The number of radial nodes in an orbital is given by the formula:

$$ \text{Number of radial nodes} = n - l - 1 $$

where $$n$$ is the principal quantum number, $$l$$ is the azimuthal quantum number also known as the angular momentum quantum number.

For a $$3p$$ orbital,

$$n = 3$$ (since it is the 3rd energy level),

$$l = 1$$ (since $$p$$ orbitals correspond to $$l = 1$$).

Let's use the formula to determine the number of radial nodes:

$$ \text{Number of radial nodes} = 3 - 1 - 1 = 1 $$

So, the correct answer is: Option C : 1