Question

The orbital that has one radial node is:

• A. $2p$
• B. $3p$
• C. $4p$
• D. $5p$

Answer 1

The correct option is B $3p$

Number of radial nodes is given by $n-l-1$, where $n$ is the principal quantum number and $l$ is the azimuthal quantum number.

For $3p$ orbital, the value of $n$ and $l$ are $3$ and $1$ respectively.

Number of radial node(s) $=n-l-1=3-1-1=1$

So, for $3p$, number of radial nodes is $1$.

The number of radial nodes for $2p,4p$ and $5p$ are $0,2$ and $3$ respectively.