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