Metals and Non-metals

Notes

8. Reactivity Series

Definition

The Reactivity Series is the arrangement of metals in the decreasing order of their reactivity.

Reactivity Series (Most Reactive → Least Reactive)

Symbol Metal

K Potassium

Na Sodium

Ca Calcium

Mg Magnesium

Al Aluminium

Zn Zinc

Fe Iron

Pb Lead

(H) Hydrogen (Reference only)

Cu Copper

Hg Mercury

Ag Silver

Au Gold

Remember: Metals above hydrogen can displace hydrogen from dilute acids, while metals below hydrogen cannot.

Memory Trick

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P – Potassium (K)

S – Sodium (Na)

C – Calcium (Ca)

M – Magnesium (Mg)

A – Aluminium (Al)

Z – Zinc (Zn)

I – Iron (Fe)

T – Tin (Sn)* (NCERT includes Pb instead of Sn in many tables; JAC mainly follows Pb after Fe.)

L – Lead (Pb)

H – Hydrogen

C – Copper (Cu)

S – Silver (Ag)

G – Gold (Au)

9. Displacement Reaction

A more reactive metal displaces a less reactive metal from its salt solution.

Example

Zn + CuSO₄ → ZnSO₄ + Cu

Observation:

Blue colour of CuSO₄ fades.

Brown copper metal is deposited.

10. Ionic Compounds

Definition

Compounds formed by the transfer of electrons from a metal to a non-metal are called ionic compounds.

Example

NaCl (Sodium Chloride)

Sodium loses 1 electron → Na⁺

Chlorine gains 1 electron → Cl⁻

Na⁺ + Cl⁻ → NaCl

Properties of Ionic Compounds

Hard and brittle.

High melting and boiling points.

Soluble in water.

Conduct electricity in molten state or aqueous solution.

Do not conduct electricity in solid state.

11. Extraction of Metals

Metals are extracted from their ores.

Steps

Mining

Concentration of Ore

Extraction of Metal

Refining (Purification)

Extraction Based on Reactivity

(A) Highly Reactive Metals

Examples:

Potassium

Sodium

Calcium

Method: Electrolysis

(B) Moderately Reactive Metals

Examples:

Zinc

Iron

Lead

Method: Reduction using carbon (coke).

Example:

ZnO + C → Zn + CO

(C) Least Reactive Metals

Examples:

…