The boundary surface diagrams for the orbitals, should be drawn using the shape of orbitals.
All p orbitals are dumb-bell shape. The three p orbitals () are identical in size, shape and energy; they differ from one another only in orientation. An electron described by one of these wave functions will not be found at the nucleus. There is a nodal plane running through the nucleus between the two lobes. For example in orbital, ‘ ’ is the nodal plane.
There are 5d-orbitals. All d orbitals () are identical in energy. They are labelled with subscripts denoting their orientation with respect to the axes and to the planes defined by them. orbitals have four lobes and these lobes lie symmetrically between the coordinate axes. For example, the lobes of orbital lie symmetrically in between axes. orbital also has four lobes along axes. orbital has a unique shape with two lobes along -axis and a ‘belt’ like space centred in the ‘ ’ plane. Each d orbital has two nodal planes.