9th ICSE - Regular Batch

• The Language of Chemistry

(i) Symbol of an element; valency; formulae of radicals and formulae of compounds. Balancing of simple chemical equations.

1. Symbol – definition; symbols of the elements used often.
2. Valency - definition; hydrogen combination and number of valence electrons of the metals and non-metals; mono, di, tri and tetra valent elements.
3. Radicals – definition; formulae and valencies.
4. Compounds – name and formulae.
5. Chemical equation – definition and examples of chemical equations with one reactant and two or three products, two reactants and one product, two reactants and two products and two reactants and three or four products; balancing of equations. (by hit and trial method).

(ii) Relative Atomic Masses (atomic weights) and Relative Molecular Masses (molecular weights): either - standard H atom or 1/12th of carbon 12 atom.

1. Definitions
2. Calculation of Relative Molecular Mass and percentage composition of a compound.

• Chemical changes and reactions

(i) Types of chemical changes.

1. Direct combination
2. Decomposition
3. Displacement;
4. Double decomposition

(The above to be taught with suitable chemical equations as examples).

(ii) Energy changes in a chemical change. Exothermic and endothermic reactions with examples – evolution/absorption of heat, light and electricity.

• Water

(i) Water as a universal solvent.

1. Solutions as 'mixtures' of solids in water; saturated solutions.
2. Qualitative effect of temperature on solubility (e.g. solutions of calcium sulphate, potassium nitrate and sodium chloride in water).

(ii) Hydrated and anhydrous substances.
(a) Hydrated substances: Water of Crystallisation – meaning and examples.
(b) Anhydrous substances: Meaning and examples only
(c) Properties:

1. Efflorescence
2. Deliquescence
3. Hygroscopy

(Definition and examples of each of the above).
(iii)Drying and Dehydrating Agents: Meaning and examples only.

• Atomic Structure and Chemical bonding

(i) Structure of an Atom, mass number and atomic number, Isotopes and Octet Rule.

1. Definition of an atom
2. Constituents of an atom - nucleus (protons, neutrons) with associated electrons; mass number, atomic number.
3. Electron distribution in the orbits - 2n2 rule, Octet rule. Reason for chemical activity of an atom.
4. Definition and examples of isotopes (hydrogen, carbon, chlorine).

(ii) Electrovalent and covalent bonding, structures of various compounds – orbit structure
(a) Electrovalent Bond

1. Definition
2. Atomic orbit structure for the formation of Electrovalent compounds (e.g. NaCl, MgCl2, CaO);

(b) Covalent Bond

1. Definition
2. Atomic orbit structure for the formation of Covalent molecules on the basis of duplet and octet of electrons (examples: hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia, carbon tetrachloride, methane.)

• The Periodic Table

Dobereiner’s Triads, Newland’s law of Octaves, Mendeleev’s contributions; Modern Periodic Law, the Modern Periodic Table. (Groups and periods)

1. General idea of Dobereiner’s triads, Newland’s law of Octaves, Mendeleev’s periodic law.
2. Discovery of Atomic Number and its use as a basis for Modern Periodic law.
3. Modern Periodic Table (Groups 1 to 18 and periods 1 to 7).
4. Special reference to Alkali metals (Group 1), Alkaline Earth metals (Group 2) Halogens (Group 17) and Zero Group (Group 18).
5. Study of the First Element -Hydrogen

Position of the non-metal (Hydrogen) in the periodic table and general group characteristics with reference to valency electrons, burning, ion formation applied to the above-mentioned element.

(i) Hydrogen from: water, dilute acids and alkalis.
(a) Hydrogen from water:

1. The action of cold water on sodium potassium and calcium.
2. The action of hot water on magnesium.
3. The action of steam on aluminium, zinc, and iron; (reversibility of reaction between iron and steam).
4. The action of steam on non-metal (carbon).
5. Students can be shown the action of sodium and calcium on water in the laboratory. They must be asked to make observations and write equations for the above reactions.
6. Application of activity series for the above-mentioned reactions.

(b) Displacement of hydrogen from dilute acids. The action of dilute sulphuric acid or hydrochloric acid on metals: Mg, Al, Zn and Fe . (To understand reasons for not using other metals and dilute nitric acid.)
(c) Displacement of hydrogen from alkalis. The action of Alkalis ((NaOH, KOH) on Al, Zn and Pb – unique nature of these elements.
(ii) The preparation and collection of hydrogen by a standard laboratory method other than electrolysis. In the laboratory preparation, the reason for using zinc, the impurities in the gas, their removal and the precautions in the collection of the gas must be mentioned.
(iii) Industrial manufacture of hydrogen by Bosch process.

1. Main reactions and conditions.
2. Separation of CO2 and CO from hydrogen.

(iv) Oxidation and reduction reactions. Differences in terms of addition and removal of oxygen / hydrogen.

• Study of Gas Laws

(i) The behaviour of gases under changes of temperature and pressure; explanation in terms of molecular motion (particles, atoms, molecules); Boyle’s Law and Charles’ Law; absolute zero; gas equation; simple relevant calculations.

1. The behaviour of gases under changes of temperature and pressure; explanation in terms of molecular motion (particles, atoms, molecules).
2. Boyle’s Law: statement, mathematical form, simple calculations.
3. Charles’ Law: statement, mathematical form, simple calculations.
4. Absolute zero Kelvin scale of temperature.
5. Gas equation P1 V1 / T1 = P2 V2 / T2; simple relevant calculations based on gas equation.

(ii) Relationship between Kelvin scale and Celsius Scale of temperature; Standard temperature and pressure. Conversion of temperature from Celsius Scale to Kelvin scale and vice versa. Standard temperature and pressure. (Simple calculations).

There will be one paper of 2 Hrs duration of 80 marks and Internal Assessment of practical work carrying 20 marks.

The paper will be divided into 2 sections, Section I (40 marks) and Section II (40 marks).

Section I (compulsory) will contain short answer questions on the entire syllabus.

Section II will contain six questions. Candidates will be required to answer any four of these six questions.

Note: All chemical process/reactions should be studied with reference to the reactants, products, conditions, observation, the (balanced) equations and diagrams.

•  Chapter : Periodic Properties and variations of Properties – Physical and Chemical.

1. Periodic properties and their variations in groups and periods. Definitions and trends of the following periodic properties in groups and periods should be studied:
   • atomic size
   • metallic character
   • non-metallic character
   • ionisation potential
   • electron affinity
   • electronegativity
2. Periodicity on the basis of atomic number for elements.
3. The study of modern periodic table up to period 3 (students to be exposed to the complete modern periodic table but no questions will be asked on elements beyond period 3 – Argon);
4. Periodicity and other related properties to be explained on the basis of nuclear charge and shells (not orbitals). (Special reference to the alkali metals and halogen groups).

Chemical Bonding

Electrovalent, covalent and co-ordinate bonding, structures of various compounds, Electron dot structure.

Electrovalent bonding:

1. Electron dot structure of Electrovalent compounds NaCl, MgCl2, CaO.
2. Characteristic properties of electrovalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), dissociation in solution and in molten state to be linked with electrolysis.

Covalent Bonding:

1. Electron dot structure of covalent molecules on the basis of duplet and octet of electrons (example: hydrogen, chlorine, nitrogen, ammonia, carbon tetrachloride, methane.
2. Polar Covalent compounds – based on difference in electronegativity: Examples – HCl and H2O including structures.
3. Characteristic properties of Covalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), ionisation in solution.
4. Comparison of Electrovalent and Covalent compounds.

Coordinate Bonding:

1. Definition
2. The lone pair effect of the oxygen atom of the water molecule and the nitrogen atom of the ammonia molecule to explain the formation of H3O+ and OH- ions in water and NH4+ ion.
3. The meaning of lone pair; the formation of hydronium ion and ammonium ion must be explained with help of electron dot diagrams.

Study of Acids, Bases and Salts

1. Simple definitions in terms of the molecules and their characteristic properties.
2. Ions present in mineral acids, alkalis and salts and their solutions; use of litmus and pH paper to test for acidity and alkalinity.
3. Examples with equation for the ionisation/dissociation of ions of acids, bases and salts.
4. Acids form hydronium ions (only positive ions) which turn blue litmus red, alkalis form hydroxyl ions (only negative ions) with water which turns red litmus blue.
5. Salts are formed by partial or complete replacement of the hydrogen ion of an acid by a metal. (To be explained with suitable examples).
6. Introduction to pH scale to test for acidity, neutrality and alkalinity by using pH paper or Universal indicator.
7. Definition of salt; types of salts.
8. Types of salts: normal salts, acid salt, basic salt, definition and examples.

• Chapter: Analytical Chemistry

1. Action of Ammonium Hydroxide and Sodium Hydroxide on solution of salts: colour of salt and its solution; formation and colour of hydroxide precipitated for solutions of salts of Ca, Fe, Cu, Zn and Pb; special action of ammonium hydroxide on solutions of copper salt and sodium hydroxide on ammonium salts.
2. On solution of salts: Colour of salt and its solution. Action on addition of Sodium Hydroxide to solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess. Formation and colour of hydroxide precipitated to be highlighted with the help of equations. Action on addition of Ammonium Hydroxide to solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess. Formation and colour of hydroxide precipitated to be highlighted with the help of equations.
3. Special action of Ammonium Hydroxide on solutions of copper salts and sodium hydroxide on ammonium salts.
4. Action of alkalis (NaOH, KOH) on certain metals, their oxides and hydroxides. The metal aluminium, its oxide and hydroxide, which react with caustic alkalis (NaOH, KOH), showing the amphoteric nature of this substance.

• Chapter: Mole Concept and Stoichiometry

1. Vapour Density and its relation to relative molecular mass.
2. Molecular mass = 2×vapour density (formal proof not required)
3. Deduction of simple (empirical) and molecular formula from: The percentage composition of a compound. The masses of combining elements.

• Chapter: Electrolysis

1. Electrolytes and non-electrolytes. Definitions and examples.
2. Substances containing molecules only, ions only, both molecules and ions.
3. Substances containing molecules only ions only, both molecules and ions.
4. Examples: relating their composition with their behaviour as strong and weak electrolytes as well as non-electrolytes.
5. Definition and explanation of electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation and reduction (on the basis of loss and gain of electrons).
6. An elementary study of the migration of ions, with reference to the factors influencing selective discharge of ions (reference should be made to the activity series as indicating the tendency of metals, e.g. Na, Mg, Fe, Cu, to form ions) illustrated by the electrolysis of: Molten lead bromide acidified water with platinum electrodes Aqueous copper (II) sulphate with copper electrodes; electron transfer at the electrodes. The above electrolytic processes can be studied in terms of electrolyte used, electrodes used, ionization reaction, anode reaction, cathode reaction, use of selective discharge theory, wherever applicable.
7. Applications of electrolysis:
8. Electroplating with nickel and silver, choice of electrolyte for electroplating.
9. Electro refining of copper. 
10. Reasons and conditions for electroplating; names of the electrolytes and the electrodes used should be given. Equations for the reactions at the electrodes should be given for electroplating, refining of copper.

• Chapter: Metallurgy

1. Occurrence of metals in nature. • Mineral and ore - meaning only. • Common ores of aluminium.
2. Extraction of Aluminium.
3. Chemical method for purifying bauxite by using NaOH – Baeyer’s Process.
4. Electrolytic extraction – Hall Heroult’s process:
5. Structure of electrolytic cell - the various components as part of the electrolyte, electrodes and electrode reactions.
6. Description of the changes occurring, purpose of the substances used and the main reactions with their equations.

• Study of Compounds

A. Hydrogen Chloride

1. Hydrogen chloride: preparation of hydrogen chloride from sodium chloride; refer to the density and solubility of hydrogen chloride (fountain experiment); reaction with ammonia; acidic properties of its solution.
2. Preparation of hydrogen chloride from sodium chloride; the laboratory method of preparation can be learnt in terms of reactants, product, condition, equation, diagram or setting of the apparatus, procedure, observation, precaution, collection of the gas and identification.
3. Simple experiment to show the density of the gas (Hydrogen Chloride) – heavier than air.
4. Solubility of hydrogen chloride (fountain experiment); setting of the apparatus, procedure, observation, inference.
5. Method of preparation of hydrochloric acid by dissolving the gas in water- the special arrangement and the mechanism by which the back suction is avoided should be learnt.

              a.  Reaction with ammonia.

              b.  Acidic properties of its solution - reaction with metals, their oxides, hydroxides and carbonates to give their chlorides; decomposition of carbonates, hydrogen carbonates, sulphides, sulphites.

              c. Precipitation reactions with silver nitrate solution and lead nitrate solution.

B. Ammonia

1. Ammonia: its laboratory preparation and collection from ammonium chloride; ammonia from ammonium salts. Manufacture by Haber’s Process; density and solubility of ammonia (fountain experiment); aqueous solution of ammonia; its reactions with hydrogen chloride and with hot copper (II) oxide and chlorine; the burning of ammonia in oxygen.
2. Laboratory preparation from ammonium chloride and collection; (the preparation to be studied in terms of, setting of the apparatus and diagram, procedure, observation, collection and identification)
3. Ammonia from ammonium salts using alkalies.
4. The reactions to be studied in terms of reactants, products, conditions and equations.Manufacture by Haber’s Process.Density and solubility of ammonia (fountain experiment). The burning of ammonia in oxygen. The catalytic oxidation of ammonia (with conditions and reaction) Its reactions with hydrogen chloride and with hot copper (II) oxide and chlorine (both chlorine in excess and ammonia in excess).
5. All these reactions may be studied in terms of reactants, products, conditions, equations, and observations.  Aqueous solution of ammonia - reaction with sulphuric acid, nitric acid, hydrochloric acid and solutions of iron (III) chloride, iron(II) sulphate, lead nitrate, zinc nitrate and copper sulphate.

C. Nitric Acid

1. Nitric Acid: one laboratory method of preparation of nitric acid from potassium nitrate or sodium nitrate. Large scale preparation. Nitric acid as an oxidizing agent.
2. Laboratory preparation of nitric acid from potassium nitrate or sodium nitrate; the laboratory method to be studied in terms of reactants, products, conditions, equations, setting up of apparatus, diagram, precautions, collection and identification. • Manufacture of Nitric acid by Ostwald’s process (Only equations with conditions where applicable).
3. As an oxidising agent: its reaction with copper, carbon, sulphur.

D. Sulphuric Acid

1. Sulphuric Acid: its behaviour as an acid when dilute, as an oxidizing agent when concentrated - oxidation of carbon and sulphur; as a dehydrating agent - dehydration of sugar and copper (II) sulphate crystals; its non-volatile nature.
2. Its behaviour as an acid when dilute - reaction with metal, metal oxide, metal hydroxide, metal carbonate, metal bicarbonate, metal sulphite, metal sulphide.
3. Concentrated sulphuric acid as an oxidizing agent - the oxidation of carbon and sulphur.
4. Concentrated sulphuric acid as a dehydrating agent- (a) the dehydration of sugar (b) Copper (II) sulphate crystals.
5. Non-volatile nature of sulphuric acid -reaction with sodium or potassium chloride and sodium or potassium nitrate.

• Chapter : Organic Chemistry

1. Introduction to Organic compounds. Unique nature of Carbon atom – tetra valency, catenation. Formation of single, double and triple bonds, straight chain, branched chain, cyclic compounds (only benzene).
2. Structure and Isomerism. Structure of compounds with single, double and triple bonds. Structural formulae of hydrocarbons. Structural formula must be given for: alkanes, alkenes, alkynes up to 5 carbon atoms. Isomerism – structural (chain, position). Homologous series – characteristics with examples.
3. Alkane, alkene, alkyne series and their gradation in properties and the relationship with the molecular mass or molecular formula.
4. Simple nomenclature. Simple nomenclature - of the hydrocarbons with simple functional groups – (double bond, triple bond, alcoholic, aldehydes, carboxylic group) longest chain rule and smallest number for functional groups rule – trivial and IUPAC names (compounds with only one functional group).
5. Hydrocarbons: alkanes, alkenes, alkynes. Alkanes - general formula; methane (greenhouse gas) and ethane, Complete combustion of methane and ethane, reaction of methane and ethane with chlorine through substitution. Alkenes – (unsaturated hydrocarbons with a double bond); ethene as an example. Alkynes - (unsaturated hydrocarbons with a triple bond); ethyne as an example of alkyne.
6. Only main properties, particularly addition products with hydrogen and halogen namely Cl2, Br2 and I2 pertaining to alkenes and alkynes.

There will be one paper of 2 Hrs duration of 80 marks and Internal Assessment of practical work carrying 20 marks.

The paper will be divided into 2 sections, Section I (40 marks) and Section II (40 marks).

Section I (compulsory) will contain short answer questions on the entire syllabus.

Section II will contain six questions. Candidates will be required to answer any four of these six questions.

Note: All chemical process/reactions should be studied with reference to the reactants, products, conditions, observation, the (balanced) equations and diagrams.

• Chapter: Basic Biology

1. Cell Cycle and Cell Division. Cell cycle – Interphase (G1, S, G2) and Mitotic phase. Cell Division:  Mitosis and its stages. A basic understanding of Meiosis as a reduction division (stages not required). A brief idea of homologous chromosomes and crossing over leading to variations.Significance and major differences between mitotic and meiotic division.
2. Structure of chromosome. Basic structure of chromosome with elementary understanding of terms such as chromatin, chromatid, gene structure of DNA and centromere.

• Chapter:  Plant Physiology

1. Absorption by roots, imbibition, diffusion and osmosis; osmotic pressure, root pressure; turgidity and flaccidity; plasmolysis and deplasmolysis; the absorption of water and minerals; active and passive transport (in brief); The rise of water up to the xylem; Forces responsible for ascent of sap. Understanding of the processes related to absorption of water by the roots. Characteristics of roots, which make them suitable for absorbing water.
2. Structure of a single full-grown root hair. A general idea of Cohesive, Adhesive forces and transpirational pull. Experiments to show the conduction of water through the xylem.
3. Transpiration - process and significance. Ganong’s potometer and its limitations. The factors affecting rate of transpiration. Experiments on transpiration. A brief idea of guttation and bleeding. Concept of transpiration and its importance to plants. Experiments related to transpiration: (a) Loss in weight of a potted plant or a leafy shoot in a test tube as a result of transpiration. (b)Use of cobalt chloride paper to demonstrate unequal rate of transpiration in a dorsiventral leaf. Mechanism of stomatal transpiration on the basis of potassium ion exchange theory. Adaptations in plants to reduce transpiration. A brief idea of guttation and bleeding.
4. Photosynthesis: the process and its importance to life in general; experiments to show the necessity of light, carbon dioxide, chlorophyll, formation of starch and release of oxygen; carbon cycle. The process and significance of Photosynthesis. The internal structure of chloroplast to be explained to give an idea of the site of light and dark reactions. Opening and closing of stomata based on potassium ion exchange theory. Overall balanced chemical equation to represent photosynthesis. Introduction of the terms "photochemical" for light phase and "biosynthetic" for dark phases. Light reaction - activation of chlorophyll followed by photolysis of water, release of O2, formation of ATP (photophosphorylation) and NADPH. Dark reaction - only combination of hydrogen released by NADP with CO2 to form glucose. (detailed equations are not required). Adaptations in plants for photosynthesis. Experiments with regard to the factors essential for photosynthesis; emphasis on detaching and the steps involved in starch test. A diagrammatic representation of “carbon cycle”.

• Chapter: Human Anatomy and Physiology

1. Circulatory System: Blood and lymph, the structure and working of the heart, blood vessels, circulation of blood (only names of the main blood vessels entering and leaving the heart, liver and kidney will be required). Lymphatic system. Composition of blood (structure and functions of RBC, WBC and platelets). Brief idea of tissue fluid and lymph. Increase in efficiency of mammalian red blood cells due to absence of certain organelles; reasons for the same. A brief idea of blood coagulation. Structure and working of the heart along with names of the main blood vessels entering and leaving the heart, the liver and the kidney. Concept of systole and diastole; concept of double circulation. Brief idea of pulse and blood pressure. Blood vessels: artery, vein and capillary to be explained with the help of diagrams to bring out the relationship between their structure and function. Brief idea of the lymphatic organs: spleen and tonsils. ABO blood group system, Rh factor.  Significance of the hepatic portal system.
2. Excretory System: A brief introduction to the excretory organs; parts of the urinary system; structure and function of the kidneys; blood vessels associated with kidneys; structure and function of nephron: A brief idea of different excretory organs in the human body. External and internal structure of the kidney. Parts of the urinary system along with the blood vessels entering and leaving the kidney; functions of various parts of the urinary system (emphasis on diagram with correct labelling). A general idea of the structure of a kidney tubule/ nephron. A brief idea of ultra-filtration (emphasis on the diagram of Malpighian capsule); selective reabsorption and tubular secretion in relation to the composition of blood plasma and urine formed.
3. Nervous system: Structure of Neuron; central, autonomous and peripheral nervous system (in brief); brain and spinal cord; reflex action and how it differs from voluntary action. Sense organs – Eye: Structure, functions, defects and corrective measures: Ear: Parts and functions of the ear. Parts of a neuron. Various parts of the external structure of the brain and its primary parts: Medulla Oblongata, Cerebrum, Cerebellum, Thalamus, Hypothalamus and Pons; their functions. Reference to the distribution of white and gray matter in Brain and Spinal cord. Voluntary and involuntary actions – meaning with examples. Diagrammatic explanation of the reflex arc, showing the pathway from receptor to effector. A brief idea of the peripheral and autonomic nervous system in regulating body activities. Differences between natural and acquired reflex. External and Internal structure and functions of the Eye and Ear and their various parts. A brief idea of stereoscopic vision, adaptation and accommodation of eye. Defects of the eye (myopia, hyperopia hypermetropia, presbyopia, astigmatism and cataract) and corrective measures (diagrams included for myopia and hyperopia only). The course of perception of sound in human ear. Role of ear in maintaining balance of the body.
4. Endocrine System: General study of the following glands: Adrenal, Pancreas, Thyroid and Pituitary. Endocrine and Exocrine glands. Differences between Endocrine and Exocrine glands. Exact location and shape of the endocrine glands in the human body. Hormones secreted by the following glands: Pancreas: insulin and glucagon; Thyroid: only thyroxin; Adrenal gland: Cortical hormones and adrenaline; Pituitary: growth hormone, tropic hormones, ADH and oxytocin. Effects of hypo secretion and hyper secretion of hormones. A brief idea of Feedback mechanism with reference to TS

• Chapter: Force, Work, Power and Energy

1. Turning forces concept; moment of a force; forces in equilibrium; centre of gravity; [discussions using simple examples and simple numerical problems]. Elementary introduction of translational and rotational motions; moment (turning effect) of a force, also called torque and its cgs and SI units; common examples - door, steering wheel, bicycle pedal, etc.; clockwise and anti-clockwise moments; conditions for a body to be in equilibrium ( translational and rotational); principle of moment and its verification using a metre rule suspended by two spring balances with slotted weights hanging from it; simple numerical problems; Centre of gravity (qualitative only) with examples of some regular bodies and irregular lamina.
2. Uniform circular motion. As an example of constant speed, though acceleration (force) is present. Differences between centrifugal and centripetal force.
3. Work, energy, power and their relation with force. Definition of work. W = FS cosθ; special cases of θ = 00, 900. W= mgh. Definition of energy, energy as work done. Various units of work and energy and their relation with SI units. [erg, calorie, kW h and eV]. Definition of Power, P=W/t; SI and cgs units; other units, kilowatt (kW), megawatt (MW) and gigawatt (GW); and horsepower (1hp=746W) [Simple numerical problems on work, power and energy].
4. Different types of energy (e.g. chemical energy, Mechanical energy, heat energy, electrical energy, nuclear energy, sound energy, light energy).
5. Mechanical energy: potential energy U = mgh (derivation included) gravitational PE, examples; kinetic energy K= ½ mv2 (derivation included); forms of kinetic energy: translational, rotational and vibrational - only simple examples. [Numerical problems on K and U only in case of translational motion]; qualitative discussions of electrical, chemical, heat, nuclear, light and sound energy, conversion from one form to another; common examples.
6. Machines as force multipliers; load, effort, mechanical advantage, velocity ratio and efficiency; pulley systems showing the utility of each type of machine. Functions and uses of simple machines: Terms- effort E, load L, mechanical advantage MA = L/E, velocity ratio VR = VE/VL = dE / dL, input (Wi), output (Wo), efficiency (η), relation between η and MA, VR (derivation included); for all practical machines η <1; MA < VR. Pulley system: single fixed, single movable, block and tackle (using single tackle).; MA, VR and η in each case.
7. Principle of Conservation of energy. Statement of the principle of conservation of energy; theoretical verification that U + K= constant for a freely falling body. Application of this law to simple pendulum (qualitative only); [simple numerical problems].

• Chapter: Light

1. Refraction of light through a glass block and a triangular prism - qualitative treatment of simple applications such as real and apparent depth of objects in water and apparent bending of sticks in water. Applications of refraction of light.
2. Partial reflection and refraction due to change in medium. Laws of refraction; the effect on speed (V), wavelength (λ) and frequency (f) due to refraction of light; conditions for a light ray to pass undeviated. Values of speed of light (c) in vacuum, air, water and glass; refractive index μ = c/V,V = fλ. Values of μ for common substances such as water, glass and diamond; experimental verification; refraction through glass block; lateral displacement; refraction through a glass prism, simple applications: real and apparent depth of objects in water; apparent bending of a stick under water. (Simple numerical problems and approximate ray diagrams required).
3. Total internal reflection: Critical angle; examples in triangular glass prisms; comparison with reflection from a plane mirror (qualitative only). Applications of total internal reflection.
4. Transmission of light from a denser medium (glass/water) to a rarer medium (air) at different angles of incidence; critical angle (C) μ = 1/sinC. Essential conditions for total internal reflection. Total internal reflection in a triangular glass prism; ray diagram, different cases - angles of prism (60º,60º,60º), (60º,30º,90º), (45º,45º,90º); use of right angle prism to obtain δ = 90º and 180º (ray diagram); comparison of total internal reflection from a prism and reflection from a plane mirror.
5. Lenses (converging and diverging) including characteristics of the images formed (using ray diagrams only); magnifying glass; location of images using ray diagrams and thereby determining magnification.
6. Types of lenses (converging and diverging), convex and concave, action of a lens as a set of prisms; technical terms; centre of curvature, radii of curvature, principal axis, foci, focal plane and focal length; detailed study of refraction of light in spherical lenses through ray diagrams; formation of images - principal rays or construction rays; location of images from ray diagram for various positions of a small linear object on the principal axis; characteristics of images. Sign convention and direct numerical problems using the lens formula are included (derivation of formula not required). Scale drawing or graphical representation of ray diagrams not required. Power of a lens (concave and convex); Only definition and basic understanding based on the curvature or thickness of lens. Applications of lenses.
7. Using a triangular prism to produce a visible spectrum from white light; Electromagnetic spectrum.
8. Deviation produced by a triangular prism; dependence on colour (wavelength) of light; dispersion and spectrum; electromagnetic spectrum: broad classification (names only arranged in order of increasing wavelength); properties common to all electromagnetic radiations; properties and uses of infrared and ultraviolet radiation.

• Chapter:  Sound

1. Reflection of Sound Waves; echoes: their use; simple numerical problems on echoes. Production of echoes, condition for formation of echoes; simple numerical problems; use of echoes by bats, dolphins, fishermen, medical field. SONAR.
2. Natural vibrations, Damped vibrations, Forced vibrations and Resonance - a special case of forced vibrations. Meaning and simple applications of natural, damped, forced vibrations and resonance.
3. Loudness, pitch and quality of sound.
4. Meaning of the terms and the factors affecting them (no examples).

• Chapter: Electricity and Magnetism

1. Ohm’s Law; concepts of emf, potential difference, resistance; resistances in series and parallel, internal resistance. Concepts of pd (V), current (I), resistance (R) and charge (Q). Ohm's law: statement, V=IR; SI units; graph of V vs I and resistance from slope; ohmic and non-ohmic resistors, factors affecting resistance (including specific resistance) and internal resistance; super conductors, electromotive force (emf); combination of resistances in series and parallel. Simple numerical problems using the above relations. [Simple network of resistors involving not more than four external resistors in a circuit].
2. Electrical power and energy. Electrical energy; examples of heater, motor, lamp, loudspeaker, etc. Electrical power; measurement of electrical energy, W = QV = VIt from the definition of pd. Combining with ohm’s law W = VIt = I2 Rt = (V2/R)t and electrical power P = (W/t) = VI = I2R = V2/R. Units: SI and commercial; Power rating of common appliances, household consumption of electric energy; calculation of total energy consumed by electrical appliances; W = Pt (kilowatt × hour = kW h), (simple numerical problems).
3. Household circuits – main circuit; switches; fuses; earthing; safety precautions; three-pin plugs; colour coding of wires. Main circuit (3 wires-live, neutral, earth) with fuse / MCB, main switch and its advantages, need for earthing, fuse, 3-pin plug and socket; Conventional location of live, neutral and earth points in 3 pin plugs and sockets. Safety precautions, colour coding of wires.

• Chapter: Heat

1. Calorimetry: meaning, specific heat capacity; principle of method of mixtures; Numerical Problems on specific heat capacity using heat loss and gain and the method of mixtures.
2. Heat and its units (calorie, joule), temperature and its units (oC,, K); thermal (heat) capacity C' = Q/T... (SI unit of C'): Specific heat Capacity C = Q/mT (SI unit of C) Mutual relation between Heat Capacity and Specific Heat capacity, values of C for some common substances (ice, water and copper). Principle of method of mixtures including mathematical statement. Natural phenomenon involving specific heat. Consequences of high specific heat of water. [Simple numerical problems].
3. Latent heat; loss and gain of heat involving change of state for fusion only.
4. Change of phase (state); heating curve for water; latent heat; specific latent heat of fusion (SI unit). Common physical phenomena involving latent heat of fusion.

• Chapter: Modern Physics

1. Radioactivity and changes in the nucleus; background radiation and safety precautions.
2. Brief introduction (qualitative only) of the nucleus, nuclear structure, atomic number (Z), mass number (A). Radioactivity as spontaneous disintegration. α, β and γ - their nature and properties; changes within the nucleus. One example each of α and β decay with equations showing changes in Z and A. Uses of radioactivity - radio isotopes. Harmful effects. Safety precautions. Background radiation.
3. Radiation: X-rays; radioactive fallout from nuclear plants and other sources.
4. Nuclear Energy: working on safe disposal of waste. Safety measures to be strictly reinforced.

• A NOTE ON SI UNITS

SI units were adopted internationally in 1968.

1. Fundamental units: The system has seven fundamental (or basic) units, one for each of the fundamental quantities.
2. Derived units: These are obtained from the fundamental units by multiplication or division; no numerical factors are involved. Some derived units are given special names due to their complexity when expressed in terms of the fundamental units. When the unit is named after a person, the symbol has a capital letter.
3. Standard prefixes: Decimal multiples and submultiples are attached to units when appropriate.