Metals and Non-Metals

Class 10 Science • Important Questions & Practice

Exam Focus: Physical and chemical properties, reactions with oxygen, water and acids, reactivity series, displacement reactions, ionic compounds, occurrence and extraction of metals, corrosion, prevention of corrosion and alloys.

A. Very Short Answer Questions

Question 1

What is malleability?

Malleability is the property by which a metal can be beaten into thin sheets.

Question 2

What is ductility?

Ductility is the property by which a substance can be drawn into thin wires.

Question 3

Name one non-metal that conducts electricity.

Graphite, an allotrope of carbon, conducts electricity.

Question 4

What is an amphoteric oxide?

An oxide that reacts with both acids and bases to form appropriate products is called an amphoteric oxide.

Question 5

What is an ore?

An ore is a mineral from which a metal can be extracted conveniently and economically.

Question 6

What is corrosion?

Corrosion is the gradual deterioration of a metal due to chemical or electrochemical reactions with its surroundings.

B. Physical Properties

Question 7

Why are metals generally used for making electrical wires?

Metals generally have high electrical conductivity and can also be drawn into wires because of their ductility.

Question 8

Why can metals generally be made into sheets?

Metals are generally malleable, which allows them to be hammered or rolled into thin sheets.

Question 9

Give two exceptions to the common physical properties of metals and non-metals.

Sodium and potassium are soft metals.
Graphite is a non-metal that conducts electricity.
Bromine is a liquid non-metal at room temperature.

C. Chemical Properties

Question 10

Write the reaction of magnesium with oxygen.

2Mg + O₂ → 2MgO

Question 11

Why is zinc oxide called an amphoteric oxide?

Zinc oxide reacts with acids as well as bases.

ZnO + 2HCl → ZnCl₂ + H₂O

ZnO + 2NaOH → Na₂ZnO₂ + H₂O

Question 12

Write the reaction of sodium with water.

2Na + 2H₂O → 2NaOH + H₂

Question 13

Why should sodium and potassium be stored carefully?

They are highly reactive metals and react vigorously with moisture and water. They are therefore stored in suitable conditions, commonly under kerosene.

D. Metals with Acids & Salt Solutions

Question 14

What happens when zinc reacts with dilute hydrochloric acid?

Zinc forms zinc chloride and hydrogen gas is evolved.

Zn + 2HCl → ZnCl₂ + H₂

Question 15

Why does copper not liberate hydrogen from dilute hydrochloric acid?

Copper is below hydrogen in the reactivity series and therefore does not displace hydrogen from dilute hydrochloric acid.

Question 16

Identify the type of reaction:

Fe + CuSO₄ → FeSO₄ + Cu

This is a displacement reaction.

E. Reactivity Series

Question 17

Write the commonly used metal reactivity series.

K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Hg > Ag > Au

Question 18

Which metal is more reactive, zinc or copper? Explain using the reactivity series.

Zinc is more reactive than copper because zinc is placed above copper in the reactivity series.

Question 19

Can copper displace zinc from zinc sulphate solution?

No. Copper is less reactive than zinc and therefore cannot displace zinc from zinc sulphate.

F. Ionic Compounds

Question 20

How is an ionic compound formed?

An ionic compound is formed through transfer of electrons between atoms, producing oppositely charged ions held together by electrostatic attraction.

Question 21

Why do ionic compounds generally have high melting points?

Strong electrostatic forces exist between oppositely charged ions in the ionic lattice. A large amount of energy is required to overcome these forces.

Question 22

Why do ionic compounds conduct electricity in molten state but generally not in solid state?

In the molten state, ions can move freely and carry electric charge. In the solid state, ions are fixed in their lattice positions.

G. Occurrence & Extraction of Metals

Question 23

Differentiate between a mineral and an ore.

A mineral is a naturally occurring substance containing a metal or its compound.

An ore is a mineral from which the metal can be extracted conveniently and economically.

Question 24

Why does the method of extraction depend on the reactivity of the metal?

Highly reactive metals form very stable compounds and require stronger extraction methods such as electrolysis, whereas less reactive metals can often be obtained by simpler reduction methods.

Question 25

Why are highly reactive metals extracted by electrolysis?

Their compounds are too stable to be reduced effectively by common reducing agents such as carbon. Electrolysis supplies electrical energy to reduce their ions.

Question 26

Give an example of extraction of zinc from zinc oxide.

ZnO + C → Zn + CO

Carbon acts as a reducing agent.

H. Corrosion & Prevention

Question 27

What conditions are important for rusting of iron?

The presence of oxygen and moisture is important for the rusting of iron.

Question 28

Give three methods of preventing corrosion.

Painting.
Oiling or greasing.
Galvanisation.
Electroplating.
Alloying.

Question 29

What is galvanisation?

Galvanisation is the process of coating iron or steel with zinc to protect it from corrosion.

I. Alloys

Question 30

What is an alloy?

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

Question 31

Give two examples of alloys and their main components.

Brass → Copper + Zinc

Bronze → Copper + Tin

J. Reasoning-Based Questions

Question 32

Why does aluminium not corrode easily even though it is reactive?

Aluminium rapidly develops a thin, adherent protective layer of aluminium oxide on its surface. This layer prevents further contact of the metal with the environment and slows corrosion.

Question 33

Why can sodium not be extracted from sodium chloride by heating it with carbon?

Sodium is highly reactive and has a greater affinity for oxygen/electron loss than carbon can overcome in the required extraction process. Molten sodium compounds are therefore extracted by electrolysis.

Question 34

Why are ionic compounds generally brittle?

When an ionic crystal is subjected to stress, layers can shift so that similarly charged ions come close together. Strong repulsion can then cause the crystal to break.

Question 35

Why can zinc displace copper from copper sulphate solution but copper cannot displace zinc?

Zinc is higher than copper in the reactivity series, so it is more reactive and can displace copper. Copper is less reactive than zinc and therefore cannot displace it.

K. Competency-Based Practice

Question 36

Metal X displaces metal Y from its salt solution. What can be concluded about the relative positions of X and Y in the reactivity series?

Metal X is more reactive than metal Y and therefore occurs above Y in the reactivity series.

Question 37

An element forms a positive ion by losing three electrons. What type of element is it likely to be?

It is likely to be a metal because metals generally form positive ions by losing electrons.

Question 38

A substance has a high melting point and conducts electricity when molten but not in its solid state. What type of compound is it likely to be?

It is likely to be an ionic compound because its ions are fixed in the solid state but can move freely in the molten state.

Question 39

A metal occurs low in the reactivity series and is found in the free state. Why is this chemically reasonable?

Metals low in the reactivity series have a lower tendency to react and therefore may occur in the native or free state.

Question 40

A metal oxide reacts with both an acid and a base. What can you infer about the oxide?

The oxide is amphoteric. Zinc oxide is a commonly studied example.

L. Long Answer Questions

Question 41

Explain the major steps involved in the extraction of metals from their ores.

The broad steps include concentration of the ore, conversion into a suitable form such as an oxide where appropriate, reduction or another extraction process and finally refining of the obtained metal.

The exact method depends on the reactivity of the metal.

Question 42

Explain the formation and properties of ionic compounds.

Metals generally lose electrons to form cations while non-metals gain electrons to form anions. The electrostatic attraction between the oppositely charged ions produces an ionic compound.

Ionic compounds generally have high melting and boiling points and conduct electricity when molten or dissolved because their ions can move.

Question 43

Explain the reactivity series and its applications.

The reactivity series arranges metals according to their relative reactivity.

It helps predict displacement reactions, reactions with water and acids and the broad extraction methods suitable for different metals.

M. Quick Revision Questions

Why are metals generally malleable and ductile?
Why does zinc displace copper from copper sulphate?
What is the significance of the reactivity series?
Why do ionic compounds conduct electricity when molten?
Differentiate between a mineral and an ore.
Why are highly reactive metals extracted by electrolysis?
What is galvanisation?
What is an alloy?

Official Practice Sources

Use official CBSE competency-based resources and NCERT material for additional practice.

CBSE Assessment Resources → CBSE Academic Curriculum 2026-27 → NCERT Official Textbooks →