Metals and Non-Metals: Properties and Uses

Introduction

Metals and non-metals are foundational to our understanding of chemistry. These two broad classifications of elements are not only part of our daily environment but also form the basis of countless scientific principles and applications. From the iron used to build skyscrapers to the oxygen essential for human life, metals and non-metals are indispensable.

Grasping the properties of metals and non-metals equips students with knowledge that supports both theoretical learning and real-world understanding. These topics form a crucial part of the Class 10 Chemistry syllabus and are commonly featured in board exams and entrance tests. This comprehensive guide will take you through their physical and chemical properties, occurrences, reactions, and practical applications, complete with relatable examples.

What Are Metals and Non-Metals?

Elements in the periodic table are broadly classified into metals, non-metals, and metalloids. While there are exceptions and overlaps, the core traits of metals and non-metals help us differentiate them clearly.

Metals:

Metals are typically hard, lustrous, malleable, ductile, and good conductors of heat and electricity. They usually have high density and melting points. Common examples include iron (Fe), aluminum (Al), copper (Cu), and gold (Au).

Non-Metals:

Non-metals are generally brittle (if solid), dull in appearance, and poor conductors of heat and electricity, though graphite is an exception. They exist in all three states of matter—solid (sulfur), liquid (bromine), and gas (oxygen, nitrogen).

Quick Comparison Table:

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Physical Properties of Metals and Non-Metals

Understanding the physical properties is key to distinguishing between metals and non-metals. These traits are observable without changing the chemical composition.

Properties of Metals:

• Lustrous: Shiny surface, easily polished
• Malleable: Can be hammered into sheets (e.g., aluminum foil)
• Ductile: Can be drawn into wires (e.g., copper wiring)
• Sonorous: Produce ringing sounds when struck
• Conductivity: High thermal and electrical conductivity
• Hardness: Most are hard (exception: sodium and potassium)
• Melting/Boiling Points: Generally high

Properties of Non-Metals:

• Non-Lustrous: Except iodine
• Brittle: Break when hammered (e.g., sulfur)
• Poor Conductors: Except graphite, which conducts electricity well
• Low Density and Soft Texture: Many are soft or gaseous
• Low Melting/Boiling Points: Especially in gaseous non-metals like nitrogen and oxygen

In-depth coverage here: Physical Properties of Metals and Non-Metals

Chemical Properties of Metals

The way metals react with air, water, acids, and other substances defines their chemical behavior.

Reaction with Air (Oxygen):

• Forms metal oxides
• Example:
• Metal oxides are basic in nature and often turn red litmus blue

Reaction with Water:

• Forms metal hydroxide + hydrogen gas
• Example:
• Not all metals react equally; sodium reacts vigorously, while gold does not react at all

Reaction with Acids:

• Produces salt and hydrogen gas
• Example:
• Hydrogen gas is seen as bubbles in lab experiments

Real-Life Example: When iron surfaces come into contact with acid rain, they corrode over time, forming rust and releasing gases.

Safety Tip: Always wear gloves and goggles during practicals involving acids.

Discover more: Chemical Properties of Metals

How Do Metals and Non-Metals React?

These reactions are usually ionic, where electrons are transferred from metals to non-metals.

Ionic Bond Formation:

• Metals lose electrons → form cations
• Non-metals gain electrons → form anions
• Result: stable ionic compound with strong electrostatic attraction

Example Reaction:

Na (metal) + Cl (non-metal) → NaCl (common salt)

Everyday Example: The salt you use in cooking is a product of a reaction between sodium and chlorine.

More examples here: How Do Metals and Non-Metals React?

Occurrence of Metals in Nature

Metals are rarely found in their pure form. Most occur in combined states within the earth’s crust.

Native State:

• Found in pure form (e.g., gold, silver)
• Usually unreactive metals

Combined State:

• Most metals occur as ores—compounds like oxides, carbonates, and sulfides
• Example: Iron as hematite (), zinc as zinc blende ()

These ores must be extracted using metallurgical processes like roasting, calcination, and reduction.

Detailed explanation: Occurrence of Metals

Uses of Metals and Non-Metals

Understanding the applications helps relate the concepts to everyday life.

Uses of Metals:

• Iron: For infrastructure like bridges, buildings, vehicles
• Aluminum: Aircraft parts, kitchen utensils, foils
• Copper: Electrical wires due to low resistance
• Zinc: Coating (galvanization) to prevent rust
• Gold & Silver: Jewelry, dentistry, electronics (high conductivity and corrosion resistance)

Uses of Non-Metals:

• Oxygen: Respiration in living organisms and in hospitals
• Nitrogen: Fertilizers (ammonium nitrate), food packaging
• Chlorine: Water disinfection, production of PVC
• Sulfur: Gunpowder, vulcanization of rubber
• Carbon: In steel production, fuels, and graphite in pencils

Frequently Asked Questions

1. What are the main differences between metals and non-metals?

Metals are lustrous, malleable, ductile, and good conductors; non-metals are dull, brittle, and poor conductors.

2. Why are metals good conductors?

They contain free electrons that allow electric and thermal energy to pass through easily.

3. How do metals react with acids?

They typically produce hydrogen gas and form salt. Example:

4. What are some common uses of non-metals?

Oxygen (breathing), nitrogen (fertilizers), chlorine (cleaning water), sulfur (industrial use).

5. How do metals and non-metals form compounds?

Metals donate electrons; non-metals accept them to form stable ionic compounds.

Conclusion

Mastering the basics of metals and non-metals is essential for building a strong foundation in Chemistry. These elements not only shape the scientific world but also influence our everyday life—from the bridges we walk on to the water we drink.

By understanding their properties, reactions, and uses, students can better appreciate the structure of matter and prepare more confidently for exams.

For additional resources, diagrams, and exam tips, visit the Chemistry section on Deeksha Vedantu’s learning portal.