Highest Occupied Molecular Orbital Puns

Thank you.

They’re homophobic

According to Molecular Orbital Theory, which diatomic molecule would have the highest bond order? A) O-F B) O-O C) F-F D) N-O

I know it’s like another theory as opposed to the localized electron model but I don’t really understand the whole bonding and antibonding principles and YouTube videos aren’t helping lol

I'm hoping a kind soul can provide advice for my high school student taking Chemistry. She's trying to better understand Molecular Orbital Theory. Can anyone explain it?

Hey guys.

I'm studying the molecular orbital theory and found some missing information while solving.

If we are asked about the MO of a polyatomic orbital, BeF2 for example, how can I know the order of the MO formed between the atomic orbitals, how can I know what atomic orbitals do bond together. Thank you

At the moment I'm learning about molecular orbital diagrams for homonuclear molecules, namely: B2, C2, N2, O2, F2, and Ne2. I understand that the energy of the 2p sigma bond is at a higher level for B2, C2, and N2, leading to the 2p sigma bond and the 2p pi bond switching places in the MO diagram (with 2p pi bond appearing under 2p sigma bond) for B, C, and N but not for O, F, or Ne. My lectures state that this is due to s and p mixing and my textbook states that it is due to electron repulsion from the 2s sigma bond's electrons towards the electrons added to the 2p sigma bond. Are these repulsions occurring because the s and p orbitals are mixing? Are these orbitals now suddenly hybrid sp orbitals? I'm having a hard time seeing the logic here. Thanks for the help!

I’m having trouble identifying which molecular orbitals of a pi system in Pericyclical Reactions are bonding, nonbonding and antibonding, can anyone please explain this concept to me?

I’ve been tasked with drawing rhe MO diagram for Sulfure Oxide and I’m not sure about the energies of the relatove orbitals. Since Oxygen is more electronegative I expect the 2s and 2p orbitals to have much lower energy than the 3s and 3p orbitals sulfur has. But the energy difference would be really high then. So I’m not sure what 2 orbitals combine to form the sigma 3s or sigma* 3s orbital. The difference in energy kevels confuses me as every example I’ve done has the same orbitals (2s,2p’s) combining to make a different molecular orbital. Not sure about SO since sulfur has valence electrons in the 3s and 3p’s while oxygen has valence electrons in the 2s and 2p’s

For both sigma and pi bonds (O is oxygen, C is carbon):

A. In terms of electronegativity: Since effective nuclear charge of O is higher than C, so the E.N. of O is higher than C. Therefore, both sigma and pi bonding orbitals will have energy closer to O as the bonding electrons are more localized to O than C, hence those orbitals will be lower in energy for C=O than C=C.

B. However, from what I am learning on bond interaction energy:

1. Atomic orbitals with more similar energy yield larger bond interaction, hence lower bonding molecular orbital energy (sigma and pi)
2. Atomic orbitals with more similar sizes yield better orbital overlap i.e. larger bond interaction, which gives the same result to (1).

As Carbon-Carbon atomic orbital interaction is higher than Carbon-Oxygen (since C-C has the same A.O. energy and their orbitals are the same size (if C and O here are all sp2) - due to no E.N. differences), I am thinking:

1. both sigma and pi bonds of C=C will be lower energy than that of C=O
2. both sigma* and pi* bonds of C=C will be higher energy than that of C=O

From (2), it can be explained why C-F bond is easier to break than C-C bond (e.g. in SN2), as sigma*(LUMO) of C-F is lower than C-C.

Question: In terms of E.N., sigma and pi bonds are lower energy for C=O than C=C. But from bond interaction, it seems those bonds are lower energy for C=C than C=O, may I ask what mistakes have I made here? (I know I am wrong since alkenes have nucleophilic pi bonds while carbonyls have electrophilic pi bonds)

My chem book says: the sidewise overlap of pi orbitals of carbon atoms in benzene produces a pi molecular orbital containing six electrons.

What is a pi molecular orbital? Can you explain it in layman terms plz?

Allo there, I’m a first year chem student at uni, and I’m struggling to get my head around the concept of molecular orbitals. In particular how anti bonding and bonding orbitals are both made when atoms bond. I understand them separately but can’t put them together in my head. Any help would be much appreciated.

Donny x

I'm a freshman, currently taking up chem. I'm having a hard time wrapping my head on the ideas on these theories. Can anyone care to explain it to me? I'll be a great help for me.

Journal of the American Chemical SocietyDOI: 10.1021/jacs.0c10791

David Trummer, Keith Searles, Alexander Algasov, Sergey A. Guda, Alexander V. Soldatov, Harry Ramanantoanina, Olga V. Safonova, Alexander A. Guda, and Christophe Copéret

https://ift.tt/2Rehc9J

I know it’s like another theory as opposed to the localized electron model but I don’t really understand the whole bonding and antibonding principles and YouTube videos aren’t helping lol