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• In this course you will learn exactly what you need to know for your chemistry exams so that you can learn as efficiently as possible.
• Understand the three states of matter in terms of the arrangement, movement and energy of the particles
• Understand the interconversions between the three states of matter in terms of: the changes in arrangement, movement and energy of the particles.
• Understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained
• Know what is meant by the terms: • solvent • solute • solution • saturated solution.
• Know what is meant by the term solubility in the units g per 100 g of solvent
• Understand how to classify a substance as an element, compound or mixture
• Describe these experimental techniques for the separation of mixtures: • simple and fractional distillation • filtration • crystallisation • chromatography.
• Understand how a chromatogram provides information about the composition of a mixture
• Understand how to use the calculation of Rf values to identify the components of a mixture
• Know what is meant by the terms atom and molecule
• Know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles
• Know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Ar)
• Be able to calculate the relative atomic mass of an element (Ar) from isotopic abundances
• Understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table
• Understand how the electronic configuration of a main group element is related to its position in the Periodic Table
• Understand how ions are formed by electron loss or gain
• Know the charges of common ions
• Write formulae for compounds formed between the ions listed above
• Draw dot-and-cross diagrams to show the formation of ionic compounds by electron transfer, limited to combinations of elements from Groups 1, 2, 3 and 5, 6, 7
• Understand ionic bonding in terms of electrostatic attractions
• Understand why compounds with giant ionic lattices have high melting and boiling points
• Know that ionic compounds do not conduct electricity when solid, but do conduct electricity when molten and in aqueous solution
• Know that a covalent bond is formed between atoms by the sharing of a pair of electrons
• Understand covalent bonds in terms of electrostatic attractions
• Understand how to use diagrams to represent covalent bonds in a range of molecules
• Explain why substances with a simple molecular structures are gases or liquids, or solids with low melting and boiling points
• Explain why the melting and boiling points of substances with simple molecular structures increase, in general, with increasing relative molecular mass
• Explain why substances with giant covalent structures are solids with high melting and boiling points
• Explain how the structures of diamond, graphite and C60 fullerene influence their physical properties, including electrical conductivity and hardness
• Know that covalent compounds do not usually conduct electricity
• Know how to represent a metallic lattice by a 2-D diagram
• Understand metallic bonding in terms of electrostatic attractions
• Explain typical physical properties of metals, including electrical conductivity and malleability
• Understand why covalent compounds do not conduct electricity
• Understand why ionic compounds conduct electricity only when molten or in aqueous solution