CBSE Class 10 Science Syllabus

Science syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Science in CBSE Class 10, not a summary of it.

1. 1

   Chemical Substances - Nature and Behaviour

   5 topics

   • Chemical Reactions
   • Acids, Bases and Salts
   • Metals and Non-metals
   • Carbon Compounds
   • Periodic Classification of Elements
2. 2

   World of Living

   4 topics

   • Life Processes
   • Control and Coordination in Animals and Plants
   • Reproduction
   • Heredity and Evolution
3. 3

   Natural Phenomena

   5 topics

   • Reflection of Light
   • Refraction of Light
   • Refraction of Light through a Prism
   • Dispersion of Light
   • Human Eye and Colourful World
4. 4

   Effects of Current

   2 topics

   • Electric Current and its Effects
   • Magnetic Effects of Electric Current
5. 5

   Natural Resources

   3 topics

   • Sources of Energy
   • Our Environment
   • Management of Natural Resources

Science flashcards for CBSE Class 10

23 of 66 cards from the Science deck — real questions with worked answers.

1. What is a combination reaction? Give the equation for slaking of lime as an example.

   A reaction in which two or more substances combine to form a single product. CaO + H2O -> Ca(OH)2 (this is also exothermic).

2. Define a decomposition reaction and name its three types based on the energy supplied.

   A single reactant breaks into two or more products. Types: thermal (heat), electrolytic (electricity), and photolytic/photochemical (light).

3. What is a redox reaction? Define oxidation and reduction in terms of oxygen/hydrogen.

   A reaction where oxidation and reduction occur simultaneously. Oxidation = gain of oxygen or loss of hydrogen; Reduction = loss of oxygen or gain of hydrogen.

4. What is a displacement reaction? Give an example with iron and copper sulphate.

   A more reactive element displaces a less reactive one from its compound. Fe + CuSO4 -> FeSO4 + Cu (iron displaces copper; blue solution turns pale green).

5. Why is the reaction between an acid and a base called neutralisation, and what is always formed?

   Because acid and base cancel each other's properties. Acid + Base -> Salt + Water (e.g. NaOH + HCl -> NaCl + H2O).

6. What is the pH scale range, and what do values below 7, equal to 7, and above 7 indicate?

   0 to 14. Below 7 = acidic, 7 = neutral, above 7 = basic/alkaline. Lower pH means higher H+ ion concentration.

7. Which ion is responsible for acidic nature and which for basic nature in aqueous solution?

   Acids produce hydrogen ions (H+ / hydronium H3O+) in water; bases produce hydroxide ions (OH-) in water.

8. Give the common name, chemical formula, and one use of washing soda.

   Washing soda: sodium carbonate decahydrate, Na2CO3.10H2O. Used for removing permanent hardness of water and in glass/soap manufacture.

9. What is the chemical formula and a key use of baking soda, and what gas does it release on heating?

   Baking soda = sodium hydrogencarbonate, NaHCO3. Used in baking and antacids. On heating it releases carbon dioxide (CO2), which makes cakes rise.

10. How is Plaster of Paris made from gypsum and what is its formula?

    Gypsum (CaSO4.2H2O) is heated to 373 K (100 C) to form Plaster of Paris, CaSO4.(1/2)H2O. It sets into a hard solid on adding water.

11. List four general physical properties of metals.

    Metals are malleable, ductile, good conductors of heat and electricity, lustrous, sonorous, and generally hard with high melting points.

12. What are amphoteric oxides? Give two examples.

    Oxides that react with both acids and bases to form salt and water. Examples: aluminium oxide (Al2O3) and zinc oxide (ZnO).

13. State the reactivity series order for these metals: K, Na, Ca, Mg, Al, Zn, Fe, Cu, Au.

    K > Na > Ca > Mg > Al > Zn > Fe > Cu > Au (potassium most reactive, gold least reactive).

14. What is an ionic (electrovalent) bond and name two properties of ionic compounds.

    A bond formed by transfer of electrons from a metal to a non-metal. Ionic compounds have high melting points and conduct electricity in molten or aqueous state.

15. What is the difference between roasting and calcination in metallurgy?

    Roasting heats sulphide ore strongly in excess air to form oxide; calcination heats carbonate ore in limited air to form oxide. Both convert ore to metal oxide.

16. What is the catenation property of carbon and why does carbon form a large number of compounds?

    Catenation is carbon's ability to form long chains/rings by bonding with other carbon atoms. Carbon forms many compounds due to catenation and tetravalency (4 bonds).

17. State the general formula of alkanes, alkenes, and alkynes.

    Alkanes: CnH2n+2 (saturated); Alkenes: CnH2n (one C=C double bond); Alkynes: CnH2n-2 (one C triple bond C).

18. What is a homologous series and how do consecutive members differ?

    A series of compounds with the same general formula and functional group, where consecutive members differ by a -CH2- group (mass difference of 14 u).

19. Name the functional groups in alcohols, carboxylic acids, aldehydes, and ketones.

    Alcohol: -OH (hydroxyl); Carboxylic acid: -COOH; Aldehyde: -CHO; Ketone: >C=O (carbonyl).

20. What is an esterification reaction and what is formed?

    Reaction of a carboxylic acid with an alcohol (in presence of acid catalyst) to form an ester (sweet-smelling) and water. Acid + Alcohol -> Ester + Water.

21. On what basis did Mendeleev arrange elements, and what was his Periodic Law?

    Mendeleev arranged elements by increasing atomic mass. His law: properties of elements are a periodic function of their atomic masses.

22. State the Modern Periodic Law and the basis of arrangement in the modern periodic table.

    Properties of elements are a periodic function of their atomic numbers. Elements are arranged by increasing atomic number (proposed by Moseley).

23. How many periods and groups are there in the modern periodic table?

    7 periods (horizontal rows) and 18 groups (vertical columns).

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