In PCl5, the central metal atom, P is in +5 oxidation state, while in PCl3, it is in +3 oxidation state. Therefore, PCl5 is more covalent than PCl5.

Atoms will often join together to form bonds because a negative force is attracted to a positive bond. Ionic bond forms oppositely charged ions. Covalent bond forms from shared electrons. You just studied 5 terms!

Atoms mainly combine to fill the outermost shell and they can combine with similar elements or different elements. Sometimes, they can achieve stability even after half-filled subshell.

Bonds form when atoms share or transfer valence electrons. Valence electrons are the electrons in the outer energy level of an atom that may be involved in chemical interactions. Valence electrons are the basis of all chemical bonds.

Bonds are formed when valence electrons, the electrons in the outermost electronic “shell” of an atom, interact. The nature of the interaction between the atoms depends on their relative electronegativity.

Answer. PCl5 is a non-polar covalent molecule because individual dipole moments of P-Cl bond cancel out each other but PCl3 is a polar covalent molecule. Therefore, PCl5 is more covalent than PCl3.

why? According to Fajan’s rule, smaller the cation, higher will be the covalent nature of the bond. Hence, BiCl3 is less covalent than PCl3.

Answer Expert Verified 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).

In pcl5 the two axial bonds are longer than three equitorial bond (bond length of axial bond 240 pm) the axial bond pairs suffer more repulsion as compaired to equtorial bons . but in pcl3 three is no any axial bond . so pcl5 is more reactive than pcl3.

PCl5 forms five bonds by using the d-orbitals to “expand the octet” and have more places to put bonding pairs of electrons. NCl5 does not exist because there are no d-orbitals in the second energy level. Therefore there is no way to arrange five pairs of bonding electrons around a nitrogen atom.

PCl5 is unstable because phosphorus forms 5 bonds with cl atoms out of which the two axial bonds have more Bond length than three equatorial Bond length this result in repulsion and thereby making the axial bonds weak.

PCl5 is a crystalline solid. It exists as PCl4+ and PCl6- ions. The former has tetrahedral and the later has octahedral structure These structures do account for efficient packing in form of crystals,which is more favourable as the two specis are ionic. So PCl5 attains a solid state .

Answer. The pentachlorides of the elements above and below arsenic in group 15, phosphorus pentachloride and antimony pentachloride are much more stable and the instability of AsCl5 appears anomalous.

Phosphorus penta chloride is one of the important compounds of phosphorus and chlorine. Preparation: Phosphorus Penta chloride is prepared by passing an excess of dry chlorine into liquid trichloride. Chlorine reacts with phosphorus trichloride and solid phosphorus penta chloride is formed.

Phosphorus pentachloride is a Lewis acid.