One of the major requirement in atomic structure is determination of location of electron inside an atom. The wave mechanical model establishes this in accordance with Heisenberg's uncertainty principle through the concept of orbitals. The orbitals are defined as that '3D' space in which probability of finding electron is maximum and are represented by wave functions `Psi_(n,l,m)` where n,l and m are quantum number. The variation of `Psi` is analysed in terms of polar coordinates and hence `Psi = f( r, 0 , phi)` where 'r' represents radius vector and 0 and `phi` represents angle `(/_)` Which the radius vector with x-axis respectively. The expressions of `Psi_(r,0, phi)` are often given in terms of `sigma` instead of r where `sigma=(2Zr)/(nalpha_(0))` and Z = atomic number and n= shell number.
If an orbital is represented as:
`Psi_(r,0,phi)=2/3((1)/(3alpha_(0)))^(3//2).(sigma-1)(sigma^(2)-8sigma+12) .sigma^(-sigma//2).cos0`
belong to which orbital?

Options

A. `6d_(x^(2)-y^(2))`
B. `5p_(z)`
C. `5p_(y)`
D. `6d_(z)^(2)`

Answer

B

Explanation

l=1,n-l-1=3
`n=5 rArr 5 p_(z)`