Bond Orders of Isoelectronic Species

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Discussion Overview

The discussion revolves around the bond orders of isoelectronic species, specifically comparing the bond orders of F2 and O2 -2 (oxygen molecule ion). Participants explore the reasons behind the bond orders and the application of molecular orbital theory in calculating these values.

Discussion Character

  • Exploratory, Technical explanation, Conceptual clarification

Main Points Raised

  • One participant questions how isoelectronic species like F2 and O2 -2 can have the same bond order, specifically asking about the bond order of the oxygen molecule ion.
  • Another participant provides a formula for calculating bond order using molecular orbital theory, suggesting that the bond order is determined by the difference between the number of electrons in bonding and anti-bonding orbitals.
  • A subsequent post reiterates the bond order calculation method and encourages others to find the bond orders of O2, O2^-, and O2^2- independently.
  • One participant expresses a desire for alternative methods to calculate bond order, indicating they have not yet learned about anti-bonding orbitals.
  • Another participant suggests that the concept is not difficult and recommends referring to standard inorganic chemistry textbooks for further understanding of molecular orbital theory.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the bond order of the oxygen molecule ion, and there are differing levels of familiarity with molecular orbital theory among participants.

Contextual Notes

Some participants express uncertainty regarding the application of molecular orbital theory, particularly in relation to anti-bonding orbitals, which may affect their ability to calculate bond orders accurately.

Who May Find This Useful

Students and individuals interested in molecular chemistry, particularly those studying bond order and molecular orbital theory.

Priyadarshini
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How and why do isoelectronic species have the same bond order? My book cites an example that says that F2 and O2 -2 (oxygen molecule ion) has a bond order of 1. I understand how fluorine gas has a bond order of 1. But how does the oxygen molecule ion have a bond order of 1? Is it because they both have the same number of valence electrons?
Thanks!
 
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You can calculate bond order using Molecular orbital theory.
Bond Order = [(number of electrons occupying bonding orbitals)-(number of electrons in anti-bonding orbitals)]/2
Try to find the bond order of ##O_2##, ##{O_2}^-## and ##{O_2}^{2-}## yourself.
 
Titan97 said:
You can calculate bond order using Molecular orbital theory.
Bond Order = [(number of electrons occupying bonding orbitals)-(number of electrons in anti-bonding orbitals)]/2
Try to find the bond order of ##O_2##, ##{O_2}^-## and ##{O_2}^{2-}## yourself.
Is there any other way to work it out? I haven't learned anti-bonding yet.
 
Its not a difficult concept. Refer some standard inorganic chemistry textbooks for MOT.
 

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