The number of radial and angular nodes in $$4d$$ orbital are, respectively

We need to find the number of radial and angular nodes in the $$4d$$ orbital.

For the $$4d$$ orbital: principal quantum number $$n = 4$$, azimuthal quantum number $$l = 2$$.

Number of angular nodes = $$l = 2$$

Number of radial nodes = $$n - l - 1 = 4 - 2 - 1 = 1$$

Total number of nodes = $$n - 1 = 3$$

Angular + Radial = $$2 + 1 = 3$$ ✓

The number of radial and angular nodes are $$1$$ and $$2$$, respectively.

The correct answer is Option A: $$1$$ & $$2$$.