Why isn't ClF3 trigonal planar?

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Discussion Overview

The discussion revolves around the molecular geometry of chlorine trifluoride (ClF3), specifically why it adopts a T-shaped structure rather than a trigonal planar configuration. The conversation touches on concepts from VSEPR theory and the spatial requirements of electron pairs.

Discussion Character

  • Technical explanation, Conceptual clarification, Debate/contested

Main Points Raised

  • One participant asserts that ClF3 has a trigonal bipyramidal arrangement and T-shaped molecular geometry, questioning why it could also be considered trigonal planar.
  • Another participant explains that according to VSEPR theory, non-bonding electron pairs are sterically more demanding than bonding pairs, which influences the molecular shape.
  • A participant seeks clarification on the term 'sterically more demanding than bound electron pairs' and expresses difficulty in understanding its meaning.
  • In response, another participant states that non-bonding pairs need more space and occupy a larger volume compared to bonding pairs.

Areas of Agreement / Disagreement

Participants express differing views on the molecular geometry of ClF3, with no consensus reached on the applicability of the trigonal planar model.

Contextual Notes

The discussion highlights the complexity of molecular geometry and the influence of electron pair repulsion, but does not resolve the assumptions or definitions related to steric demands and VSEPR theory.

prakhargupta3301
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I know ClF3 has triagonal bi-pyramidal arrangement and T-shape molecular geometry. (as shown in first diag.). However, it can also be 2nd case. In this one, the shape will be triagonal planar. Also, electrons will be farthest. So why isn't ClF3 like second case?
 

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In VSEPR theory, non-bonding electron pairs are sterically more demanding than bound electron pairs. In the first formula, each non-bonding electron pair has only two neighbours in a 90 degree separation while in the 2nd one, each has 3. Whether the distance between the two non-bonding pairs is 120 or 180 degrees will be rather irrelevant compared to the next neighbour repulsion.
 
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I get what you mean. Thank you.
But would you be kind enough to explain what
DrDu said:
'sterically more demanding than bound electron pairs'
means?
[I did look up the meaning of steric but the meaning still isn't clear]
Thanks.
 
Need more space for themselves, occupy larger volume.
 

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