Chapter U1.24, Problem 4E

Interpretation Introduction

Interpretation:

The number of subshells in the given shell needs to be determined.

Concept introduction:

Electrons revolve around the nucleus in orbits. These orbits are called shells. The shells are numbered as n = 1, 2, 3, 4…. Number of shells in an atom is the same as the number of period where the atom is located on the periodic table. Each shell is divided into further layers called subshells. Each subshell is a collection of orbitals. Subshells are denoted by using the shell number and the subshell letter; 1s, 2p, 3d, etc.

Explanation of Solution

The maximum number of subshells is equal to the shell number. For example - When n = 1(first shell), only one subshell is possible (only 1s sub shell).

Thus,

When n=2 (second shell), two sub shells are possible (2s, 2p).

When n=3 (third shell), three sub shells are possible (3s, 3p, 3d).

When n=4 (fourth shell), four sub shells are possible (4s, 4p, 4d, 4f).

There are four different types of sub shells. These various sub shells can be represented as s, p, d, f. The s sub shell is the lowest energy sub shell and the highest energy sub shell is f-sub shell.