Summary Short Notes

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
Can exist in all three states:
S + O₂ → SO₂
Solid at room solids (e.g., Sulfur,
State temperature (except Phosphorus), liquid (Bromine - Oxygen - Metals
Metal + Oxygen → Metal Oxide (Basic)
Mercury - liquid) only liquid), gases (e.g.,
Example: 2Mg + O₂ → 2MgO
Oxygen, Nitrogen)
Amphoteric Metals: Beryllium (Be), Zinc (Zn), Tin (Sn),
Lustre Shiny (metallic lustre) Dull (except Iodine - lustrous)
Lead (Pb), Aluminium (Al), (Antimony (Sb)
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
Good conductors Poor conductors (except NO₂ + H₂O → HNO₃ + HNO₂
Conductivity
(except Lead, Graphite - conducts Water- Metal
(Heat &
Mercury - poor electricity but not heat Metal + Water → Metal Hydroxide + H₂
Electricity)
conductors of heat) efficiently)
Na₂O, K₂O, CaO, and MgO dissolve in water to form metal
hydroxides
Generally high
Generally low (Diamond - Example: 2Na + 2H₂O → 2NaOH + H₂
Melting & (except Gallium,
exception, extremely high K, Na react violently with water; Ca reacts mildly;
Boiling Point Caesium - low melting
melting point) Ca+2H2​O→Ca(OH)2​+H2​
points)
Mg reacts with hot water. Al, Fe, Zn react with steam;
2Al+3H2​O (steam)→Al2​O3​+3H2​
Produces sound when
Sonority Does not produce sound 3Fe+4H2​O (steam)→Fe3​O4​+4H2
struck
Pb, Cu, Ag, Au do not react with water.

Acids- Non - metals No Reaction
Acids- Metal Property Description
Metal + dil. Acid → Salt + H₂
Example: Zn + 2HCl → ZnCl₂ + H₂
Hydrogen gas isn't produced when metals react with HNO₃ Solid, hard, brittle due to strong ionic
Physical nature
because it oxidizes H₂ to water and reduces to nitrogen oxides. 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
Melting &
Mn + 2HNO₃ → Mn(NO₃)₂ + H₂ attractions requiring more energy to
Boiling points
Other Metals + Dilute nitric acid → Salt + Water + NO₂/N₂O/NO 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
Soluble in water, insoluble in organic
and platinum. Solubility
solvents like kerosene and petrol.
Metal Salts Non - metals
No Reaction
Electrical Conducts in molten and aqueous states,
Metal Salts Metal
conductivity not in solid due to immobile ions.
More reactive metals displace less reactive metals from
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.
Ores: Minerals from which metals can be extracted
Metal + Non-metal → Ionic compound PROPERTIES?
economically and conveniently

Gangue Particles: Impurities in ores (sand, oil, etc.)


Enrichment of Ore/Concentration: Process of removing
gangue particles from ore