PCl5 is formed but NCl5 is not why?

Question

Answer

D orbital absent in Nitrogen

Answer

Nitrogen is a 2nd period element which has no vacant d-orbital whereas Phosphorus is the element of 3rd period which has vacant d-orbital. Hence Phosphorus can form bonds with 5 Chlorine atoms but Nitrogen can't.

Answer

IT IS DUE TO 'N' LIES IN SECOND PERIOD AND 'P' IN SECOND PERIOD HENCE 'N' DOESN'T HAVE VACANT d-ORBITAL
THEREFORE 'P' CAN FORM PCl5 BUT NCl5 DOESN'T FORM NCl5

Answer

Because nitrogen is much smaller than phosphorus. ... N cannot partake in d orbital-based hybridization. Second row elements don't have d orbitals. NCl5 would have sp3d hybridization (trigonal pyramid) which is possible beginning with 3rd Row elements and allows for the expanded octet of the central atom.

Answer

Introduction:
PCl5 (phosphorus pentachloride) is a compound that exists, while NCl5 (nitrogen pentachloride) does not. This difference in behavior can be attributed to several factors, including the electronic configuration and size of the atoms involved.

Electronic Configuration:
Phosphorus (P) has an electronic configuration of 1s2 2s2 2p6 3s2 3p3, while nitrogen (N) has an electronic configuration of 1s2 2s2 2p3. In the case of PCl5, phosphorus undergoes hybridization to form five sp3d orbitals, each of which can accommodate a chlorine (Cl) atom. This allows for the formation of five P-Cl bonds. In contrast, nitrogen lacks the available d-orbitals for hybridization that would be necessary to accommodate the five chlorine atoms in NCl5.

Size of the Atom:
Another important factor to consider is the size of the atom. Nitrogen is a smaller atom compared to phosphorus. The smaller size of nitrogen makes it difficult to accommodate five chlorine atoms around it due to the increased electron-electron repulsion. This repulsion destabilizes the molecule, making NCl5 highly reactive and prone to decomposition.

Stability and Reactivity:
The stability of a compound is also influenced by the strength of the bond formed between the atoms. In the case of PCl5, each chlorine atom forms a covalent bond with the phosphorus atom, resulting in a stable molecule. However, due to the electronic configuration and smaller size of nitrogen, the bonds formed between nitrogen and chlorine in NCl5 would be weaker. This weak bonding leads to increased reactivity and a higher tendency for NCl5 to decompose into more stable compounds.

Conclusion:
In summary, PCl5 can exist because phosphorus has the necessary electronic configuration and size to form stable bonds with five chlorine atoms. On the other hand, NCl5 does not exist due to the lack of available d-orbitals for hybridization in nitrogen and its smaller size, which makes it highly reactive and prone to decomposition.

Answer

Due to absence of d orbital and inert pair effect

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