Curriculum Shule Direct Kenya Secondary School Form 2 Chemistry Kenya

Chemistry Kenya Form 2 Syllabus

  1. Structure of the Atom and the Periodic Table
    1. Structure of the Atom and the Periodic Table
      1. The Structure of the Atom
      2. Names and symbols of the first twenty elements of the periodic table
      3. Simple structure of the atom; protons, electrons and neutrons; electron energy levels in atoms
      4. Atomic characteristics
      5. Definitions of atomic number, mass number, isotopes and relative atomic mass(reference C-12); examples of isotopes
      6. Calculation of relative atomic mass from relative abundance of isotopes of an element
      7. The periodic table
      8. Build up of the periodic table for the 1st twenty elements on the basis of energy levels(rows=periods, columns=groups)
      9. Ion formation
      10. Formation of simple ions and cations
      11. Qualitative treatment of the ionisation energy and electron affinity
      12. Writing electron arrangement of ions formed from atoms:lithium, Na,Fl,Mg,Al, Cl,S
      13. Definition of valency and oxidation numbers
      14. Derive valency and oxydation number of an element from atoms(it's position in the periodic table)
      15. Names and formulae of common radicals
      16. Use of valencies in determining the chemical formulae of common compounds
      17. Writing simple balanced equations
      18. Chemical equations with state symbols
  2. Chemical Families
    1. Chemical Families
      1. Alkali metals (Group 1); (lithium,sodium and potassium)
      2. Electron arrangement, gradation in size of the atom, ions and trends in ionisation energy.
      3. Physical properties; appearance, melting point, boiling point
      4. Thermal and electrical conductivity
      5. Reaction with air, water and chlorine
      6. Similarity of ions and formulae of hydroxides, oxides and chlorides of alkali metals
      7. Uses of alkali metals (sodium only)
      8. Alkaline-earth metals (Group 2); (Beryllium,magnesium, and calcium)
      9. Physical properties; appearance, melting point, boiling point, thermal and electrical conductivity
      10. Reaction with air, water, chlorine and dilute acids: CAUTION: Reaction between calcium and acid is violent. Use very dilute acid)
      11. Similarity of ions and formulae of oxides, hydroxides, and chlorides
      12. Importance of alkaline-earth metals
      13. Halogens (Group 7); (Fluorine, chlorine, bromine and iodine)
      14. Electron configuration of fluorine and chlorine, gradation in size of the atoms and ions
      15. Physical properties (appearance, melting point, boiling point, thermal and electrical conductivity)
      16. Reaction with metals, sodium, zinc, iron and water
      17. Similarity of ions and formulae of compounds
      18. Importance of fluorine, chlorine, bromine and iodine
      19. Noble gases (Group 8);(Helium, neon, argon)
      20. Electron arrangement and gradation in size of the atoms
      21. Electron arrangement- the basis of low reactivity of helium, neon and argon
      22. Importance of noble gases
      23. Properties and trends across a period
      24. Period three elements (sodium, magnesium, aluminium, silicon, phosphorus, sulphur,chlorine and argon)
      25. Electron arrangement of the elements
      26. Physical properties of period three elements (atomic size, ionisation energy, melting point, boiling point, thermal and electrical conductivity)
      27. Reaction of period three elements with with oxygen, water and dilute acids. (CAUTION: Reaction of sodium with acids is explosive. Give theoretical treatment only)
  3. Structure and Bonding
    1. Structure and Bonding
      1. The role of outer electrons in chemical bonding
      2. Significance of the outer electrons in chemical bonding.
      3. The noble gas electron arrangement
      4. Electron transfer and ionic bonding
      5. Electron sharing and covalent bonding
      6. Use dot(.) and cross (x) diagrams to illustrate bonding, electrostatic forces of attraction in the following: molecular (iodine), giant covalent( diamond, graphite and silicon (IV) oxide), giant ionic (sodium chloride) and giant metallic (copper)
      7. Other types of bonds: coordinate, hydrogen bond, Van der waals forces of attraction (simple explanation only)
      8. The influence of hydrogen bonds and Van der waals forces on physical properties (melting point, boiling point, solubility, electrical and thermal conductivity)
      9. Types of bonds across a period (period 3)
      10. Changes in types of chemical bonds in oxides and chlorides of sodium, magnesium, aluminium, silicon, phosphorus, Sulphur and chlorine. NOTE: Use of models to illustrate bonding should be encouraged.
      11. Applications: Selection of materials for various uses; e.g. diamond, graphite and aluminium
  4. Salts
    1. Salts
      1. Methods of preparing salts
      2. Preparation of soluble salts by reaction of acids with; metals, metal hydroxides, metal oxides, metal carbonates and metal hydrogen carbonates
      3. Preparation of insoluble salts by precipitation (ionic equations required)
      4. Direct combination reaction (e.g. sodium with chlorine, iron with sulphur)
      5. Types of salts; normal, acid and double salts.
      6. Solubility of salts
      7. Solubility of sulphates, chlorides, nitrates and carbonates in water
      8. Relationship between method of preparation and solubility. NOTE: The solubility of hydroxides and oxides should be considered along with others.
      9. Action of heat on salts
      10. Effects of heat on the following salts; carbonates, nitrates, sulphates and hydrated salts (include ammonium salts)
      11. Applications:- use of lime to change pH, use of salts as anti-acids, use of salts as inorganic fertilizers
  5. Effect of an Electric Current on Substances
    1. Effect of an Electric Current on Substances
      1. Conduction of electricity
      2. Conductors and non-conductors
      3. Test for conduction of electricity by; Solids, metals and non-metals;( wood, aluminium foil, sodium chloride, sugar and lead (II) bromide), aqueous solutions of sugar, urea, copper (II) chloride, sodium chloride and mineral acids, melts: Sulphur, lead (II)bromide or lead (II)iodide and sugar
      4. Electrolytes and non-electrolytes
      5. Ions as the particles in electrolyte solutions and melts
      6. Molecules as the particles i non-electrolyte solutions and melts
      7. Passage of a direct electric current through an electrolyte (electrolysis of molten lead (II)bromide or lead(II)iodide
      8. Anode and cathode
      9. Applications of electrolysis: - electroplating, production and purification of metals. NOTE: Details of the processes not required at this point.
  6. Carbon and some of its Compounds
    1. Carbon and some of its Compounds
      1. Forms of carbon
      2. Diamond,graphite and charcoal: structure, physical properties and uses (relate uses to structure and physical properties)
      3. Chemical properties of carbon
      4. Combustion, reaction with acids and reducing action
      5. Preparation and properties of Carbon (IV) oxide (carbon dioxide)(Relate methods of collection to the properties of the gas)
      6. Reactions of the gas with water, calcium hydroxide and alkalis
      7. Uses of carbon (IV) oxide (carbon dioxide)
      8. Preparation and properties of Carbon (II) oxide (carbon monoxide)
      9. Preparation of carbon(II)oxide (carbon monoxide)
      10. Physical properties, chemical properties, combustion, reducing action, poisonous nature such as car exhausts fumes and charcoal fire. NOTE: Only theoretical treatment required because of its poisonous nature.
      11. Carbonates and hydrogen carbonates
      12. Action of heat and dilute acids on carbonates and hydrogen carbonates
      13. Production and manufacture of sodium carbonate (Magadi Soda Company and solvay process). NOTE: Use simple schematic diagrams to illustrate solvay process.
      14. Importance of carbon and its oxides
      15. Carbon cycle
      16. Soft drinks manufacturer
      17. Fire extinguishers
      18. The effects of Carbon(IV)oxide (carbon dioxide) and carbon(II)oxide (carbon monoxide) on the environment

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