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shedrick94
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If an atom described by spin-orbit coupling is in a 4P state, why is the spin quantum number s=3/2?
The exponent is 2S+1, so for a quadruplet, 2S+1 = 4 means S=3/2.shedrick94 said:So the angular momentum quantum number is l=1 as it's a P state? How is the value of s determined?
It's a legacy from the earlier days of atomic physics. It follows the same nomenclature as orbitals: s, p, d, f, etc., but with uppercase letters (just as the total orbital angular momentum is L, instead of l for the orbital angular momentum of a single electron).shedrick94 said:Sorry I've never seen this notation before so I wasn't aware of the relationship. So why do we have L=P then?
The spin quantum number, denoted as "s", represents the intrinsic angular momentum of an electron within an atom. It determines the direction of the electron's spin and is an important factor in understanding an atom's electronic structure.
The spin quantum number can have only two possible values: +1/2 or -1/2. These values correspond to the two possible spin orientations of an electron, either "spin up" or "spin down".
The Pauli exclusion principle states that no two electrons within an atom can have the same set of quantum numbers. This means that electrons in the same energy level must have different spin quantum numbers, ensuring that each electron has a unique set of quantum numbers.
No, the spin quantum number can vary for different electrons within the same atom. This is because electrons in different energy levels and orbitals have different sets of quantum numbers, including the spin quantum number.
The spin quantum number determines the magnetic moment of an electron, which in turn contributes to an atom's overall magnetic properties. Atoms with unpaired electrons, each with a spin quantum number of +1/2 or -1/2, will have a net magnetic moment and exhibit magnetic behavior.