Question

The manganate and permanganate ions are tetrahedral, due to:

• A. The \(\pi\) bonding involves overlap of p-orbitals of oxygen with d-orbitals of manganese
• B. There is no \(\pi\) bonding
• C. The \(\pi\) bonding involves overlap of p-orbitals of oxygen with p-orbitals of manganese
• D. The \(\pi\) bonding involves overlap of d-orbitals of oxygen with d-orbitals of manganese

Answer 1

The Correct Option is A

The given question asks about the tetrahedral shape of manganate and permanganate ions and the type of bonding responsible for this geometry. Let's explore the correct option and reasoning behind it:

1. Tetrahedral Shape Explanation:
   • Manganate (\(\text{MnO}_4^{2-}\)) and permanganate (\(\text{MnO}_4^{-}\)) ions are known to have a tetrahedral geometry.
   • This geometry arises due to the electronic structure and specific types of bonding present in these ions.
2. Type of Bonding:
   • The tetrahedral shape is primarily due to the overlap of orbitals between manganese and oxygen atoms.
   • In these compounds, manganese is in a high oxidation state, specifically \(+6\) in manganate and \(+7\) in permanganate after losing its electrons, which allows it to utilize its d-orbitals for \(\pi\) bonding.
   • Oxygen uses its p-orbitals to form \(\pi\) bonds with the d-orbitals of manganese. This type of bonding is known as p-d \(\pi\) bonding.
3. Choice Justification:
   • The \(\pi\) bonding involves overlap of p-orbitals of oxygen with d-orbitals of manganese: This statement is correct as explained above. The p-d \(\pi\) bonding strengthens the overall structure, resulting in the stable tetrahedral shape of both ions.
   • Other Options:
     • There is no \(\pi\) bonding: Incorrect, because \(\pi\) bonding is essential for the stability and geometry.
     • The \(\pi\) bonding involves overlap of p-orbitals of oxygen with p-orbitals of manganese: Incorrect, because manganese uses its d-orbitals, not p-orbitals, for \(\pi\) bonding.
     • The \(\pi\) bonding involves overlap of d-orbitals of oxygen with d-orbitals of manganese: Incorrect, because oxygen typically uses its p-orbitals for bonding.

Hence, the correct answer is: The \(\pi\) bonding involves overlap of p-orbitals of oxygen with d-orbitals of manganese.