Below is the structure of benzene (C_2H_6). Both VBLE) and MO Theories are used

Question

Below is the structure of benzene (C_2H_6). Both VBLE) and MO Theories are used to describe its bonding. Below are its pi Mo energy levels and simplified pictures of those MO's next to the energy levels. (a) How many total p orbitals are mathematically combined to form the pi MO's shown below for this molecule? How many ambybridized p orbtials are available after applying hybridization to each of the atoms? What is the relationship between the number of MOs and the number of atomic orbitals used to make them by LCAO? (b) Circle below the pictures of the MO's that represent Pi* Mo's What is the relative energy of this type of pi MO among other pi MO's and what it their typical number and distribution among energy levels compared to pi bonding MOs? (c) State which orbitals overlap to form the C-C bonds in benzene. (d) Are pi nonbonding MO's present? Considering your answer to the question to consider in (b) above, how do the typical number and distribution of pi nonbonding MOs differ from that of pi and pi* MOs? (e) Six electrons (representing the 3 pi bonding electron pairs) occupy the pi MO energy levels to the left. Correctly place those electrons in the MO energy level diagram. Use the orbital to state whether benzene relatively stable according to Mo theory. Briefly explain.

Explanation / Answer

2. (a) Total 6 p-orbitals are combined to form the pi-M.O's for this molecule.

1. There are one unhybridised p-orbital present for every carbon atom, six unhybridised p-orbital in total.

After hybridisation and the formation of pi-bond there are no unhybridised p-orbital left for any carbon atom.

2. Numbers of atomic orbitals used to form LCAO is equal to the number of M.O's formed.

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