The orbital filled by the last electron from the S element is 3p
<h3>Further explanation </h3>In an atom there are levels of energy in the skin and sub skin.
This energy level is expressed in the form of electron configurations.
Writing electron configurations starts from the lowest to the highest sub-shell energy level. There are 4 sub skins in the skin of an atom, namely s, p, d and f. The maximum number of electrons for each sub skin is
• s: 2 electrons
• p: 6 electrons
• d: 10 electrons and
• f: 14 electrons
Charging electrons in the sub skin uses the following sequence:
<em>1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc. </em>
Each sub-skin also has an orbital depicted in the form of a square 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
An sulfur atom (S) has 16 electrons means having an electron configuration as follows:
1s², 2s², 2p⁶, 3s², 3p⁴
or we can write with the noble gas symbol
[Ne] 3s² 3p⁴
From this configuration, it has been seen that the last electron (16th electron) occupies a 3p orbital (3p⁴) orbital with a downward symbol
The quantum number:
n = 3
l = 1
ml = -1
ms = -1/2
<h3>Learn more </h3>
electron transitions
the locations and properties of two electrons
It's sublevel
a possible full set of quantum numbers
Keywords: orbitals, subshells, quantum numbers
