Unit 11: Reactivity of Metals

Vocabulary flashcards on the reactivity of metals, their reactions with oxygen, water, and acids, displacement reactions, extraction, compound stability and the thermit reaction.

Reactivity Series

K, Na, Ca, Mg,Al, Zn, Fe,Sn, Pb, Cu, H, Hg,Ag,Cu

Sodium Reaction with Oxygen

Ignites easily by gentle heating: 4Na(s) + O2(g) → 2Na₂O(s)

Calcium Reaction with Oxygen

Requires strong heating to start burning: 2Ca(s) + O2(g) → 2CaO(s)

Magnesium Reaction with Oxygen

Requires strong heating to start burning: 2Mg(s) + O2(g) → 2MgO(s)

Aluminum Reaction with Oxygen

Requires strong heating to start burning: 4Al(s) + 3O2(g) → 2Al2O3(s)

Zinc Reaction with Oxygen

Reacts to form oxides: 2Zn(s) + O2(g) → 2ZnO(s)

Iron Reaction with Oxygen

Reacts to form oxides: 3Fe(s) + 2O2(g) → Fe3O4(s)

Lead Reaction with Oxygen

Reacts to form oxides: 2Pb(s) + O2(g) → 2PbO(s)

Copper Reaction with Oxygen

Reacts to form oxides: 2Cu(s) + O2(g) → 2CuO(s)

Silver reaction with oxygen

No reaction

Sodium Reaction with Water

Reacts with cold water explosively: 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

Calcium Reaction with Water

Reacts with cold water: Ca(s) + 2H2O(1) → Ca(OH)2(s) + H2(g)

Magnesium Reaction with Steam

Reacts with steam: Mg(s) + H2O(g) → MgO(s) + H2(g)

Aluminum Reaction with Steam

Reacts with steam: 2Al(s) + 3H₂O(g) → Al2O3(s) + 3H2(g)

Zinc Reaction with Steam

Reacts with steam: Zn(s) + H2O(g) → ZnO(s) + H2(g)

Iron Reaction with Steam

Reacts with steam: 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g)

lead, copper and silver reaction with water

No reaction

Sodium reaction with dilute acids

Explosive

Calcium Reaction with Acids

Reacts with dilute hydrochloric acid: Ca(s) + 2HCl(aq) → CaCl2(aq) + H2(g). Reacts with dilute sulphuric acid: Ca(s) + H2SO4(aq) → CaSO4(s) + H2(g)

Magnesium Reaction with Acids

Reacts with dilute hydrochloric acid: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g). Reacts with dilute sulphuric acid: Mg(s) + H2SO4(aq) → MgSO4(aq) + H2(g)

Aluminum Reaction with Acids

Reacts with dilute hydrochloric acid: 2Al(s) + 6HCl(aq) → 2AICI3(aq) + 3H2(g). Reacts with dilute sulphuric acid: 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)

Zinc Reaction with Acids

Reacts with dilute hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g). Reacts with dilute sulphuric acid: Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)

Iron Reaction with Acids

Reacts with dilute hydrochloric acid: Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g). Reacts with dilute sulphuric acid: Fe(s) + H2SO4(aq) → FeSO4(aq) + H2(g)

Copper and silver reaction with dilute acids

No reaction

Reactivity and Electron Loss

A metal that readily reacts with water and dilute hydrochloric acid has the highest tendency to lose outermost shell electron(s) to form a positive ion.

Displacement Reaction

A more reactive metal displaces a less reactive metal from a compound of the less reactive metal in a solution. Example: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

Metal Extraction

The more reactive a metal is, the more difficult it is to extract it from its ore.

Compound Stability

The higher a metal is in the reactivity series, the more stable its compounds are likely to be.

Decomposition of Metal Oxides

The lower a metal is in the reactivity series, the more readily its oxide decomposes when heated.

Thermit Reaction

A reaction where a powdered mixture of zinc and copper(II) oxide is heated, and the mixture keeps burning even after the Bunsen burner is removed: Zn(s) + CuO(s) → ZnO(s) + Cu(s)