A certain orbital has $$n = 4$$ and $$m_l = -3$$. The number of radial nodes in this orbital is ________. (Round off to the Nearest Integer).

We are given $$n = 4$$ and $$m_l = -3$$. Since the magnetic quantum number $$m_l$$ ranges from $$-l$$ to $$+l$$, having $$m_l = -3$$ requires $$l \geq 3$$. For $$n = 4$$, the allowed values of $$l$$ are 0, 1, 2, and 3, so the minimum (and only possible) value is $$l = 3$$. This corresponds to the 4f orbital.

The number of radial nodes is given by the formula $$n - l - 1$$. Substituting the values, we get $$4 - 3 - 1 = 0$$.

Therefore, the 4f orbital has 0 radial nodes.