Education For All

Metals usually have several common physical properties.

1. Metallic Lustre

Most metals have a shiny surface when freshly cut or polished. This property is called metallic lustre.

Examples include iron, copper, aluminium, and magnesium.

2. Hardness

Most metals are hard, although hardness varies from one metal to another.

For example, sodium is soft compared with many other metals.

3. Malleability

The ability of a metal to be beaten into thin sheets is called malleability.

Gold and silver are highly malleable metals.

4. Ductility

The ability of a metal to be drawn into thin wires is known as ductility.

This property makes metals useful for electrical wiring.

Conductivity and Sonority

Most metals are good conductors of heat and electricity.

This is why metals such as copper are widely used in electrical applications.

Metals are also sonorous, meaning they produce a ringing sound when struck.

That is why metals are used in objects such as:

Bells
Musical instruments
Electrical wires
Cooking utensils

Physical Properties of Non-metals

In general, non-metals have characteristics that are in opposition to those of metals.

They are usually:

Dull
Not malleable
Not ductile
Poor conductors of heat
Poor conductors of electricity

Non-metals may exist as solids or gases at room temperature.

Important Exception

Br is a nonmetal that exists as a liquid at room temperature.

Some non-metals also show unusual properties. For example:

Iodine is lustrous.
Graphite conducts electricity.

This shows why exceptions are important in the metals and non-metals class 10.

Important Exceptions You Should Remember

Science often has general rules, but some elements behave differently.

Metals with Exceptions

Mercury is a metal but is liquid at room temperature.
Sodium and potassium are soft metals.
Ga and Cs have relatively low melting points.

Non-metals with Exceptions

Iodine is lustrous.
Graphite conducts electricity.
Diamond (C) — Diamond is a form of carbon and is extremely hard.

These exceptions are important for exams and conceptual understanding.

  Chemical Properties: Reaction with Oxygen

Metals react with oxygen to form metal oxides.

General Reaction

Metal + Oxygen → Metal Oxide

For example:

2Cu + O₂ → 2CuO

4Al + 3O₂ → 2Al₂O₃

Most metal oxides are basic in nature.

Amphoteric Oxides
Certain metal oxides react with both acidic and basic substances. These are called amphoteric oxides.

Important examples include:

Aluminum oxide (Al₂O₃)
Zinc oxide (ZnO)

How Do Metals React with Water?

Different metals react differently with water.

Highly Reactive Metals

Sodium and potassium react very vigorously with water.

Moderately Reactive Metals

Calcium reacts less vigorously, while magnesium reacts with hot water.

Metals That React with Steam

Al, Zn, and Fe react with steam under suitable conditions.

Metals That Do Not React with Water

Pb, Cu, Ag, and Au do not react with H₂O .

A metal reacts according to its position in the reactivity series.

Metals and Dilute Acids

Many metals react with dilute acids to form salts and hydrogen gas.

General Reaction

Metal + Dilute Acid → Salt + Hydrogen Gas

Different metals react at different speeds.

For example, Mn reacts more vigorously than Zn and Fe.

Copper does not react with dilute hydrochloric acid.

Special Case: Nitric Acid
The behaviour of nitric acid is different because of its strong oxidising nature. Therefore, the usual hydrogen gas reaction does not generally occur.

What Is Aqua Regia?

Aqua regia is a freshly prepared mixture of concentrated

Hydrochloric acid
Nitric acid

The ratio is:

3:1

Aqua regia is known for its ability to dissolve metals such as gold and platinum.

Displacement Reactions

A more reactive metal can displace a less reactive metal from its salt solution.

For example, iron is more reactive than copper.

Therefore, when an iron nail is placed in a copper sulfate solution, iron displaces copper.

Simple Rule

More Reactive Metal + Salt Solution → New Salt + Less Reactive Metal

Displacement reactions help us understand the relative reactivity of metals.

The Reactivity Series

The reactivity series arranges metals according to their chemical reactivity.

Highly reactive metals are placed near the top, while less reactive metals are placed near the bottom.

The position of a metal helps predict the following:

Its reaction with water
Its reaction with acids
Its extraction method
Whether it can displace another metal

Understanding the reactivity series is one of the most important parts of the Metals and Non-metals Class 10.

How Do Metals and Nonmetals React?

Atoms react to achieve a stable electronic configuration.

Metals Lose Electrons

Metals generally lose electrons and form positively charged ions called cations.

For example:

Na → Na⁺ + e⁻

Non-metals Gain Electrons

Non-metals generally gain electrons and form negatively charged ions called **anions**.

For example:

Cl + e⁻ → Cl⁻

  Formation of Ionic Compounds

When a metal transfers electrons to a non-metal, oppositely charged ions are formed.

These ions attract each other due to electrostatic forces.

For example, sodium and chlorine form sodium chloride.

Example

Na⁺ + Cl⁻ → NaCl

Compounds formed through the transfer of electrons are called:

Ionic compounds or electrovalent compounds.

Properties of Ionic Compounds

Ionic compounds generally:

Are solids
Are hard and brittle
Have high melting and boiling points
Are usually soluble in water
Conduct electricity in molten or aqueous states

They do not usually conduct electricity in solid form because their ions cannot move freely.

Less Reactive Metals

Gold and silver may occur in their native or free state.

Roasting, Calcination and Reduction

These processes are important in metallurgy.

Roasting

Heating sulfide ores strongly in the presence of excess air is called roasting.

Calcination

Heating carbonate ores in limited or no air is called calcination.

Reduction

The process of converting metal oxides into metals is called reduction.

These steps help extract useful metals from their ores.

The Thermite Reaction

The thermite reaction is a highly exothermic reaction involving aluminium and iron oxide.

The heat produced is sufficient to form molten iron.

This reaction is used in joining railway tracks and repairing certain machine parts.

Corrosion: Why Do Metals Get Damaged?

The gradual destruction of metals due to reactions with their environment is called corrosion.

Examples include:

Rusting of iron
Black coating on silver
Green coating on copper

Iron rusts when both air and water are present.

How Can Corrosion Be Prevented?

Common methods include:

Painting
Oiling
Greasing
Chrome plating
Anodizing
Galvanization

What Is Galvanization?

Galvanization is the process of protecting iron or steel by coating it with zinc.

This method helps prevent rusting.

Alloys: Improving Metal Properties

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

Alloys are created to improve properties such as strength, hardness, and resistance to corrosion.

Important Alloys

Brass: Copper + Zinc
Bronze: Copper + Tin
Stainless Steel: Iron + Chromium + Nickel
Solder: Lead + Tin

Alloying allows metals to be modified for specific uses.

How to Study Metals and Non-metals Class 10

Use this simple revision strategy:

1. Learn the Properties

Compare metals and non-metals using a table.

2. Remember the Exceptions

Focus on mercury, bromine, iodine, graphite, sodium, and diamond.

3. Practice Chemical Equations

Write and balance important reactions regularly.

4. Understand the Reactivity Series

Do not simply memorize it. Understand how it predicts chemical behavior.

5. Learn Key Definitions

Important terms include:

Ore
Mineral
Alloy
Corrosion
Roasting
Calcination
Ionic compound
Cation
Anion

6. Revise Through Questions

Practice MCQs, assertion-reason questions, and chemical equations.

Quick Revision Questions

Test yourself:

Q1. What property allows metals to be drawn into wires?

Q2. Why does graphite conduct electricity despite being a non-metal?

Q3. What are amphoteric oxides?

Q4. Why are ionic compounds good conductors in molten form?

Q5. What is galvanization?

Q6. What is the difference between roasting and calcination?

Frequently Asked Questions

What is the main topic of Metals and Non-metals?

The chapter explains the physical and chemical properties of metals and non-metals, their reactions, ionic compounds, extraction methods, corrosion, and alloys.

What are the main properties of metals?

Metals are generally lustrous, malleable, ductile, sonorous, and good conductors of heat and electricity.

What is an ionic compound?

An ionic compound is formed when electrons are transferred from one atom to another, creating positively and negatively charged ions.

Why are metals extracted using different methods?

The extraction method depends on the reactivity of the metal. Highly reactive metals require electrolysis, while moderately reactive metals can often be extracted through reduction.

What is corrosion?

Corrosion is the gradual damage or destruction of a metal caused by reactions with substances in its surroundings, such as air and moisture.

What is galvanization?

Galvanization is the process of coating iron or steel with zinc to protect it from rusting.

Remember This

Properties → Reactions → Reactivity → Extraction → Protection

Exam Tip

Focus on exceptions, chemical equations, the reactivity series, ionic compounds, and methods of preventing corrosion. These topics are especially useful for building strong conceptual understanding.

Final Takeaway

Metals and Non-metals Class 10 is not just about memorizing properties and reactions. It explains how the chemical nature of elements determines their behavior, extraction, and everyday uses.

Once you understand the connection between properties, reactivity, and applications, the entire chapter becomes much easier to revise.