Explain $2p$ orbitals.

If $n=2$ and $l=1$,then it is a $2p$ orbital. The number of orbitals is given by $2l+1 = 2(1)+1 = 3$.
These three $2p$ orbitals have magnetic quantum numbers $(m_l): +1, 0, -1$. These values can be assigned to any orbital,and $p_x$ can be given any of these values.
Based on their orientation along the axes,these orbitals are known as $2p_x, 2p_y, 2p_z$.
The number of radial nodes in $2p$ orbitals is zero as per the formula $(n-l-1) = (2-1-1) = 0$. However,the number of angular nodes (nodal planes) is one. At the nodal plane where the two lobes meet,the electron density is zero.