cordination basics

9. Coordination Compounds Coordination compounds are complex compounds in which transition metal atoms are bound to a number of anions or neutral molecules. Postulates of Werner’s theory of coordination compounds:   In coordination compounds, there are two types of linkages (valences) – primary and secondary.   The primary valences are ionisable and are satisfied by negative ions.   The secondary valences are non-ionisable and are satisfied by negative ions or neutral molecules. The secondary valence is equal to the coordination number of a metal and remains fixed for a metal.   Different coordination numbers have characteristic spatial arrangement of the ions or groups bound by the secondary linkages. Difference between a double salt and a complex:   In water, a double salt dissociates completely to give simpler ions. Examples of double salt: carnallite (KCl. MgCl2.  6H2O), Mohr’s salt [FeSO4. (NH4)2 SO4. 6H2O]   Complex ions do not dissociate further to give simpler ions. For example, [Fe(CN)6] –4 , [Fe(C2O4)3] 3– Ligands: Ions or molecules bound to the central metal atom or ion in the coordination entity   Didentate – 2 222224 HNCHCHNHCO Ethane1,2diamineOxalate   Polydentate –   Ambidentate – (Can bind through two different atoms) Coordination number: Number of ligand donor atoms bonded directly to the metal Coordination polyhedral: Homoleptic and heteroleptic complexes:   Homoleptic complexes: In which metal is bound to only one kind of donor groups, e.g., [Co(NH3)6] 3+   Heteroleptic complexes: In which metal is bound to more than one kind of donor groups, e.g., [Co(NH3)4Cl2] + Naming of mononuclear coordination compounds:   The cation is named first in both physically and negatively charged coordination entities.   The ligands are named in alphabetical order, before the name of the central atom/ion.   Names of the anionic ligands end in –o. [Exceptions: aqua (H2O), ammine (NH3), carbonyl (CO), nitroryl (NO)]   To indicate the number of the individual ligands, the prefixes mono–, di–, tri–, etc., are used. If these prefixes are present in the names of ligands, then the terms bis–, tris–, tetrakis–, etc., are used.   Oxidation state of the metal is indicated in Roman numerals, in parentheses.   If the complex ion is cation, then the metal is named as the element. If the complex ion is anion, then the metal is named with ‘–ate’ ending.   The neutral complex molecule is named as the complex cation. Isomerism in coordination compounds:   Stereoisomerism –   Geometrical isomerism:   Optical isomerism: Optical isomers (enantiomers) are mirror images which cannot be superimposed on one another.   The molecules or ions which cannot be superimposed are called chiral.   Structural isomerism –   Linkage isomerism: Arises due to the presence of ambidentate ligand   Coordination isomerism: Arises due to the interchange of ligands between cationic and anionic entities of different metal ions 33 6666 CoNHCrCNandCrNHCoCN   Ionisation isomerism: Arises due to the interchange of ligands between the inside and the outside of the coordination sphere 3434 55 CoNHSOBrandCoNHBrSO   Solvate isomerism (Hydrate isomerism when solvent is water): Arises depending upon whether a solvent molecule is directly bonded to the metal ion or is present as a free solvent molecule. 263222 5 CrHOCl and CrHOClClHO violet(greygreen) Valence bond theory: Coordination number Type of hybridisation Distribution of hybrid orbitals in space 4  sp3   Tetrahedral 4 5 6 6 dsp2 sp3 d sp3 d2 d2 sp3 Square planar Trigonal bipyramidal Octahedral Octahedral   Inner-orbital or low spin or spin-paired complexes: Complexes that use inner d– orbitals in hybridisation, e.g., [Co(NH3)6] 3+   Outer-orbital or high spin or spin-free complexes: Complexes that use outer d– orbitals in hybridisation, e.g., [CoF6] 3– Limitations of valence bond theory:   A number of assumptions are involved.   Quantitative interpretation of magnetic data is not given.   The exhibition of colour by coordination compounds is not explained.   The thermodynamic or kinetic stabilities of coordination compounds are not quantitatively interpreted.   Whether a complex of coordination number 4 is tetrahedral or square planar cannot be exactly predicted.   Weak and strong ligands cannot be distinguished. Crystal-field theory: [Crystal-field splitting is the splitting of the degenerate energy levels due to the presence of ligands.]   Crystal-field splitting in octahedral coordination entities:   Spectrochemical series: 22 24 4 23 IBrSCNClSFOHCO HONCSEDTANHenCNCO   Ligands for which  0 (crystal-field splitting) < P (pairing energy) are called weak-field ligands, and form high-spin complexes.   Ligands for which  o (crystal-field splitting) > P (pairing energy), are called strong-field ligands, and form low-spin complexes.   Crystal-field splitting in tetrahedral coordination entities: t  = (4/9)  0 Colour in coordination compounds: The colour of the coordination compounds is attributed to d–d transition of electrons. Limitations of the crystal-field theory:   Anionic ligands are assumed to exert the greatest splitting effect. But the anionic ligands are found at the lower end of the spectrochemical series.   Crystal-field theory does not take into account the covalent character of bonding between ligand and the central metal atom. Bonding in metal carbonyls:   Synergic bonding – Stability of coordination compounds: n = K1 × K2 × K3 × K4…Kn Where,  → Overall stability constant K → Stepwise stability constant Applications of coordination compounds:   EDTA is used in the treatment of lead poisoning.   Cis–platin is used in the treatment of cancer.		draft		07:15:00	by shijus world of chemistry	Delete
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