PRASHANT KIRAD
Metals and Non Metals Reactions of Metals and Non Metals
Oxygen - Non - metals
Property Metals Non-Metals
Non-Metal + Oxygen →
Non-Metal Oxide (Acidic/Neutral)
Example: C + O₂ CO₂→
Solid at room
Can exist in all three states:
solids (e.g., Sulfur,
S + O₂ →SO₂
Oxygen - Metals
State temperature (except Phosphorus), liquid (Bromine -
Metal + Oxygen →
Metal Oxide (Basic)
Mercury - liquid) only liquid), gases (e.g.,
Oxygen, Nitrogen)
Example: 2Mg + O₂ →
2MgO
Amphoteric Metals: Beryllium (Be), Zinc (Zn), Tin (Sn),
Lead (Pb), Aluminium (Al), (Antimony (Sb)
Lustre Shiny (metallic lustre) Dull (except Iodine - lustrous)
Aluminium with Oxygen: 4Al(s) + 3O₂(g) →
2Al₂O₃(s)
Generally hard Generally soft (Diamond -
Zinc with Oxygen: 2Zn(s) + O₂(g) →
2ZnO(s)
Hardness (except Sodium, exception, hardest natural Aluminium Oxide Reactions:
Potassium - soft) substance) Al₂O₃(s) + 6HCl(aq) →
2AlCl₃(aq) + 3H₂O(l)
Al₂O₃(s) + 2NaOH(aq) →
2NaAlO₂(aq) + H₂O(l)
Can be beaten into Brittle, cannot be beaten into Water- Non - metals
Malleability
sheets sheets Non metals don’t react with water
Non-Metal Oxide + Water Acid→
Can be drawn into Non-ductile, cannot be drawn SO₂ + H₂O →
H₂SO₃
Ductility
wires into wires SO₃ + H₂O →
H₂SO₄
CO₂ + H₂O →
H₂CO₃
Conductivity
Good conductors Poor conductors (except NO₂ + H₂O →
HNO₃ + HNO₂
(except Lead, Graphite - conducts Water- Metal
(Heat &
Electricity)
Mercury - poor
conductors of heat)
electricity but not heat
efficiently)
Metal + Water →
Metal Hydroxide + H₂
Na₂O, K₂O, CaO, and MgO dissolve in water to form metal
hydroxides
Melting &
Generally high
(except Gallium,
Generally low (Diamond - Example: 2Na + 2H₂O →
2NaOH + H₂
exception, extremely high K, Na react violently with water; Ca reacts mildly;
Boiling Point Caesium - low melting
points)
melting point) →
Ca+2H2O Ca(OH)2+H2
Mg reacts with hot water. Al, Fe, Zn react with steam;
→
2Al+3H2O (steam) Al2O3+3H2
Sonority
Produces sound when
struck
Does not produce sound →
3Fe+4H2O (steam) Fe3O4+4H2
Pb, Cu, Ag, Au do not react with water.
Acids- Non - metals No Reaction
Acids- Metal
Metal + dil. Acid Salt + H₂ → Property Description
Example: Zn + 2HCl ZnCl₂ + H₂ →
Hydrogen gas isn't produced when metals react with HNO₃ Solid, hard, brittle due to strong ionic
because it oxidizes H₂ to water and reduces to nitrogen oxides. Physical nature
bonds.
Only Mg and Mn with very dilute HNO₃ release H₂ gas.
Metal (Mg and Mn) + Dilute nitric acid Salt + Hydrogen gas →
2Mg + 4HNO₃ 2Mg(NO₃)₂ + H₂ → High, due to strong inter-ionic
Mn + 2HNO₃ Mn(NO₃)₂ + H₂ → Melting &
attractions requiring more energy to
Other Metals + Dilute nitric acid Salt + Water + NO₂/N₂O/NO→ Boiling points
break.
Aqua regia is a mix of concentrated hydrochloric and nitric
acids in a 3:1 ratio. It’s highly corrosive and can dissolve gold
and platinum. Soluble in water, insoluble in organic
Solubility
solvents like kerosene and petrol.
Metal Salts Non - metals
No Reaction
Metal Salts Metal Electrical Conducts in molten and aqueous states,
More reactive metals displace less reactive metals from conductivity not in solid due to immobile ions.
their salt solutions (displacement reaction).
Metal A + Salt solution of B →
Salt solution of A + Metal B Metallurgy: Science & tech of metals' properties,
Example: Pb + CuCl₂ PbCl₂ + Cu → production, purification
When metals react with non-metals, electrons transfer from
Minerals: Naturally occurring elements/compounds in
metals to non-metals, forming ions. The compound formed is
Earth's crust
ionic.
Metal + Non-metal → Ionic compound PROPERTIES?
Ores: Minerals from which metals can be extracted
economically and conveniently
Gangue Particles: Impurities in ores (sand, oil, etc.)
Enrichment of Ore/Concentration: Process of removing
gangue particles from ore
Metals and Non Metals Reactions of Metals and Non Metals
Oxygen - Non - metals
Property Metals Non-Metals
Non-Metal + Oxygen →
Non-Metal Oxide (Acidic/Neutral)
Example: C + O₂ CO₂→
Solid at room
Can exist in all three states:
solids (e.g., Sulfur,
S + O₂ →SO₂
Oxygen - Metals
State temperature (except Phosphorus), liquid (Bromine -
Metal + Oxygen →
Metal Oxide (Basic)
Mercury - liquid) only liquid), gases (e.g.,
Oxygen, Nitrogen)
Example: 2Mg + O₂ →
2MgO
Amphoteric Metals: Beryllium (Be), Zinc (Zn), Tin (Sn),
Lead (Pb), Aluminium (Al), (Antimony (Sb)
Lustre Shiny (metallic lustre) Dull (except Iodine - lustrous)
Aluminium with Oxygen: 4Al(s) + 3O₂(g) →
2Al₂O₃(s)
Generally hard Generally soft (Diamond -
Zinc with Oxygen: 2Zn(s) + O₂(g) →
2ZnO(s)
Hardness (except Sodium, exception, hardest natural Aluminium Oxide Reactions:
Potassium - soft) substance) Al₂O₃(s) + 6HCl(aq) →
2AlCl₃(aq) + 3H₂O(l)
Al₂O₃(s) + 2NaOH(aq) →
2NaAlO₂(aq) + H₂O(l)
Can be beaten into Brittle, cannot be beaten into Water- Non - metals
Malleability
sheets sheets Non metals don’t react with water
Non-Metal Oxide + Water Acid→
Can be drawn into Non-ductile, cannot be drawn SO₂ + H₂O →
H₂SO₃
Ductility
wires into wires SO₃ + H₂O →
H₂SO₄
CO₂ + H₂O →
H₂CO₃
Conductivity
Good conductors Poor conductors (except NO₂ + H₂O →
HNO₃ + HNO₂
(except Lead, Graphite - conducts Water- Metal
(Heat &
Electricity)
Mercury - poor
conductors of heat)
electricity but not heat
efficiently)
Metal + Water →
Metal Hydroxide + H₂
Na₂O, K₂O, CaO, and MgO dissolve in water to form metal
hydroxides
Melting &
Generally high
(except Gallium,
Generally low (Diamond - Example: 2Na + 2H₂O →
2NaOH + H₂
exception, extremely high K, Na react violently with water; Ca reacts mildly;
Boiling Point Caesium - low melting
points)
melting point) →
Ca+2H2O Ca(OH)2+H2
Mg reacts with hot water. Al, Fe, Zn react with steam;
→
2Al+3H2O (steam) Al2O3+3H2
Sonority
Produces sound when
struck
Does not produce sound →
3Fe+4H2O (steam) Fe3O4+4H2
Pb, Cu, Ag, Au do not react with water.
Acids- Non - metals No Reaction
Acids- Metal
Metal + dil. Acid Salt + H₂ → Property Description
Example: Zn + 2HCl ZnCl₂ + H₂ →
Hydrogen gas isn't produced when metals react with HNO₃ Solid, hard, brittle due to strong ionic
because it oxidizes H₂ to water and reduces to nitrogen oxides. Physical nature
bonds.
Only Mg and Mn with very dilute HNO₃ release H₂ gas.
Metal (Mg and Mn) + Dilute nitric acid Salt + Hydrogen gas →
2Mg + 4HNO₃ 2Mg(NO₃)₂ + H₂ → High, due to strong inter-ionic
Mn + 2HNO₃ Mn(NO₃)₂ + H₂ → Melting &
attractions requiring more energy to
Other Metals + Dilute nitric acid Salt + Water + NO₂/N₂O/NO→ Boiling points
break.
Aqua regia is a mix of concentrated hydrochloric and nitric
acids in a 3:1 ratio. It’s highly corrosive and can dissolve gold
and platinum. Soluble in water, insoluble in organic
Solubility
solvents like kerosene and petrol.
Metal Salts Non - metals
No Reaction
Metal Salts Metal Electrical Conducts in molten and aqueous states,
More reactive metals displace less reactive metals from conductivity not in solid due to immobile ions.
their salt solutions (displacement reaction).
Metal A + Salt solution of B →
Salt solution of A + Metal B Metallurgy: Science & tech of metals' properties,
Example: Pb + CuCl₂ PbCl₂ + Cu → production, purification
When metals react with non-metals, electrons transfer from
Minerals: Naturally occurring elements/compounds in
metals to non-metals, forming ions. The compound formed is
Earth's crust
ionic.
Metal + Non-metal → Ionic compound PROPERTIES?
Ores: Minerals from which metals can be extracted
economically and conveniently
Gangue Particles: Impurities in ores (sand, oil, etc.)
Enrichment of Ore/Concentration: Process of removing
gangue particles from ore
