Nothing Special   »   [go: up one dir, main page]
Scribd Logo
Upload

Welcome to Scribd!

  • 4K views

    Limitation of CFT

    Uploaded by

    Guttu Das
    The Crystal Field Theory has several limitations: 1. It cannot explain the color of substances with full or empty d orbitals like KMnO4. 2. It does not account for charge transfer electron transitions which are more powerful than d-d transitions. 3. It treats metal-ligand bonds as purely ionic and cannot be used to explain complexes with covalent bonds like sulfides.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd

    Limitation of CFT

    Uploaded by

    Guttu Das
    4K views2 pages
    The Crystal Field Theory has several limitations: 1. It cannot explain the color of substances with full or empty d orbitals like KMnO4. 2. It does not account for charge transfer electron transitions which are more powerful than d-d transitions. 3. It treats metal-ligand bonds as purely ionic and cannot be used to explain complexes with covalent bonds like sulfides.

    Original Description:

    asdddfdsew

    Copyright

    © © All Rights Reserved

    Available Formats

    DOCX, PDF, TXT or read online from Scribd

    Did you find this document useful?

    Is this content inappropriate?

    The Crystal Field Theory has several limitations: 1. It cannot explain the color of substances with full or empty d orbitals like KMnO4. 2. It does not account for charge transfer electron transitions which are more powerful than d-d transitions. 3. It treats metal-ligand bonds as purely ionic and cannot be used to explain complexes with covalent bonds like sulfides.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    4K views2 pages

    Limitation of CFT

    Uploaded by

    Guttu Das
    The Crystal Field Theory has several limitations: 1. It cannot explain the color of substances with full or empty d orbitals like KMnO4. 2. It does not account for charge transfer electron transitions which are more powerful than d-d transitions. 3. It treats metal-ligand bonds as purely ionic and cannot be used to explain complexes with covalent bonds like sulfides.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    of 2

    Limitation of CFT

    1. The CFT can not explain thee color of substances with a full or empty d orbital.(since it only
    consider d orbitals) an example of these substances is KMnO4 in which the d orbital is empty.
    2. There is another kind of electron transfer called Charge Transfer(CT) which is more
    powerful than
    dd
    transfer and is between metal and ligand. this type of electron transfer is not covered in
    crystal
    field theory and can only be explained using MOT(molecular orbital theory)
    3. It treats metal ligand as purely ionic. Hence it cannot be used for sulfides as sulfides forms
    mostly
    covalent bond.
    4. . It cannot satisfactorily explain chemical bonding. Complexes may also be formed between
    neutral
    metal atoms and neutral or cationic ligands. Crystal Field Theory is poorly suited to explain
    such
    interactions.
    5. Crystal Field Theory fails in explaining why a neutral ligand such as CO can cause a very
    large
    crystal field splitting. Molecular Orbital Theory explains why the CO ligand leads to a higher
    crystal field splitting.
    6. It assumes that anionic ligands are present at low end of the spectrochemical series.

    Limitations of Valence Bond Theory :


    While the VB theory, to a larger extent, explains the formation, structures and magnetic
    behaviour of coordination compounds, it suffers from the following shortcomings:
    (i)
    (ii)
    (iii)
    (iv)
    (v)
    (vi)

    It involves a number of assumptions.


    It does not give quantitative interpretation of magnetic data.
    It does not explain the colour exhibited by coordination compounds.
    It does not give a quantitative interpretation of the thermodynamic or kinetic
    stabilities of coordination compounds.
    It does not make exact predictions regarding the tetrahedral and square
    planar structures of 4-coordinate complexes.
    It does not distinguish between weak and strong ligands.

    HgS, Bi2S3, PbS, CdS and CuS can be separated by differential solubility. HgS is insoluble
    in nitric acid while the rest of the group II cations are soluble
    Adding the nitric acid will cause the white AgCl to precipitate out

    You might also like