Metals & Non-metals Topic Hub

Metals & Non-metals — Class 10 Notes

CBSE 2027 — dates, rules and official papers →
Chemistry · Ch 3Class 10 · CBSE 2026–27High weightage

Metals and Non-metals

What the board actually asks: Distinguish metals from non-metals by their physical properties (lustre, malleability, ductility, conductivity, sonority) and their chemical behaviour; write and balance the equations for metals reacting with oxygen, water, dilute acids and salt solutions; use the reactivity (activity) series to predict displacement and to choose the right extraction method; explain how metals occur as minerals and ores and how they are enriched, reduced (by carbon or electrolysis) and refined; show how an ionic (electrovalent) compound forms by the transfer of electrons and list its properties; and explain corrosion, its prevention and alloys. The balanced equation and activity-series reasoning carry most of the marks here.

NCERT VERBATIM sourced, word-for-wordAUTHORED LazyTopper teaching scaffolding
The Big Idea AUTHORED

Metals give up electrons - and that one habit explains all their chemistry.

Metals are lustrous, malleable, ductile conductors that tend to LOSE electrons and form positive ions, so they react with oxygen, water and acids and can push a less reactive metal out of its salt. Ordering metals by how readily they react gives the reactivity (activity) series, and that single list then tells us how each metal occurs in nature and how it must be extracted and refined. Non-metals behave in the opposite way - they gain electrons - so a metal and a non-metal together form an ionic compound. Most board marks here come from writing the correct balanced equation and reasoning with the activity series.

Formulae
Metal + Oxygen
(mostly basic; and are amphoteric)
Tip: Metal oxides are mostly basic; Al₂O₃, ZnO amphoteric.
Metal + Water
·
Tip: Reactivity decides cold water, hot water, steam, none.
Metal + Acid
Tip: Cu, Hg, Ag, Au do not release hydrogen.
Displacement
(A more reactive than B)
Tip: More reactive displaces less reactive.

Reactivity Series of Metals (Activity Series)

Activity series
K > Na > Ca > Mg > Al > Zn > Fe > Pb > [H] > Cu > Hg > Ag > Au
Tip: K Na Ca Mg Al Zn Fe Pb H Cu Hg Ag Au (top most reactive).
Roasting / Calcination
Roasting: sulphide ore + excess air oxide · Calcination: carbonate ore + limited air oxide
Tip: Roasting: sulphide ore, excess air. Calcination: carbonate ore, limited air.
Thermit reaction
(aluminium reduces iron(III) oxide; the iron is molten)
Tip: Aluminium reduces iron(III) oxide; used to join rails.
Physical Properties of Metals and Non-metals (with Exceptions)
Metals are lustrous, malleable, ductile, sonorous and good conductors of heat and electricity; non-metals are brittle and poor conductors. Exceptions: mercury is a liquid metal; gallium and caesium melt at very low temperatures; iodine is a lustrous non-metal; diamond is the hardest natural substance; graphite conducts electricity; the alkali metals (lithium, sodium, potassium) are so soft that they can be cut with a knife; lead and mercury are poor conductors of heat; non-metals are solids or gases except bromine, which is a liquid.
Properties of Ionic Compounds
Ionic compounds are solids, somewhat hard and brittle; they have high melting and boiling points; they dissolve in water; they conduct electricity in solution and in the molten state but not as solids.
Extraction of Metals by Position in the Reactivity Series
Top of the series (K, Na, Ca, Mg, Al): electrolysis of the molten chloride; the metal is deposited at the cathode. Middle (Zn, Fe, Pb): roast or calcine the ore to the oxide, then reduce with carbon. Bottom: mercury from cinnabar (HgS) and copper from Cu₂S are obtained by heating in air alone; silver and gold are found free.
Electrolytic Refining of Copper
The impure metal is made the anode and a thin strip of pure metal the cathode, in a solution of acidified copper sulphate. On passing current, pure copper deposits on the cathode.
Prevention of Corrosion
Painting, oiling, greasing, galvanising, chrome plating, anodising and making alloys. Galvanising is coating iron or steel with a thin layer of zinc; the article stays protected even if the zinc coating is broken.
Alloys
An alloy is a homogeneous mixture of two or more metals, or of a metal and a non-metal. Pure iron is soft; with a little carbon (about 0.05%) it becomes hard and strong; with nickel and chromium it gives stainless steel. Brass is copper and zinc; bronze is copper and tin. An alloy with mercury is an amalgam. The conductivity and melting point of an alloy are lower than those of the pure metals.
Metals and Water: Who Reacts How
Potassium and sodium react violently with cold water. Calcium reacts less violently. Magnesium reacts only with hot water. Aluminium, iron and zinc react only with steam, giving the metal oxide and hydrogen. Lead, copper, silver and gold do not react with water at all.
Formation of an Ionic Compound (NaCl)
A metal atom loses electrons to form a positive ion; a non-metal atom gains electrons to form a negative ion; the opposite charges attract. and , giving .

Shortcuts & memory tricks →

Definitions the board rewards NCERT VERBATIM

State these in NCERT’s exact words

Metallic lustre
NCERT verbatim — memorise this exact wording· Ch 3,
“Metals, in their pure state, have a shining surface. This property is called metallic lustre.”
What it means: The natural shine of a clean metal surface - which is why freshly rubbed iron or copper looks bright.
Malleability
NCERT verbatim — memorise this exact wording· Ch 3,
“Some metals can be beaten into thin sheets. This property is called malleability.”
What it means: The ability to be hammered into thin sheets without breaking - gold and silver are the most malleable metals.
Ductility
NCERT verbatim — memorise this exact wording· Ch 3,
“The ability of metals to be drawn into thin wires is called ductility.”
What it means: The ability to be pulled out into thin wires - gold is the most ductile metal.
Amphoteric oxides
NCERT verbatim — memorise this exact wording· Ch 3,
“Such metal oxides which react with both acids as well as bases to produce salts and water are known as amphoteric oxides.”
What it means: Oxides that behave both as a base (with acids) and as an acid (with bases) - aluminium oxide and zinc oxide are the standard examples.
Reactivity (activity) series
NCERT verbatim — memorise this exact wording· Ch 3,
“The reactivity series is a list of metals arranged in the order of their decreasing activities.”
What it means: The ranking K > Na > Ca > Mg > Al > Zn > Fe > Pb > [H] > Cu > Hg > Ag > Au - a more reactive metal displaces a less reactive one.
Ionic (electrovalent) compounds
NCERT verbatim — memorise this exact wording· Ch 3,
“The compounds formed in this manner by the transfer of electrons from a metal to a non-metal are known as ionic compounds or electrovalent compounds.”
What it means: Compounds like NaCl or made when a metal donates electrons to a non-metal, giving oppositely charged ions held by strong electrostatic attraction.
Minerals
NCERT verbatim — memorise this exact wording· Ch 3,
“The elements or compounds, which occur naturally in the earth's crust, are known as minerals.”
What it means: Naturally occurring elements or compounds in the earth's crust that contain a metal.
Ores
NCERT verbatim — memorise this exact wording· Ch 3,
“At some places, minerals contain a very high percentage of a particular metal and the metal can be profitably extracted from it. These minerals are called ores.”
What it means: The minerals from which a metal can be extracted profitably - every ore is a mineral, but not every mineral is rich enough to be an ore.
Metallurgy
NCERT verbatim — memorise this exact wording· Ch 3,
“The extraction of metals from their ores and then refining them for use is known as metallurgy.”
What it means: The whole process of getting a pure, usable metal from its ore - enrichment, then reduction, then refining.
Corrosion
NCERT verbatim — memorise this exact wording· Ch 3,
“The surface of some metals, such as iron, is corroded when they are exposed to moist air for a long period of time. This phenomenon is known as corrosion.”
What it means: The slow eating-away of a metal surface by air and moisture - the rusting of iron is the everyday example, and it needs BOTH air and water.
Alloy
NCERT verbatim — memorise this exact wording· Ch 3,
“An alloy is a homogeneous mixture of two or more metals, or a metal and a non-metal.”
What it means: A uniform mixture made by melting a base metal and dissolving other elements in it - e.g. steel (iron + carbon), brass, bronze, solder.
Key terms — NCERT verbatim (state word-for-word)
Sonorous
The metals that produce a sound on striking a hard surface are said to be sonorous. (Ch 3, )
Allotrope
Carbon is a non-metal that can exist in different forms. Each form is called an allotrope. (Ch 3, )
Gangue
Ores mined from the earth are usually contaminated with large amounts of impurities such as soil, sand, etc., called gangue. (Ch 3, )
Roasting
The sulphide ores are converted into oxides by heating strongly in the presence of excess air. This process is known as roasting. (Ch 3, )
Calcination
The carbonate ores are changed into oxides by heating strongly in limited air. This process is known as calcination. (Ch 3, )
Amalgam
If one of the metals is mercury, then the alloy is known as an amalgam. (Ch 3, )
Must-know concepts AUTHORED FRAMING

…and where they’re tested

Physical properties of metals
Metals in their pure state have a shining surface (metallic lustre), are generally hard, and are malleable (beaten into sheets) and ductile (drawn into wires). They are good conductors of heat and electricity, have high melting points, are sonorous, and are solids at room temperature - mercury is the one liquid exception. Silver and copper are the best conductors of heat.
1-mark: name a metal that is liquid / can be cut with a knife / is the best conductor; or explain malleable and ductile.
Physical properties of non-metals
Non-metals show properties opposite to metals: they are neither malleable nor ductile and are bad conductors of heat and electricity. There are exceptions worth remembering - iodine is a lustrous non-metal, graphite (an allotrope of carbon) conducts electricity, and diamond (another allotrope) is the hardest natural substance. Non-metals are solids or gases, except bromine which is a liquid.
2-mark: state exceptions (iodine lustrous, graphite conducts) and differentiate metals from non-metals.
Reaction of metals with oxygen
Almost all metals combine with oxygen to form metal oxides, which are generally basic. Different metals react at different rates: sodium and potassium catch fire in air (so they are kept in kerosene), while silver and gold do not react even at high temperatures. Aluminium oxide and zinc oxide are amphoteric - they react with both acids and bases. Some oxides (sodium oxide, potassium oxide) dissolve in water to form alkalis.
3-mark: write equations for metals burning in oxygen; define amphoteric oxides with two examples.
Reaction of metals with water and acids
Metals react with water to give a metal oxide (or hydroxide) and hydrogen, but not all metals react. Potassium and sodium react violently with cold water; calcium reacts less violently and floats; magnesium reacts with hot water; aluminium, iron and zinc react only with steam; lead, copper, silver and gold do not react at all. With dilute acids the reactivity order is Mg > Al > Zn > Fe, while copper gives no reaction. Hydrogen is usually not evolved with nitric acid, because is a strong oxidising agent.
3-mark: write equations for iron with steam and calcium/potassium with water; explain why sodium is stored in kerosene.
Reactivity series and displacement
Arranging metals in decreasing order of reactivity gives the activity series (K at the top, Au at the bottom). Displacement reactions give the clearest evidence of reactivity: if metal A displaces metal B from its salt solution, A is more reactive than B. For example, an iron nail placed in copper sulphate solution displaces copper, whereas a copper wire in iron sulphate solution shows no reaction - so iron is more reactive than copper.
3-mark: tabulated reactivity comparison (metals A, B, C, D); predict displacement and arrange in decreasing reactivity.
Ionic (electrovalent) compounds and their properties
When a metal transfers electrons to a non-metal, oppositely charged ions form and are held by strong electrostatic forces - for example sodium loses one electron to chlorine to give and , which aggregate as sodium chloride. Such ionic compounds are solids that are hard and brittle, have high melting and boiling points, are generally soluble in water but not in petrol or kerosene, and conduct electricity in the molten or aqueous state (ions free to move) but not as solids.
NCERT Fig 3.5Formation of sodium chloride.
Sodium (2,8,1) loses one electron to become the sodium cation (2,8); chlorine (2,8,7) gains that electron to become the chloride anion (2,8,8). The oppositely charged ions attract to form the ionic compound sodium chloride (electron-dot / cross diagram shown).
3-mark: show the formation of or MgO by electron transfer; give the ions present; explain the high melting point.
Occurrence and extraction of metals
Metals occur either free (gold, silver, platinum, copper) or as compounds; the naturally occurring forms are minerals, and a mineral rich enough to extract the metal profitably is an ore. Ores are first enriched to remove the gangue. The extraction method follows the activity series: metals high up (K, Na, Ca, Mg, Al) are obtained by electrolysis of their molten compounds; middle metals (Zn, Fe, Pb, Cu) have their sulphide/carbonate ores converted to oxides by roasting or calcination and then reduced to metal with carbon; metals low down are found native or obtained by heating alone.
NCERT Fig 3.10Steps involved in the extraction of metals from ores.
The extraction route branches on the activity series: high-reactivity metals electrolysis of molten ore pure metal; medium-reactivity metals carbonate ore (calcination) or sulphide ore (roasting) oxide of metal reduction to metal purification; low-reactivity metals sulphide ores roasting metal refining.
3-mark: define mineral, ore, gangue; state the chemical process used to obtain a metal from its oxide.
Refining of metals
The metals produced by reduction are impure and are purified, most commonly by electrolytic refining. The impure metal is made the anode, a thin strip of pure metal the cathode, and a solution of the metal's salt the electrolyte; on passing current, pure metal dissolves from the anode and deposits on the cathode. Soluble impurities stay in solution while insoluble impurities collect below the anode as anode mud. Copper, zinc, tin, nickel, silver and gold are all refined this way.
NCERT Fig 3.12Electrolytic refining of copper.
The electrolyte is a solution of acidified copper sulphate; the anode is impure copper and the cathode is a strip of pure copper. On passing current, pure copper dissolves from the anode and is deposited on the cathode, while insoluble impurities settle below the anode as anode mud. Labels: Key, Cathode, Anode, Acidified copper sulphate solution, , Tank, Impurities (anode mud).
3-mark: in the electrolytic refining of a metal M, state what is taken as anode, cathode and electrolyte.
Corrosion, its prevention and alloys
Corrosion is the attack on a metal by moisture and acids around it - iron rusts, silver blackens, copper gains a green coat. Activity 3.14 shows iron rusts only when BOTH air and water are present. Rusting is prevented by painting, oiling, greasing, galvanising (a zinc coat), chrome plating, anodising or alloying. Alloying also improves a metal's properties: iron mixed with a little carbon becomes hard steel, and iron with nickel and chromium becomes rust-resistant stainless steel. If mercury is one of the metals, the alloy is an amalgam.
NCERT Fig 3.13Investigating the conditions under which iron rusts (Activity 3.14).
Three test tubes with clean iron nails: A has both air and water (nails rust); B has boiled distilled water under a layer of oil so no air is dissolved (no rust); C has dry air over anhydrous calcium chloride, a drying agent (no rust). Rusting therefore needs BOTH air and water. Labels: A/B/C, Air, Air, Dry air, Rusty iron nails, Water, Layer of oil.
2-mark: state two ways to prevent rusting; explain the conditions needed for iron to rust; what are alloys.
Worked examples — real solved problems NCERT VERBATIM

Solved exactly as the source does them

Every problem is a real sourced item, quoted verbatim with its page; the step-by-step decoding and mark-logic are LazyTopper-authored coaching.

Ch 3,
“[authored prompt] Copper and aluminium are each heated strongly in air. Write the balanced equation for each reaction and state the nature of the oxides formed.”
Copper.Copper heated in air combines with oxygen to form a black layer of copper(II) oxide.
Concept: metal + oxygen metal oxide
1 mark
Aluminium.Aluminium combines with oxygen to form aluminium oxide.
1 mark
Nature of the oxides.Metal oxides are generally basic; but aluminium oxide is amphoteric, reacting with both acids and bases.Concept: basic vs amphoteric oxide
1 mark
Mark-scheme logic (authored): 3-mark: the balanced equation for copper (1) + the balanced equation for aluminium (1) + stating the oxides are basic, with amphoteric (1). Balance oxygen first, then the metal.
Ch 3,
“[authored prompt] Sodium, calcium and iron are each brought into contact with water. Write a balanced equation in each case and state which metal reacts with cold water and which reacts only with steam.”
Ch 3,
“[authored prompt] Magnesium, zinc and copper are each added to dilute hydrochloric acid (Activity 3.11). Write the equation for the reaction of zinc, arrange Mg, Al, Zn and Fe in decreasing order of reactivity, and explain the observation with copper.”
Ch 3,
“[authored prompt] In Activity 3.12 an iron nail is placed in copper sulphate solution and a copper wire in iron sulphate solution. In which test tube does a reaction occur? Write the balanced equation and name the type of reaction.”
Ch 3,
“[authored prompt] The thermit reaction between iron(III) oxide and aluminium is used to join railway tracks. Write the balanced equation, state which substance is oxidised and which is reduced, and explain why the iron is produced in the molten state.”
Ch 3,
“[authored prompt] Zinc occurs as zinc sulphide and as zinc carbonate. Write the balanced equation for converting each ore to zinc oxide, name the two processes, and give the equation for reducing zinc oxide to zinc metal.”
Problem-solving strategies AUTHORED
Metal or non-metal?Test for lustre, malleability/ductility and conductivity - metals shine, bend and conduct. Keep the exceptions ready: mercury is a liquid metal, iodine is a lustrous non-metal, and graphite (carbon) conducts electricity.
Which metal reacts?Read down the activity series. K and Na react even with cold water, Mg with hot water, Al/Fe/Zn only with steam, and Cu/Ag/Au not with water at all. With dilute acids the order is Mg > Al > Zn > Fe, and copper does not react.
Which extraction method?Tie the method to the series: top metals (K, Na, Ca, Mg, Al) electrolysis of the molten compound; middle metals (Zn, Fe, Pb, Cu) roast or calcine the ore to the oxide, then reduce with carbon; bottom metals (Ag, Au) found native or reduced by heat alone.
Roasting or calcination?Sulphide ore heated in EXCESS air is roasting; carbonate ore heated in LIMITED air is calcination. Both give the metal oxide, which is the easy form to reduce.
Oxidised or reduced?Follow the oxygen. The substance that GAINS oxygen is oxidised; the one that LOSES oxygen is reduced. In the thermit reaction aluminium is oxidised and iron(III) oxide is reduced.
Common mistakes that cost marks

Where students lose easy marks

Swapping roasting and calcination. Roasting = sulphide ore + excess air; calcination = carbonate ore + limited air.
Saying metals form acidic oxides. Metals form BASIC oxides; aluminium oxide and zinc oxide are the amphoteric exceptions. Non-metals form acidic or neutral oxides.
Claiming all metals react with water. Lead, copper, silver and gold do not react with water at all, and aluminium, iron and zinc react only with steam, not with cold or hot water.
Reversing the electrodes. In electrolytic reduction and refining the metal is deposited at the cathode (negative electrode); chlorine is liberated at the anode (positive electrode), where the impure metal dissolves.
Expecting hydrogen gas when a metal reacts with nitric acid. is a strong oxidising agent, so it usually oxidises the hydrogen to water and no is evolved (very dilute with Mg or Mn is the exception).
Thinking ionic compounds conduct as solids. They conduct only in the molten or aqueous state, when the ions are free to move; in the solid state the ions are locked in a rigid structure.
Formulae
Metal + Oxygen
(mostly basic; and are amphoteric)
Tip: Metal oxides are mostly basic; Al₂O₃, ZnO amphoteric.
Metal + Water
·
Tip: Reactivity decides cold water, hot water, steam, none.
Metal + Acid
Tip: Cu, Hg, Ag, Au do not release hydrogen.
Displacement
(A more reactive than B)
Tip: More reactive displaces less reactive.

Reactivity Series of Metals (Activity Series)

Activity series
K > Na > Ca > Mg > Al > Zn > Fe > Pb > [H] > Cu > Hg > Ag > Au
Tip: K Na Ca Mg Al Zn Fe Pb H Cu Hg Ag Au (top most reactive).
Roasting / Calcination
Roasting: sulphide ore + excess air oxide · Calcination: carbonate ore + limited air oxide
Tip: Roasting: sulphide ore, excess air. Calcination: carbonate ore, limited air.
Thermit reaction
(aluminium reduces iron(III) oxide; the iron is molten)
Tip: Aluminium reduces iron(III) oxide; used to join rails.
Physical Properties of Metals and Non-metals (with Exceptions)
Metals are lustrous, malleable, ductile, sonorous and good conductors of heat and electricity; non-metals are brittle and poor conductors. Exceptions: mercury is a liquid metal; gallium and caesium melt at very low temperatures; iodine is a lustrous non-metal; diamond is the hardest natural substance; graphite conducts electricity; the alkali metals (lithium, sodium, potassium) are so soft that they can be cut with a knife; lead and mercury are poor conductors of heat; non-metals are solids or gases except bromine, which is a liquid.
Properties of Ionic Compounds
Ionic compounds are solids, somewhat hard and brittle; they have high melting and boiling points; they dissolve in water; they conduct electricity in solution and in the molten state but not as solids.
Extraction of Metals by Position in the Reactivity Series
Top of the series (K, Na, Ca, Mg, Al): electrolysis of the molten chloride; the metal is deposited at the cathode. Middle (Zn, Fe, Pb): roast or calcine the ore to the oxide, then reduce with carbon. Bottom: mercury from cinnabar (HgS) and copper from Cu₂S are obtained by heating in air alone; silver and gold are found free.
Electrolytic Refining of Copper
The impure metal is made the anode and a thin strip of pure metal the cathode, in a solution of acidified copper sulphate. On passing current, pure copper deposits on the cathode.
Prevention of Corrosion
Painting, oiling, greasing, galvanising, chrome plating, anodising and making alloys. Galvanising is coating iron or steel with a thin layer of zinc; the article stays protected even if the zinc coating is broken.
Alloys
An alloy is a homogeneous mixture of two or more metals, or of a metal and a non-metal. Pure iron is soft; with a little carbon (about 0.05%) it becomes hard and strong; with nickel and chromium it gives stainless steel. Brass is copper and zinc; bronze is copper and tin. An alloy with mercury is an amalgam. The conductivity and melting point of an alloy are lower than those of the pure metals.
Metals and Water: Who Reacts How
Potassium and sodium react violently with cold water. Calcium reacts less violently. Magnesium reacts only with hot water. Aluminium, iron and zinc react only with steam, giving the metal oxide and hydrogen. Lead, copper, silver and gold do not react with water at all.
Formation of an Ionic Compound (NaCl)
A metal atom loses electrons to form a positive ion; a non-metal atom gains electrons to form a negative ion; the opposite charges attract. and , giving .
Shortcuts & Tricks
A metal displaces any metal BELOW it in the reactivity series from its salt solution.
MCQ / check only: don't write this as working
Only metals above hydrogen displace H₂ from dilute acids; Cu, Hg, Ag, Au do not.
MCQ / check only: don't write this as working
Top: electrolysis. Middle: carbon reduction (after roasting/calcination). Bottom: heat alone.
Safe in written answers
Metal oxides are basic; non-metal oxides acidic; aluminium and zinc oxides are amphoteric.
MCQ / check only: don't write this as working
Sulphide ore ⇒ roasting (excess air). Carbonate ore ⇒ calcination (limited air).
Safe in written answers
Refining: impure metal at the anode, pure metal at the cathode.
Safe in written answers
Memory Tricks

Reactivity Series Trick (K to Au)

Kal Naani Car Mein Aloo Zeera Fry Paka Hain, Cupboard Hi Agle Aunty.
Most reactive → least reactive, 13 members, hydrogen in position 9. Kal = K · Naani = Na · Car = Ca · Mein = Mg · Aloo = Al · Zeera = Zn · Fry = Fe · Paka = Pb · Hain = H (hydrogen) · Cupboard = Cu · Hi = Hg · Agle = Ag · Aunty = Au. The five words that share a first letter (Ca, Al, Cu, Ag, Au) now carry the whole symbol (Car, Aloo, Cupboard, Agle, Aunty).
Anode = Ashuddh, Cathode = Chokha.
Electrolytic refining. anode: impure metal · cathode: pure metal strip.
K, Na bhadak jaate; Ca kam bhadakta aur tairta hai; Mg sirf garam paani; Al-Zn-Fe sirf bhaap; Pb se Au kuch nahi.
Metals and water. K, Na violent · Ca less violent · Mg hot water · Al, Fe, Zn steam · Pb, Cu, Ag, Au nothing.
Upar: Bijli. Beech: Bhatti. Neeche: Aanch.
Extraction method by position. top: electrolysis · middle: carbon reduction (furnace) · bottom: heat alone (Hg, Cu) or found free (Ag, Au).
Metal ka oxide Base; non-metal ka oxide Acid; Aluminium-Zinc dono taraf.
Nature of oxides. basic · acidic · amphoteric (Al₂O₃, ZnO).
Pintu Oye Gaya Gaon Chhodke Aaj Aaya.
Seven prevention methods, NCERT order. P = painting · O = oiling · G = greasing · G = galvanising · C = chrome plating · A = anodising · A = alloying (making alloys).
Metal de, non-metal le.
Ionic bond formation. metal loses electrons (cation); non-metal gains (anion).
Pital = Cu + Zn; Kaansa = Cu + Sn.
Brass and bronze. brass: copper + zinc · bronze: copper + tin.
Mindmap
      • Metals: lustrous, malleable, ductile, sonorous
      • Metals: good conductors, high m.p., solids (except mercury)
      • Non-metals: brittle, poor conductors (graphite conducts)
      • Exceptions: mercury liquid, iodine lustrous, diamond hardest
      • With oxygen metal oxide (basic; /ZnO amphoteric)
      • With water oxide/hydroxide + (Na/K violent, Al/Fe steam)
      • With dilute acid salt + (Mg > Al > Zn > Fe)
      • With salt solution displacement
      • K > Na > Ca > Mg > Al > Zn > Fe > Pb > [H] > Cu > Hg > Ag > Au
      • More reactive metal displaces less reactive one
      • Above hydrogen displaces from dilute acids
      • Metal transfers electrons to non-metal ()
      • High melting and boiling points; hard, brittle solids
      • Soluble in water, not in petrol/kerosene
      • Conduct in molten / aqueous state, not as solids
      • Minerals and ores; gangue removed by enrichment
      • Top metals electrolysis of molten compound
      • Middle metals roasting/calcination then reduction with carbon
      • Refining electrolytic refining (anode mud)
      • Rusting of iron needs both air and water
      • Prevention: painting, oiling, galvanising, alloying
      • Alloys: steel, stainless steel, brass, bronze, solder
      • Amalgam = alloy containing mercury

For Chemistry the third tab holds the chapter's key balanced equations - the formal core you must be able to reproduce, grouped by the way metals react and by how they are extracted. Every equation is a real NCERT Ch 3 reaction; the condition (Heat, Electricity) sits above or beside the arrow.

Metal + oxygen (general)
Metal + Oxygen Metal oxide
Almost all metals combine with oxygen to form metal oxides (mostly basic)
Copper burnt in air
Copper heated in air forms a black layer of copper(II) oxide
Aluminium burnt in air
Aluminium combines with oxygen to form aluminium oxide
Amphoteric oxide with an acid
Aluminium oxide (amphoteric) behaves as a base towards acid
Amphoteric oxide with a base
Aluminium oxide (amphoteric) behaves as an acid towards base; gives sodium aluminate
Soluble metal oxide alkali
Sodium oxide dissolves in water to form an alkali
Sodium + cold water
Violent and exothermic; the evolved hydrogen catches fire
Calcium + water
Less violent; calcium floats on the hydrogen bubbles
Iron + steam
Iron reacts only with steam, not with cold or hot water
Metal + dilute acid (general)
Metal + Dilute acid Salt + Hydrogen
Reactivity Mg > Al > Zn > Fe; copper does not react with dilute HCl
Displacement (general)
Metal A + Salt solution of B Salt solution of A + Metal B
A more reactive metal (A) displaces a less reactive one (B) from its salt
Roasting - zinc sulphide
Sulphide ore heated in excess air is converted to the oxide (roasting)
Calcination - zinc carbonate
Carbonate ore heated in limited air is converted to the oxide (calcination)
Reduction by carbon - zinc oxide
The metal oxide is reduced to metal by heating with carbon
Extraction of mercury (low reactivity)
;
Cinnabar is roasted to the oxide, which is then reduced to mercury by heat alone
Thermit reaction
Highly exothermic; molten iron produced is used to join railway tracks
Electrolytic reduction - at cathode
Reactive metals obtained by electrolysis of the molten chloride; metal deposits at the cathode
Electrolytic reduction - at anode
Chlorine is liberated at the anode
Formation of an ionic compound
; ;
Electron transfer from the metal to the non-metal gives oppositely charged ions

3 competency questions from the CBSE board pattern, with the full step-marked solution for each — the marks are shown per step, as the official scheme awards them.

1 markSection A

Galvanisation is a process of coating iron articles with a layer of zinc to prevent the iron from rusting. The iron is protected even if the zinc coating is scratched and iron is exposed. Which of the following is true about how zinc prevents the rusting of iron? P) A galvanised iron article does not undergo oxidation. Q) The zinc coating prevents contact of iron with air. R) Zinc undergoes corrosion more easily than iron.

  1. (A) only P
  2. (B) only Q
  3. (C) only P and Q
  4. (D) only Q and R
Step-marked solution
  1. [0.5 mark] Q correct: zinc coating blocks air/moisture from iron surface.
  2. [0.5 mark] R correct: zinc is more reactive than iron (sacrificial anode), so it corrodes preferentially. P false: oxidation still occurs but on zinc, not iron.
1 markSection A

Metals are lustrous and shine especially when their freshly cut surfaces are exposed. Salma cut pieces and compared the lustre of the freshly cut surfaces of: aluminium, sodium, copper, iron. The freshly cut surface of which of these metals is likely to lose its lustre first on exposure to air?

  1. (A) aluminium
  2. (B) sodium
  3. (C) copper
  4. (D) iron
Step-marked solution
  1. [1 mark] Sodium is the most reactive among the four (highest in reactivity series). It rapidly reacts with O2 and moisture in air, forming a dull oxide layer fastest. (Sodium is stored under kerosene to prevent this.)
1 markSection A

Assertion (A): Zinc oxide can be reduced to zinc metal on heating with carbon. Reason (R): Carbon is less reactive than zinc.

  1. (A) Both A and R are true, and R is the correct explanation of A.
  2. (B) Both A and R are true, and R is not the correct explanation of A.
  3. (C) A is true but R is false.
  4. (D) A is false but R is true.
Step-marked solution
  1. [0.5 mark] A is true: ZnO + C → Zn + CO (carbon reduces ZnO to Zn at high temperature).
  2. [0.5 mark] R is false: carbon is MORE reactive than zinc in the reactivity context — that's why it can reduce ZnO.
Practise Metals and Non-metals competency questions

Read NCERT Chapter 3 on LazyTopper (jesc103)

Official NCERT chapter PDF (jesc103) — ncert.nic.in

Sources: NCERT 2026-27 (tap to view)
Source ledger PROVENANCE

Source edition: NCERT Reprint 2026-27, Class 10 Science, Ch 3. One row per sourced item — every verbatim, example and NCERT figure traces to its page.

ItemTypeSource
Metallic lustreverbatimNCERT 2026-27 Ch3
MalleabilityverbatimNCERT 2026-27 Ch3
DuctilityverbatimNCERT 2026-27 Ch3
Amphoteric oxidesverbatimNCERT 2026-27 Ch3
Reactivity (activity) seriesverbatimNCERT 2026-27 Ch3
Ionic (electrovalent) compoundsverbatimNCERT 2026-27 Ch3
MineralsverbatimNCERT 2026-27 Ch3
OresverbatimNCERT 2026-27 Ch3
MetallurgyverbatimNCERT 2026-27 Ch3
CorrosionverbatimNCERT 2026-27 Ch3
AlloyverbatimNCERT 2026-27 Ch3
SonorousverbatimNCERT 2026-27 Ch3
AllotropeverbatimNCERT 2026-27 Ch3
GangueverbatimNCERT 2026-27 Ch3
RoastingverbatimNCERT 2026-27 Ch3
CalcinationverbatimNCERT 2026-27 Ch3
AmalgamverbatimNCERT 2026-27 Ch3
Metals burnt in air (metal + oxygen)exampleNCERT 2026-27 Ch3 Eqs. on
Metals react with water / steamexampleNCERT 2026-27 Ch3 Eqs. on
Metals react with dilute acid + reactivity orderexampleNCERT 2026-27 Ch3 Activity 3.11,
Displacement (metal + salt solution)exampleNCERT 2026-27 Ch3 Activity 3.12,
Thermit reaction (reduction / redox in extraction)exampleNCERT 2026-27 Ch3 Eq. on
Extraction of zinc from its oresexampleNCERT 2026-27 Ch3 Eqs. on
NCERT Fig 3.10figureNCERT 2026-27 Ch3 Fig 3.10
NCERT Fig 3.12figureNCERT 2026-27 Ch3 Fig 3.12
NCERT Fig 3.13figureNCERT 2026-27 Ch3 Fig 3.13
NCERT Fig 3.5figureNCERT 2026-27 Ch3 Fig 3.5

Metals and Non-metals · spec-rendered note · NCERT Reprint 2026-27, Class 10 Science, Ch 3

Practise writing answers the way examiners mark them → Guide