Shells and subshells

Shells and subshells - (lowest energy state) of a...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Shells and subshells As usual, for historical reasons we have more than one way to characterize an electron state in an atom. We can do it using the 4 quantum numbers, or we can use the notion of shells and subshells. A shell consists of all those states with the same value of n, the principal quantum number. A subshell groups all the states within one shell with the same value of , the orbital quantum number. The subshells are usually referred to by letters, rather than by the corresponding value of the orbital quantum number. The letters s, p, d, f, g, and h stand for values of 0, 1, 2, 3, 4, and 5, respectively. Using these letters allows us to use a shorthand to denote how many electrons are in a subshell; this is useful for specifying the ground state
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: (lowest energy state) of a particular atom. The ground state configuration for oxygen, for instance, can be written as : This means that the lowest energy configuration of oxygen, with 8 electrons, is to have two electrons in the n=1 s-subshell, two in the n=2 s-subshell, and four in the n=2 p-subshell. Potassium (Z = 19) has an interesting ground state configuration: That's interesting because there is a d-subshell in the n = 3 shell, but instead of the last electron going into that subshell it goes into the s-subshell of the n=4 shell. It does this to minimize the energy: the 4s subshell is at a lower energy than the 3d subshell....
View Full Document

This note was uploaded on 11/22/2011 for the course PHY PHY2053 taught by Professor Davidjudd during the Fall '10 term at Broward College.

Ask a homework question - tutors are online