CBSE Class 10 Science Revision Notes Chapter 3 Metals and Non-metals 2026–27

Metals and Non-metals explains how elements differ in physical properties, chemical reactions, bonding and extraction.

In CBSE Class 10 Science, Chapter 3 covers reactivity series, ionic compounds, metallurgy, corrosion and alloys.

Metals and Non-metals is an important chemistry chapter in Class 10 Science. It explains why metals are used for wires, utensils and machines, while non-metals are used in forms such as oxygen, sulphur, carbon and iodine.

Use these CBSE Class 10 Science Revision Notes Chapter 3 to revise the chapter quickly for the 2026–27 exams. Start with the physical properties of metals and non-metals, then revise reactions, reactivity series, ionic compounds, extraction of metals, corrosion and alloys.

Key Takeaways

• Metals: Metals are generally lustrous, malleable, ductile, sonorous and good conductors of heat and electricity.
• Non-metals: Non-metals are usually brittle, non-sonorous and poor conductors, except graphite.
• Reactivity series: More reactive metals displace less reactive metals from their salt solutions.
• Ionic compounds: Metals lose electrons and non-metals gain electrons to form ionic compounds.
• Corrosion: Rusting happens when iron reacts with both air and moisture.

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CBSE Class 10 Science Chapter 3 Metals and Non-metals at a Glance

This chapter compares metals and non-metals through their properties and reactions. It also explains how metals are extracted from ores and why corrosion damages metal objects.

These Class 10 Science Chapter 3 Notes help students revise reactions, definitions and examples in a board-exam-friendly format.

What Are Metals and Non-metals?

Metals are elements that generally lose electrons and form positive ions. They are usually hard, shiny and good conductors.

Examples of metals include iron, copper, aluminium, magnesium, zinc, sodium, potassium, silver and gold.

Non-metals are elements that usually gain electrons and form negative ions. They may exist as solids, liquids or gases.

Examples of non-metals include carbon, sulphur, iodine, oxygen, hydrogen, nitrogen and bromine.

Physical Properties of Metals and Non-metals

The physical properties of metals and non-metals help us understand their uses in daily life.

Metals like copper and aluminium are used for electric wires because they conduct electricity. Metals like iron are used in machines and construction because they are hard and strong.

Exceptions in Physical Properties

Some elements do not follow the general pattern. These exceptions are important in CBSE Notes Class 10 Science Chapter 3.

These exceptions are often used in short-answer and reasoning questions.

Chemical Properties of Metals

The chemical properties of metals depend on how easily they lose electrons. Metals form positive ions and react with oxygen, water, acids and salt solutions.

Reaction of Metals with Oxygen

Metals react with oxygen to form metal oxides.

Metal + Oxygen → Metal oxide

Example:

2Cu + O₂ → 2CuO

Copper forms black copper oxide on heating.

4Al + 3O₂ → 2Al₂O₃

Aluminium forms aluminium oxide. This oxide forms a protective layer on the surface of aluminium.

Most metal oxides are basic in nature. Some metal oxides, such as aluminium oxide and zinc oxide, are amphoteric.

Amphoteric oxides react with both acids and bases to form salt and water.

Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O

Al₂O₃ + 2NaOH → 2NaAlO₂ + H₂O

Reaction of Metals with Water

Metals react with water to form metal oxide or metal hydroxide and hydrogen gas.

Metal + Water → Metal oxide + Hydrogen

Metal oxide + Water → Metal hydroxide

Highly reactive metals such as potassium and sodium react violently with cold water.

2K + 2H₂O → 2KOH + H₂ + heat

2Na + 2H₂O → 2NaOH + H₂ + heat

Calcium reacts less violently with water.

Ca + 2H₂O → Ca(OH)₂ + H₂

Magnesium reacts with hot water.

Mg + 2H₂O → Mg(OH)₂ + H₂

Aluminium, zinc and iron react with steam.

2Al + 3H₂O → Al₂O₃ + 3H₂

3Fe + 4H₂O → Fe₃O₄ + 4H₂

Lead, copper, silver and gold do not react with water.

Reaction of Metals with Acids

Metals react with dilute acids to form salt and hydrogen gas.

Metal + Dilute acid → Salt + Hydrogen gas

Example:

Zn + 2HCl → ZnCl₂ + H₂

The reaction is faster when the metal is more reactive.

Metals above hydrogen in the reactivity series can displace hydrogen from dilute acids.

Copper does not react with dilute hydrochloric acid because it is less reactive than hydrogen.

Nitric acid usually does not produce hydrogen gas with metals because it is a strong oxidising agent. Magnesium and manganese can produce hydrogen with very dilute nitric acid.

Reaction of Metals with Salt Solutions

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

Metal A + Salt solution of B → Salt solution of A + Metal B

Example:

Fe + CuSO₄ → FeSO₄ + Cu

Iron displaces copper from copper sulphate solution because iron is more reactive than copper.

Another example:

Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag

Copper displaces silver from silver nitrate solution because copper is more reactive than silver.

Reactivity Series of Metals

The reactivity series arranges metals in decreasing order of reactivity.

The reactivity series helps students predict displacement reactions and extraction methods.

A metal placed higher in the series can displace a metal placed lower in the series from its salt solution.

How Do Metals and Non-metals React?

Metals lose electrons and form cations. Non-metals gain electrons and form anions.

The oppositely charged ions attract each other strongly. This forms an ionic bond.

Example: Formation of sodium chloride

Na → Na⁺ + e⁻

Cl + e⁻ → Cl⁻

Na⁺ + Cl⁻ → NaCl

Sodium loses one electron and becomes Na⁺. Chlorine gains one electron and becomes Cl⁻.

Ionic Compounds

Ionic compounds are formed by the transfer of electrons from a metal to a non-metal.

Examples include NaCl, MgO, CaO and MgCl₂.

Ionic compounds conduct electricity in molten or aqueous state because ions are free to move. They do not conduct electricity in solid state because ions are fixed in position.

Occurrence of Metals

Metals occur in nature in free state or combined state.

The elements or compounds found naturally in the earth’s crust are called minerals.

Minerals from which metals can be extracted profitably are called ores.

The unwanted impurities present in an ore are called gangue.

Gold, silver, platinum and copper may occur in free state because they are less reactive. Potassium, sodium, calcium, magnesium and aluminium are highly reactive, so they are not found in free state.

Extraction of Metals

The extraction method depends on the position of the metal in the reactivity series.

This section of Chapter 3 Science Class 10 Notes is important because extraction questions often depend on the reactivity series.

Enrichment of Ores

Ores mined from the earth contain impurities such as sand and soil. These impurities are called gangue.

The process of removing gangue from ore is called enrichment of ore.

Different methods are used depending on the physical or chemical properties of ore and gangue.

Roasting and Calcination

Roasting and calcination convert ores into metal oxides. Metal oxides are easier to reduce into metals.

Roasting and calcination are frequently asked as difference-based questions.

Reduction of Metal Oxides

Metal oxides are reduced to metals by removing oxygen.

Metal oxide + Carbon → Metal + Carbon dioxide

Example:

ZnO + C → Zn + CO

For some metal oxides, aluminium is used as a reducing agent.

Fe₂O₃ + 2Al → 2Fe + Al₂O₃ + heat

This reaction is called the thermit reaction. It is used for joining railway tracks and cracked machine parts.

Electrolytic Refining

The metals obtained after extraction may contain impurities. Refining removes these impurities.

Electrolytic refining is a common method used for metals such as copper, zinc, tin, nickel, silver and gold.

In electrolytic refining:

When electric current passes through the electrolyte, pure metal is deposited on the cathode. Insoluble impurities settle below the anode as anode mud.

Corrosion

Corrosion is the gradual damage of a metal due to the action of air, moisture or chemicals.

Rusting of iron is the most common example.

Iron + Oxygen + Water → Hydrated iron oxide

4Fe + 3O₂ + xH₂O → 2Fe₂O₃·xH₂O

Rust is brown and flaky. It weakens iron articles over time.

Copper forms a green coating due to basic copper carbonate.

Silver turns black due to silver sulphide.

Prevention of Corrosion

Corrosion can be reduced by stopping air and moisture from reaching the metal surface.

Galvanisation protects iron even when the zinc layer is slightly broken because zinc is more reactive than iron.

Alloys

An alloy is a homogeneous mixture of two or more metals, or a metal and a non-metal.

Alloying improves hardness, strength and resistance to corrosion.

Pure gold is very soft. It is mixed with copper or silver to make it suitable for jewellery.

Formula and Reaction Table for Class 10 Metals and Non-metals

Chapter 3 Metals and Non-metals Summary

Metals are generally lustrous, malleable, ductile, sonorous and good conductors. Non-metals usually show opposite properties, but graphite, iodine and diamond are important exceptions.

Metals react with oxygen to form metal oxides. Most metal oxides are basic, while aluminium oxide and zinc oxide are amphoteric.

Metals react with water, acids and salt solutions according to their reactivity. The reactivity series helps predict these reactions.

Metals lose electrons and non-metals gain electrons to form ionic compounds. Ionic compounds have high melting points and conduct electricity in molten or aqueous state.

Metals are extracted from ores using different methods based on their reactivity. Corrosion damages metals, while painting, galvanisation, electroplating and alloying help prevent it.

Useful Links for Class 10 Science