Answer Expert Verified PCl3 is more stable than PCl5 because PCl5 has more steric hindrance (triangular bipyramidal shape and sp3d2 hybridization) than PCl3 (triangular planar structure and sp3 hybridization).
Why is PCl5 more reactive than PCl3?
In pcl5, both axial bonds are longer than three equatorial bonds (bond length of axial bond 240 pm), axial bond pairs experience more repulsion than equatorial bonds. … so pcl5 is more responsive than pcl3 .
Why is PCl5 unstable?
PCl5 is unstable because phosphorus forms 5 bonds with cl atoms whose two axial bonds have longer bond lengths than three equatorial bond lengths, resulting in repulsion and thus weakening the axial bonds.
What is the difference between PCl3 and PCl5?
PCl3 is trigonal pyramidal with a lone pair of electrons on phosphorus. PCl5 is trigonal bipyramidal without a lone pair of electrons. However, PCl5 has 2 axial bonds and 3 equitorial bonds, the axial bonds are longer and weaker than the equitorial bonds because they are subject to more b.p.b.p repulsions than the equitorial bonds.
Which is the most covalent PCl3 or PCl5?
(i) The greater the positive oxidation state of the central metal atom, the greater its polarizing power and hence the greater the covalent character of the bond formed between the central metal atom and the other atoms. … Therefore, PCl5 is more covalent than PCl5.
Why is PCl5 asymmetric?
There is a theoretical reason (VSEPR) for PCl5 to be non-polar. The electron pairs in the five PCl bonds repel each other (while being attracted to the phosphorus nucleus). … For contrast, consider PCl3, which has a trigonal pyramidal geometry (with a lone pair of electrons on the phosphorus atom) according to VSEPR theory.
Why is PCl5 highly reactive?
⏩Answer: In PCl5, in addition to the equitorial ties that are in the same plane, there are axial ties that are subject to more repulsion and are longer than the other ties. Again these are weak bonds and therefore these bonds can break for these reasons PCl5 is very reactive.
Why is there PCl5 but no NCl5?
PCl5 forms five bonds using the dormitals to extend the octet and have more places to place bonding electron pairs. NCl5 does not exist because there are no dormitories on the second energy plane. So there is no way to arrange five bonding electron pairs around a nitrogen atom.
Why is PCl5 solid at room temperature?
Phosphorus(V) chloride (Phosphorus pentachloride), PCl 5 Solid phosphorus(V) chloride contains ions, which is why it is a solid at room temperature. Two PCl5 molecules are involved in the formation of the ions.
Why is bicl3 less covalent than PCl3?
Why? According to Fajans rule, the smaller the cation, the higher the covalency of the bond. … Therefore, BiCl3 is less covalent than PCl3.
Why is pentahalide more covalent than trihalides?
The oxidation state of +5 in the pentahalide is higher than that of +3 in the trihalides because of the higher positive oxidation state of the central atom in the pentahalide. These atoms have a greater polarizing power than the halogen atom attached to them. … Pentahalides are more covalent than trihalides.