Explanation:

Atomic orbitals are mathematical functions that describe the probability of finding an electron in a particular region around the nucleus of an atom. These functions are characterized by a set of quantum numbers, which include the principal quantum number (n), the azimuthal quantum number (l), and the magnetic quantum number (m).

Radial Nodes:

A radial node is a region in an atomic orbital where the probability of finding an electron is zero. It occurs when the radial wave function changes sign, which implies that the electron spends equal amounts of time on either side of the node. The number of radial nodes is equal to n - l - 1, where n is the principal quantum number and l is the azimuthal quantum number.

Angular Nodes:

An angular node is a plane that passes through the nucleus and divides the orbital into two lobes of opposite phase. It occurs when the angular wave function changes sign, which implies that the electron has zero probability of being found on the plane of the node. The number of angular nodes is equal to l.

Answer:

If an atomic orbital has 2 radial nodes and 1 angular node, it is a 4p orbital. This is because:

- The principal quantum number for a 4p orbital is 4.
- The azimuthal quantum number for a 4p orbital is 1, which corresponds to a single angular node.
- The number of radial nodes for a 4p orbital is 4 - 1 - 1 = 2.

Therefore, the only option in the given choices that satisfies these conditions is option D, which is a 4p orbital.