates are soluble
- Most chlorides, bromides, and iodides are soluble, except for those of silver, lead, and mercury
- Most sulfates are soluble, except for those of calcium, strontium, and barium
- Most hydroxides and oxides are insoluble, except for those of sodium, potassium, and ammonium

Metals can be arranged in a reactivity series, from most reactive to least reactive, to predict the outcome of single displacement reactions
Metals high in the series can displace metals lower in the series from their salts
Higher metals in the series are more reactive than lower metals

Ionic compounds are formed through the reaction between a metal and a non-metal
Metals lose electrons to form cations, while non-metals gain electrons to form anions
The electrostatic attraction between oppositely charged ions holds the compound together

Oxidation involves the loss of one or more electrons by an atom, molecule, or ion
Reduction involves the gain of one or more electrons by an atom, molecule, or ion
Oxidation and reduction occur simultaneously in a redox reaction
Oxidation states can be used to identify the species being oxidized or reduced

Acids donate protons (H+), while bases accept protons (H+)
Neutralization reactions involve the combination of an acid and a base to form a salt and water
Strong acids and bases completely dissociate in water, while weak acids and bases partially dissociate

Sodium, potassium, and ammonium salts are always soluble
Nitrates and acetates are always soluble
Chlorides, bromides, and iodides are generally soluble, except for those of silver, lead, and mercury
Sulfates are generally soluble, except for those of calcium, strontium, and barium
Hydroxides and oxides are generally insoluble, except for those of sodium, potassium, and ammonium