<h3>Further explanation
</h3>
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
- 9. 2,-2,-2,-1/2 : invalid
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
<h3>Learn more</h3>
electron transitions
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the locations and properties of two electrons
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It's sublevel
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a possible full set of quantum numbers
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Keywords: orbitals, subshells, quantum numbers