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ADVANCED HIGHER LEARNING OUTCOMES ELECTRONIC STRUCTURE Electromagnetic spectrum and associated calculations o Know that electromagnetic radiation can be described in terms of waves o Define wavelength, frequency, give the symbols and units for these values o Give a value for the speed of light with appropriate units o Know the equation that relates velocity (speed), wavelength and frequency o Explain the dual nature of light/radiation o Know the equations that enable the energy of a photon or of a mole of photon to be calculated o Know the name of the constants represented by h and L and where to find their values. Electron configuration and the periodic table o State the name of the element whose emission spectra provide the evidence for energy levels o Define the terms quanta and quantised o Know the which energy transition is associated with the release of a photon o Understand how to use an emission spectrum to calculate the energy associated with the release of a photon. o Understand what the energy associated with a photon corresponds to within the atom o Know why spectra of elements with more than 1 electron give evidence of sublevels or orbital’s o Understand the terms principle energy level and sublevel o Know that electrons have a dual nature o Give a definition for ‘orbital’ in terms of probability o Name the types of orbital, their characteristic shapes and identify which orbitals and how many are found in each principle energy level. o State the Pauli exclusion principle and state how it governs the maximum number of electrons in an orbital o Define the term degenerate o State the Aufbau principle and explain how it relates to the filling of orbitals o Be able to draw a diagram to show the relative energies of orbitals in the first 4 shells o State Hunds rule and explain how it relates to the way electrons fill degenerate orbitals Write electronic configurations using box notation or spectroscopic notation for elements 1-36 o o Identify the 4 blocks of the periodic table and explain how the blocks relate to electron filling of orbitals o Explain how the first ionisation of elements gives evidence of the different stabilities of different electron configurations o Explain how the first, second and third ionisation energies give evidence of the stabilities of the electron configuration of the species from which the electron is being removed Spectroscopy o Understand the difference between emission and absorption spectroscopy in terms of electron transitions and the spectra seen o State the approximate wavelength range of visible and u.v. spectra o Understand how spectra give evidence of the identity and quantity of a species BONDING Covalent Bonding o Understand that there is a continuum of bonding and know where ionic, non-polar covalent and polar covalent bonding lie on the continuum. o Explain dative bonding and give a common example o Relate the type of bonding likely to be present to the difference in electronegativity of the elements involved. o Use different theories to explain the behaviour of electrons during the formation of covalent bonds o Use Lewis diagrams to show bonding and non-bonding electrons in molecules o Explain what is meant by a resonance structure and give 3 examples. Shapes of molecules and polyatomic ions o Predict the shapes of molecules from the number of bonding and non-bonding electron pairs present. o Understand the terms linear, trigonal, tetrahedral, trigonal bipyramidal and octahedral and relate these to the number of electron pairs present. o State the order of repulsion of electron pairs o Explain how electron pair repulsion accounts for the differing bond angles seen in methane, ammonia and water. Transition Metals o Give a definition of a transition metal o Explain how the Aufbau principle applies to the atoms of Cu and Cr o Know which electrons are lost first when transition metals form ions and explain why. o Know how to determine the oxidation state of an element in a compound o Explain why transition metals can have ions in different oxidation states with different stabilities o Understand why compounds of the same element can have different colours o Explain oxidation and reduction in terms of oxidation number o Give a general rule about the oxidation number of oxidising and reducing agents. Transition Metal Complexes o Define o Understand the terms monodentate, bidentate and hexadentate as applied to ligands o Explain why d orbitals are no longer degenerate in a complex ion o Know the IUPAC rules for naming complexes o Explain how the position of a ligand in the spectrochemical series affects the size of the ligand field o Explain in terms of d-d transitions why complexes are coloured o Define absorption and emission spectroscopy a) complex ion b) ligand c) co-ordination number o Relate the wavelengths 200-400nm and 400-700nm to the appropriate type of spectroscopy o Explain how spectrometers use light intensity to determine absorption o Explain how transition metals can act as catalysts in terms of their variable oxidation state, reaction pathways and intermediate complexes