Class 10 Science – Chapter 3: Metals and Non-metals (Complete Notes) 🧪

Meta Description: Comprehensive guide on metal and non metal for Class 10. Learn difference between metal and non metal, their properties, examples, and important question answers with notes.

Introduction – Metals aur Non-metals kya hote hain?

Definition:

Metals – Elements jo electrons easily lose karte hain aur positive ions (cations) banate hain
Non-metals – Elements jo electrons easily gain karte hain aur negative ions (anions) banate hain

Examples:

Metals: Iron (Fe), Copper (Cu), Aluminium (Al), Gold (Au), Silver (Ag)
Non-metals: Oxygen (O), Carbon (C), Sulphur (S), Phosphorus (P), Chlorine (Cl)

3.1 Physical Properties of Metals and Non-metals

Physical Properties of Metals ⚡

Property	Description	Examples
Metallic Lustre	Metals have shiny appearance	Gold, Silver ki chamak
Malleability	Metals can be beaten into thin sheets	Aluminium foil, Gold leaf
Ductility	Metals can be drawn into wires	Copper wires, Iron wires
Good Conductors	Heat aur electricity ko well conduct karte hain	Copper wires in electrical appliances
High Density	Generally metals ka density high hota hai	Iron, Lead
High Melting Point	Most metals high temperature pe melt hote hain	Iron – 1538°C
Sonorous	Metals produce ringing sound when struck	Bell metal, Gong

Memory Trick: “MALGOOD-HS” = Malleable, Alternating lustre, Good conductors, Obviously Onerous (heavy), Ductile, High melting point, Sonorous

Physical Properties of Non-metals ❌

Property	Description	Examples
No Metallic Lustre	Dull appearance (except Iodine and Graphite)	Sulphur, Phosphorus
Brittle	Break easily when hammered	Coal, Sulphur
Non-ductile	Cannot be drawn into wires	Carbon, Oxygen
Poor Conductors	Heat aur electricity poorly conduct karte hain	Rubber, Wood
Low Density	Generally light weight hote hain	Hydrogen, Helium
Low Melting Point	Most non-metals low temperature pe melt/boil	Bromine – liquid at room temp
Non-sonorous	No ringing sound	Plastic

Exceptions to Remember 🚨

Metals with Exceptions:

Mercury – Room temperature pe liquid hai
Gallium – Low melting point (29°C)
Lead – Low density compared to other metals

Non-metals with Exceptions:

Graphite – Good conductor of electricity
Diamond – Hardest natural substance (not brittle)
Iodine – Metallic lustre

3.2 Chemical Properties of Metals

1) Reaction with Oxygen 🔥

General Reaction:

Metal + Oxygen → Metal Oxide (Basic Oxide)

Examples:

4Al + 3O₂ → 2Al₂O₃ (Aluminium Oxide)
2Mg + O₂ → 2MgO (Magnesium Oxide)
4Na + O₂ → 2Na₂O (Sodium Oxide)

Important Points:

Metal oxides are basic in nature
React with water to form alkalis
React with acids to form salt + water

Activity Series based on Oxygen Reaction:

Most Reactive: K > Na > Ca > Mg > Al > Zn > Fe > Pb > Cu > Ag > Au : Least Reactive

2) Reaction with Water 💧

Highly Reactive Metals:

2Na + 2H₂O → 2NaOH + H₂↑ (Violent reaction)
2K + 2H₂O → 2KOH + H₂↑ (Very violent)

Moderately Reactive Metals:

Mg + 2H₂O → Mg(OH)₂ + H₂↑ (Hot water ke saath)

Less Reactive Metals:

3Fe + 4H₂O → Fe₃O₄ + 4H₂↑ (Steam ke saath)

Least Reactive Metals:

Gold, Silver, Copper – No reaction with water

3) Reaction with Acids 🧪

General Reaction:

Metal + Acid → Salt + Hydrogen gas

Examples:

Zn + H₂SO₄ → ZnSO₄ + H₂↑
Mg + 2HCl → MgCl₂ + H₂↑
2Al + 6HCl → 2AlCl₃ + 3H₂↑

Important Notes:

Hydrogen gas pop sound deti hai with burning splinter
Copper and metals below it don’t react with dilute acids
Nitric acid is special – usually no H₂ gas (oxidizing agent hai)

4) Reaction with Salt Solutions (Displacement) ⚗️

More reactive metal displaces less reactive metal:

CuSO₄ + Zn → ZnSO₄ + Cu (Blue solution becomes colorless)
AgNO₃ + Cu → Cu(NO₃)₂ + Ag (Silver deposited)

Activity Series (Reactivity Series):

K > Na > Ca > Mg > Al > Zn > Fe > Pb > (H) > Cu > Hg > Ag > Au

Memory Trick: “Please Send Charlie’s Monkeys And Zebras In London, Having Cold Morning And Gold“

3.3 Chemical Properties of Non-metals

1) Reaction with Oxygen 🌬️

General Reaction:

Non-metal + Oxygen → Non-metal Oxide (Acidic Oxide)

Examples:

C + O₂ → CO₂ (Carbon dioxide)
S + O₂ → SO₂ (Sulphur dioxide)
4P + 5O₂ → 2P₂O₅ (Phosphorus pentoxide)

Important Points:

Non-metal oxides are acidic in nature
React with water to form acids
React with bases to form salt + water

2) Reaction with Water 💦

Most non-metals don’t react directly with water

Exceptions:

Cl₂ + H₂O → HCl + HOCl (Hypochlorous acid)

3) Reaction with Hydrogen 🎈

Examples:

H₂ + Cl₂ → 2HCl (Hydrogen chloride)
H₂ + S → H₂S (Hydrogen sulphide)
3H₂ + N₂ → 2NH₃ (Ammonia – Haber process)

4) Reaction with Metals 🔗

Non-metals gain electrons from metals:

2Na + Cl₂ → 2NaCl (Sodium chloride)
Mg + S → MgS (Magnesium sulphide)

3.4 Uses of Metals and Non-metals

Uses of Metals 🛠️

Metal	Uses	Properties Used
Iron	Construction, Tools, Vehicles	Strong, Malleable
Copper	Electrical wires, Pipes	Good conductor, Ductile
Aluminium	Aircraft, Foils, Utensils	Light weight, Corrosion resistant
Gold	Jewelry, Electronics	Noble metal, Good conductor
Silver	Jewelry, Photography	Lustrous, Antibacterial
Lead	Batteries, X-ray shields	Dense, Malleable

Uses of Non-metals 🧬

Non-metal	Uses	Properties Used
Oxygen	Respiration, Combustion	Supports burning
Carbon	Steel making, Pencils	Forms strong bonds
Nitrogen	Fertilizers, Food packaging	Inert nature
Chlorine	Water purification, PVC	Disinfectant
Sulphur	Gunpowder, Medicines	Chemical reactivity

3.5 Occurrence of Metals in Nature

Native State (Free State) 🏔️

Least reactive metals occur in free state:

Gold – River sands, Quartz rocks
Silver – Combined with gold
Platinum – Native form

Combined State ⛏️

Most metals occur as compounds:

Common Ores:

Metal	Ore	Chemical Formula
Iron	Haematite	Fe₂O₃
Iron	Magnetite	Fe₃O₄
Aluminium	Bauxite	Al₂O₃.2H₂O
Copper	Copper Pyrites	CuFeS₂
Zinc	Zinc Blende	ZnS
Lead	Galena	PbS
Sodium	Rock Salt	NaCl

Types of Compounds in Ores:

Oxides – Most common (Fe₂O₃, Al₂O₃)
Sulphides – Common for Cu, Zn, Pb
Carbonates – Some metals (CaCO₃)
Halides – Alkali metals (NaCl, KCl)

3.6 Extraction of Metals

Steps in Metallurgy 🏭

Step 1: Concentration of Ore

Remove impurities (gangue) from ore

Methods:

Hydraulic Washing – Density difference use karte hain
Magnetic Separation – Magnetic properties use karte hain
Froth Floatation – Surface properties use karte hain

Step 2: Conversion to Oxide

Most reduction processes need oxide form

Calcination (Carbonates):

ZnCO₃ → ZnO + CO₂↑ (Heat in absence of air)

Roasting (Sulphides):

2ZnS + 3O₂ → 2ZnO + 2SO₂↑ (Heat in presence of air)

Step 3: Reduction of Metal Oxide

Remove oxygen to get pure metal

Methods depend on reactivity:

A) Highly Reactive Metals (K, Na, Ca, Mg, Al)

Electrolytic Reduction:

2Al₂O₃ → 4Al + 3O₂ (Electrolysis)
NaCl → Na + ½Cl₂ (Electrolysis)

B) Moderately Reactive Metals (Zn, Fe, Pb)

Carbon Reduction:

ZnO + C → Zn + CO
Fe₂O₃ + 3CO → 2Fe + 3CO₂

C) Less Reactive Metals (Cu, Hg)

Heat Alone:

2HgO → 2Hg + O₂ (Just heating)

Step 4: Refining

Remove remaining impurities

Methods:

Electrolytic Refining – Pure metal at cathode
Distillation – For volatile metals

3.7 Thermite Process 🔥

Special process for Welding:

Fe₂O₃ + 2Al → Al₂O₃ + 2Fe + Heat

Uses:

Railway track welding
Repair of machine parts
Military applications

Why Aluminium?

High affinity for oxygen
Produces lot of heat
Iron produced in molten state

3.8 Corrosion 🦠

Definition

Slow destruction of metals by reaction with environment

Examples of Corrosion

Rusting of Iron 🔴

Most common example:

Conditions Required:

Oxygen (O₂)
Water (H₂O)
Both essential – either absent, no rusting

Chemical Process:

4Fe + 3O₂ + 6H₂O → 2Fe₂O₃.3H₂O (Rust)

Color: Reddish-brown

Other Examples

Copper – Green coating (CuCO₃.Cu(OH)₂)
Silver – Black coating (Ag₂S)
Aluminium – White powder (Al₂O₃)

Prevention of Corrosion 🛡️

1) Physical Barriers

Painting – Iron gates, bridges
Greasing/Oiling – Machine parts
Chrome Plating – Car parts, taps

2) Galvanization

Coating with Zinc:

Zinc more reactive than iron
Sacrificial protection
Used in: Buckets, pipes, sheets

3) Alloying

Mix with other metals:

Stainless Steel = Iron + Chromium + Nickel
Doesn’t rust
Used in: Utensils, surgical instruments

3.9 Alloys 🔗

Definition

Homogeneous mixture of two or more metals (or metal + non-metal)

Why Make Alloys? 🤔

Advantages:

Increase Strength – Pure metals are soft
Prevent Corrosion – Better resistance
Change Properties – Color, hardness, melting point
Reduce Cost – Mix expensive with cheap metals

Important Alloys

Alloy	Composition	Uses
Steel	Fe + C (0.1-1.5%)	Construction, Tools
Stainless Steel	Fe + Cr + Ni	Utensils, Medical instruments
Brass	Cu + Zn	Musical instruments, Decorative
Bronze	Cu + Sn	Statues, Medals
Solder	Pb + Sn	Joining metals, Electronics
Amalgam	Hg + other metals	Dental fillings
Duralumin	Al + Cu + Mg + Mn	Aircraft parts

Special Properties

Alloys don’t have sharp melting point (unlike pure metals)
Generally harder than constituent metals
Better corrosion resistance

Metal and Non Metal Notes Class 10 notes

3.10 Important Chemical Equations 📝

Metals with Oxygen

4Al + 3O₂ → 2Al₂O₃
2Mg + O₂ → 2MgO
4Na + O₂ → 2Na₂O
2Cu + O₂ → 2CuO

Metals with Water

2Na + 2H₂O → 2NaOH + H₂↑
Ca + 2H₂O → Ca(OH)₂ + H₂↑
Mg + 2H₂O → Mg(OH)₂ + H₂↑ (hot water)

Metals with Acids

Zn + H₂SO₄ → ZnSO₄ + H₂↑
Mg + 2HCl → MgCl₂ + H₂↑
Fe + 2HCl → FeCl₂ + H₂↑

Displacement Reactions

CuSO₄ + Zn → ZnSO₄ + Cu
FeSO₄ + Zn → ZnSO₄ + Fe
AgNO₃ + Cu → Cu(NO₃)₂ + Ag

Non-metals with Oxygen

C + O₂ → CO₂
S + O₂ → SO₂
4P + 5O₂ → 2P₂O₅

Extraction Reactions

2Al₂O₃ → 4Al + 3O₂ (Electrolysis)
ZnO + C → Zn + CO
Fe₂O₃ + 3CO → 2Fe + 3CO₂
2HgO → 2Hg + O₂

Memory Tricks and Tips 🧠

1) Activity Series

“Please Send Charlie’s Monkeys And Zebras In London, Having Cold Morning And Gold” = K, Na, Ca, Mg, Al, Zn, Fe, Pb, (H), Cu, Hg, Ag, Au

2) Properties of Metals

“MALGOOD-HS” = Malleable, lustrous, Good conductors, Heavy, Ductile, High melting point, Sonorous

3) Corrosion Prevention

“PGGA” = Paint, Grease, Galvanization, Alloying

4) Types of Ores

“OSCH” = Oxides, Sulphides, Carbonates, Halides

5) Metallurgy Steps

“CCRE” = Concentration, Conversion, Reduction, Refining

Exam-Important Points 🎯

High Weightage Topics

Activity Series – Displacement reactions
Corrosion – Causes and prevention
Extraction methods – Different for different metals
Alloys – Properties and uses
Chemical equations – Balancing and products

Common Numerical Types

Displacement reactions – Predicting products
Corrosion prevention – Method selection
Alloy composition – Percentage calculations
Activity series – Arranging metals

Practical Applications

Thermite welding – Process and uses
Galvanization – Why zinc used
Stainless steel – Composition and advantages
Electrolytic refining – Copper purification

Quick Revision Checklist ✅

Definitions to Remember:

✅ Metals, Non-metals, Metalloids
✅ Ore, Gangue, Activity Series
✅ Corrosion, Alloys, Galvanization
✅ Roasting, Calcination, Smelting

Chemical Equations:

✅ Metal + Oxygen reactions
✅ Metal + Water reactions
✅ Metal + Acid reactions
✅ Displacement reactions
✅ Extraction reactions

Properties:

✅ Physical properties of metals/non-metals
✅ Chemical properties differences
✅ Exceptions to general properties

Applications:

✅ Uses of common metals
✅ Corrosion prevention methods
✅ Important alloys and their uses
✅ Extraction methods for different metals