# What is wrong with the following quantum notation numbers? 2, 3, 1, -1/2 4, 1, 3, 1/2 1, 1, 1, -1/2

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### 1 Answer

The quantum numbers identify the location of an electron in one of the orbitals. The principal quantum number (n) has allowed values of integers of 1 or greater (i.e. 1, 2, 3). This number determines the shell of the electron.

The angular momentum quantum number (l) has values of 0 through n-1 and determines the type of orbital (i.e. s, p, d, or f)

The magnetic quantum number has possible values of -l to +l including zero (where l is the angular momentum quantum number). This identifies the specific orbital (i.e. px, py, or pz).

The magnetic spin quantum number determines whether an electron is "spin up" or "spin down". It has possible values of +1/2 or -1/2.

2, 3, 1, -1/2 The value of the angular momentum number is too large. It has a maximum value of 1 for n=2.

4, 1, 3, 1/2 The value of the magnetic quantum number is too large (-l to +1) so it must be -1, 0, +1.

1, 1, 1, -1/2 The value of the angular momentum quantum number is too large. For n=1, the maximum value is 0. The magnetic quantum number would only have a possible value of 0.