Which of the following quantum number combinations is not allowed in an atom? n = 2, l = 1, m subscript l = 0 n = 1, l = 0, m subscript l = 0 n = 4, l = 3, m subscript l = -3 n = 2, l = 3, m subscript l = 2

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Which of the following quantum number combinations is not allowed in an atom? n = 2, l = 1, m subscript l = 0 n = 1, l = 0, m subscript l = 0 n = 4, l = 3, m subscript l = -3 n = 2, l = 3, m subscript l = 2

Chemistry
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n = 2 is the energy level principle quantum number; l = 1 means that this is the shape and mL is 0, if L = 1 then mL can be from positive 1 to negative 1 so mL can take on -1,0,1 this is a p orbital sot his is possible. n = 1, l = 0 mL = 0. I believe that this is an s orbital which has one orientation. so this is correct. n = 4, l = 3, mL = -3. let's see if l = 3 mL can be -3,-2-,-1,0,1,2,3 I believe this is possible n =2, L =3, mL = 2 if L is 3 that means mL can be -3,-2,-1,0,1,2,3 but this is the configuration for an f orbital. how do we know? because if l =3 there are 7 possible orbitals, which each can hold 2 electrons to give us a total of 14 electrons. n the principle quantum number is too low, given that an f orbital starts at n = 4, I would say this is wrong.

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