How many electrons in an atom can have each of the following quantum number or sublevel designations?

(a) n = 2, l = 1

(b) 3d

(c) 4s

Answer: a:6 electrons, b:10electrons, c: 2electrons

Explanation:

1. Principle quantum number (n)

n is the number of shell, it is a positive integer. The maximum number of electrons in a shell is 2 (n2)

2. Azimuthal quantum number (l)

l is the number of subshell in the principal shell

The name of subshell are s, p, d, f

The number of nodes in each subshell is

s is l=0, p is l=1, d is l=2, f is l=3.

Each shell can have 2 x l + 1 sublevels, and each sublevel can accommodate maximum of 2 electrons and have two electrons.

A. n=2, l=1 then 2 x 1 + 1 = 3 subshell, 3*2 = 6 electrons in the p subshell

b. 3d, d is l = 2 then 2 x 2 + 1 = 5 sublevels, 5*2=10 electrons in the d subshell

c. 4s, s is l=0 then 2 x 0 + 1 = 1 sublevel, 1*2=2 electrons in the s subshell.