The oxides of Period 3, Na - Cl
 

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1. Basic oxides and hydroxides: Na2O, NaOH, MgO and Mg(OH)2

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Sodium oxide:                         Na2O (s)  +  H2O (l)  "   2NaOH (aq)

Na+ (aq) +  OH - (aq) +  H+ (aq)   "   Na+ (aq) + H2O (l)

Magnesium oxide:            MgO (s)  +  2H+ (aq)   "   Mg2+ (aq)  +  H2O (l)

Mg(OH)2 (s)  +  2H+ (aq)  "   Mg2+ (aq)  +  2H2O (l)


Inorganic catalogue contents

Basic oxides
Amphoteric oxide
Acidic oxides


2. Amphoteric oxide and hydroxide: Al2O3, Al(OH)3.

 

Basic properties: Aluminium oxide is very resistant to attack by acids and so the first reaction is slow. Aluminium hydroxide reacts easily with dilute acids.

Al2O3 (s)  +  6H+ (aq)   "   2Al3+ (aq)+3H2O(l)  

Al(OH)3 (s)  +  3H+ (aq)  "   Al3+ (aq)  +  3H2O (l)

Acidic properties: Alkaline attack on aluminium oxide is slow unless the alkali is hot and concentrated or molten. The formula of the aluminate ion shown is accepted in exams; you may also see [Al(OH)4]- or AlO2-, though the latter only really comes from reaction with molten alkali.

Al2O3(s) + 6OH(aq) + 3H2O(l)  "   2 [Al(OH)6]3 –(aq)

Aluminium hydroxide reacts readily with sodium hydroxide solution:

Al(OH)3 (s)  +  3OH(aq)   "   [Al(OH)6]3 – (aq)


 

3. Acidic oxides (acid anhydrides) SiO2, P4O10, SO2, SO3, Cl2O.

 

Silicon dioxide, silica. Silica’s giant covalent lattice means it is very resistant to attack; the alkali solution must be concentrated and needs heating.

SiO2 (s) +  2 OH(aq)  "   SiO3 2 – (aq)  +  H2O(l)

Phosphorus(V) oxide. The reaction is violent with cold water.

P4O10 (s) + 2H2O (l)   "  4HPO3(aq)

On heating the solution further reaction occurs forming phosphoric(V) acid:

HPO3(aq)  +  H2O(l)   "  H3PO4(aq)

Sulphur dioxide:

SO2(g)  +  H2O (l)   "  H2SO3 (aq)

Sulphur trioxide: This reaction is violent, and is not used directly to make sulphuric acid.

SO3(g)  +  H2O (l)  "   H2SO4 (aq)

Dichlorine oxide:                         Cl2O (aq)  +  H2O(l)   "  2 HClO (aq)


 

© JRG Beavon 2007