Which of the following statements is false ab | vedclass

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(B) $1$. Oxygen has the electronic configuration $[He] 2s^2 2p^4$,which contains $2$ unpaired electrons in the $2p$ orbitals.$2$. Sulphur has the elec

Vedclass · Accepted Answer

Oxygen and sulphur show $-2, +4$ and $+6$ oxidation states.

Vedclass · Answer

(B) $1$. Oxygen has the electronic configuration $[He] 2s^2 2p^4$,which contains $2$ unpaired electrons in the $2p$ orbitals.$2$. Sulphur has the electronic configuration $[Ne] 3s^2 3p^4$,which also contains $2$ unpaired electrons in the $3p$ orbitals.$3$. Oxygen is highly electronegative and typically exhibits an oxidation state of $-2$. It does not show $+4$ or $+6$ oxidation states because it lacks $d$-orbitals.$4$. Sulphur can show $-2, +2, +4,$ and $+6$ oxidation states due to the availability of vacant $d$-orbitals.$5$. Therefore,the statement that both oxygen and sulphur show $-2, +4,$ and $+6$ oxidation states is false.

Which of the following statements is false about oxygen and sulphur?

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