Schooling · Class 10 · Science · Metals and Non-metals · Chapter on a page
CBSE Class 10 · Science · NCERT Science
Metals and Non-metals: chapter on a page
A cut of Shishya's notes for this chapter: the first paragraph of the introduction and the key ideas, formulas and facts, common mistakes and quick revision lists, word for word. Nothing is added or reworded; the worked examples are left out (they are on the chapter page).
About the notes: Written by Shishya's AI on 26 Sept 2026 from the chapter's title and class level, in Shishya's own words — not a copy or summary of the textbook. Read the official chapter for the book's own text, activities and exercises.
This note's current text has no applied fact-check on record.
Mind map
Drawn from the same notes by a fixed rule (no AI): each label is the item's own words — its bold term, its label before a colon, a short formula as written, or its first words.
The mind map as a list
- Key ideas
- Metals are generally lustrous…
- Metals form positive ions (cations)…
- The reactivity series arranges…
- Ionic compounds are formed when…
- Extraction method depends on…
- Corrosion is the slow chemical…
- Alloys are homogeneous mixtures of…
- Formulas and facts
- Metal + Oxygen
- Metal + Water
- Metal + Dilute acid
- More reactive metal displaces less…
- Metal oxide + Carbon
- Copper, silver, gold and platinum…
- Amphoteric oxides react with both…
- Watch out for
- Thinking all metals react with…
- Writing hydrogen as H instead of H₂…
- Believing aluminium does not corrode…
- Confusing calcination and roasting
- Assuming alloys are compounds
What this chapter is about
This chapter explores the two broad categories into which most elements are classified: metals and non-metals. A Class 10 student learns to distinguish these categories based on their physical and chemical properties, and understands why they behave differently in reactions.
Key ideas
- Metals are generally lustrous, malleable, ductile, good conductors of heat and electricity, and have high melting points. Non-metals are generally brittle, dull, poor conductors, and have low melting points.
- Metals form positive ions (cations) by losing electrons; non-metals form negative ions (anions) by gaining electrons.
- The reactivity series arranges metals in order of decreasing reactivity: potassium, sodium, calcium, magnesium, aluminium, zinc, iron, lead, copper, mercury, silver, gold.
- Ionic compounds are formed when metals transfer electrons to non-metals. These compounds have high melting points, conduct electricity when molten or dissolved, and are usually soluble in water.
- Extraction method depends on reactivity: highly reactive metals (sodium, aluminium) need electrolysis; moderately reactive metals (zinc, iron) are reduced using carbon; least reactive metals (copper, silver) occur free or need simple heating.
- Corrosion is the slow chemical attack on metal surfaces by air, water or chemicals. Rusting of iron requires both oxygen and moisture.
- Alloys are homogeneous mixtures of metals (or metal with non-metal) made to improve properties. Examples: brass (copper + zinc), bronze (copper + tin), stainless steel (iron + chromium + nickel + carbon).
Formulas and facts to remember
- Metal + Oxygen → Metal oxide (basic oxide). Example: 2Mg + O₂ → 2MgO
- Metal + Water → Metal hydroxide + Hydrogen. Example: 2Na + 2H₂O → 2NaOH + H₂
- Metal + Dilute acid → Salt + Hydrogen. Example: Zn + 2HCl → ZnCl₂ + H₂
- More reactive metal displaces less reactive metal from its salt solution. Example: Fe + CuSO₄ → FeSO₄ + Cu
- Metal oxide + Carbon → Metal + Carbon monoxide (reduction). Example: ZnO + C → Zn + CO
- Copper, silver, gold and platinum are least reactive and do not react with dilute acids.
- Amphoteric oxides react with both acids and bases. Examples: aluminium oxide, zinc oxide.
- Rusting of iron: 4Fe + 3O₂ + 2xH₂O → 2Fe₂O₃·xH₂O (hydrated iron(III) oxide)
Common mistakes
- Thinking all metals react with dilute acids → Copper, silver and gold are below hydrogen in reactivity and do not displace hydrogen from acids.
- Writing hydrogen as H instead of H₂ in equations → Hydrogen exists as diatomic molecules; always write H₂.
- Believing aluminium does not corrode because it looks shiny → Aluminium corrodes quickly, but its oxide layer is protective and sticks to the surface, preventing further damage.
- Confusing calcination and roasting → Calcination heats ore in absence of air (for carbonates); roasting heats ore in presence of air (for sulphides).
- Assuming alloys are compounds → Alloys are mixtures, not compounds; their composition can vary.
Quick revision
- Metals lose electrons to form cations; non-metals gain electrons to form anions.
- Reactivity series: K, Na, Ca, Mg, Al, Zn, Fe, Pb, H, Cu, Hg, Ag, Au (decreasing order).
- More reactive metal displaces less reactive metal from its salt solution.
- Highly reactive metals: electrolysis; moderately reactive: carbon reduction; least reactive: simple heating or occur free.
- Rusting needs both oxygen and water; prevent by coating, galvanising or alloying.
- Ionic compounds have high melting points and conduct electricity only when molten or in solution.