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NEETChemistryClassification of Elements and Periodicity in Properties

Considering the stability of oxidation states, which of the following relationships is correct for Group 14 chlorides?

Options

  1. ASnCl₂ > SnCl₄
  2. BGeCl₂ > GeCl₄
  3. CPbCl₂ > PbCl₄
  4. DSiCl₂ > SiCl₄

Correct answer

C. PbCl₂ > PbCl₄

Step-by-step solution

In Group 14 elements (C, Si, Ge, Sn, Pb), the general valence shell electronic configuration is ns^2 np^2 . They primarily exhibit +4 and +2 oxidation states. Down the group, the stability of the higher oxidation state (+4) decreases and that of the lower oxidation state (+2) increases due to the inert pair effect (the reluctance of ns^2 electrons to participate in bond formation). For lighter elements like Si, Ge, and Sn, the +4 state is more stable than the +2 state. Therefore, SiCl₄ , GeCl₄ , and SnCl₄ are more

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