Oxygen and sulfur resemble each other in all respects except ____________?

Oxygen (O) and sulfur (S) are both elements of Group 16 (the oxygen family or chalcogens) in the periodic table. They possess similar outer electronic configurations — ns² np⁴ — which results in comparable chemical properties such as forming oxides, showing allotropy, and existing as non-metals. However, despite these similarities, there are some key differences due to the variation in atomic size, electronegativity, and availability of d-orbitals.

Oxygen is a second-period element, while sulfur lies in the third period. This difference introduces the availability of vacant 3d orbitals in sulfur, allowing it to show higher oxidation states, unlike oxygen.

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  Oxygen’s oxidation states: It usually exhibits −2 (in oxides) and sometimes −1 (in peroxides) or 0 (in O₂). Higher oxidation states such as +2 are extremely rare and unstable due to the absence of d-orbitals and high electronegativity.

  
  


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  Sulfur’s oxidation states: Sulfur, on the other hand, shows a much wider range: −2, 0, +2, +4, and +6, found in compounds like H₂S, S₈, SO₂, and SO₃ respectively. This versatility arises from the ability of sulfur to expand its octet using the available 3d orbitals.

  
  

Apart from this difference, both elements:

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  Exist in allotropic forms (oxygen as O₂ and O₃; sulfur as rhombic and monoclinic sulfur).

  
  


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  Form polymeric or chain structures (especially sulfur, due to its larger size).

  
  


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  Exhibit similar valence shell configurations, leading to comparable bonding patterns in many compounds.

  
  

Therefore, while oxygen and sulfur resemble each other in electronic configuration, allotropy, and polymeric nature, they differ in oxidation states because only sulfur can exhibit higher positive oxidation states like +4 and +6.

Hence, the correct answer is D) Show same oxidation states