What are the physical properties that distinguish metals from non-metals?

Metals and non-metals differ significantly in their physical properties. Metals are generally lustrous (shiny), hard, malleable (can be beaten into sheets), ductile (can be drawn into wires), and good conductors of heat and electricity. They also have high melting and boiling points and high densities. For example, iron, copper, and gold show these properties. Non-metals, on the other hand, are generally dull, brittle, poor conductors (except graphite), and have lower melting points. Sulphur, phosphorus, and iodine are typical non-metals. However, there are exceptions — sodium and potassium are soft metals, mercury is liquid at room temperature, and diamond (a form of carbon) is extremely hard despite being a non-metal.

What is the reactivity series and how does it help predict chemical reactions?

The reactivity series is a list of metals arranged in decreasing order of their chemical reactivity. From most reactive to least, it runs: potassium, sodium, calcium, magnesium, aluminium, zinc, iron, lead, hydrogen, copper, silver, gold, and platinum. This series helps predict which metals can displace others from their compounds. A more reactive metal always displaces a less reactive metal from its salt solution. For example, zinc displaces copper from copper sulphate solution. Metals above hydrogen in the series react with dilute acids to release hydrogen gas, while those below (like copper, silver, and gold) do not. The reactivity series also guides the choice of extraction methods — highly reactive metals require electrolysis while less reactive ones can be extracted by reduction.

How are metals extracted from their ores? Explain the main steps.

Metal extraction from ores involves several steps depending on the reactivity of the metal. First, the ore is concentrated by removing gangue (impurities) through methods like hydraulic washing, froth flotation, or magnetic separation. Next, the concentrated ore is converted into metal oxide through roasting or calcination. Then, the oxide is reduced to obtain the metal — less reactive metals like copper can be reduced by heating alone; moderately reactive metals like iron and zinc require reduction with carbon or carbon monoxide. Highly reactive metals like sodium, potassium, and aluminium are extracted using electrolysis because carbon cannot reduce their oxides. Finally, the crude metal undergoes refining through processes like electrolytic refining to obtain pure metal.

What is corrosion and how can it be prevented?

Corrosion is the gradual deterioration of metals due to their reaction with substances in the environment such as oxygen, moisture, and acids. The most common example is rusting of iron: when iron is exposed to oxygen and water, it forms hydrated iron oxide, which is the reddish-brown rust. Corrosion weakens structures, damages machinery, and costs industries billions of rupees every year. Prevention methods include painting, oiling, or greasing the metal surface to block contact with moisture and air. Galvanisation — coating iron with zinc — protects because zinc is more reactive and corrodes first (sacrificial protection). Alloying iron with chromium and nickel creates stainless steel, which resists corrosion. Electroplating with chromium or silver also provides a protective coating.

What are ionic compounds and how are they formed by metals and non-metals?

Ionic compounds are formed when metals transfer electrons to non-metals, resulting in the formation of oppositely charged ions that attract each other. Metals tend to lose electrons to form positively charged cations, while non-metals tend to gain electrons to form negatively charged anions. The electrostatic force of attraction between these oppositely charged ions forms an ionic bond. For example, sodium (Na) gives one electron to chlorine (Cl), forming Na⁺ and Cl⁻, which combine to form sodium chloride (NaCl). Ionic compounds have high melting and boiling points due to strong ionic bonds, conduct electricity when dissolved in water or melted (because ions become free to move), and are generally soluble in water. They exist as crystalline solids at room temperature.

NCERT Solutions for Class 10 Science Chapter 3 Metals and Non-Metals

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NCERT Solutions for Class 10 Science Chapter 3: Metals and Non-Metals

Metals and Non-Metals is a chapter that connects everyday life to the periodic table in the most practical way possible. From the iron in your kitchen utensils to the carbon in your pencil, this chapter explains what makes certain elements behave differently from others and why those differences matter. NCERT Solutions for Class 10 Science Chapter 3 on Myclass24 are built to ensure that every student, whether in urban schools or rural learning centres across Bihar, Jharkhand, Chhattisgarh, Odisha, Assam, or Telangana, gets access to clear, stepwise explanations.

The chapter covers physical and chemical properties of metals and non-metals, the reactivity series, extraction of metals from ores, and the prevention of corrosion. These topics are not just important for CBSE board exams but also form the basis for higher-level Chemistry in Classes 11 and 12. Myclass24 solutions are designed to help students understand the underlying science rather than just memorising answers, leading to better performance in both boards and competitive exams. Every solution is aligned with the NCERT textbook and follows CBSE marking guidelines strictly.

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Chapter 3 Explained: Metals and Non-Metals — Facts and Tables

Metals and Non-Metals is a content-heavy chapter that becomes much easier when you organise it visually. Below are essential concepts with structured tables designed for mobile-friendly reading and quick revision before exams.

Physical Properties: Metals vs Non-Metals

Property	Metals	Non-Metals
State at Room Temp	Mostly solid (except Hg)	Solid, liquid, or gas
Lustre	Shiny (metallic lustre)	Dull (except iodine, graphite)
Malleability	Malleable (can be beaten into sheets)	Brittle (except graphite)
Ductility	Ductile (can be drawn into wires)	Non-ductile
Conductivity	Good conductors of heat & electricity	Poor conductors (except graphite)
Sonorous	Produce sound when struck	Not sonorous
Density	Generally high	Generally low

Chemical Properties of Metals

Reaction	Equation Example	Observation
With oxygen	4Na + O₂ → 2Na₂O	Oxide formed (basic in nature)
With water	2Na + 2H₂O → 2NaOH + H₂	Hydrogen gas released
With dilute acids	Fe + H₂SO₄ → FeSO₄ + H₂	Salt + hydrogen gas
With salt solutions	Zn + CuSO₄ → ZnSO₄ + Cu	Displacement occurs

Reactivity Series of Metals (Most to Least Reactive)

Position	Metal	Symbol	Key Behaviour
Most reactive	Potassium	K	Reacts violently with water
Very high	Sodium	Na	Reacts with cold water
High	Calcium	Ca	Reacts with cold water slowly
Moderate	Aluminium	Al	Reacts with steam
Moderate	Zinc	Zn	Reacts with steam & dilute acids
Moderate	Iron	Fe	Reacts with steam
Low	Copper	Cu	No reaction with water/steam
Least reactive	Gold / Platinum	Au / Pt	No reaction with acids

Ionic Bond Formation: Example with NaCl

When sodium (Na) donates one electron to chlorine (Cl), sodium becomes Na⁺ (cation) and chlorine becomes Cl⁻ (anion). These oppositely charged ions attract each other, forming an ionic bond. The result is sodium chloride (NaCl) — common salt. Ionic compounds have high melting and boiling points, are soluble in water, and conduct electricity in molten or dissolved state.

Extraction of Metals — Based on Reactivity

Reactivity Level	Extraction Method	Example Metals
Low reactivity	Found as free elements	Gold, Silver, Platinum
Medium reactivity	Reduction with carbon	Iron, Copper, Zinc
High reactivity	Electrolytic reduction	Sodium, Calcium, Aluminium