Question

What are the nodal planes of ${\mathrm{dz}}^2$ orbital? How can we find nodal planes?

Answer 1

Nodal plane:

• A nodal plane is defined as the region where the possibility of finding an electron is nil/zero.
• The number of planes corresponds to $\text{'}\mathrm{l}\text{'}$.
• The nodal planes have two nodes which are given below:

1. Radial node
2. Angular node

The number of radial nodes can be calculated by using the formula: $\mathrm{n}-\mathrm{l}-1$, where n is the principal quantum number and l is the azimuthal quantum number.

The number of angular nodes can be calculated by knowing the value of $\text{'}\mathrm{l}\text{'}$.

Nodal planes of ${\mathrm{dz}}^2$ orbital:

• For d orbital, the value of azimuthal quantum number i.e. $\text{'}\mathrm{l}\text{'}$ is $2$. Thus the minimum value of principal quantum number n is $3$. The value for $\mathrm{l}$ cannot be greater than $\mathrm{n}-1$.
• Hence, ${\mathrm{dz}}^2$ orbital has no nodal plane.