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Sulphur and rest of the elements of grou...

Sulphur and rest of the elements of group `16` are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire `ns^2 np^6` configuration by sharing two electrons with the atoms of other elements and thus, exhibit `+2` oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the `p` and s-orbitals of the same shell. As a result, they can show `+4` and `+ 6` oxidation states.
Like sulphur, oxygen does not show `+ 4` and `+6` oxidation states. The reason is

A

That oxygen is a gas while sulphur is a solid

B

That oxygen has high ionisatio enthalpies in comparison to sulphur

C

That oxygen has high electron affinity in comparison to sulphur

D

That oxygen has no d-orbitals in its valence shell.

Text Solution

Verified by Experts

The correct Answer is:
D
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Knowledge Check

  • Sulphur and rest of the elements of group 16 are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire ns^2 np^6 configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the same shell. As a result, they can show +4 and + 6 oxidation states. Oxygen exhibits +2 oxidation state in

    A
    `H_2 O`
    B
    `OF_2`
    C
    `Cl_2 O`
    D
    `H_2 O_2`

  • Sulphur and rest of the elements of group 16 are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire ns^2 np^6 configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the same shell. As a result, they can show +4 and + 6 oxidation states. The oxidation state of sulphur in Na_2 S_4 O_6 is

    A
    `2//3`
    B
    `3//2`
    C
    `3//5`
    D
    `5//2`

  • Sulphur and rest of the elements of group 16 are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire ns^2 np^6 configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the same shell. As a result, they can show +4 and + 6 oxidation states. The nature of the compounds of sulphur having +4 oxidation state is

    A
    Act as oxidising agents
    B
    Acts as reducing agents
    C
    Act as oxidising as well as reducing agents
    D
    Cannot be predicted

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    Explore conceptually related problems

    Sulphur and rest of the elements of group 16 are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire ns^2 np^6 configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the same shell. As a result, they can show +4 and + 6 oxidation states. The oxidation state of of sulphur in S_8, SO_3 and H_2 S respectively are.

    No two electrons in an atom of an element have

    Which is the valence shell electronic configuration 16^(th) group elements ?

    Which of the following atom with outer electronic configuration exhibit maximum oxidation state ?

    Valence electrons in the atom of element A is 4 and in the element B is 2. Most probable compound formed from A and B is

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