Question

What are the number of sublevels and electrons for the first four principal quantum numbers?

Answer 1

Hint: We have to know the arrangement of numbers used to portray the position and energy of the electron in a particle are called quantum numbers. There are four quantum numbers, to be specific, head, azimuthal, attractive, and turn quantum numbers. The upsides of the saved amounts of a quantum framework are given by quantum numbers.

Complete step by step answer:
We have to know the rules for calculating the number of sublevels and first four principal quantum numbers.
- We have to know the first quantum number, here, the quantity of the sub-level is one and the quantity of electrons is two.
- We have to know the second quantum number, here the quantity of sub-level is two and the quantity of electrons is eight.
- We have to know the third quantum number, here the quantity of sub-level is three and the quantity of electrons is eighteen.
- We have to know the fourth quantum number, here the quantity of sublevels is four and the quantity of electrons is thirty-two.
You can easily calculate it with this method,
Suppose, the principal quantum number is represented as $n$ , the Azimuthal or secondary quantum number is represented as $l$ , the magnetic quantum number is represented as $m$ , and the spin quantum number is represented as $s$ .
$n$ = which energy shell it is;
$l$ = number of sub-shells;
$m$ = number of orbitals as well as electrons.
Where,
$l = 0{\text{, n - 1 }}$
${\text{m = }} \pm {\text{1 = - 1,0, + 1}}$

Note: Suppose, in the case of principal quantum number is $2$.
$l = n - 1 = 2 - 1 = 1$
Where, two subshells are present. They are ${\text{0}}$ and $1$.
Then,
$m = 0$
One orbital subshell is present. That is $s$ . The quantity of electrons is two.
$m = 1$
Three orbitals of subshell are present. That is $p$ . The quantity of electrons is six. Because each orbital contains two electrons.