inorganic

• a transition metal is an element which was partially filled d/f electron subshells in any common oxidation states
• properties of transition metals are

  shiny, bendy, high melting and boiling points

  multiple oxidation states

  have coloured ions

  form paramagnetic compounds (compounds with unpaired electrons)

  have many uses
• oxygen have oxidation state of -2
• F, Cl, Br, and I have oxidation state of -1
• H had an oxidation state of 1-
• acyl groups (e.g.COCH3) have oxidation states of -1
• CN has oxidation state of -1
• H20, NH3, CO, PMe3 have oxidation states of 0
• Alkenes have oxidation states of 0
• Allyl (e.g. CH2CH=CH2) have oxidation states of -1
• Cyclobutadiene has an oxidation state of -2
• cyclopentadiene has an oxidation state of -1
• Benzene's have an oxidation state of 0
• atomic radii decreases across the period with a slight increase at the end
• atomic radii increases slightly at the end of the period because of the stable outermost valence shell
• atomic radii increases from period four to period 5/6 (which are almost identical)
• core electrons are better shields than valence electrons
• shielding value of core electrons = 1
• shielding value of 4s electrons = 0
• shielding value of 3d electrons = 0.35
• Z* (ENC) = Z (total charge on nucleus) - S ( shielding or screening effect)
• lanathides lie between the 6s and 5d elements
• unpaired electrons are easier to remove than paired electrons
• as ionisation energy increases, the ease of oxidation decreases
• reactions proceed if Gibbs Free energy deltaG is negative
• delta G = delta H - T delta S
• hess's law states that if a reaction can be written as the sum of a number of steps it overall enthalpy change is the same as the sum of the emthalpy changes for all steps
• products with lower energies than their reactants are more stable
• max oxidation states are given by the total number of electrons in valence shells
• the number of oxidation’s states increases from 2 to 7 from scandium to manganese, then starts to decrease as ENC increases and paired electrons arise and become more difficult to remove
• when naming complex ions cations must have a + and anions must have a -
• when naming complex ions ligands must be named in alphabetical order and then the metal
• simple ligand prefixes include di, tri, tetra, petra, hexa
• complex ligand prefixes include bis, tris, tetrakis, pentrakis, hexakis
• anionic ligands end in an "o"
• neutral ligand just use the name of the molecule except ammine, carbonyl and aqua
• the oxidation state of the metal is given in roman numerals in brackets after the metal
• ate is added to the metal if it is an anion
• binary compounds with low oxidation states have lattice structures, lots of oxide/ halide ions, transition metals in nodes in the lattice and are neutral
• binary compounds with high oxidation states are more covalent often molecular (or covalent polymers)