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Matter and its Composition
(i) Inter-conversion of states of matter; m.p., b.p. (relevant experiments).
(ii) Explanation of change of state of matter on the basis of Kinetic Theory of Matter.
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 (Kelvin) zero; gas equation; simple relevant calculations.
(ii) Relationship between Kelvin Scale and Celsius Scale of temperature; Standard
temperature and pressure (reduction to S.T.P. required)
Elements, Compounds and Mixtures
(i) General characteristics and differences between elements, compounds and mixtures.
(ii) Separation of mixtures involving use of a solvent, filtration, evaporation and distillation, fractional distillation, simple paper chromatography (limited to separation of colouring matter in ink); immiscible liquids (separating funnel).
(iii) Types of mixtures: of two solids, a solid and a liquid, two liquids, liquid and gas, two
gases.
The language of Chemistry
Symbol of an element; valency; formulae of radicals and formulae of compounds. Balancing of simple chemical equations.
Physical and Chemical Changes
(i) Definitions and comparison of Physical and Chemical changes.
(ii) Conditions for chemical change.
(iii) Types of chemical change.
(iv) Energy changes in a chemical change.
(v) Burning: Definition and conditions of burning. Water
(i) Physical Properties: Water as a compound and as a universal solvent; its physical states
and chief physical properties; solutions as 'mixtures' of solids in water; saturated solutions; qualitative effect of temperature on solubility (e.g. solutions of calcium sulphate, potassium nitrate, sodium chloride in water).
(ii) Water of crystallization: removal of water of crystallization; idea of anhydrous substances; air dissolved in water and its biological importance.
(iii) Chemical Properties: The action of cold water on sodium and calcium; the action of
hot water on magnesium and steam on iron; reversibility of reaction between iron and steam; reactivity series.
Atomic Structure
(i) Atom consists of a nucleus (protons, neutrons) with associated electrons, mass number and atomic number.
(ii) Isotopes of hydrogen, carbon, chlorine. Reason for chemical activity of an atom (electronic configuration). Octet Rule.
The Periodic Table
(i) Dobereiner’s Triads, Newland’s Octaves, Mendeleev’s contributions; Modern Periodic Law, the representative periodic table for 8 groups up to period 3.
(ii) Uses of Modern Periodic Table._ Study of the First Element -Hydrogen
Position of the non-metal (Hydrogen) in the periodic table and general group characteristics applied to the above mentioned element.
(i) Hydrogen from water.
(ii) Displacement of hydrogen from dilute sulphuric acid or hydrochloric acid by zinc or iron (no reaction with copper).
(iii) Displacement of hydrogen from alkalis (NaOH, KOH) by Zn, Al.
(iv) The preparation and collection of hydrogen by a standard laboratory method other than electrolysis.
_ Study of the Group 14 (Fourth Group) Element - Carbon
Position of the non-metal (Carbon) in the periodic table and general group characteristics applied to the above mentioned element. Natural occurrence; Allotropy (definition); Allotropes of Carbon – diamond, graphite and fullerene; burning of these in O2 giving CO2. Other forms of Carbon: wood, bone charcoal, soot, gas carbon – their uses.
_ Study of the Group 15 (Fifth Group) Element - Nitrogen
Position of the non-metal (Nitrogen) in the periodic table and general group characteristics applied to the above mentioned element.
(i) Laboratory preparation and collection of nitrogen.
(ii) Properties of nitrogen.
_ Study of the Group 16 (Sixth Group) Elements – Oxygen, Sulphur Position of the non-metals (Oxygen, Sulphur) in the periodic table and general group characteristics applied to the above mentioned elements.
(i) Occurrence of oxygen in air, water and oxides.
(ii) The preparation and collection of oxygen in the laboratory e.g. from:
(i) hydrogen peroxide (ii) potassium chlorate with manganese (IV) oxide.
(iii) oxygen from higher oxides like Pb3O4, PbO2.
(iii) Density of oxygen as compared to air.
(iv) Solubility of oxygen in water.
(v) The burning of common elements in oxygen (e.g. carbon, sulphur, phosphorus, sodium, calcium, magnesium, iron); burning of a candle in air – products formed: water and carbon dioxide.
(vi) Conditions for and prevention of rusting.
(vii) Sulphur - extraction by Frasch process. Structure and process.
(viii) Chemical properties of sulphur.
(ix) Uses of sulphur. _ Study of Group 17 (Seventh Group) Element - Chlorine Position of the non-metal (Chlorine) in the periodic table and general group characteristics applied to the above mentioned element.
(i) Preparation and collection of chlorine; refer to the density, solubility andpoisonous nature of chlorine; oxidation of concentrated hydrochloric acid by MnO2; NaCl and concentrated sulphuric acid and MnO2; bleaching powder; PbO2 and Pb3O4.
(ii) Reaction of chlorine with burning sodium, hot iron, phosphorus. Sodium hydroxide solutions, cold and hot, potassium iodide solution, hydrogen sulphide and ammonia; uses of Chlorine: in water purification, bleaching agent, manufacture of hydrochloric acid and other important uses.
Study of Carbon Monoxide and Carbon Dioxide
(i) Carbon monoxide formed by incomplete combustion of carbon or carbon compounds (e.g. exhaust fumes from cars); methods of preparing and collecting carbon monoxide (preparation of CO from oxalic and formic acids); conversion of CO2 into CO and viceversa; separation of CO2 or CO from a mixture of the two; reducing property of CO with reference to metallic oxides (refer to the density, solubility and poisonous nature of carbon monoxide).
(ii) Carbon dioxide: an oxide of carbon; its formation when charcoal, wood or other organic substances (e.g. ethanol) are burned in air or oxygen; the main concept that hydrocarbons mostly contain carbon and hydrogen, which on burning produce water and carbon dioxide should be understood (can be demonstrated by burning of candle).
(iii) Obtaining CO2 from sodium hydrogen carbonate and carbonates; reaction with quicklime, slaked lime, lime water and their important uses.
(iv) The reactions of carbon dioxide with lime water, sodium hydroxide solution and magnesium; difference between CO and CO2 with reference to their densities, combustibility and action of lime water; use of carbon dioxide in refrigeration, fire extinguishers and photosynthesis.
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