## PCl6

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

vanessas0123
Posts: 100
Joined: Wed Sep 11, 2019 12:17 am

### PCl6

Why is the hybridization of P in PCl6 sp3d2?

Serena Siddiq 3D
Posts: 51
Joined: Fri Aug 30, 2019 12:17 am

### Re: PCl6

Since P is bonded to 6 other atoms, its shape is an octahedral and has 6 regions of electron density. Therefore, its hybridization must be sp3d2, which accounts for all 6 of those regions. Hope that helps!

Chris Tai 1B
Posts: 102
Joined: Sat Aug 24, 2019 12:16 am

### Re: PCl6

The reason octahedral shapes need to have an extra two valence d electrons is because the p suborbitals can only hold up to three valence electrons in such a given orbital, so atoms like Xe and P must go into the d orbital regions (which mix with the preexisting s and p orbitals) to gain more valence electrons.

Joelle 3L
Posts: 50
Joined: Sat Jul 20, 2019 12:16 am

### Re: PCl6

The P in PCl6 has six regions of electron density. Therefore, to account for all these six regions the hybridization would be sp3d2. The p orbital can only hold up to three valence electrons