How many angular nodes are present in the 3s orbital?

The 3s orbital is characterized by its principal quantum number, which is 3. The number of angular nodes in an orbital is determined by the angular momentum quantum number, denoted as l. For s orbitals, the value of l is always 0, regardless of the principal quantum number. Since angular nodes are defined as regions in which the probability of finding an electron is zero and are related to the value of l, an s orbital having l = 0 means that it has no angular nodes.

In summary, the 3s orbital has 0 angular nodes because it is an s orbital, where the angular momentum quantum number l is always 0. Therefore, the correct answer reflects that there are no angular nodes present in the 3s orbital.