Energy diagram for hybridized oxygen in CO

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Discussion Overview

The discussion revolves around the energy diagram for hybridized oxygen in carbon monoxide (CO), focusing on the number of electrons represented in the diagram and the implications of hybridization in this context. Participants explore the correctness of the diagram and its relevance to bonding and molecular orbital theory.

Discussion Character

  • Homework-related, Debate/contested, Conceptual clarification

Main Points Raised

  • One participant questions the accuracy of the energy diagram, noting that oxygen has six electrons but the diagram shows only five.
  • Another participant asserts that oxygen is not charged in CO, suggesting the diagram must be incorrect.
  • A different viewpoint proposes that the diagram might be considering bonding electrons from both carbon and oxygen, referencing bonding and anti-bonding orbitals.
  • One participant mentions that the molecular orbital (MO) diagram for CO is isoelectronic to N2 and can have either six or ten electrons, depending on the inclusion of certain bonding-antibonding pairs.
  • Concerns are raised about the hybridization of the diagram, with one participant questioning the necessity of hybridization for oxygen in CO.
  • Another participant agrees that hybridization may not be applicable for a diatomic molecule like CO, suggesting that the exercise may be poorly designed.

Areas of Agreement / Disagreement

Participants express disagreement regarding the accuracy of the energy diagram and the relevance of hybridization for oxygen in CO. Multiple competing views remain about the interpretation of the diagram and the number of electrons involved.

Contextual Notes

There are limitations regarding the assumptions made about hybridization and the representation of electrons in the diagram, as well as the potential for confusion surrounding bonding and anti-bonding orbitals.

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Homework Statement


Please look at the screenshot attached. The answer is "Yes", but I am not sure why.

Homework Equations


N/A

The Attempt at a Solution


Oxygen have six electrons, but the energy diagram shows only five. That was why I thought it was wrong, but the diagram shown is correct. Can anyone explain why?
 

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There have to be six electrons. Oxygen isn’t charged in CO. The diagram must be wrong.
 
TeethWhitener said:
The diagram must be wrong.
..., unless, it's for bonding electrons from both carbon and oxygen? Seem to recall some sort of quasi-quantum mechanical argument for "bonding/anti-bonding orbitals."
 
The MO diagram for CO is isoelectronic to N2 and will have either 6 or 10 electrons, depending on whether you choose to include the σ-σ* bonding-antibonding pair generated from the 2s electrons. The point of the exercise is doubtless to highlight the energy splitting due to the hybridization of s and p orbitals on oxygen, but in no world is 5 electrons correct.
 
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How the heck do you hybridize a diagram?
Furthermore, there is no reason why O in CO should be hybridized at all.
 
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Likes   Reactions: TeethWhitener
I agree, it doesn’t make much sense for a diatomic. I imagine the point was to show the effects of hybridization on s and p orbital energies, but that’s probably the least of the problems with this example.
 

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