metal complex's

for 4 ligands, if the metal is platinum of palladium then its square planar. otherwise its tetrahedral

6 (H2O) ligands: pale blue solution 4 (H2O), 2(OH) ligands: blue precipitate 2 (H2O), 4(NH4) ligands: dark blue solution

6 (H2O) ligands: pale green solution 4 (H2O), 2(OH) ligands: green precipitate (slowly turns brown due to oxidation to Fe3+)

6 (H2O) ligands: yellow solution 3 (H2O), 3 (OH) ligands: orange precipitate

6 (H2O) ligands: pale pink solutions 4 (H2O), 2 (OH) ligands: pink precipitate

6 (H2O) ligands: green solution 3 (H2O), 3(OH) ligands: grey-green precipitate 6 (OH) ligands: dark green solution 6 (NH3) ligands: purple solution

Cu with NH3 to form [Cu(NH3)4 (H2O)2]^2+ Cr with OH- to form [Cr(OH)6]^3- Cr with NH3 to form [Cr(NH3)6]^3+

they bond to haemoglobin in a ligand substitution reaction instead of oxygen, preventing oxygen transfer

prevents DNA replication by a ligand substitution reaction. two coordinate bonds are formed between the platinum and nitrogen atoms on 2 adjacent bases. the nitrogen replaces the 2 chlorine ligands. it also targets healthy cells

identity of the metal, oxidation state, ligands type, coordination number.

the difference in energy of the split d orbitals corresponds to the energy of light absorbed. electrons are excited to higher energy levels. the colour of the complex corresponds to the frequencies of light not absorbed

the d-orbitals have different energies because each orbital interacts differently with the bonding ligands.