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This question already has an answer here:

According to these sites:

  1. Chemistry Help

  2. Molbase

in $\ce{PCl2F3}$, both $\ce{Cl}$ and one $\ce{F}$ atom are on equatorial position, and other 2 $\ce{F}$ atoms are on axial position as follows:

enter image description here

The first site mentions that to minimise repulsions of $\ce{F - F}$ bonds. But this structure is in fact increasing the repulsions, and decreasing stability, since the bond angle of $\ce{F - P - F}$ bond will be about $\mathrm{90^\circ}$

If instead all the $\ce{F}$ atoms are on equatorial position, and the 2 $\ce{Cl}$ on axial positions, then the repulsion may be further minimized.

So according to me, the structure should be:

enter image description here

Question: Why is my structure wrong? Please explain. Thank you!

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marked as duplicate by orthocresol, Todd Minehardt, bon, Klaus-Dieter Warzecha, M.A.R. Feb 10 '16 at 16:38

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    $\begingroup$ See, the repulsion is not only between fluorines. $\endgroup$ – Ivan Neretin Feb 10 '16 at 12:03
  • $\begingroup$ @IvanNeretin But $\rm F$ on equitorial position is a menace for all. It will repel the two $\rm F$ on axial very strongly, and also repel the chlorine. $\endgroup$ – Max Payne Feb 10 '16 at 12:05
  • $\begingroup$ True, but chlorine would repel chlorine even stronger. $\endgroup$ – Ivan Neretin Feb 10 '16 at 12:06
  • $\begingroup$ @IvanNeretin Thats why i placed the $\rm Cl$ atoms on axial position. This also gives symmetry to molecule. The site I linked said that Fluorine's bond $e^-$ repel more strongly due to its greater electronegativity $\endgroup$ – Max Payne Feb 10 '16 at 12:10
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    $\begingroup$ Strongly related: chemistry.stackexchange.com/questions/18427/… $\endgroup$ – bon Feb 10 '16 at 13:02