Metals and Non-metals Class 10 Notes

Metals and Non-metals is Chapter 3 of NCERT Class 10 Science and one of the most important Chemistry chapters for CBSE board exam preparation. This chapter explains the physical and chemical properties of metals and non-metals, reactivity series, ionic bond formation, extraction of metals, corrosion, alloys, and important daily-life applications.

These Metals and Non-metals Class 10 Notes are written in a simple and exam-focused format to help students revise the chapter quickly. The notes include comparison tables, important exceptions, chemical equations, electron dot structures, activity series tricks, extraction flowcharts, lab precautions, important questions, MCQs, assertion-reason questions, and case-based questions.

Students can use these notes for school exams, pre-board revision, CBSE board exams, NCERT questions, previous year questions, and quick last-minute revision.

Metals and Non-Metals Class 10 Notes: Chapter Overview

This chapter is one of the most important and scoring chapters in Class 10 Science Notes. Understanding it properly not only helps you score well in CBSE board exams but also builds a strong foundation for Class 11 and 12 Chemistry, as well as competitive exams like JEE and NEET.

This chapter is important for CBSE Class 10 exams because it includes many reaction-based, reasoning-based, diagram-based, and application-based questions.

Metals and Non-metals Class 10 Notes PDF Download

Students can download the Metals and Non-metals Class 10 Notes PDF for offline revision. The PDF is useful for quick preparation because it includes chapter summary, reactions, diagrams, tables, important questions, MCQs, and previous year question patterns.

What are Metals?

Metals are elements that generally show properties like lustre, malleability, ductility, sonority, and good conductivity of heat and electricity. Most metals are solids at room temperature and form positive ions by losing electrons.

Examples of Metals

What are Non-metals?

Non-metals are elements that generally do not show metallic properties. They are usually poor conductors of heat and electricity, brittle in solid state, and form negative ions by gaining electrons or form covalent compounds by sharing electrons.

Examples of Non-metals

Physical Properties of Metals and Non-metals

The physical properties of metals and non-metals help us identify and compare them. Metals are generally hard, lustrous, malleable, ductile, sonorous, and good conductors. Non-metals are generally dull, brittle, non-sonorous, and poor conductors.

Difference Between Metals and Non-metals Class 10

Important Exceptions in Metals and Non-metals

Some elements do not follow the general properties of metals and non-metals. These exceptions are very important for CBSE exams because they are often asked in one-mark and reasoning questions.

Why is Graphite a Good Conductor of Electricity?

Graphite is a non-metal, but it conducts electricity because each carbon atom in graphite is bonded to three other carbon atoms, leaving one electron free. These free electrons can move through the layers of graphite and conduct electricity.

This is an important exception because most non-metals do not conduct electricity.

Why is Diamond Hard but Graphite Soft?

Diamond and graphite are both forms of carbon, but their structures are different. In diamond, each carbon atom is strongly bonded to four other carbon atoms, forming a rigid three-dimensional structure. This makes diamond extremely hard.

In graphite, carbon atoms are arranged in layers. These layers can slide over each other, making graphite soft and slippery.

Chemical Properties of Metals

Metals show chemical reactions with oxygen, water, acids, and salt solutions. The reactivity of a metal decides how strongly it reacts with these substances.

Reaction of Metals with Oxygen

Metals react with oxygen to form metal oxides. Metal oxides are generally basic in nature, but some metal oxides are amphoteric.

General Reaction

Metal + Oxygen → Metal oxide

Examples

2Cu + O₂ → 2CuO

4Al + 3O₂ → 2Al₂O₃

2Mg + O₂ → 2MgO

Important Point

Magnesium burns in air with a bright white flame and forms magnesium oxide.

2Mg + O₂ → 2MgO

Magnesium oxide is basic in nature.

What are Amphoteric Oxides?

Amphoteric oxides are oxides that react with both acids and bases to form salt and water. Aluminium oxide and zinc oxide are common examples of amphoteric oxides.

Examples

Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O

Al₂O₃ + 2NaOH → 2NaAlO₂ + H₂O

ZnO + 2HCl → ZnCl₂ + H₂O

ZnO + 2NaOH → Na₂ZnO₂ + H₂O

Reaction of Metals with Water

Metals react with water to form metal hydroxides or metal oxides and hydrogen gas. Highly reactive metals react with cold water, while less reactive metals may react with hot water or steam.

General Reaction

Metal + Water → Metal hydroxide + Hydrogen gas

Examples

2Na + 2H₂O → 2NaOH + H₂ + heat

Ca + 2H₂O → Ca(OH)₂ + H₂

Mg + H₂O → MgO + H₂

Why does Calcium Float on Water?

Calcium reacts with water and produces hydrogen gas. Bubbles of hydrogen gas stick to the surface of calcium, making it float on water.

Ca + 2H₂O → Ca(OH)₂ + H₂

Why is Sodium Stored in Kerosene Oil?

Sodium is a highly reactive metal. It reacts vigorously with oxygen and moisture present in air and may catch fire. Therefore, sodium is stored under kerosene oil to prevent contact with air and water.

This is a very common Class 10 board exam question.

Reaction of Metals with Acids

Most metals react with dilute acids to form salt and hydrogen gas.

General Reaction

Metal + Dilute acid → Salt + Hydrogen gas

Example

Zn + 2HCl → ZnCl₂ + H₂

Mg + 2HCl → MgCl₂ + H₂

Fe + 2HCl → FeCl₂ + H₂

Test for Hydrogen Gas

Hydrogen gas burns with a pop sound when a burning splinter is brought near it.

Why is Hydrogen Gas Not Evolved When Metals React with Nitric Acid?

Hydrogen gas is generally not evolved when metals react with nitric acid because nitric acid is a strong oxidising agent. It oxidises hydrogen gas into water and itself gets reduced to nitrogen oxides such as NO₂, NO, or N₂O.

Exception: Magnesium and manganese may produce hydrogen gas with very dilute nitric acid.

Reaction of Metals with Salt Solutions

A more reactive metal displaces a less reactive metal from its salt solution. This reaction is called a displacement reaction.

General Reaction

More reactive metal + Salt solution of less reactive metal → Salt solution of more reactive metal + Less reactive metal

Example: Iron and Copper Sulphate

Fe + CuSO₄ → FeSO₄ + Cu

Iron is more reactive than copper, so it displaces copper from copper sulphate solution.

Observation

The blue colour of copper sulphate solution gradually changes to green due to the formation of iron sulphate. A reddish-brown layer of copper gets deposited on the iron nail.

Chemical Properties of Non-metals

Non-metals react with oxygen to form non-metal oxides. These oxides are generally acidic or neutral in nature. Non-metals usually do not react with water and dilute acids like metals do.

Reaction of Non-metals with Oxygen

Non-metals react with oxygen to form non-metal oxides. These oxides are generally acidic.

Examples

C + O₂ → CO₂

S + O₂ → SO₂

Nature of Non-metal Oxides

Difference Between Metal Oxides and Non-metal Oxides

Reactivity Series Class 10

The reactivity series is an arrangement of metals in decreasing order of their reactivity. Metals at the top are highly reactive, while metals at the bottom are least reactive.

Reactivity Series of Metals

Reactivity Series Mnemonic

Use this memory trick for the order:

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K → Potassium
Na → Sodium
Ca → Calcium
Mg → Magnesium
Al → Aluminium
Zn → Zinc
Fe → Iron
Pb → Lead
H → Hydrogen
Cu → Copper
Hg → Mercury
Ag → Silver
Au → Gold

Why is Hydrogen Included in the Reactivity Series?

Hydrogen is included in the reactivity series as a reference point. Metals placed above hydrogen can displace hydrogen from dilute acids, while metals placed below hydrogen usually cannot displace hydrogen from dilute acids.

Example

Zinc is above hydrogen, so it reacts with dilute hydrochloric acid:

Zn + 2HCl → ZnCl₂ + H₂

Copper is below hydrogen, so it does not react with dilute hydrochloric acid to release hydrogen gas.

Ionic Bond Formation in Metals and Non-metals

Metals generally lose electrons and form positive ions. Non-metals generally gain electrons and form negative ions. The strong electrostatic attraction between positive and negative ions forms an ionic bond.

Formation of Sodium Chloride

Sodium has one electron in its outermost shell, while chlorine needs one electron to complete its octet. Sodium transfers one electron to chlorine.

Electron Transfer

Na → Na⁺ + e⁻

Cl + e⁻ → Cl⁻

Na⁺ + Cl⁻ → NaCl

Electron Dot Representation

Na•  +  :Cl:  →  Na⁺ [:Cl:]⁻

Sodium loses one electron and becomes Na⁺. Chlorine gains one electron and becomes Cl⁻. The oppositely charged ions attract each other and form sodium chloride.

Formation of Magnesium Oxide

Magnesium has two valence electrons, while oxygen needs two electrons to complete its octet. Magnesium transfers two electrons to oxygen.

Electron Transfer

Mg → Mg²⁺ + 2e⁻

O + 2e⁻ → O²⁻

Mg²⁺ + O²⁻ → MgO

Electron Dot Representation

Mg••  +  :O:  →  Mg²⁺ [:O:]²⁻

Properties of Ionic Compounds

Ionic compounds have strong forces of attraction between oppositely charged ions. Because of this, they show high melting points, high boiling points, and conduct electricity in molten or aqueous state.

Why Do Ionic Compounds Have High Melting Points?

Ionic compounds have high melting points because their positive and negative ions are held together by strong electrostatic forces of attraction. A large amount of heat energy is required to break these forces.

Why Do Ionic Compounds Conduct Electricity Only in Molten or Aqueous State?

Ionic compounds conduct electricity only when their ions are free to move. In solid state, ions are fixed in their positions and cannot carry charge. In molten or aqueous state, ions become mobile and conduct electricity.

Occurrence of Metals

Metals occur in nature either in free state or combined state. Highly reactive metals are found in combined form, while less reactive metals may be found in free state.

Minerals, Ores and Gangue

Difference Between Minerals and Ores

Extraction of Metals Class 10

The method used for extracting a metal depends on its position in the reactivity series. Highly reactive metals are extracted by electrolysis, moderately reactive metals are extracted by reduction, and less reactive metals may be obtained by simple heating or from native state.

Extraction of Highly Reactive Metals

Highly reactive metals such as potassium, sodium, calcium, magnesium, and aluminium cannot be extracted by heating their oxides with carbon. They have strong affinity for oxygen, so they are extracted by electrolytic reduction.

Examples

Extraction of Moderately Reactive Metals

Moderately reactive metals such as zinc, iron, lead, and copper are usually found as sulphide or carbonate ores. These ores are first converted into metal oxides and then reduced to metals.

Step 1: Concentration of Ore

The removal of impurities from ore is called concentration or enrichment of ore.

Step 2: Conversion into Oxide

Sulphide ores are converted into oxides by roasting. Carbonate ores are converted into oxides by calcination.

Step 3: Reduction of Oxide

Metal oxides are reduced to metals using reducing agents such as carbon, carbon monoxide, or aluminium.

Difference Between Roasting and Calcination

Reduction of Metal Oxides

Metal oxides are reduced to metals using reducing agents.

Example

ZnO + C → Zn + CO

Fe₂O₃ + 2Al → Al₂O₃ + 2Fe + heat

The second reaction is called the thermite reaction.

What is Thermite Reaction?

The thermite reaction is a highly exothermic reaction in which aluminium reduces iron oxide to molten iron. It is used in welding railway tracks and repairing broken machine parts.

Equation

Fe₂O₃ + 2Al → Al₂O₃ + 2Fe + heat

Extraction of Less Reactive Metals

Less reactive metals such as mercury, silver, gold, and platinum occur either in free state or can be obtained easily from their compounds.

Example: Mercury from Cinnabar

Cinnabar is mercury sulphide, HgS. It is heated in air to form mercury oxide, which is then reduced to mercury.

2HgS + 3O₂ → 2HgO + 2SO₂

2HgO → 2Hg + O₂

Refining of Metals

The metals obtained after extraction usually contain impurities. The process of removing impurities from metals is called refining. The most common method is electrolytic refining.

Electrolytic Refining of Copper

Electrolytic refining is used to obtain pure copper from impure copper.

During electrolysis, copper from the anode dissolves into the solution and gets deposited on the cathode as pure copper. Insoluble impurities settle below the anode as anode mud.

Corrosion Class 10

Corrosion is the slow destruction of metals due to the action of air, moisture, acids, or other chemicals present in the environment. Rusting of iron is the most common example of corrosion.

Rusting of Iron

Iron rusts in the presence of oxygen and moisture. Rust is hydrated iron oxide.

Fe₂O₃·xH₂O

Conditions Necessary for Rusting

• Presence of oxygen
• Presence of moisture

How Can Corrosion Be Prevented?

Corrosion can be prevented by stopping the contact of metal with air and moisture.

Why Does Aluminium Resist Corrosion?

Aluminium is reactive, but it does not corrode easily because it forms a thin, strong layer of aluminium oxide on its surface. This oxide layer prevents further reaction with air and moisture.

Alloys Class 10

An alloy is a homogeneous mixture of two or more metals, or a metal and a non-metal. Alloys are made to improve the properties of metals such as strength, hardness, resistance to corrosion, and usefulness.

Examples of Alloys

Why is Pure Gold Not Used for Making Jewellery?

Pure gold is very soft and can easily change shape. Therefore, it is mixed with small amounts of copper or silver to make it harder and suitable for jewellery.

Real-life Applications of Metals and Non-metals

Lab Activities and Safety Notes

Lab-based questions are important because CBSE often asks observation-based and reasoning-based questions from activities.

Burning Magnesium Ribbon

Magnesium burns in air with a bright white flame and forms white magnesium oxide.

2Mg + O₂ → 2MgO

Safety Notes

• Perform the activity only under teacher supervision.
• Do not look directly at the bright flame.
• Use proper lab tools and keep flammable materials away.
• Do not touch hot magnesium oxide immediately.

Iron Nail in Copper Sulphate Solution

When an iron nail is placed in copper sulphate solution, iron displaces copper because iron is more reactive than copper.

Fe + CuSO₄ → FeSO₄ + Cu

Observation

• Blue copper sulphate solution turns green.
• Reddish-brown copper gets deposited on the iron nail.

Conclusion

Iron is more reactive than copper.

Reaction of Metal with Dilute Acid

When zinc reacts with dilute hydrochloric acid, hydrogen gas is evolved.

Zn + 2HCl → ZnCl₂ + H₂

Test

Hydrogen gas burns with a pop sound.

Safety Notes

• Do not smell gases directly.
• Keep flames away unless instructed by the teacher.
• Use small quantities under supervision.

Important Chemical Equations from Metals and Non-metals

Metals and Non-metals Short Notes

• Metals are generally lustrous, malleable, ductile, sonorous, and good conductors.
• Non-metals are generally dull, brittle, non-sonorous, and poor conductors.
• Mercury is the only liquid metal at room temperature.
• Bromine is a liquid non-metal.
• Graphite is a non-metal but conducts electricity.
• Iodine is a lustrous non-metal.
• Sodium and potassium are soft and highly reactive metals.
• Metals form positive ions by losing electrons.
• Non-metals form negative ions by gaining electrons.
• Ionic compounds are formed by transfer of electrons.
• Ionic compounds conduct electricity in molten or aqueous state.
• Reactivity series arranges metals in decreasing order of reactivity.
• More reactive metals displace less reactive metals from their salt solutions.
• Highly reactive metals are extracted by electrolysis.
• Sulphide ores are converted into oxides by roasting.
• Carbonate ores are converted into oxides by calcination.
• Corrosion is the slow damage of metals due to air and moisture.
• Rusting requires both air and water.
• Galvanisation prevents rusting by coating iron with zinc.
• Alloys are mixtures of metals or metals with non-metals.

Common Mistakes Students Should Avoid

Metals and Non-metals Class 10 MCQs

1. Which of the following is a liquid metal?

A. Sodium
B. Mercury
C. Aluminium
D. Copper

Answer: B. Mercury

2. Which non-metal conducts electricity?

A. Sulphur
B. Phosphorus
C. Graphite
D. Iodine

Answer: C. Graphite

3. Which metal is stored in kerosene oil?

A. Iron
B. Sodium
C. Copper
D. Zinc

Answer: B. Sodium

4. Which gas is evolved when zinc reacts with dilute hydrochloric acid?

A. Oxygen
B. Nitrogen
C. Hydrogen
D. Carbon dioxide

Answer: C. Hydrogen

5. Which method is used to prevent rusting by coating iron with zinc?

A. Alloying
B. Galvanisation
C. Roasting
D. Calcination

Answer: B. Galvanisation

Assertion and Reason Questions

Question 1

Assertion: Sodium is stored in kerosene oil.
Reason: Sodium reacts vigorously with air and moisture.

Answer: Both Assertion and Reason are true, and Reason is the correct explanation of Assertion.

Question 2

Assertion: Graphite is used as an electrode.
Reason: Graphite can conduct electricity.

Answer: Both Assertion and Reason are true, and Reason is the correct explanation of Assertion.

Question 3

Assertion: Ionic compounds do not conduct electricity in solid state.
Reason: Ions are not free to move in solid ionic compounds.

Answer: Both Assertion and Reason are true, and Reason is the correct explanation of Assertion.

Case-based Question on Metals and Non-metals

A student places an iron nail in a blue copper sulphate solution. After some time, the colour of the solution changes from blue to green, and a reddish-brown deposit appears on the nail.

Questions

1. Name the reaction taking place.
2. Write the balanced chemical equation.
3. Why does iron displace copper?
4. What is the green solution formed?
5. What is the reddish-brown deposit?

Answers

1. Displacement reaction.
2. Fe + CuSO₄ → FeSO₄ + Cu
3. Iron is more reactive than copper.
4. Iron sulphate, FeSO₄.
5. Copper.

Metals and Non-metals Class 10 Important Questions

One-mark Questions

1. Name one liquid metal.
2. Name one liquid non-metal.
3. Which non-metal conducts electricity?
4. What is an alloy?
5. What is galvanisation?
6. Name the metal stored in kerosene oil.
7. What is the formula of rust?
8. Name one amphoteric oxide.

Two-mark Questions

1. Why is sodium stored in kerosene oil?
2. Why is graphite a good conductor of electricity?
3. Why does calcium float on water?
4. Why is hydrogen included in the reactivity series?
5. Why do ionic compounds have high melting points?
6. Why does aluminium resist corrosion?
7. What is the difference between minerals and ores?
8. What is the difference between roasting and calcination?

Three-mark Questions

1. Write three physical differences between metals and non-metals.
2. Explain the formation of sodium chloride by electron transfer.
3. Explain the reaction of metals with oxygen, water, and acids.
4. Explain electrolytic refining of copper.
5. Write three methods to prevent corrosion.
6. Explain the extraction of metals from the middle of the reactivity series.

Five-mark Questions

1. Explain the physical and chemical properties of metals and non-metals with examples.
2. Explain the reactivity series and displacement reactions with examples.
3. Explain ionic bond formation in NaCl and MgO using electron transfer.
4. Explain the extraction of metals based on their position in the reactivity series.
5. Explain corrosion, rusting of iron, and methods of prevention.

To score well in Metals and Non-metals Class 10, focus on the comparison table, exceptions, reactivity series, displacement reactions, ionic bond formation, extraction of metals, roasting vs calcination, corrosion, alloys, and important chemical equations. Practise MCQs, assertion-reason questions, and case-based questions because this chapter is commonly tested through application-based questions.