Question

1. A shell includes all orbitals with the same principal quantum number (n). In this figure the principal quantum numbers are designated along the bottom (n = 1, n = 2, etc.) and the orbitals contained within the shell are shown as individual, colored boxes. The first shell (n=1) contains only 1 orbital, represented by 1 yellow box. The second shell (n=2) contains a total of 4 orbitals, represented by 1 yellow box and 3 blue boxes. Use the figure to fill in the following chart, and then look for a pattern that will help you complete the entry for the 5th shell.

Shell number (Principal quantum number)	Total number of orbitals in shell	Number of different colored orbitals in shell
n=1	1	1
n=2	4	2
n=3
n=4
n=5

Answer 1

Answer – We are given the principal quantum numbers and the orbitals contained within the shell are shown as individual, colored boxes. For the same number of principal quantum numbers there are different suborbitals, so the number of color boxes = number of orbitals like s, p, d and f

The number of subcell for each principal quantum numbers is the total number of orbitals and there are suborbital. Example for n = 3 there are 3s, 3p and 3d orbital , s has 1subcell , p has 3 and d has 5 so total 1+3+5 = 8 and number of color boxes for s, p and d are 3

So the n is the principal quantum numbers and the following table filled -