• Transition element complexes can exhibit?stereoisomerism

?Geometrical (cis-trans) isomerism

• Even though transition element complexes do not have a?double bond, they can still have?geometrical?isomers
• Square planar?and?octahedral?complexes with?two pairs?of different?ligands exhibit?cis-trans?isomerism
• An example of a square planar complex with two pairs of ligands is the anti-cancer drug?cis-platin
  • Whereas?cis-platin has beneficial medical effects by binding to DNA in cancer cells,?trans-platin cannot be used in cancer treatment

Cis-platin is an example of a square planar transition element complex that exhibits geometrical isomerism

• As long as a complex ion has two ligands attached to it that are different to the rest, then the complex can display geometric isomerism
• Examples of octahedral complexes that exhibit geometrical isomerism are the [Co(NH₃)₄(H₂O)₂]²⁺?and [Ni(H₂NCH₂CH₂NH₂)₂(H₂O)₂]²⁺?complexes
  • [Ni(H₂NCH₂CH₂NH₂)₂(H₂O)₂]²⁺?can also be written as [Ni(en)₂(H₂O)₂]²⁺
• Like in the square planar complexes, if the two ‘different’ ligands are next to each other then that is the ‘cis’ isomer, and if the two ‘different’ ligands are opposite each other then this is the ‘trans’ isomer
  • In [Co(NH₃)₄(H₂O)₂]²⁺, the two water ligands are next door to each other in the cis isomer and are opposite each other in the trans isomer

Octahedral transition metal complexes exhibiting geometrical isomerism

Optical isomerism

• Octahedral?complexes with?bidentate ligands?also have?optical isomers
• This means that the two forms are?non-superimposable mirror images?of each other
  • They have no plane of symmetry, and one image cannot be placed directly on top of the other
• The optical isomers only differ in their ability to rotate the plane of polarised light in opposite directions
• Examples of octahedral complexes that have optical isomers are the [Ni(H₂NCH₂CH₂NH₂)₃]²⁺and [Ni(H₂NCH₂CH₂NH₂)₂(H₂O)₂]^2+?complexes
  • The ligand H₂NCH₂CH₂NH₂?can also be written as ‘en’ instead

Octahedral transition metal complexes exhibiting optical isomerism

• The isomers of transition elements complexes may be?polar?or?non-polar
• This is caused by differences in?electronegativity?of the atoms in the ligands that form the dative bond to the complex ion

Polarity in square planar complexes

• In?cis-platin, the two chlorine atoms are on the same side
• These atoms have a stronger pull on the electrons in the dative bond and will carry a?partial negative charge
• As a result, there is an imbalance of charge causing the complex to become?polar
• In?trans-platin, the same ligands are on opposite sides of each other
• The pull on electrons in the dative bonds to the complex ion are therefore balanced
• The overall charge is balanced and the complex is?non-polar
• Trans-platin does not have the same benefits medically as?cis-platin does

Example of a square planar complex and its polar and non-polar geometric isomers

Polarity in octahedral complexes

• Again, the?trans-isomer in octahedral complexes is?non-polar?whereas the?cis-isomer is slightly?polar
• In?cis-[Co(NH₃)₄(H₂O)₂]²⁺?for example, the oxygen atoms in the H₂O ligands are more electronegative than the nitrogen atoms in the NH₃?ligands
• This causes the side of the water ligands to be?partially negative
• Resulting in a charge imbalance causing the complex to become?polar
• The?symmetrical arrangement?in the?trans?isomers means that the charge is evenly distributed in the complex
• Trans-isomers are therefore?non-polar

Example of an octahedral complex and its polar and non-polar geometric isomers