Sage-Tips

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

The hybrization of P in PCl3 is sp3 and in PCl5 is sp3d. Cl is more electronoegative than P so it tends to pull electron density away from P. This will weaken the strength of the bond between the other P—Cl bonds.

Why all P Cl bonds lengths are not equivalent in PCl5?

(i) In gaseous and liquid state, PCl5 has a trigonal bipyramidal structure. In this structure, the two axial P-Cl bonds are longer and less stable than the three equatorial P-Cl bonds. This is because of the greater bond pair – bond pair repulsion in the axial bonds. Hence, all the bonds in PCl5 are not equivalent.

What causes differences in bond length?

The length of the bond is determined by the number of bonded electrons (the bond order). The higher the bond order, the stronger the pull between the two atoms and the shorter the bond length. Generally, the length of the bond between two atoms is approximately the sum of the covalent radii of the two atoms.

How bond length is affected by hybridization?

The greater s character of the sigma bonds of acetylene and alkynes affects their physical properties. The length of a bond between a carbon atom and another atom is the shortest for a carbon atom with sp hybrid orbitals. The length of a carbon–carbon sigma bond depends on the hybridization of both carbon atoms.

What is the bond energy of P Cl?

Common Bond Energies (D

Bond	D (kJ/mol)	r (pm)
P=O	544	150
P=S	335	186
P-F	490	154
P-Cl	326	203

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.

Why all PF bonds in PF5 molecule are not of the same length?

Answer Expert Verified concept :- bond length depends upon hybridization of molecule . we know, structure of SP³d is an Triangular bipyramidal . in which three bonds have equal length but two bonds (axial bond) are longer. so, all bonds of PF5 isn’t equal .

Why all PF bonds in PF5 are not equivalent?

PF5 has sp3 hybridisation, out of P−F bonds two are equatorial which have different lengths. C. Out of five P−F bonds two are axial and three equatorial. PF5 is made up of two types of bond namely covalent and coordinate, hence are not equivalent.

What is effect of hybridization on bond length and bond strength?

Key Principle On Orbital Hybridization And Bond Strengths: The Greater The s-character, The Stronger The Bond. In other words, the more s-character on carbon, the stronger the bond.

Why is P-Cl bond not stable in PCl5?

Hence due to inter electronic repulsion the bond length increases and P-Cl bond is not stable. Because pcl5 has one smaller and one bigger bond angle of 90 and 120 so their bond length increase due to repulsion Please find below the solution to your problem.

Which pair of bonds is more polar P-Br and P-Cl?

Which pair of bonds is more polar: P-Br and P-Cl? The P – Cl bond is more polar. A polar bond is basically a bond where electrons are more drawn to one atom over the other atom. That one atom will have a greater electronegativity, which means that it has a greater tendency to hog electrons in a bond.

What is the hybridization geometry of PCl5?

In PCl5 , P is undergoing sp3d hybridization geometry of the molecule is trigonal bi pyramidal with bond angle 90° and 120° . Hence due to inter electronic repulsion the bond length increases and P-Cl bond is not stable.

What is the difference between PCl3 and PCl5?

However if its not, then consider the structures of these compounds according to the VSEPR theory. PCl3 has a trigonal pyramid structure whereas, PCl5 has a TBP (trigonal bipyramidal) structure. In TBP, the longitudinal and equatorial bond lengths differ. So PCl5 would obviously have two different types of bond lengths.