When excited electron of phosphorus goes in d orbital from p orbital then particularly in which orbital of d (5 coz there are 5 suborbitals in d) that electron goes? And why?
http://wwwchem.uwimona.edu.jm/courses/selrules.html
When an excited electron of phosphorus transitions from the p orbital to the d orbital, it will occupy a specific suborbital within the d orbital. The d orbital has five suborbitals, labeled as dxy, dyz, dzx, dx2-y2, and dz2.
To determine which suborbital the electron will occupy, we can use the Aufbau principle and Hund's rule:
1. Aufbau principle: Electrons fill orbitals starting from the lowest energy level. In terms of the d orbitals, they fill in the order of increasing energy: 3dxy, 3dyz, 3dzx, 3dx2-y2, and 3dz2.
2. Hund's rule: Electrons will initially occupy each suborbital of the same energy with parallel spins before pairing up. This means that if there are multiple suborbitals available at the same energy level, the electron will occupy separate suborbitals with the same spin.
In the case of phosphorus, it has an atomic number of 15, which means there are 15 electrons distributed among the orbitals. The ground state electron configuration of phosphorus is 1s2 2s2 2p6 3s2 3p3.
Before the transition, the p orbital of phosphorus is partially filled with 3 electrons in the 3p suborbitals (3px, 3py, 3pz). When excited, one of these electrons can transition to the d orbital.
Since the electron is transitioning from a p orbital to a d orbital, it will occupy the lowest energy suborbital available in the d orbital, which is 3dxy. This is determined by the Aufbau principle, which dictates that electrons fill orbitals from lowest to highest energy.
Therefore, when a phosphorus electron transitions from the p orbital to the d orbital, it will occupy the 3dxy suborbital.