Chapter 6, Problem 71QP

Interpretation Introduction

Interpretation:

Among the pairs of hydrogen orbitals, the orbital higher in energy is to be identified.

Concept introduction:

The lower energy orbitals are filled before the higher energy orbitals.

Electrons first enter the orbitalthat contains lower energy.

In equal energy orbitals, electrons first enter in an orbital with parallel spins.

The energies of orbitals in hydrogen atom, or any other one-electron ion, depend on the value of principal quantum number $(n)$.

Energy increases as $n$ increases. Hence orbital in the same shell have the same energy regardless of their subshell.

In a hydrogen atom, if two orbitals have the same value of $n$ then they have equal energy.

In a hydrogen atom, the sequence of orbital energy levels is as follows:

$1s<2s=2p<3s=3p=3d<4s=4p=4d=4f$