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Hybridisation is the mixing of atomic or...

Hybridisation is the mixing of atomic orbital of comparable energy and the number of hybrid orbitals formed is equal to the number of pure atomic orbitals mixed up and hybrid are occupied by `sigma`-bond pair and lone pair.
Which of the following geometry is most likely to not form from `sp^(3)d` hybridisation of the central atom.

A

Linear

B

Tetrahedral

C

T-Shaped

D

See-Saw

Text Solution

Verified by Experts

The correct Answer is:
B
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Number of hybrid orbitals formed in 'sp' hybridisation of carbon are

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Knowledge Check

  • Hybridisation is the mixing of atomic orbital of comparable energy and the number of hybrid orbitals formed is equal to the number of pure atomic orbitals mixed up and hybrid orbitals are occupied by sigma -bond pair and lone pair. ''The hybrid orbitals are at at angle of X^(@) to one another''. This statement is not valid for which of the following hybridisation?

    A
    `sp^(3)`
    B
    `sp^(2)`
    C
    `sp^(3)d^(2)`
    D
    `sp`

  • Spin pairing and overlapping theory cannot explain the equal bond length as well as equal bond angles in CH_(4) molecule. To explain the above facts we are in need of hybridization theory. Hybridization is the mixing of atomic orbitals of comparable energy and the numbe of atomic orbitals involved is equal to the number of hybrid orbitals formed of equal energy. The number of axial and equatorial positions in trigonal bipyramidal geometry having sp^(3)d hybridizaton are respectively :

    A
    2, 4
    B
    4, 2
    C
    3, 3
    D
    2, 3

  • The geometry and the type of hybrid orbitals present about the central atom in BF_3 is :

    A
    linear ,sp
    B
    trigonal planar , `sp^2`
    C
    tetrahedral `sp^3`
    D
    pyramidal , `sp^3`

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    d^(2)sp(3) hybridisation of the atomic orbital gives :

    Which of the following geometry is associated with the compound in which the central atom assumes sp^3d hybridisation?

    Spin pairing and overlapping theory cannot explain the equal bond length as well as equal bond angles in CH_(4) molecule. To explain the above facts we are in need of hybridization theory. Hybridization is the mixing of atomic orbitals of comparable energy and the numbe of atomic orbitals involved is equal to the number of hybrid orbitals formed of equal energy. According to hybridization theory, the %s character in sp^(3) hybrid orbitals is :

    In which of the following central atom makes use of sp^(3) hybrid orbitals

    In which of the following the central atom does not use sp^3 hybrid orbitals in its bonding

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