Metals and non-metals represent crucial topics within the Class 10 Chemistry syllabus, delving into the distinct attributes, reactions, and applications of these elemental groups. Through the "Metals and Non-metals Class 10 Notes," students will unravel the differences between these categories, particularly in terms of their physical and chemical characteristics, the ways they interact with other substances, and their everyday significance. Mastering these concepts is key to understanding the fundamental nature of elements, empowering students to excel in examinations and navigate more sophisticated chemistry concepts with ease.

Metals and Non-metals

1. Physical Properties of Metals:

Metals are malleable, ductile, good conductors of heat and electricity, and have high melting and boiling points. They are generally solid at room temperature except mercury (liquid).
Examples: Iron (Fe), Copper (Cu), Aluminum (Al).

2. Physical Properties of Non-metals:

Non-metals are generally brittle, non-ductile, and poor conductors of heat and electricity. They may exist in solid, liquid, or gas states.
Examples: Sulfur (S), Oxygen (O₂), Carbon (C).

3. Chemical Properties of Metals:

a) Reaction of Metals with Oxygen:

Metals react with oxygen to form metal oxides, which are generally basic in nature.
Example: 4Na(s) + O₂(g) → 2Na₂O(s).

b) Reaction of Non-metals with Oxygen:

Non-metals react with oxygen to form non-metallic oxides, which are acidic in nature.
Example: C(s) + O₂(g) → CO₂(g).

c) Reaction of Metals with Water:

Metals react with water to form metal hydroxides and hydrogen gas.
Example: 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g).

Less reactive metals, like iron, react with steam.
Example: 3Fe(s) + 4H₂O(g) → Fe₃O₄(s) + 4H₂(g).

d) Reaction of Metals with Acids:

Metals react with acids to form salt and hydrogen gas.
Example: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g).

e) Reaction of Metals with Solutions of Other Metal Salts:

A more reactive metal displaces a less reactive metal from its salt solution (displacement reaction).
Example: Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s).

4. Reactivity Series of Metals:

The reactivity series arranges metals in order of their reactivity, from most reactive to least reactive:
K > Na > Ca > Mg > Al > Zn > Fe > Pb > Cu > Hg > Ag > Au.

5. Extraction of Metals:

a) Extraction of Metals Low in the Reactivity Series:

Metals low in the reactivity series (e.g., Au, Ag) are found in their free state and can be obtained by physical methods.

-b) Extraction of Metals in the Middle of the Reactivity Series:

Metals like iron, zinc, and copper are extracted by reduction of their oxides using carbon or carbon monoxide.
Example: ZnO(s) + C(s) → Zn(s) + CO(g).

c) Extraction of Metals High in the Reactivity Series:

Metals like sodium, calcium, and aluminum are extracted by electrolytic reduction of their molten compounds.
Example: 2NaCl(l) → 2Na(s) + Cl₂(g) (Electrolysis of molten sodium chloride).

6. Corrosion:

Corrosion is the gradual destruction of metals due to reactions with air, water, or other chemicals.
Example: Fe(s) + O₂(g) + H₂O(l) → Fe₂O₃·xH₂O(s) (Rust).

Prevention of Corrosion:

Galvanization: Coating iron with a layer of zinc.
Alloying: Mixing metals with other elements to prevent corrosion.

7. Properties of Ionic Compounds:

Ionic compounds are formed by the transfer of electrons from metals to non-metals, resulting in strong electrostatic forces of attraction.
They have high melting and boiling points, are soluble in water, and conduct electricity in molten or aqueous state.
Example: NaCl(s), MgO(s).

8. Occurrence of Metals:

Minerals are naturally occurring compounds of metals.
Ores are minerals from which metals can be extracted profitably.

9. Metallurgy:

Metallurgy involves three main steps:

Concentration of Ore: Removal of impurities (gangue) from ore.
Reduction of Ore: Converting concentrated ore into metal using reduction methods (carbon reduction, electrolytic reduction).
Refining of Metal: Purification of the crude metal obtained from the ore.

10. Alloys:

An alloy is a homogeneous mixture of two or more metals or metals with non-metals. Alloys have properties different from their constituent metals.
Example: Brass is an alloy of copper and zinc.