S3.1.5- Metal and non-metal oxides

ionic period 3 oxides

Na₂O, MgO, Al₂O₃

giant covalent period 3 oxides

SiO₂

period 3 molecular covalent oxides

P₄O₁₀, P₄O₆, SO₃, SO₂, Cl₂O₇, Cl₂O

properties period 3 molecular covalent oxides

• no conductivity

• acidic

properties period 3 giant covalent oxides

• low conductivity

• acidic

properties giant ionic period 3 oxides

• high conductivity

• basic

• except Al₂O₃, which is amphoteric

reactions basic oxides with water

Na₂O + H₂O → 2NaOH

MgO + H₂O → Mg(OH)₂

reactions amphoteric oxides with water

Acid base reaction with sulfuric acid, producing salt and water

Al₂O₃+ 6H → 2 Al³⁺+ 3H₂O

Al₂O₃+ 3H₂SO₄→ Al₂(SO₄)₃+ 3H₂O

behaves as an acid when reacted with alkalis

Al₂O₃ + 3H₂O + 2OH^- —> 2Al(OH)_4^-

reactions acidic oxides with water

Non- metal oxides react with water to produce acidic solutions

H₂O + CO₂ → H₂CO₃ (carbonic acid)

SO₃+ H₂O → H₂SO₄ (sulfuric v acid)

SO₂+ H₂O → H₂SO₃ (sulfuric iv acid)

sulfuric oxdes producing acid rain

• SO₂ is produced from burning fossil fuels

• sulfur dioxide or sulfur trioxide dissolves in rain water to form sulfourus acid

nitrogen oxides proudces acid rain

nitrogen dissolving in rain water:

• H₂O+2NO₂→ HNO₂+ HNO₃

• 2H₂O + 4NO₂+ O₂→ 4HNO₃