Chapter 6, Problem 80QP

Interpretation Introduction

Interpretation:

The total number of $p$ electrons in N $(z=7)$, $s$ electrons in Si $(z=14)$, and $3d$ electrons in S $(z=16)$ is to be determined.

Concept introduction:

An atom consists of a positivelycharged nucleus, which is surrounded by negativelycharged electrons. The electrons revolve around the nucleus in their orbitals (or shells). Each orbital has subshells.

The arrangement of electrons in the orbitals of an atom is called electronic configuration. It is written with the help of quantum numbers.

Every electron occupies orbitals in the increasing order of their energies.

Pauli Exclusion Principle states that no two electrons of the same atom can have the same quantum numbers.

Hund’s Rule states that when electrons occupy degenerate orbitals (i.e., orbitals having the same energies), they should occupy all the empty orbitals of the subshell before occupying the orbital with one electron.