11. The set of orbitals associated with a particular value of are sometimes collectively called a " subshell ". 12. The + 6 state would be less stable due to the strong binding of the 7p 1 / 2 subshell . 13. A subshell is the set of states defined by a common azimuthal quantum number, !, within a shell. 14. The maximum number of electrons that can be placed in a subshell is given by 2 ( 2 ! + 1 ). 15. For many theoretical purposes, the valence electron configuration may be represented to reflect the 7p subshell split as 7p7p } }. 16. The electrons inside each subshell all have a magnetic quantum number; this describes the shape of the electron's orbit. 17. For this reason, orbitals with the same value of " n " are said to comprise a " subshell ". 18. Let's say we want to calculate transition dipole moments for an electron to transition from a 4d to a 2p subshell . 19. This is because the argon atoms have a larger antibonding interaction with the 7s 1 electron, forcing it into a different subshell . 20. For instance, one may speak of the subshell with n = 2 and \ ell = 0 as a'2s subshell '.
