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Questions and Answers
Which type of isomerism occurs due to the exchange of ligands between the complex ion and ions outside it?
In which type of isomerism does an H2O molecule replace other ligands in a complex?
Which type of isomerism occurs when there is an ambidentate ligand in a complex?
In which type of isomerism does ligand exchange happen between cation and anion complexes?
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Which type of isomerism occurs due to the interchange of ligands between different metal nuclei of a polynuclear complex?
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In tetrahedral complexes with coordination number 4, which type of isomerism is not possible?
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In tetrahedral complexes with coordination number 4, when is optical isomerism possible?
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What type of hybridization do tetrahedral complexes with coordination number 4 exhibit?
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Limitations of EAN rule arise when dealing with...
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According to Valence Bond Theory, what condition must be met for a complex to exhibit optical isomerism?
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Study Notes
Coordination Compounds
- Four electron pairs from 4 NH3 ligands are accommodated in the dsp2 hybrid orbitals, resulting in a square planar geometry.
- The complex is paramagnetic because it contains one unpaired electron.
Limitations of Valence Bond Theory
- It cannot predict whether a coordination compound will be tetrahedral or square planar.
- It fails to predict whether a complex is an inner orbital complex or outer orbital complex.
- It does not predict any distortion in symmetrical complexes (Jahn-Teller distortions).
- It does not attempt to explain the color of the complexes.
- It cannot explain the temperature-dependent paramagnetism of the complexes.
Nomenclature of Coordination Compounds
- The basic rules of nomenclature are: name the cation first, then the anion, with a space in between.
- Naming of complex portion: use di, tri, tetra, penta, hexa, or bis, tris, tetrakis, etc. as necessary.
- Naming of ligands: in alphabetical order, regardless of their charges, and anions end in 'o'.
Coordination Geometry Hybridization Examples
- Linear: sp (sp²) [Ag(NH3)2]+
- Trigonal planar: sp² (sp²xpy) [Ag(PR3)3]
- Tetrahedral: sp³ (sp³xpy pz) [Ni(CO)4]
- Square planar: dsp² (dx²-y²sp²xpy) [Ni(CN)4]2-
- Trigonal bipyramidal: sp³d (sp³xpy pzdz²) [CuCl5]3-
- Square pyramidal: sp³d (sp³xpy pzdx²-y²) [VO(acac)2]
- Octahedral (outer orbital complex): sp³d² (sp³xpy pzdx²-y²dz²) [Cu(H2O)6]2+
- Octahedral (inner orbital complex): d²sp³ (dx²-y²dz²sp³xpy pz) [Fe(CN)6]4-
Examples of Geometries
- [Ag(NH3)2]+: ground state electronic configuration of 47Ag is [Kr]4d¹⁰4s¹, and geometry is linear.
- [Ni(CN)4]4-: ground state electronic configuration of 28Ni is [Ar]3d⁸4s², and geometry is tetrahedral.
Types of Isomerism
- Ionization Isomerism: due to exchange of ligands between the complex ion and ions outside it.
- Hydrate Isomerism: a special kind of ionization isomerism in which H2O molecules replace other ligands.
- Linkage Isomerism: occurs when there is an ambidentate ligand in the complex.
- Coordination Isomerism: occurs because of ligand exchange between cation and anion complexes.
- Coordination Position Isomerism: occurs because of ligand interchange between different metal nuclei of a polynuclear complex.
Stereoisomerism
- Occurs because of different orientations of ligands in space.
- There are two types of stereoisomerism: Geometrical Isomerism and Optical Isomerism.
- Stereoisomerism in Complexes with Coordination Number 4:
- Tetrahedral complexes: Geometrical isomerism is not possible, and optical isomerism is possible only in those tetrahedral complexes in which the central metal atom is bonded with four different ligands and is asymmetric.
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Description
Explore the application of molecular orbital theory in coordination compounds, determining the hybridization and geometry of complexes. Learn about the limitations of the theory in predicting certain complex structures.
