1. First, Get the Big Picture 🎯

In Class 10 Chemistry, “Metals and Non-metals” is not just about learning lists of elements. The real aim is to connect three ideas:

1. Physical properties – What they look and feel like
2. Chemical properties – How they react
3. Uses and extraction – Where we use them and how we get them from ores

This chapter forms a base for higher classes and competitive exams (JEE Main, NEET, Olympiads), where you will study more about the periodic table, bonding and metallurgy.

2. Quick Visual Snapshot: Metals vs Non-metals 🧾

Concept Table – Compare at a Glance

Memory tip:
“MALDA CONSO” – MALleable, Ductile, Alloy-forming, good CONductors, SOnorous → features of metals.

3. Physical Properties Explained with Simple Examples 🔍

3.1 Lustre, Malleability and Ductility

• Lustre (shining surface):
  Gold, silver, copper and aluminium shine when freshly cut or polished.
  That is why metals are used to make jewellery, utensils, decorative items.

• Malleability:
  Ability to be beaten into thin sheets.
  Example: Aluminium foil, gold leaf used in sweets.

• Ductility:
  Ability to be drawn into wires.
  Example: Copper and aluminium wires used in electrical wiring.

Board Exam Tip (CBSE Class 10):
A very common 2-mark question is: “Why are metals used for making cooking utensils and electrical wires?”
Answer must mention: good conductor + high melting point (for utensils) and ductility + conductivity (for wires).

3.2 Conductivity and Sonority

• Good conductors: Copper, aluminium, silver conduct heat and electricity well.

  • Cooking utensils: metals transfer heat quickly to food.
  • Electric wires: metals allow current to pass easily.

• Sonorous:
  When you hit a metal plate or bell, it produces a ringing sound.
  That’s why bells in schools and temples are made of metal.

3.3 Non-metals in Everyday Life

Non-metals may not shine or conduct like metals, but they are equally important:

• Oxygen – for breathing, combustion.
• Nitrogen – used in fertilizers (as ammonia, urea).
• Sulphur – used in vulcanization of rubber and in medicines.
• Chlorine – used in water purification.
• Iodine – in antiseptics.

4. Chemical Behaviour: How Metals React ⚗️

Chemical properties are very important for both board exams and competitive exams because they test your understanding, not memory.

4.1 Reaction with Oxygen (Air)

• Metals react with oxygen to form metal oxides.

Examples:

• Magnesium burns in air to form magnesium oxide:
  2Mg + O2 → 2MgO (magnesium oxide, a white powder)
• Aluminium forms a thin layer of aluminium oxide that protects it from further corrosion.

Some metal oxides (like aluminium oxide, zinc oxide) are amphoteric – they react with both acids and bases.

• Non-metals form non-metallic oxides, which are generally acidic.
  Example: Sulphur + oxygen → sulphur dioxide (acidic oxide).

4.2 Reaction with Water

• Highly reactive metals like sodium and potassium react vigorously with water and release hydrogen gas.
  Sodium + water → sodium hydroxide + hydrogen (with lot of heat).

  That’s why sodium is stored in kerosene, not in water or air.

• Less reactive metals like magnesium react slowly with cold water but faster with hot water or steam.

• Very unreactive metals like gold and platinum do not react with water at all.

4.3 Reaction with Acids

Metals generally react with dilute acids (like HCl, H2SO4) to form salt + hydrogen gas.

Example:

• Zinc + dilute sulphuric acid → zinc sulphate + hydrogen
• Iron + dilute hydrochloric acid → iron chloride + hydrogen

Lab Clue:
The colourless gas formed is confirmed as hydrogen by bringing a burning matchstick near it. It burns with a ‘pop’ sound.

Non-metals usually do not react with dilute acids like metals do (they don’t displace hydrogen).

4.4 Reaction with Bases

Some metals react with strong bases like sodium hydroxide to form complex salts and hydrogen gas.
Example: Zinc reacts with sodium hydroxide to give sodium zincate and hydrogen.

This shows again that zinc is amphoteric (forms soluble salts with both acids and bases).

5. Reactivity Series: Who Is More Powerful? ⚡

Not all metals are equally reactive. To arrange them, we use the Reactivity Series of Metals.

Simplified Reactivity Series (Top = Most Reactive)

Potassium > Sodium > Calcium > Magnesium > Aluminium > Zinc > Iron > Lead > (Hydrogen) > Copper > Silver > Gold

• Metals above hydrogen in the series can displace hydrogen from acids.
• Metals higher up can displace metals lower down from their compounds.

Common CBSE Question Pattern

• “Why does zinc displace copper from copper sulphate solution, but copper cannot displace zinc from zinc sulphate solution?”

Answer idea:

• Zinc is more reactive than copper as per the reactivity series.
• Therefore, zinc can displace copper from its salt solution, but copper cannot displace zinc from zinc sulphate.

6. How We Get Metals from Ores (Metallurgy Basics) ⛏️

Metals are rarely found in pure form in the earth. They are mostly present as ores (compounds mixed with impurities).

Important Terms

• Mineral: A naturally occurring substance containing metal (may or may not be economically profitable).
• Ore: Mineral from which metal can be profitably extracted.
• Gangue: Unwanted impurities like sand, soil, etc.

Main Steps of Extraction (Class 10 Level)

1. Ores → Concentration of ore (removal of gangue).
2. Concentrated ore → Metal oxide (by roasting or calcination).
3. Metal oxide → Metal (by reduction using carbon or other reducing agents).
4. Metal → Refining (to get very pure metal).

Different Reactivity, Different Methods

• Highly reactive metals (e.g., Na, K, Ca, Al):
  Extracted by electrolysis of their molten salts (e.g., NaCl, Al2O3).

• Moderately reactive metals (e.g., Zn, Fe, Pb):
  Extracted by reduction of their oxides with carbon or carbon monoxide.
  Example: Iron is extracted from iron oxide in a blast furnace using coke (carbon).

• Least reactive metals (e.g., Au, Ag, Pt):
  Often found in native (free) state. They may just be refined or extracted by mild methods.

7. Corrosion and Protection of Metals 🛡️

7.1 What is Corrosion?

Corrosion is the slow eating away of metals due to reaction with moisture, oxygen and other chemicals.

• Rusting of iron is the most common example.
  It requires both air (oxygen) and water (moisture).

7.2 Preventing Corrosion

Very important for 3–5 mark questions.

Methods:

1. Painting / Oiling / Greasing

   • Forms a protective layer so that air and moisture cannot reach the metal.

2. Galvanization

   • Coating iron with a thin layer of zinc.
   • Zinc is more reactive and protects iron from rusting.

3. Alloying

   • Mixing metal with other metals or non-metals to improve properties.
   • Example: Stainless steel (iron + carbon + chromium + nickel) is harder and rust-resistant.

4. Electroplating

   • Deposition of a thin layer of a more expensive or less reactive metal (like chromium, silver) on the surface of a cheaper metal.
   • Used in taps, car parts, jewellery, decorative items.

8. Alloys: Super-Metals for Special Uses 🧪

An alloy is a homogeneous mixture of a metal with other metals or non-metals to improve its properties.

Important Alloys for Class 10

Did you know?
Pure metals are often too soft or too reactive. That’s why we rarely use them in pure form. Most industrial uses involve alloys, which are stronger, harder or more resistant to corrosion.

9. Non-metals: Not Weak, Just Different 🌿

Non-metals may not be shiny or ductile, but they are chemically very important.

Key Roles of Non-metals

• Oxygen (O2): Essential for respiration and combustion.
• Nitrogen (N2): Major part of air, used to make ammonia and fertilizers.
• Chlorine (Cl2): Water purification, production of PVC plastic.
• Sulphur (S): In gunpowder, fertilizers, vulcanization of rubber.
• Phosphorus (P): In safety matches, fertilizers, DNA in our body.
• Iodine (I2): Antiseptics (e.g., tincture iodine).

Nature of Non-metal Oxides

• Non-metals form acidic oxides (like sulphur dioxide, carbon dioxide) that dissolve in water to form acids.
• Some form neutral oxides (like carbon monoxide, nitrous oxide) that are neither acidic nor basic.

10. Common Mistakes Students Make 🚫

1. Thinking all metals are hard and all non-metals are soft

   • Sodium and potassium are so soft they can be cut with a knife.
   • Diamond (a form of carbon, a non-metal) is the hardest natural substance.

2. Assuming all metals are solid at room temperature

   • Mercury (metal) is a liquid at room temperature.

3. Saying “all metal oxides are basic”

   • Some metal oxides like aluminium oxide and zinc oxide are amphoteric.

4. Forgetting that graphite is a good conductor

   • It is a non-metal but conducts electricity due to free electrons.

5. Confusing ore and mineral

   • Every ore is a mineral, but not every mineral is an ore.

Exam Strategy:
When you see the words “justify with reason” or “explain” in CBSE questions, always add a reason linked to properties or reactivity series, not just the final answer.

11. Lightning Revision Sheet ⚡ (Use Before Exam)

Rapid Revision – Metals and Non-metals (Class 10)

• Metals: lustrous, malleable, ductile, good conductors, sonorous, form basic or amphoteric oxides.
• Non-metals: generally dull, brittle (if solid), poor conductors, form acidic or neutral oxides.
• Highly reactive metals (Na, K, Ca): stored carefully, often extracted by electrolysis.
• Moderately reactive metals (Zn, Fe, Pb): extracted by reduction with carbon.
• Least reactive metals (Au, Ag, Pt): found in free state, need simple extraction.
• Corrosion: slow damage of metals; rusting needs air and moisture.
• Protection: painting, galvanization, alloying, electroplating.
• Alloys: mixtures to improve strength, durability, corrosion resistance.
• Reactivity series: helps predict displacement reactions and extraction method.
• CBSE focus: definitions, reactions with oxygen/water/acids, reactivity series, corrosion, alloys, and reasoning questions.

12. Practice to Master: Try the Metals And Non Metals Quiz 📝

Ready to test your understanding and identify weak spots before the exam?

👉 Practice “Metals And Non Metals” Quiz