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What is the hybridization of P in ##PF_3## and ##PF_5##?
In this answer, I will first teach you a general way to find the hybridization of , And finally I will answer your question.
- To find hybridization ,first draw the Lewis structure.
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Next count the electron regions around the central atom
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Electron regions : Places which are regions of high electron .
- A triple bond ##rArr## one electron region..
- A single bond ##rArr## one electron region.
- An electron lone pair ##rArr## one electron region.
And,
- If there are
- 8 electron regions; hybridization is ##sp^3d^4##.
- 7 electron regions; hybridization is ##sp^3d^3##.
- 6 electron regions; hybridization is ##sp^3d^2##.
- 5 electron regions; hybridization is ##sp^3d##.
- 4 electron regions; hybridization is ##sp^3##.
- 3 electron regions; hybridization is ##sp^2##
- 2 electron regions; hybridization is ##sp##
In
- ##PF_3##==> One lone pair & three single bonds.
In ##PF_3## there are 4 electron regions, so hybridization is ##sp^3##
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In ##PF_5##, there are ##5## electron regions around the central atom (5 single bonds)
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So the hybridization is ##sp^3d##.
I hope this is helpful, what is your feedback?
Meantime don't forget to check this also