Question

Use a molecular orbital energy diagram to explain why we can never expect to see more than a triple bond.

Answer 1

Answer: the molecular diagram with explanation is given as follows,

• os. There are two types of Molecular orbital e diagram. 1. If more ual or than less 14 electrons are present than 14 electrons present ALMO 000 oool 7000.000/ ) ooo px P P2 000 Papy P2 Paap, P2 Px PY P2 0 110 V TTY ABMD 25 O 25 BMOIS AU - 15 or M. O Diagram M. O of B2, Cele Diagram of O2, Fa etc (Equal less than Care & More than 1460) Equalfless than 14 eos) 14 If we are taking No for M. O Diagram than No has 14 00. 450 First 4 electrons will go to ist & 188* nie Bonding & antibonding then 254 & 250 orbital will be filled then 28. Te, 21lgh will be filled by remaining electrons & 36 Orbital will get eletrons. The electronic configuration of No is: No = (as)[48][*]* [ Tapa] [ Tomy]*[T5:)"

o No (Bond order) = No. of Bonding Orbit of Bonding Orbital's eg - No. of antibondin Pr 2 No 2.0 - 6 - 0 - 6 2 2 GITISATISH & Tas, Tis eos cancel each other) If we are taking On then. e.configuration of Oz = (Tis] G] [6] [435][17px) [Tlapa"]' (,) ooooooooooooooo B.0 = 65.2 - 4 - 2 6-27 Because 3 Bonding Orbital and only can never expect Orbitals are be electrons to see more present in Molecular can occupy B.O we than a tripal bond.