In a hydrogen like species,an electron jumps from an orbital having two radial and two angular nodes to the orbital, having same sign of wave function in all direction,at any distance and having zero radial node.
If the energy of emitted photon is `326.4eV` ,the atom or ion is

The orbital having two radial as well as two angular nodes is

Orbital having 2 radial, 2 angular nodes

An electron jumps to higher excited state of a orbital which is non directional and have 4 radial node then shell with which electron belong?

" (A) Principal quantum number of orbital having non-planar angular node and "2" radial nodes may be "5

A hydrogen like species is in a spherical symmetrical orbital S_(1) having 3 radial nodes. It gets de-excited to another level S_(2) having no radial node. Energy of S_(2) orbital is 2.25 times energy of 1st Bohr robit of hydrogen atom. Identify the species involvedgt

A hydrogen like species is in a spherical symmetrical orbital S_(1) having 3 radial nodes. It gets de-excited to another level S_(2) having no radial node. Energy of S_(2) orbital is 2.25 times energy of 1st Bohr robit of hydrogen atom. ltbr. What is the combined total number of nodes ("radial" +"angular) is" S_(1) and S_(2)?