transition metal - incomplete d-orbital in at least one ion, Aufbau - orbitals fill in order of increasing energy, Hunds rule - maximise parallel spin before pairing, Pauli exclusion prinicple - no 2 electrons can have same 4 QN, principle QN - n (energy level) 1,2,...., angular momentum QN - l (orbital) 0,1..., magnetic QN - ml (subshell) -l...+l, spin QN - ms (spin) 1/2, emission spectrum - black background with coloured lines, shows electrons falling from excited state, absorption spectrum - coloured background with black lines shows electrons being promoted to excited state, EM spectrum - range of waves from micro to gamma, relationship between frequency and wavelength - f = c/ƛ, s orbital - sphere, orbital that starts every energy level, p orbital - 2 lobes, present every level from 2 onwards, d orbital - most have 4 lobes, present in TM onwards, octahedral - 6 electron pairs, square based pyramid - 6 pairs, 5 bonds, square planar - 6 pairs, 4 bonds, trigonal bypyramidal - 5 electron pairs, tetrahedral - 4 electron pairs, VSEPR Theory - counts electrons to find electron pairs, colorimetry - technique measuring wavelength and intensity of colour, spectroscopic notation - orbitals and e number written out, complex - TM surrounded by ligands, ligand - negative / lone eelctron pairs, dative bond - both electrons from same atom, coordination number - number of bonds to central TM in complex, complementary colour - colour we see in TM complex is opposite of colour absorbed,

AH Inorganic

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