Question

The nature of $\pi$- bond in perchlorate ion is-

• A. O (dπ)- Cl (pπ)
• B. O (pπ) -Cl (dπ)
• C. O (dπ)- Cl (dπ)
• D. O (dπ) - Cl (dπ)

Answer 1

The correct option is B O (pπ) -Cl (dπ)

Ground state outer electronic configuration of Cl is

Thus, Cl atom exhibits $s{p}^3$ hybridizaion to form $4\pi$ bonds. Therefore, 3 $\pi$ bonds in perchlorate ion are formed by overlap of p-orbitals of O and d-orbitals of Cl.