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) |
Basic
oxides |
2.
Amphoteric oxide and hydroxide: Al2O3, Al(OH)3. |
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Basic properties: Al2O3 (s) + 6H+ (aq) " 2Al3+ (aq)+3H2O(l) Al(OH)3 (s) + 3H+ (aq) " Al3+ (aq) + 3H2O (l) Acidic properties: 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) |
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3.
Acidic oxides (acid anhydrides) SiO2, P4O10,
SO2, SO3, Cl2O. |
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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) |
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© JRG Beavon 2007