Metals and Non-metals
INTRODUCTION:
Table of Contents
Physical Properties: The Visible Differences
The first step in differentiating metals from non-metals lies in their
observable physical characteristics.
Metals
Metals are typically hard (except sodium and potassium), have a characteristic metallic lustre, and are good conductors of heat and electricity. They are malleable (can be hammered into sheets) and ductile (can be drawn into wires). They are generally solid at room temperature (except mercury) and have high density and melting points.
Non-Metals
Non-metals are generally soft (except diamond), lack lustre, and are poor conductors of heat and electricity. They are neither malleable nor ductile but are brittle. They exist in all three states: solids (sulphur), liquids (bromine), and gases (oxygen).
Quick Comparison Table: Physical Properties
|
Property |
Metals |
Non-metals |
|
Appearance |
Usually shiny (lustrous) |
Usually dull |
|
Malleability |
Yes |
No (brittle) |
|
Ductility |
Yes |
No |
|
Heat & electricity |
Good conductors |
Poor conductors |
|
Sonorous |
Yes |
No |
|
State at room temp |
Mostly solids (Hg is liquid) |
Solids/gases (Br is liquid) |
Important exceptions (very common in exams)
· Mercury is a metal but liquid at room temperature.
· Gallium and caesium have very low melting points (can melt on the palm).
· Iodine is a non-metal but lustrous.
· Carbon allotropes: Diamond is extremely hard; graphite conducts electricity.
Chemical Properties
This is where things get
interesting! The chemical behavior of metals and non-metals explains why
they're used in specific ways.
Metals + oxygen (burning in air)
Almost all metals combine with oxygen to form metal oxides. Many metal oxides are basic in nature.
Example: When copper is heated in air, it forms black copper(II) oxide.
Equation: 2Cu + O₂ → 2CuO
Example: Aluminium forms aluminium oxide.
Equation: 4Al + 3O₂ → 2Al₂O₃
Amphoteric oxides (very important)
Some metal oxides behave as both acids and bases. NCERT specifically mentions aluminium oxide and zinc oxide as amphoteric.
· Aluminium oxide reacts with acids and also with bases to form salts and water.
· Equation: Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O
Al₂O₃ + 2NaOH → 2NaAlO₂ + H₂O (sodium aluminate)
Why sodium and potassium are stored in kerosene
Sodium and potassium react so vigorously with oxygen (and also with water) that they can catch fire if kept in the open, so they are stored in kerosene oil for safety.
Protective oxide layer and anodising
Metals like magnesium, aluminium, zinc, and lead get a thin oxide layer at room temperature that protects them from further oxidation. NCERT also explains anodising, where aluminium is given a thicker oxide layer to improve corrosion resistance and allow dyeing.
Metals + water
In words: Metals react with water to form a metal oxide (or metal hydroxide) and hydrogen gas, but all metals do not react with water.
General idea from NCERT:
Metal + water → metal oxide + hydrogen
Metal oxide + water → metal hydroxide
Highly reactive metals (K, Na)
Potassium and sodium react violently with cold water, and the reaction is so exothermic that the hydrogen gas catches fire.
Equations:
2K + 2H₂O →
2KOH + H₂ + heat
2Na + 2H₂O →
2NaOH + H₂ + heat
Calcium
Calcium reacts with water less violently and starts floating because hydrogen bubbles stick to its surface.
Equation: Ca + 2H₂O → Ca(OH)₂ + H₂
Magnesium
Magnesium does not react with cold water; it reacts with hot water and can also react with steam. It may float due to hydrogen bubbles.
Aluminium, iron, zinc
These metals do not react with cold/hot water but react with steam to form metal oxide and hydrogen.
Equations:
2Al + 3H₂O
(steam) → Al₂O₃
+ 3H₂
3Fe + 4H₂O
(steam) → Fe₃O₄
+ 4H₂
Lead, copper, silver, gold
These
metals do not react with water at all.
Chapter 2 Science : Acids, Bases & Salts. (Complete Notes: Download PDF)
Metals + acids
Metals react with dilute acids to form salt + hydrogen gas, but not all metals react equally.
General equation:
Metal + dilute acid → salt + hydrogen
Special point (nitric acid): Hydrogen gas is generally not evolved with nitric acid because HNO₃ is a strong oxidising agent; however Mg and Mn can produce H₂ with very dilute HNO₃.
Metals + salt solutions (displacement)
A more reactive metal can displace a less reactive metal from its salt solution.
General
form:
Metal A + salt solution of B → salt solution of A + metal B
This concept is used to build the reactivity series
.The Reactivity Series
The reactivity series is a list of metals arranged in decreasing reactivity.
Memorize this series:
Potassium > Sodium > Calcium > Magnesium > Aluminium > Zinc > Iron > Tin > Lead > [Hydrogen] > Copper > Mercury > Silver > Gold
Helpful Mnemonic: "Please Stop Calling Me A Zebra I Think Lead Halogens Can Make Silver Gold"
Key Points:
· Metals above hydrogen can displace hydrogen from acids/water.
· Metals higher in the series can displace lower metals from solutions.
· This series determines the extraction method of metals.
How metals and non-metals react (ionic bonding)
Metals generally lose electrons and form positive ions; non-metals gain electrons and form negative ions.
Example: Sodium chloride formation (concept)
Sodium loses one electron to become Na⁺ and chlorine gains one electron to become Cl⁻; opposite charges attract and form NaCl as an ionic compound (as ion aggregates, not molecules).
Ionic (electrovalent) compounds
Compounds formed by transfer of electrons are called ionic/electrovalent compounds.
Properties of ionic compounds:
· Hard solids and brittle due to strong attraction between ions.
· High melting/boiling points because lots of energy is needed to break attractions.
· Generally soluble in water and insoluble in kerosene/petrol.
· Conduct electricity in molten state and in aqueous solution, not in solid state (ions can move only when free).
Complete Notes on Nationalism in India (First World War, Khilafat & Non-Cooperation Movement).
Extraction of Metals: From Ores to Pure Metals
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The extraction process depends
entirely on the metal's position in the reactivity series.
|
Metal's Position |
Extraction Method |
Examples |
|
Top (K, Na, Ca, Mg, Al) |
Electrolytic Reduction (Electrolysis). |
Aluminum from bauxite (Al₂O₃) |
|
Middle (Zn, Fe, Pb) |
Reduction using Carbon (Smelting). |
Iron from haematite (Fe₂O₃) |
|
Bottom (Cu, Hg, Ag) |
Reduction by Heating Alone. |
Mercury from cinnabar (HgS) |
Important Terms:
· Ore: Naturally occurring mineral from which metal can be extracted profitably.
· Enrichment/Concentration: Removing impurities (gangue) from ore.
· Roasting/Calcination: Heating ore in presence/absence of air.
· Reduction: Extracting metal from its oxide.
· Refining: Purifying the extracted metal (e.g., electrolytic refining of copper).
Class 10 Science Chapter-1: Chemical Reactions and Equations.
Corrosion: The Enemy of Metals
Corrosion is the gradual destruction of metals by chemical reactions with their environment (mainly oxygen and moisture).
· Iron: Rusting (forms hydrated ferric oxide - Fe₂O₃.xH₂O)
· Copper: Green coating (basic copper carbonate)
· Silver: Black coating (silver sulphide)
Prevention Methods:
1. Galvanization: Coating with zinc (e.g., iron buckets)
2. Alloying: Making stainless steel
3. Painting/Greasing: Creating barrier layer
4. Electroplating: Coating with another metal (e.g., chromium plating)
Alloys
An alloy is a homogeneous mixture of
two or more metals, or a metal and a non-metal. Alloys often have lower
electrical conductivity and lower melting points than pure metals; solder (Pb +
Sn) has low melting point and is used for welding electrical wires; brass and
bronze are not as good conductors as copper.
Why make alloys?
· Increases hardness and strength
· Lowers melting point
· Enhances resistance to corrosion
· Improves appearance
MCQs PYQ
Q1. Oxides
of aluminium and zinc are:
(a) Acidic
(b) Basic
(c) Amphoteric
(d) Neutral
Answer: (c) Amphoteric. (CBSE
2024)
Q2. The metals found both in free state and combined state
are:
(a) Gold and platinum
(b) Sodium and potassium
(c) Copper and silver
(d) Aluminium and magnesium
Answer: (c) Copper and silver. (CBSE 2024)
Q3. A metal ‘X’
is used in thermite process. When X is burnt in air it gives an amphoteric
oxide ‘Y’. ‘X’ and ‘Y’ are respectively:
(a) Fe and Fe₂O₃
(b) Al and Al₂O₃
(c) Fe and Fe₃O₄
(d) Al and Al₃O₄
Answer: (b) Al and Al₂O₃. (CBSE 2023)
Q4. Assertion
(A): A piece of zinc metal gets reddish-brown coating when kept
in copper sulphate solution for some time.
Reason (R):
Copper is more reactive metal than zinc.
(a) Both A and R true; R explains A
(b) Both A and R true; R doesn’t explain A
(c) A true, R false
(d) A false, R true
Answer:
(c) A true, R false. (CBSE
2024)
Q5. Reverse of the reaction is not possible:
Zn(s) + CuSO₄(aq) →
ZnSO₄(aq) +
Cu(s). Reason is:
(a) Zn is less reactive than Cu
(b) Cu is less reactive than Zn
(c) Both have same reactivity
(d) Zn is a non-metal
Answer:
(b) Cu is less reactive than Zn, so it can’t displace Zn back. (Board Term I, 2016)
Q6. Amphoteric oxides from the list Na₂O, ZnO, CO₂, Al₂O₃, H₂O are:
(a) Na₂O and H₂O
(b) ZnO and Al₂O₃
(c) CO₂ and H₂O
(d) Na₂O and CO₂
Answer: (b) ZnO and Al₂O₃. (Board Term I, 2014)
Q7. Calcium starts floating when it reacts with water
because:
(a) CO₂ bubbles
stick on it
(b) O₂ bubbles
stick on it
(c) H₂ bubbles
stick on it
(d) It becomes lighter than water instantly
Answer: (c) H₂
bubbles stick on it. (Board
Term I, 2015)
Q8. Most metals do not evolve hydrogen gas with nitric acid
because:
(a) HNO₃ is weak
acid
(b) HNO₃ is
strong oxidising agent
(c) Metals are non-reactive
(d) Hydrogen is insoluble
Answer: (b) HNO₃
oxidises the H₂ formed.
(Board Term I, 2016)
Q9. In galvanisation, iron is coated with:
(a) Copper
(b) Aluminium
(c) Zinc
(d) Tin
Answer: (c) Zinc. (Board
Term I, 2013)
Q10. Which metal is most ductile (best for making thin wires)?
(a) Iron
(b) Copper
(c) Aluminium
(d) Gold
Answer: (d) Gold. (Board
Term I, 2015).
Short
Answer Questions (PYQ)
Q1. What happens when zinc pieces are placed in blue copper sulphate solution? (Board Term I, 2014)
Answer: Blue colour fades and reddish-brown copper deposits on zinc because Zn displaces Cu from CuSO₄ solution.
Q2. Why does calcium start floating when it reacts with water? Write balanced equation. (Board Term I, 2015)
Answer: Hydrogen bubbles stick to calcium and make it float. Reaction: Ca + 2H₂O → Ca(OH)₂ + H₂.
Q3. What is meant
by amphoteric oxides? Give examples. (Board Term I, 2014)
Answer: Oxides that react with both acids and bases to form salt and water are amphoteric; ZnO and Al₂O₃ are examples.
Q4. Define corrosion and rusting. (Board Term I, 2017)
Answer: Corrosion is slow eating up of metals by air/moisture forming surface compounds; rusting is corrosion of iron.
Q5. State reasons: (i) Sodium is kept in kerosene. (ii) Metals conduct electricity. (Board Term I, 2016)
Answer: (i) Sodium reacts vigorously with air/water so stored in kerosene. (ii) Metals have free electrons that carry current.
Long Answer Questions (PYQ)
Q1. An ore on treatment with dilute HCl produces brisk effervescence. Name the type of ore with example. Steps to obtain metal from enriched ore with equations. (AI 2019)
Answer: It is a carbonate ore; example calamine (ZnCO₃). Steps: calcination (ZnCO₃ → ZnO + CO₂) then reduction (ZnO + C → Zn + CO).
Q2. (a) List in
tabular form three chemical properties to differentiate metals and non-metals.
(b) Give reasons: (i) metals conduct electricity (ii) Fe₂O₃ + Al reaction used to join tracks. (Delhi 2019)
Answer: (a) Metals form basic oxides; non-metals form acidic oxides. Metals may displace H₂ from water/acids; non-metals generally don’t. Metals are usually reducing agents; non-metals oxidising agents. (b) (i) Free electrons. (ii) Thermite reaction is highly exothermic and produces molten iron for welding.
Q3. Carbon cannot
reduce oxides of Na, Mg, Al. Why? Where are they in reactivity series? How
obtained? Explain with one example with equations. (2020)
Answer: These metals have higher affinity for oxygen; they are at top of reactivity series; extracted by electrolytic reduction of molten salts/oxides. Example given: electrolysis of molten NaCl with electrode reactions (Na⁺ + e⁻ → Na at cathode; 2Cl⁻ → Cl₂ + 2e⁻ at anode).
Q4. (a) Complete & balance: (i) Al₂O₃ + HCl → (ii) K₂O + H₂O → (iii) Fe + H₂O → (b) Element X displaces iron from FeSO₄. Predict observations with CuSO₄, ZnSO₄, AgNO₃ and arrange reactivity order. (2020)
Answer:
(a) (i) Al₂O₃ + 6HCl →
2AlCl₃ + 3H₂O (ii) K₂O + H₂O →
2KOH (iii) 3Fe + 4H₂O
→ Fe₃O₄
+ 4H₂. (b) X
is more reactive than Fe; it displaces Cu and Ag from their salts; may or may
not displace Zn—so possible orders: Ag < Cu < Fe < Zn < X or Ag
< Cu < Fe < X < Zn.
Q5. A metal X combines with non-metal Y by transfer of electrons to form compound Z. (i) bond type (ii) melting/boiling (iii) solubility in kerosene/petrol (iv) electrical conductivity. (Board Term I, 2017)
Answer: (i) Ionic bond. (ii) High melting/boiling points. (iii) Insoluble in kerosene/petrol. (iv) Does not conduct in solid state but conducts in molten/aqueous state.
Conclusion
Metals and Non-metals becomes easy
when you connect three things: (1) key properties with daily-life examples, (2)
the reactivity series to predict reactions, and (3) a few standard reaction
patterns like metal + oxygen, metal + water, metal + acids, and displacement
reactions. NCERT also links these ideas to real applications like extraction
methods (roasting/calcination, reduction, electrolysis), electrolytic refining,
and corrosion prevention—so if you understand the “why” behind each step, the
chapter stops feeling like memorization. Revise the tables (properties, ionic
compounds, extraction) and practice writing reactions in “words first, then
equation” format to score confidently in Board Exam 2026.
Download Class 10 Science Notes PDF
Looking for class 10 science notes PDF download or class 10 METALS & NON METALS notes PDF? This complete guide covers all topics from Chapter 3 with NCERT-based explanations, making it perfect for your CBSE Board 2026 preparation.
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