Hello,

None.

S Orbital have no nodal Planes Because,

There are no angular nodes in spherical orbitals

Any s orbital has an angular momentum quantum number l Of 0

It has spherical shell nodes known as radial nodes

They are lighter regions of orbital probability densities and where electrons cannot exist

The number of angular nodes are given by l

It can be

• Nodal planes
• In the case of dz^2 or fz^3 , conical nodes

Since l=0 for any s orbital, there are zero nodal planes in 4 s orbital

The ns orbital has (n-1) radial nodes, hence 4s Orbital has (4-1) = 3 radial nodes

Therefore, 4s orbital has no nodal Planes and has 3 nodes

Hope it helps