Given a set of quantum numbers, determine whether each is permitted for an orbital in an atom (a) n = -2, 1 = 0, m, = 0 %3D possible impossible (b) n = 2, 1 = 1, m = -1 O possible impossible (c) n = 3,1 = -2, m, = 0 possible O impossible
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Here, we have to first know that each electron in an atom is described by a set of different quantum numbers. n, l, ml specify the particular orbital of interest in the atom.
1. Principal Quantum Number (n): n = 1, 2, 3, …
It specifies the energy of an electron and the size of the orbital and also the distance from the nucleus of the atom denoting as shells.
2. Angular Momentum (Secondary, Azimunthal) Quantum Number (l): l = 0 ... n-1.
Specifies the shape of an orbital, it divides the shells into smaller groups of orbitals called subshells (sublevels).
3. Magnetic Quantum Number (ml): ml = -l... 0 ... +l.
Specifies the orientation of an orbital with respect to the energy (n) and shape (l)and thus dividing the subshell into individual orbitals which hold the electrons; there are 2l+1 orbitals in each subshell.
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