Metals and non-metals form two broad categories of elements, each with distinct properties and characteristics. Chapter 3 of CBSE Class 10 Science focuses on understanding these properties, their chemical reactions, and their applications. This blog will provide a concise overview of the key topics from this chapter to help students prepare efficiently for their exams.

Introduction to Metals and Non-Metals

Metals and non-metals are distinguished based on their physical and chemical properties.

• Metals are typically shiny, good conductors of heat and electricity, and possess high malleability and ductility.
• Non-metals, on the other hand, are generally dull, poor conductors of heat and electricity, and tend to be brittle in solid form.

Physical Properties of Metals

Metals possess several key physical properties:

• Malleability: Metals can be hammered into thin sheets without breaking.
• Ductility: They can be drawn into thin wires.
• Conductivity: Metals are excellent conductors of heat and electricity due to free-moving electrons.
• Luster: Metals have a shiny appearance because they reflect light.

Physical Properties of Non-Metals

Non-metals have contrasting properties to metals:

• Dull Appearance: Non-metals lack the shiny luster of metals.
• Poor Conductors: They do not conduct heat and electricity efficiently.
• Brittle: Non-metals are typically brittle in solid form and break easily.

Chemical Properties of Metals

Metals react with various substances to form compounds:

• Reaction with Oxygen: Metals form metal oxides when they react with oxygen. For example, magnesium reacts with oxygen to form magnesium oxide (MgO).
• Reaction with Water: Some metals like sodium react with water to form metal hydroxides and hydrogen gas.
• Reaction with Acids: Metals react with acids to form metal salts and release hydrogen gas. For instance, zinc reacts with hydrochloric acid to form zinc chloride (ZnCl₂) and hydrogen gas.

Reactivity Series

The reactivity series is a list of metals arranged in order of their reactivity. Highly reactive metals like potassium are placed at the top, while less reactive metals like gold and platinum are found at the bottom. This series helps predict the outcomes of displacement reactions and determines how metals react with other substances.

Extraction of Metals

The extraction of metals involves obtaining metals from their ores, often through processes like:

• Smelting: Heating ores with a reducing agent (like carbon) to extract the metal.
• Electrolysis: Using electric current to extract metals from their compounds.

Alloys

An alloy is a mixture of two or more elements, where at least one is a metal. Alloys have improved properties compared to pure metals. Examples include:

• Brass: A mixture of copper and zinc.
• Steel: A combination of iron and carbon.

Alloys are commonly used in construction, transportation, and manufacturing due to their enhanced strength and durability.

Corrosion and Its Prevention

Corrosion is the process of metal deterioration due to chemical reactions with substances like oxygen and water. For example, iron rusts when it reacts with water and oxygen to form iron oxide (rust).

To prevent corrosion:

• Galvanization: Coating metal with a layer of zinc.
• Painting: Applying a protective paint layer.
• Using corrosion-resistant alloys: Metals like stainless steel are resistant to corrosion due to their alloy composition.

Conclusion

Chapter 3, “Metals and Non-Metals,” covers the essential properties, reactions, and applications of these elements. Understanding the physical and chemical properties, as well as the reactivity series, helps students not only in exams but also in everyday applications of science. With these short notes, you are now equipped to revise the topic efficiently and score well in your exams.

Stay organized, keep revising, and make use of additional study resources like Physics Wallah notes for further clarification and practice. Best of luck with your preparations!

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