The number of radial nodes for a 3p orbital is 1.

Explanation:
Radial nodes are regions where the probability of finding an electron is zero. These nodes occur as a result of the wave-like nature of electrons in an atom. In the case of a 3p orbital, the principal quantum number (n) is 3, and the azimuthal quantum number (l) is 1.

1. Understanding the quantum numbers:
- Principal quantum number (n): It determines the energy level or shell of the electron. In this case, n = 3, indicating the third energy level.
- Azimuthal quantum number (l): It determines the shape of the orbital. For p orbitals, l = 1, representing a dumbbell-shaped orbital with two lobes.

2. Determining the number of radial nodes:
The total number of radial nodes (nr) can be calculated using the formula: nr = n - l - 1.

In this case, nr = 3 - 1 - 1 = 1. Therefore, the number of radial nodes for a 3p orbital is 1.

3. Visualization:
To visualize this, imagine the 3p orbital as a dumbbell-shaped region in space, with one radial node in the middle. The electron has a higher probability of being found in the lobes of the orbital and zero probability in the node.

In conclusion, the number of radial nodes for a 3p orbital is 1.