Metals and Non metals Class 10 Worksheet with Online Quiz

• Learn general properties together with their exceptions.
• Use the reactivity series to predict displacement.
• Do not apply the metal–acid hydrogen rule to every acid.
• Balance ionic charges to find the simplest formula ratio.
• Distinguish mobile ions from mobile electrons.
• Compare roasting with calcination using the ore and air supply.
• Label impure anode, pure cathode and electrolyte in copper refining.
• Use controls to explain the conditions for rusting.

• Ask for a counterexample to an overgeneralised property statement.
• Let learners predict displacement before running the virtual test.
• Use ion counts to explain why MgCl₂ contains two chloride ions.
• Switch conductivity states and ask what changed at particle level.
• Use the rusting controls to distinguish evidence from assumption.

This Metals and Non-metals Class 10 worksheet page brings together written practice, an online quiz, virtual experiments and interactive particle diagrams. Revise physical properties, chemical reactions, the reactivity series, ionic compounds, extraction, refining and corrosion. Use the worksheet download already provided on the page for written work, then practise the concepts above.

Metals and Non-metals Properties and Exceptions

Malleability means forming sheets; ductility means drawing wires. These properties should not be confused. Non-metals also have exceptions, including very hard diamond. Chemical identity cannot be established from shine or hardness alone.

Metals and Non-metals Class 10 Reactivity Series

K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Hg > Ag > Au

Hydrogen is included as a reference, although it is a non-metal. A more reactive metal can displace a less reactive metal from a suitable salt solution in the school model. Very reactive metals such as sodium also react with water, so they should not be treated as ordinary aqueous displacement demonstrations.

Metals Reacting with Oxygen Water and Acids

Magnesium burns to form magnesium oxide. Sodium and calcium react with cold water to form hydroxides and hydrogen. In the school comparison, magnesium reacts with hot water; hot iron reacts with steam to form Fe₃O₄ and hydrogen. Copper does not react with water or steam in that comparison.

Metals above hydrogen commonly release H₂ with suitable dilute acids such as HCl. Nitric acid usually oxidises the metal without giving hydrogen in this simple pattern. NCERT notes exceptions for magnesium and manganese with very dilute HNO₃. Avoid the claim that every metal with every acid produces hydrogen.

Ionic Bonding and Electron Dot Structures Class 10

In the school electron-transfer model, metals lose electrons to form positive ions and non-metals gain electrons to form negative ions. Electrostatic attraction holds these ions in a lattice. The formula gives the simplest ratio, not a separate molecule.

For Al₂O₃, two Al³⁺ ions give total charge +6 and three O²⁻ ions give −6. Six electrons are transferred per formula-unit ratio in the model.

Why Ionic Compounds Conduct When Molten or Dissolved

Solid ionic compounds have ions fixed in lattice positions and do not conduct through ion movement. When molten, or dissolved if sufficiently soluble, mobile ions can carry charge. Metallic conduction instead involves mobile electrons. Strong attractions between oppositely charged ions also explain the generally high melting points of ionic compounds.

Extraction of Metals Class 10 Flow Chart Explained

An ore is a mineral deposit from which extraction is economically viable under relevant conditions. Gangue refers to unwanted earthy impurities. Ore treatment depends on the actual mineral and economics; a reactivity table is a guide, not a complete industrial recipe.

Roasting and Calcination Difference

Roasting heats a suitable sulphide ore in air to form an oxide. Calcination heats a suitable ore, commonly a carbonate, in limited or no air. They are different pretreatment routes.

Electrolytic Refining of Copper Labelled Diagram

The virtual activity shows impure copper as the positive anode, a thin pure copper sheet as the negative cathode, and acidified copper sulphate as electrolyte. Copper enters solution from the anode and deposits on the cathode. Insoluble impurities can collect as anode mud; some other impurities remain in solution.

Corrosion Rusting and Prevention Class 10

Ordinary rusting of iron requires oxygen and moisture. The three-tube activity compares air plus water, boiled water protected by oil, and dry air with a drying agent. Rust is expected where both required conditions are available. Painting, oiling, galvanisation and appropriate alloying can reduce corrosion. Aluminium forms a protective oxide layer despite being reactive.

Silver tarnish is mainly silver sulphide in sulphur-containing air. Copper’s green coating is commonly described as basic copper carbonate. Brass contains copper and zinc; bronze mainly copper and tin. Alloying changes properties for particular uses.

Important Questions and Competency Based Practice

1. Explain a property exception rather than memorising an absolute rule.
2. Infer a reactivity order from displacement observations.
3. Draw electron transfer and justify the ion ratio.
4. Compare conductivity in solid, molten and dissolved states.
5. Choose an extraction route and distinguish roasting from calcination.
6. Label the refining setup and explain corrosion controls.

Current Syllabus and Sample Paper Update

The official CBSE Science syllabus for 2026–27 lists material properties, reactivity, ionic compounds, basic metallurgy and corrosion. The official Science sample paper includes comparisons of heat conduction in metal rods and evaluation of a proposed metal displacement observation. Practise reading evidence and controlling experimental variables. The tasks here are original practice, not a claimed list of repeated board questions.

Malleability means forming thin sheets; ductility means drawing thin wires. Many metals show both properties.

Mercury is a liquid metal at ordinary room temperature. Sodium and potassium are soft metals. Graphite conducts electricity, iodine is lustrous and diamond is very hard despite being non-metal forms.

Compare the metals in the reactivity series. A more reactive metal can replace a less reactive metal from a suitable salt solution in the stated school-model conditions.

Copper is less reactive than zinc, so it does not produce the proposed displacement under the usual conditions.

Magnesium forms Mg²⁺ and chlorine forms Cl⁻. One magnesium ion needs two chloride ions to balance the charge.

Molten ions can move and carry charge. In a solid lattice the ions are fixed. Suitable aqueous solutions also conduct through mobile ions.

They react with both acids and bases. Aluminium oxide and zinc oxide are standard Class 10 examples.

Roasting commonly heats sulphide ore in air. Calcination commonly heats carbonate ore in limited or no air. Both can produce oxides for further extraction.

Their compounds can be too stable for reduction by carbon in the school extraction model. Electrical energy drives reduction from suitable molten compounds.

Impure copper is the positive anode and a thin pure copper sheet is the negative cathode. The electrolyte is a suitable copper salt solution, commonly acidified copper sulphate.

Ordinary rusting needs oxygen and moisture. Protective coatings, oiling, galvanisation and suitable alloying can reduce corrosion.

Practise property exceptions, reactivity predictions, electron-transfer diagrams, ionic conductivity, extraction routes, balanced equations, refining labels and interpretation of corrosion experiments. Use verified papers for actual previous-year questions.