2. Compound having same molecular formula but different physical &
chemical properties
difference properties because of
different structure
difference properties because of
different orientation
3. STRUCTURAL ISOMERISM :
Compound having same mol. formula difference in physical properties because of
different structure.
(A) Ionisation isomerism :
This type of isomerism occurs when the counter ion in a coordination compound
is itself a potential ligand and can displace a ligand which can then become the
counter ion.
For example:
(B) Solvate / hydrate isomerism :
It occurs when water forms a part of the coordination entity or is outside it. This is
similar to ionisation isomerism.
For examples:
4. (C) Linkage isomerism :
In some ligands, like ambidentate ligands, there are two possible coordination
sites. In such cases, linkage isomerism exist.
NO2 group can be bonded to metal ions through (-NO2) or (-ONO),
SCN : (-SCN) or (-NCS).
(D) Coordination isomerism :
Coordination compounds made up of cationic and anionic coordination entities
show this type of isomerism due to the interchange of ligands between the cation
and anion entities.
For examples:
5. (E) Ligand isomerism :
Since many ligands are organic compounds which have possibilities for
isomerism, the resulting complexes can show isomerism from this source.
For example :
ligands 1,2-diaminopropane(propylenediamine or pn) and
1,3-diaminopropane(trimethylenediamine or tn)
(F) Polymerisation isomerism :
Considered to be a special case of coordination isomerism, in this the various
isomers differ in formula weight from one another
For example :
These all have the empirical formula [Pt(NH3)2Cl2] 1: 2 :2
[Pt(NH3)2Cl2] Pt:NH3:Cl 1: 2 :2
[Pt(NH3)4] [PtCl4] Pt:NH3:Cl 2: 4 :4
6. Stereoisomers : Compound having same mol. formula difference in physical
properties because of different orientation.
Geometrical Isomerism
Cis isomer
When ligands are present on
same side
When ligands are present at 90
to each other
trans isomer
When ligands are present on
opposite side
When ligands are present at 180
to each other
7. Coordination Number Four :
Tetrahedral Complex :
The tetrahedral compounds can not show geometrical isomerism as we all know
that all four positions are equivalent in tetrahedral geometry.
[MA4], [MA3B] not show G. I.
Square Planar Complex :
In a square planar complex of formula [MA2B2] [A and B are unidentate], the two
ligands .A. may be arranged adjacent to each other in a cis isomer, or opposite to
each other in a trans isomer as depicted.
[MA2B2], [M(AB)2], [MA2BC], [MABCD] show G. I.
8. Coordination Number 6 :
Geometrical isomerism is also possible in octahedral complexes.
[MA6], [MA5B], [M(AA)3] not show G. I.
[MA2B2C2], [MA2B2CD], [MA2BCE], [MABCDEF], [M(AB)3], [MA4B2], [MA3B3]
show G. I.
Optical Isomerism :
Plane of symmetry
Center of symmetry
Axis of symmetry
Should not be present
9. • Tetrahedral complexes with formula [MABCD] show optical isomers and
octahedral complexes (cis form) exhibit optical isomerism.
• Optical isomerism is common in octahedral complexes involving didentate
ligands. Cis-isomer of [PtCl2(en)2]2+ show optical isomerism as shown below
because of the absence of plane of symmetry as well as centre of symmetry.
