Question

How many nodes are in a $2\mathrm{p}$ orbital?

Answer 1

To determine the number of nodes in $2p$ orbitals:

• The region in which the probability of finding the electron is zero electrons is known as the node. There are two types of node: Angular node and Radial node.
• Radial nodes are the spherical surface with zero electron probability. It depends on upon the principle quantum number(n).
• The angular node is the plane that passes from the center of the nucleus. It is equal to the angular quantum number(l).
• The p orbitals form a dumbbell shape and nodes are present at the center of the nucleus.

Step 1: The number of nodes can be calculated by $\mathrm{n}-\mathrm{l}-1$where, $\mathrm{n}=$principal quantum number, $\mathrm{l}=$azimuthal quantum number

Step 2: For $2\mathrm{p}$, $\mathrm{n}=2$

Number of radial node $$\begin{gathered} =\mathrm{n}-\mathrm{l}-1 \\ =2-1-1 \\ =0 \end{gathered}$$

Number of angular node $$\begin{gathered} =\mathrm{l} \\ =1 \end{gathered}$$

Hence, $2\mathrm{p}$ orbitals contain zero radial node and one angular node.