Node is a point where the electron probability is zero. For a given orbital there are two types of nodes. 1) Radial node 2) Angular node
Radial node is also called a nodal region. Radial node is a spherical surface where the probability of finding an electron is zero. The number of radial nodes increases with the principal quantum number (n).
Angular node is also called a nodal plane. It is a plane that passes through the nucleus. Angular node is equal to the azimuthal quantum number (l). The total number of nodes present in this orbital is equal to n-1. In this case, 3-1=2, so there are 2 total nodes. The quantum number ℓ determines the number of angular nodes; there is 1 angular node, specifically on the XY plane because this is a Pz orbital.