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Presence of a lone pair of electrons dis...

Presence of a lone pair of electrons distrots the geometry of a covalent molecule.Explain.

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A
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The number of lone pair of electrons in OF_(2) molecule is

Hybridisation helps us to understand the geometry of the molecules. This is because hybridised orbitals are directed in space in some preferred directions to have stable arrangement, which determine the geometry. The common hybridisation are sp (linear), sp^(2) (trigonal planar), sp^(3) (tetrahedral), sp^(3)d (trigona bipyramidal), sp^(3)d^(2) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal). The presence of lone pairs in addition to bond pairs distort the geometry because "lone pair "-" lone pair repulsion"gt" lone pair "-" bond repulsion" gt" bond pair" -"bond pair repulsion" . Give an example of molecule involving sp^(3) hybridisation.

Knowledge Check

  • A lone pair of electrons in an atom implies

    A
    a pair of valence electrons
    B
    a pair of electrons
    C
    a pair of electrons involved in bonding
    D
    a pair of valence electrons not involved in bonding.

  • A lone pair of electrons in an atom implies

    A
    A pair of valence electrons
    B
    A pair of electrons
    C
    A pair of electrons involved in bonding
    D
    A pair of valence electrons not involved in bonding

  • A lone pair of electrons in an atom implies

    A
    `pair of electrons
    B
    pair of electrons
    C
    a pair of electrons involved in bonding
    D
    a pair of valence electrons not involved in bonding

    • Similar Questions

    Explore conceptually related problems

    Hybridisation helps us to understand the geometry of the molecules. This is because hybridised orbitals are directed in space in some preferred directions to have stable arrangement, which determine the geometry. The common hybridisation are sp (linear), sp^(2) (trigonal planar), sp^(3) (tetrahedral), sp^(3)d (trigona bipyramidal), sp^(3)d^(2) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal). The presence of lone pairs in addition to bond pairs distort the geometry because "lone pair "-" lone pair repulsion"gt" lone pair "-" bond repulsion" gt" bond pair" -"bond pair repulsion" . What is the hybridisation and shape of XeF_(4) molecule?

    Hybridisation helps us to understand the geometry of the molecules. This is because hybridised orbitals are directed in space in some preferred directions to have stable arrangement, which determine the geometry. The common hybridisation are sp (linear), sp^(2) (trigonal planar), sp^(3) (tetrahedral), sp^(3)d (trigona bipyramidal), sp^(3)d^(2) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal). The presence of lone pairs in addition to bond pairs distort the geometry because "lone pair "-" lone pair repulsion"gt" lone pair "-" bond repulsion" gt" bond pair" -"bond pair repulsion" . Give an example of a molecule involving sp^(3)d hybridisation of the central atom and two lone pairs.

    The number of lone pair of electrons on the central atom of XeF_4 molecule is

    How many lone pair of electrons are present on chlorine in ClF_(3) molecule ?

    When the number of electron pairs on the central atom is six, the geometry of the molecule is :

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