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Periodic Properties and variations of Properties – Physical and Chemical
(i) Periodic properties and their variations in groups and periods.
(ii) Relation between atomic number for light elements (proton number) and periodicity and atomic mass for light elements; the 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); periodicity and other related properties to be described in terms of shells (not orbitals); special reference to the alkali metals and halogen groups.
Chemical Bonding – Covalent and ionic compounds – structures of various
compounds – orbit structure and electron dot structure
(i) Types of bonding: electrovalent and covalent. Compounds: characteristic properties of electrovalent and covalent compounds and differences between them; oxidation and reduction in terms of loss or gain of electrons by atoms of an element.
(ii) Structure of electrovalent compounds: NaCl, MgCl2, CaO; covalent molecules like hydrogen, chlorine, nitrogen, water, ammonia, carbon tetrachloride, methane.
(iii) Coordinate Bond: Formation of H3O+ and NH4 + ion.
Study of Acids, Bases and Salts
(i) Simple definitions in terms of the molecules and their characteristic properties.
(ii) Ions present in mineral acids, alkalis and salts and their solutions; use of litmus to test for acidity and alkalinity.
(iii) Definition of salt; types of salts.
(iv) General properties of salts:
_ Deliquescence, efflorescence, water of crystallization
_ Decomposition of bicarbonates, carbonates, chlorides and nitrates by appropriate acids with heating if necessary (relevant laboratory work must be done).
(v) Preparation: laboratory preparation of salts (normal and acid salts) – relevant laboratory work is essential.
Analytical Chemistry – Use of Ammonium Hydroxide and Sodium Hydroxide and
Standard Tests
(i) On solution of salts: colour of salt and its solution; formation and colour of hydroxide precipitated for solutions of salts of Mg, Fe, Cu, Zn and Pb; special action of ammonium hydroxide on solutions of copper salts.
(ii) On certain metals and their oxides (relevant laboratory work is essential).
Mole Concept and Stoichiometry
(i) Gay Lussac’s Law of Combining Volumes; Avogadro’s Law.
(ii) Refer to the atomicity of hydrogen, oxygen,nitrogen and chlorine (proof not required).
(iii) Relative atomic masses (atomic weight) and relative molecular masses (molecular weights): either H=1 or 12C=12 will be accepted; molecular mass = 2?vapour density (formal proof not required). Deduction of simple (empirical) and molecular formula from the percentage composition of a compound; the molar volume of a gas at S.T.P.; simple calculations based on chemical equations; both reacting weight and volumes.
Electrolysis
(i) Electrolytes and non-electrolytes.
(ii) Substances containing molecules only, ions only, both molecules and ions.
(iii) An elementary study of the migration of ions, illustrated by the electrolysis of: molten lead bromide; acidified water with platinum electrodes and aqueous copper (II) sulphate with copper electrodes; electron transfer at the electrodes.
(iv) Application of electrolysis: electroplatingwith nickel and silver; purification of copper.
(v) Acids, bases and salts as electrolytes: reference should be made to the activity series as indicating the tendency of metals, e.g. Na, Mg, Fe, Cu, to form ions; action of alkalis on certain metals and their oxides; action of acids on oxides and salts.
Metallurgy
(i) Definition of Metal and Non-metals.
(ii) Position of the metals (alkali metals and alkaline earth metals) in the Periodic table and general characteristics applied to these elements.
(iii) Comparison of Metals and Non-metals.
(iv) General properties with special reference to physical properties: state, lustre, melting point, density, ductility, malleability, brittleness, conduction of electricity (exceptions to be specifically noted - e.g. graphite, mercury); chemical properties: a metal forms at least one basic oxide; non-metal, an acidic or neutral oxide; discharge of metallic ions at the cathode from fused metallic chlorides (link with bonding and ion formation); many metals liberate hydrogen from dilute HCl and H2SO4.
(v) Reduction of metallic oxides; some can be reduced by hydrogen, carbon and carbon monoxide (e.g. copper oxide, lead oxide, iron (II) oxide) and some cannot (e.g. Al2O3, MgO - refer to activity series).
(vi) Extraction of metals based on the activity series.
(vii) Metals and their alloys: common ores of iron, aluminium and zinc. Extraction of Aluminium
(a) Uses of iron, aluminium and zinc and their alloys.
(b) Other important alloys – bronze, fuse metal.
Study of Compounds
_ Hydrogen Chloride
Hydrogen chloride: preparation of hydrogen chloride from sodium chloride; refer to the density and solubility of hydrogen chloride (fountain experiment); reaction withammonia; acidic properties of its solution.
_ Ammonia
(i) Ammonia: its laboratory preparation from ammonium chloride and collection; ammonia from nitrides like Mg3N2 and AlN and ammonium salts; preparation from air and from ammonium nitrite; 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; uses of ammonia.
(ii) The catalytic oxidation of ammonia, as the source of nitric acid; simple diagram
for a catalytic oxidation of ammonia in the laboratory (with conditions and reactions only). _ Nitric Acid and Nitrates:
(i) Nitric Acid: one laboratory method of preparation of nitric acid from potassium nitrate or sodium nitrate. Nitric acid as an oxidizing agent.
(ii) Nitrates: salts of nitric acid. Action of heat on the nitrates of potassium, sodium, lead, copper and ammonium.
_ Sulphur Dioxide, Hydrogen Sulphide and Sulphuric Acid
(i) Formation of sulphur dioxide by burning sulphur and by the action of dilute acid on sodium sulphite and other sulphites; one laboratory method of preparing and collecting sulphur dioxide; density and solubility; ease of liquefaction and poisonous nature of sulphur dioxide; comparison of bleaching action of chlorine and sulphur dioxide; reactions of sulphur dioxide with water, sodium hydroxide solution and chlorine. Uses, including: manufacturing of sulphuric acid by first converting SO2 to SO3; bleaching and food preserving.
(ii) Hydrogen sulphide: its peculiar smell and its tendency to form sulphides and be converted to sulphur (study of its preparation not required).
(iii) 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.
Organic Chemistry
(i) Introduction to Organic compounds.
(ii) Structure and Isomerism.
(iii) Homologous series.
(iv) Simple nomenclature.
(v) Hydrocarbons: alkanes, alkenes, alkynes.
(vi) Alcohols: methanol, ethanol – preparation and properties; its uses.
(vii) Carboxylic acids (aliphatic – mono carboxylic acid): Acetic acid – properties and uses of acetic acid.
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