Redox Reactions And Electrochemistry Ques 679
Question: Which of the following do not show disproportionation reaction- $ ClO_4^{-},,F_2,,Cl_2,,ClO_2^{-},,ClO_2^{-},,P_4,,S_8 $ and $ Cl{{O}^{-}} $
Options:
A) $ ClO_2^{-},,ClO_4^{-}, $ and $ Cl{{O}^{-}} $
B) $ F_2 $ only
C) $ F_2 $ and $ ClO_4^{-} $
D) $ ClO_4^{-} $ only
Show Answer
Answer:
Correct Answer: C
Solution:
[c] $ F_2 $ being most electronegative element cannot exhibit any positive oxidation state. In $ ClO_4^{-} $ chlorine is present in its highest oxidation state i.e +7. Therefore it does not show disproportionation reaction.
