Question

Which of the following is incorrect statement regarding compound $C{l}_2{O}_6$?

• A. In covalent (gaseous) state, each $Cl$ atom has a hybridisation of $s{p}^3$ in $C{l}_2{O}_6$
• B. $C{l}_2{O}_6$ exists as $Cl{O}_2^{+}$ and $Cl{O}_4^{-}$ in ionic form
• C. In ionic form of $C{l}_2{O}_6$, hybridisation of $Cl$ atoms is $s{p}^2$ and $s{p}^3$
• D. In ionic form of $C{l}_2{O}_6$, hybridisation of both the $Cl$ atoms is $s{p}^3$

Answer 1

The correct option is D In ionic form of $C{l}_2{O}_6$, hybridisation of both the $Cl$ atoms is $s{p}^3$

In covalent form, $C{l}_2{O}_6$ have a hybridisation of $s{p}^3$ for each $Cl$ atom since chlorine atom forms 4 sigma bonds


In ionic bond, $C{l}_2{O}_6$ exists as $Cl{O}_2^{+}$ and $Cl{O}_4^{-}$ since $Cl{O}_2^{+}$ have a steric number of 3 so hybridisation is $s{p}^2$ and $Cl{O}_4^{-}$ has a hybridisation of $s{p}^3$