The number of angular and radial nodes for 4d orbital is respectively
[amp_mcq option1=”2 and 1″ option2=”1 and 2″ option3=”3 and 1″ option4=”4 and 0″ correct=”option1″]
This question was previously asked in
UPSC CAPF – 2018
– The number of angular nodes is equal to *l*.
– The total number of nodes is equal to *n* – 1.
– The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* – 1) – *l*.
For a 4d orbital:
– Principal quantum number *n* = 4.
– For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3).
– Number of angular nodes = *l* = 2.
– Number of radial nodes = (*n* – 1) – *l* = (4 – 1) – 2 = 3 – 2 = 1.
The question asks for the number of angular and radial nodes *respectively*.