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Bond angle in H(2)S is lower than in H(2...

Bond angle in `H_(2)S` is lower than in `H_(2)O`. Justify.

Text Solution

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Bond angle in `H_(2)O (104.5^(@))` is higher than the bond angle in `H_(2)S (92^(@))`. The difference in the bond angles is linked with the electronegativities of the oxygen and sulphur atoms. As the electronegativity of the central atom decreases, bond angle decreases. In the present case, S is less electronegative than oxygen. Now, since oxygen is more electronegative than sulphur therefore, the electron density around oxygen in `H_(2)O` is more than around sulphur in `H_(2)S`. As a result, the bond angle in `H_(2)O` is more than the bond angle in `H_(2)S` .
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Knowledge Check

  • Bond angle in H_(2)O is

    A
    `104.5^(@)`
    B
    `120^(@)`
    C
    `109.5^(@)`
    D
    `107^(@)`

  • The bond angle in H_2S is

    A
    `gt NH_3`
    B
    Same as in `BeCl_2`
    C
    `gt H_2Se`, `lt H_2O`
    D
    Same as in `CH_4`

  • The bond angle in H_(2)S

    A
    `gt NH_(3)`
    B
    Same as in `BeCl_(2)`
    C
    `gt H_(2)Se lt H_(2)O`
    D
    Same as in ` CH_(4)`

    • Similar Questions

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    The bond angle in H_(2) S is:

    The bond angle in H_(2) S is:

    Bond angle in H_(2)S molecule is

    Assertion : Bond angle in H_(2)O is less than that in H_(2)S . Reason : Electronegativity of O is more than that of S.

    Assertion (A) The O-O bond length in H_(2)O_(2) is shorter than that in O_(2) . Reason (R ) H_(2)O_(2) is ionic compound.

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