Reactivity of metals

4.1.1 Metal oxides

Metal oxides

Metal_(s) + oxygen_(g) → metal oxides_(s)

OIL RIG

Oxidation is loss of electrons, gain of O₂

Reduction is gain of electrons, loss of O₂ (using carbon)

4.1.2 The reactivity series

Reactivity series – need to memorize

Please send lions, cats, monkeys and cute zebras into the lovely, hot countries, signed general penguin

			Reaction with water	Native metals so unreactive
Most reactive	Potassium	Ka	Fizz Giving off H2(g) Leaving an alkaline solution of metal hydroxide	Explode
	Sodium	Na
	Lithium	Li
	Calcium	Ca		Fizz Giving off H2(g) Forming a salt
	Magnesium	Mg	Very slow reaction
	Aluminium	AI
	Carbon	C
	Zinc	Zn	Very slow reaction	Fizz Giving off H2(g) Forming a salt
	Iron	Fe
	Tin	Sn	Slight reaction with steam	React slowly with warm acid
	Lead	Pb
	Hydrogen	H
	Copper	Cu	Native metals so unreactive
	Silver	Ag
	Gold	Au
Least reactive	Tin	Pt

Extraction of metals and reduction

Ore – a rock that contains enough metal to make it economical to extract

			Extraction of metals
Most reactive	Potassium	Ka	Extract by electrolysis
	Sodium	Na
	Lithium	Li
	Calcium	Ca
	Magnesium	Mg
	Aluminium	AI
	Carbon	C
	Zinc	Zn	Metal ore Extract by metal oxide by reduction using carbon Why carbon? C is more reactive
	Iron	Fe
	Tin	Sn
	Lead	Pb
	Hydrogen	H	Occur native in the ground
	Copper	Cu
	Silver	Ag
	Gold	Au
Most reactive	Tin	Pt

4.1.4 Oxidation and reduction in terms of electrons (HT only)

Displacement reaction

• More reactive displace less reactive elements
• More reactive(s) + compound(aq) → less reactive(s) + compound(aq)

Eg Magnesium + copper chloride → copper + magnesium chloride

Mg + CuCl₂ → Cu + MgCl₂

• Magnesium loses 2e^– & become Mg2⁺ → oxidation

Mg → Mg²⁺ + 2e^–

• Copper gains 2e^– & become Cu → reduction

Cu²⁺ + 2e^– → Cu

Ionic equation

Solid and liquid don’t separate