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Elements of Groups 16, 17 and 18 — Chemistry STD 12 Science — Question

Maharashtra BoardEnglish MediumSTD 12 ScienceChemistryElements of Groups 16, 17 and 183 Marks
Question
Explain the oxidation states of Group $16$ elements.
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Answer

  • Group $16$ elements have general electronic configuration, $ns^2 np^4,$
  • They show variable oxidation states, $– 2, + 2, + 4$ and $-6.$
  • Since all elements have $6$ valence electrons, they tend to gain or share $2$ electrons to complete an octet, and show common oxidation state $– 2.$
  • Oxygen being highly electronegative, it shows the common oxidation state $-2$ in oxides $(H_2O, MgO).$ It shows $– 1$ oxidation state in peroxides $(H_2O_2, Na_2O_2)$ and $+ 2$ oxidation states in $OF_2.$
  • Except oxygen all other elements have vacant d-orbitals, hence they show higher oxidation states $+ 4$ and $+ 6$. For example
    Image
  • The stability of the $+ 6$ oxidation state decreases but the stability of the $+4$ oxidation state increases down the group due to the inert pair effect.
  • Bonding in $+4$ and $+6$ oxidation states is covalent in nature.

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