Home
Class 11
CHEMISTRY
Describe the hybridisation in case of PC...

Describe the hybridisation in case of `PCl_5`. Why are the axial bonds longer as compared to equatorial bonds?

Text Solution

Verified by Experts

The hybridisation in the molecule of `PCl_(5)` because the central atom is the same in both the molecules and the two halogens chlorine (Cl) and fluorine (F) also belong to the same group (group 17). They anexpected to have same hybridisation as well as same geometry. The P atom is `sp^(3)` d hybridised and the molecile has tregonal bipyrramidal geometry. The details of hybridisation of `PF_(5)` have been given in sections 4.14
Promotional Banner

Similar Questions

Explore conceptually related problems

Describe the hybridisation in case of PCl_(5) . Why are the axiial bonds longer as compared to equatorial bonds?

Describe hybridisation in the case of PCl_(5) and SF_(6) The axial bonds are longer as compared to equatorial bonds in PCl_(5) whereas in SF_(6) both axial bonds and equatorial bonds and have the same bond length. Explain.

Explain why the axial bonds in PC l_(5) are longer than the equatorial bonds.

Why are the pi -bonds weaker and more reactive than the sigma -bonds?

Why are the P-Cl bonds in PC l_(5) not of same length?

In case of CO_3^(2-) ion,all the C-O bond lengths are equal explain.

All the P - Cl bonds in PCl_(5) are not equivalent - why ?

Why is a coordinate bond referred to as a semipolar bond?

Why are the four C - CI bonds in CCI_(4) equivalent?.

sp^(3) hybridisation is involved in CH_(4), H_(2)O and NH_(3) . Why are the bond angles different in three cases?