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 inA. `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 electronegativ

1.	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 inA. `H_2 O`B. `OF_2`C. `Cl_2 O`D. `H_2 O_2`
Answer» Correct Answer - B Let the oxidation state of `O` in `OF_2` be `x` `x + (-1) xx 2 = 0 rArr x = + 2`.