Chapter 5, Problem 111CP

Interpretation Introduction

Interpretation: The term energy level, a sublevel and an orbital should be explained.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

1. All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
2. The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
3. The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
4. The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of $l=0$ , for p orbital it is $l=1$ , for d orbital it is $l=2$ and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.