CBSE Class 10 Board Exam 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 Board Exam, not a summary of it.

1. 1

   Chemical Substances - Nature and Behaviour

   4 topics

   • Chemical Reactions and Equations
     • Writing and balancing chemical equations
     • Types of reactions (combination, decomposition, displacement, double displacement)
     • Oxidation, reduction and redox; corrosion and rancidity
   • Acids, Bases and Salts
     • Properties and reactions of acids and bases
     • pH scale and its importance
     • Preparation and uses of common salts
   • Metals and Non-metals
     • Physical and chemical properties
     • Reactivity series
     • Extraction of metals and metallurgy
     • Ionic compounds and corrosion prevention
   • Carbon and its Compounds
     • Covalent bonding and allotropes
     • Hydrocarbons, saturated and unsaturated
     • Functional groups and homologous series
     • Ethanol, ethanoic acid, soaps and detergents
2. 2

   World of Living

   4 topics

   • Life Processes
     • Nutrition (autotrophic and heterotrophic)
     • Respiration in organisms
     • Transportation in plants and animals
     • Excretion in humans and plants
   • Control and Coordination
     • Nervous system and reflex action
     • Coordination in plants - tropisms
     • Hormones in animals
   • How do Organisms Reproduce
     • Asexual reproduction methods
     • Sexual reproduction in plants
     • Human reproductive system and reproductive health
   • Heredity
     • Mendel's laws of inheritance
     • Sex determination
3. 3

   Natural Phenomena

   3 topics

   • Light - Reflection and Refraction
     • Spherical mirrors and mirror formula
     • Refraction and refractive index
     • Lenses and lens formula, magnification
   • Human Eye and the Colourful World
     • Structure and working of the human eye
     • Defects of vision and their correction
     • Dispersion, scattering, atmospheric refraction
   • Power of Accommodation and optical instruments basics
4. 4

   Effects of Current

   3 topics

   • Electricity
     • Electric current, potential difference, Ohm's law
     • Resistance and factors affecting it
     • Series and parallel combination of resistors
     • Heating effect of current and electric power
   • Magnetic Effects of Electric Current
     • Magnetic field due to current-carrying conductor
     • Force on a current-carrying conductor; electric motor
     • Electromagnetic induction and generator
     • Domestic electric circuits and safety
   • Magnetic Field Patterns and Right-hand Rules
5. 5

   Natural Resources

   3 topics

   • Ecosystem and its components
   • Food chains, food webs and trophic levels
   • Ozone depletion and waste management

Science flashcards for CBSE Class 10 Board Exam

23 of 64 cards from the Science deck — real questions with worked answers.

1. What is a balanced chemical equation, and why must equations be balanced?

   An equation in which the number of atoms of each element is equal on both the reactant and product sides. It must be balanced to obey the Law of Conservation of Mass (mass is neither created nor destroyed).

2. Name and define the four main types of chemical reactions with one example each.

   Combination (A+B→AB, e.g. CaO+H2O→Ca(OH)2); Decomposition (AB→A+B, e.g. 2FeSO4→Fe2O3+SO2+SO3); Displacement (A+BC→AC+B, e.g. Fe+CuSO4→FeSO4+Cu); Double displacement (AB+CD→AD+CB, e.g. Na2SO4+BaCl2→BaSO4+2NaCl).

3. Differentiate between oxidation and reduction in terms of oxygen and hydrogen.

   Oxidation = gain of oxygen or loss of hydrogen. Reduction = loss of oxygen or gain of hydrogen. They occur together in a redox reaction.

4. What is a redox reaction? Identify the oxidised and reduced species in CuO+H2→Cu+H2O.

   A reaction where oxidation and reduction occur simultaneously. Here CuO is reduced to Cu (loses oxygen) and H2 is oxidised to H2O (gains oxygen).

5. What are exothermic and endothermic reactions? Give one example of each.

   Exothermic releases heat (e.g. respiration, burning of natural gas). Endothermic absorbs heat (e.g. decomposition of calcium carbonate, photosynthesis).

6. Define acids and bases according to the Arrhenius concept.

   An acid produces H+ (hydronium, H3O+) ions in aqueous solution; a base produces OH- (hydroxide) ions in aqueous solution.

7. What is the pH scale, and what do values below, at, and above 7 indicate?

   A scale from 0–14 measuring H+ ion concentration. pH<7 = acidic, pH=7 = neutral, pH>7 = basic/alkaline. Lower pH means stronger acidity.

8. What is the general reaction of a metal with a dilute acid, and which gas is produced?

   Metal + dilute acid → salt + hydrogen gas. Example: Zn+H2SO4→ZnSO4+H2. The gas burns with a 'pop' sound, confirming hydrogen.

9. State the reaction of an acid with a base (neutralisation) in general form.

   Acid + Base → Salt + Water. Example: HCl+NaOH→NaCl+H2O. The H+ and OH- combine to form water.

10. What is water of crystallisation? Give the formula and use of Plaster of Paris.

    Fixed water molecules in a salt's crystal structure (e.g. CuSO4·5H2O). Plaster of Paris is CaSO4·½H2O, made by heating gypsum; used for setting fractured bones and making casts.

11. List the physical properties common to most metals.

    Lustrous, malleable, ductile, good conductors of heat and electricity, sonorous, generally hard, high melting/boiling points, and solid at room temperature (except mercury).

12. What is the reactivity series, and name three metals at the top and three at the bottom.

    An arrangement of metals in decreasing order of reactivity. Top (most reactive): Potassium (K), Sodium (Na), Calcium (Ca). Bottom (least reactive): Silver (Ag), Gold (Au), Platinum (Pt).

13. What is an ionic compound, and list two general properties of ionic compounds.

    A compound formed by transfer of electrons from a metal to a non-metal (e.g. NaCl). Properties: high melting/boiling points; conduct electricity in molten or aqueous state; usually soluble in water; solid and brittle.

14. Define corrosion and give the special name for the corrosion of iron.

    Corrosion is the gradual eating away of a metal surface by reaction with air/moisture/chemicals. The corrosion of iron is called rusting (forms hydrated iron(III) oxide, Fe2O3·xH2O).

15. What are alloys? Name the constituents of brass, bronze, and steel.

    Alloys are homogeneous mixtures of a metal with other metals or non-metals. Brass = copper + zinc; Bronze = copper + tin; Steel = iron + carbon.

16. Why does carbon mostly form covalent compounds, and what are catenation and tetravalency?

    Carbon shares electrons (covalent bonding) because gaining/losing 4 electrons is energetically unfavourable. Tetravalency = it forms 4 bonds. Catenation = carbon's ability to form long chains/rings by bonding with itself.

17. Differentiate between saturated and unsaturated hydrocarbons with examples.

    Saturated have only single C–C bonds (alkanes, e.g. ethane C2H6). Unsaturated have at least one double or triple bond (alkenes e.g. ethene C2H4; alkynes e.g. ethyne C2H2).

18. Name the functional groups of alcohols, carboxylic acids, aldehydes, and ketones.

    Alcohol: –OH; Carboxylic acid: –COOH; Aldehyde: –CHO; Ketone: >C=O (carbonyl between carbons).

19. What is the difference between complete and incomplete combustion of carbon compounds?

    Complete combustion (sufficient oxygen) gives CO2, water, heat, and a blue flame. Incomplete combustion (limited oxygen) gives CO, soot/carbon, and a yellow sooty flame.

20. What is the conversion of ethanol to ethanoic acid called, and what is the saponification reaction?

    Ethanol → ethanoic acid is oxidation (by alkaline KMnO4 or acidified K2Cr2O7). Saponification is the reaction of an ester (or fat) with NaOH to form soap and alcohol.

21. Define nutrition and distinguish autotrophic from heterotrophic nutrition.

    Nutrition is the process of obtaining and using food for energy and growth. Autotrophic organisms make their own food (e.g. green plants by photosynthesis); heterotrophic organisms depend on others for food (e.g. animals, fungi).

22. Write the balanced equation for photosynthesis and name the site where it occurs.

    6CO2 + 6H2O --(sunlight, chlorophyll)--> C6H12O6 + 6O2. It occurs in the chloroplasts (containing chlorophyll) of green plant cells.

23. What is the role of stomata in plants?

    Stomata are tiny pores (mainly on leaves) that allow exchange of gases (CO2 and O2) and release of water vapour during transpiration. They are opened and closed by guard cells.

See more Science flashcards →

Planning Science for CBSE Class 10 Board Exam

Science (CBSE Class 10 Board Exam) FAQ