Question

An atomic orbital has a total of 4 nodes in which two are radial nodes. The orbital is:

• A. $6p$
• B. $6s$
• C. $5p$
• D. $5d$

Answer 1

The correct option is D $5d$

Number of radial nodes = $n-l-1$
where, $n$ is the Principal quantum number and $l$ is the Azimuthal quantum number.
Total number of nodes = $n-1$
So, $n-1$ = 4 i.e., $n=5$
and $5-l-1=2$ i.e., $5-l-1$ = 2
On solving, $l=2$ which is $d$ - subshell
The atomic orbital is $5d$.