Why is bond energy of P-Cl bond different in PCl3 and PCl5?

The P−Cl bond in PCl3 is stronger (322 kJ/mol) than that in PCl5 (260 kJ/mol). However the 326 kJ/mol value comes from the average of all P−Cl bonds found in all known molecules containing P−Cl bonds (including but not limited to PCl3 and PCl5).

Which is stronger PCl3 or PCl5?

(b) PCl5 is larger than PCl3 so the induced dipole-induced dipole forces (London dispersion forces) in PCl5 are stronger than in PCl3.

What is the difference between PCl5 and PCl3?

Phosphorus Trichloride is more stable than Phosphorus pentachloride because PCl5 has more density (trigonal bipyramidal and sp3d2 hybridisation) than PCl3 (structure of the trigonal planet and sp3 hybridisation).

How many types of CL P-Cl bonds are present in PCl5?

For molecules adopting trigonal bipyramidal geometry there are 5 bonds. The three bonds in the plane called planar bonds or equatorial bonds. And the remaining two bonds – one lying above the plane and one lying below the plane called axial bond.

What is the bond energy of P CL?

Common Bond Energies (D

What is the en difference of P and Cl in pcl5?

P (EN = 2.1) is less electronegative than chlorine (EN = 3.0) so P is the central atom. The Lewis structure is: The electronegativity difference between P and Cl is 0.9 so the C–Cl bond is nonpolar.

What type of bond is P Cl?

covalent bonds
Phosphorus(V) chloride, PCl In the case of phosphorus, 5 covalent bonds are possible – as in PCl5.

Which is more stable PCl3 or PCl5 and why?

PCl3 is more stable than PCl5 because PCl5 has steric crowding(triagonal bipyramidal shape and sp3d2 hybridisation) than PCl3(triagonal planar structure and sp3 hybridisation).

Why is PCl3 less stable than bicl3?

P3+ is smaller in size as compared to Bi3+. According to Fajan’s rule, smaller the cation, higher will be the covalent nature of the bond. Hence, BiCl3 is less covalent than PCl3.

Why is PCl5 not planar?

We can see from the discussion that the geometry is trigonal bipyramidal also the equatorial bonds are planar and one of the axial bonds lie above the plane and the other lies below the plane. Hence, the structure is non-planar.

Why axial bonds are longer in PCl5?

Geometry of PCl5 The axial bonds are longer than equatorial bonds because of greater repulsion from equatorial bonds. So axial bonds are nearer to equatorial bonds and this causes greater repulsion resulting in elongation of bond length.

How are bond length and bond energies related?

The higher the bond energy, the ‘stronger’ we say the bond is between the two atoms, and the distance between them (bond length) is smaller. The bond energy is the average of the bond dissociation energies in a molecule.