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No, because is n=1, the electron is in the first energy level, therefore cannot have a l=2, because l= n-1. Or more simply put l=2 is a d-orbital, and there are no d-orbitals in the first energy level. ml=0 is correct because ml= +-l through 0.

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Q: Is the set of quantum numbers of n equals 2 l equals 2 ml equals 0 allowed?
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Related questions

Which set of quantum numbers cannot occur together to specify an orbital?

The set of quantum numbers n=1, l=2, ml=0 cannot occur together to specify an orbital. This is because the quantum number l (azimuthal quantum number) ranges from 0 to n-1, meaning l cannot be greater than or equal to n.


Can two electron have the same set of quantum number?

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The set of quantum numbers for nitrogen can be written as follows: n=2, l=1, ml=0, ms= +1/2 or -1/2. This corresponds to the second energy level, p orbital, zero magnetic quantum number, and either spin up or down.


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The highest energy electron in Zirconium (Zr) corresponds to the 4th energy level (n=4) with an angular momentum quantum number of l=3 (d-orbital), a magnetic quantum number ml ranging from -3 to 3, and a spin quantum number of ms=+1/2. This set of quantum numbers specifies the 4d subshell in which the electron resides.


What are allowable sets of quantum numbers?

The allowable sets of quantum numbers are n (principal quantum number), l (azimuthal quantum number), ml (magnetic quantum number), and ms (spin quantum number). n determines the energy level and size of an orbital, l determines the shape of an orbital, ml determines the orientation of an orbital in space, and ms determines the spin of an electron in an orbital. Each set of quantum numbers must follow specific rules based on the principles of quantum mechanics.


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The Pauli exclusion principle, which states that no two electrons in an atom can have the same set of quantum numbers. This includes the spin quantum number, which can have values of +1/2 (up) or -1/2 (down). So, in the 1s orbital, the two electrons must have different spin quantum numbers to adhere to this principle.


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