CHEMISTRY TOPIC            DESCRIPTION OF CHEMISTRY TOPICS Basic Chemistry .......... Atomic information on protons, electrons and neutrons. .............................................................................................. Chemical Change .......... Exothermic and Endothermic reactions responsible for the change of reactants into products such as the decomposition reaction of water into hydrogen and oxygen.  The role of electrolysis is also described. .............................................................................................. Discovery of the Atomic Structure .......... Scientists responsible for describing the various sections of the atoms - Bohr (electrons) ; Chadwick (Neutrons). .............................................................................................. Formation of Chemical Bonds ......... Detailed information on the formation of non-polar covalent bonds, polar covalent bonds and ionic bonds. .............................................................................................. Hydrosphere and Precipitation Reactions .......... Water soluble substances could react with each other with the formation of non-soluble substances - precipitation (ion-exchange) reactions. .............................................................................................. Introduction to the Atom and Chemistry ......... A summary of all concepts and principles in basic chemistry. .............................................................................................. Matter and Materials .......... Description of elements, compounds and mixtures as well as techniques to separate substances from each other. .............................................................................................. Nitrogen Cycle Different processes in the nitrogen cycle as well as reactions related to the fixation of nitrogen.  Importance of nitrogen in fertilizers. .............................................................................................. Periodic Table and Balancing of Chemical Formulae .......... Information on the periodic table - columns, rows, atomic number, mass number and quidelines for the correct balancing of chemical formulae. .............................................................................................. Periodicity of Elements .......... How and why the volume, radius and size of atoms change in periods of the periodic table. ............................................................................................. Type and Balancing of Chemical Reactions .......... Illustration of various types of chemical reactions - combustion reactions, synthesis reactions, decomposition reactions, displacement reactions and rules for the correct balancing of chemical reactions. .............................................................................................. Water Cycle .......... Evaporation of water and different precipitation procedures of water. xxxxxxxxxxxxxxxxxxxxxxxx xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx Acid - Base Reactions ..........  Definition of strong and weak acids and bases. Titration calculations of the concentration of acids and bases. .............................................................................................. Atomic, Molecular and Formula Mass ......... Use of atomic masses to calculate the molecular and formulae masses of chemical substances. .............................................................................................. Balancing of Chemical .......... Rules for the correct balancing of chemical reactions. .............................................................................................. Bond Energy and Potential Energy Graphs .......... Exothermic and endothermic reactions.  Graphs reflecting the energy change during exothermic and endothermic reactions.  Bond energy - amount of energy needed to break a chemical bond. .............................................................................................. Concentration of Solutions .......... Calculate the concentration of solutions in terms of number of moles of a substances dissolved in a volume of a solvents. .............................................................................................. Chemical processes in the Atmosphere .......... Earth atmosphere - Troposphere, Stratosphere, Mesophere, Thermosphere, Ozone, Greenhouse Gases. ............................................................................................. Energy Sources .......... Fossil fuels, oil, natural gases, renewable energy. ............................................................................................. Electric Conduction of Metals .......... Formation of metallic bonds.  Semi-conductors: p-type and n-type semiconductors. ............................................................................................. Gas Laws .......... Motion of gas particles, Boyles Law, Charles Law, general gas equation, ideal gas model, pressure and temperature of a gas. ............................................................................................. Gold .......... Gold as an element.  Characteristics of gold.  Use of gold.  Extraction of gold. ............................................................................................. Iron .......... Iron as an element.  Use of iron.  Mining and refining of iron ore. .............................................................................................. Lewis structure .......... Representation of atoms with symbols and valence electrons. .............................................................................................. Mole and Avogadros Constant .......... Calculate the number of moles of a substance, n = m/M.  Use Avogadros constant to determine the number of atoms, molecules. ............................................................................................. Organic Chemistry (Reactions) .......... Chemistry of the element carbon (C), studying homologous groups, alkanes, alkenes, alkynes.  Substitution, addition, elimination, cracking and oxidation reactions.  IUPAC names of organic molecules. ............................................................................................. Oxidation Numbers .......... Resultant electric charge of atoms in elements and chemical substances.  Description of oxidation and reduction. .............................................................................................. Percentage Composition and Emperical Formula .......... Percentage mass contribution of each element to the molecular mass of a substance.  Simplest ratio which atoms combine with each other forming chemical substances. ............................................................................................. Polar Covalent Bonds and Molecules .......... Formation of covalent bonds due to the sharing of electrons between atoms of non-metals.  Electronegativity of atoms determine the type of chemical bond between atoms. ............................................................................................. Redox Reactions .......... Oxidation numbers, oxidation half reaction, reduction half reaction.  Change in oxidation numbers. .............................................................................................. Stochiometrical Calculations .......... Chemical change in terms of mole ratios of a balanced chemical reaction.  Calculations at STP. ............................................................................................. VEPR Model and Shapes of Molecules .......... Prediction of the shapes of molecules according to the arrangement of electrons around and between atoms in a molecule. xxxxxxxxxxxxxxxxxxxxxxxx xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx Balancing of Redox Reactions .......... Use the reduction potential table to identify oxidation and reduction half reactions.  Net balanced reaction. ............................................................................................. Battery Industry .......... Primary and secondary cells.  Energy stored in a battery.  Capacity of a cell.  Dry cells.  Chemical reactions in a dry cell. ............................................................................................. Chemical Equilibrium .......... Reversible chemical reaction.  Kc-value. Le Chateliers principle. ............................................................................................. Electrolytic Cells .......... Electrolysis of melted substances and solutions sodium chloried as well as copper(II)chloride.  Electroplating.  Extraction of Aluminium. .............................................................................................. Inorganic Chemistry Industry .......... Chlorine-alkaline industry. Electrolysis of sodium chloride.  Membrabe cell electrolysis. .............................................................................................. Organic Chemistry Chemistry of the element carbon.  Alkanes, alkenes, alkynes, alcohols, carboxylic acids, eaters.  IUPAC naming. Reactions such as substitution, addition, elimination, combustion and cracking.  Chemical and physical properties.   ............................................................................................. Rate of Chemical Reactions Collision theory.   Non-reversible reactions and factors influencing the rate of the reaction. xxxxxxxxxxxxxxxxxxxxxxx xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx