Identify which sets of quantum numbers are valid for an electron. each set is ordered (n,ℓ,mℓ,ms).
3,2,0,1/2
2,2,-1, 1/2
4,3,-4,1/2
1,0,0,1/2
2,2,1,-1/2
3,2,1,1
0,1,1,-1/2
3,3,1,1/2
2,-2,-2,-1/2
3,2,2,1/2
4,2,1,1/2
2,1,-1,-1/2

In an atom, there are energy levels in the shell and sub shell.

This energy level is expressed in terms of electron configurations.

Writing the electron configuration starts from the lowest to the highest subshell's energy level. There are 4 sub-shells in an atom's shell, namely s, p, d, and f. The maximum number of electrons for each subshell is

s: 2 electrons

p: 6 electrons

d: 10 electrons and

f: 14 electrons

Electron filling in subshells using the following sequence:

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.

Each sub-shell also has orbitals drawn in the form of a square box in which there are electrons symbolized by half arrows.

Each orbital in an atom consists of 4 quantum numbers

n is the principal quantum number.

l is the angular momentum / azimuthal quantum number

ml, the magnetic quantum number

ms, the electron-spin quantum number

Value of n: positive integer

value of l: s = 0, p = 1, d = 2, f = 3 , ..(n-1)

ml value: between -l to + l

ms value: +1/2 or -1/2

n = 3

l = 2 = d

ms = -2,-1,0,1,2

ml = +1/2 or -1/2

n = 2

l = 2 >>>the maximum value is at n-1

n = 4

l = 3

ml = -3,-2,-1,0,1,2,3 >>> there is no -4

ms = +1/2 or -1/2

n = 1

l = 0

ml = 0

ms = +1/2 or -1/2

n = 2

l = 2 >>> l must be n-1

n = 3

l = 2

ms = -2,-1,0,1,2

ml = +1/2 or -1/2  >>>  there is no 1

n = 0 >>> there is no n = 0, it starts from 1

n = 3

l = 3 >>>the maximum value is at n-1

n = 2

l = -2 >>> no negative value for l

n = 3,

l = 2

ml = -2,-1,0,1,2

ms = +1/2 or -1/2

n = 4

l = 2

ml = -2,-1,0,1,2

ms = ms = +1/2 or -1/2

n = 2

l = 1

ml = -1,0,1

ms = +1/2 or -1/2

electron transitions

link

the locations and properties of two electrons

link

It's sublevel

link

a possible full set of quantum numbers

link

Keywords: orbitals, subshells, quantum numbers

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