How metals and non metals react?

1

Reaction with
Oxygen

Metal + Oxygen→Metal oxide
4Na(s) + O₂(g) →2Na₂O(s)
4Al(s) + 3O₂(g) →2Al₂O₃
Metals form basic oxides
Zn and Al form amphoteric oxides (they show the properties of both acidic and basic oxides)
Most of the metal oxides are insoluble in water Some of them dissolve to form Alkali
Na₂O(s) + H₂O(l) →2NaOH(aq)

Non-metal + Oxygen →Non-metal oxide
C + O₂ →CO₂
S + O₂ →SO₂
Non-metals form acidic
oxides
CO and HO₂O are neutral oxides(they are neither acidic nor basic in nature)  Non- metal oxides are soluble in water
They dissolve in water to form acids
SO₂ + H₂O →H₂SO₃

2

Reaction
with water

Metals react with water to
form metal oxides or metal hydroxide and H2 gas is released.
2Na(s) + 2H₂O(l) →2NaOH +
H₂(g) + heat

Non-metals do not react
with water, steam to evolve hydrogen gas. Because  Non-metals cannot give electrons to hydrogen in water so that it can be released as H₂ gas.

3

Reaction
with dilute
Acids

Metal + Acid →Metal salt + Hydrogen

HCl
Mg(s) + 2HCl(aq)→ MgCl₂(aq) + H₂(g)
H₂SO₄
2Na(s) + H₂SO₂→ Na₂SO₄(aq) +H₂(g)
HNO₃
Metal + HNO₃→ H₂ gas is not displaced.
Reason- HNO₃ is strong oxidizing agent.

Non-metals do not react with acids to release H₂ gas                  
Reason- Non-metals cannot loose electrons and give it to Hydrogen ions of acids so that the gas is released.
Mn + 2HNO₃→ Mn(NO₃)₂ + H₂
H₂ gas from HNO₃

4

Reaction
with salt solutions

When metals react with salt
solution, more reactive metal will displace a less reactive metal from its salt solution.
CuSO₄(aq) + n(s)→ ZnSO₄(aq) + Cu(s)

When non-metals react
with salt solution, more reactive non-metal will displace a less reactive non-metal from its salt solution.
2NaBr(aq) + Cl₂(g)→ 2NaCl(aq) + Br₂(aq)