You are designing a new product that requires the use of a stable, nonreactive
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There are 7 values of ml are allowed for an electron in a 5f subshell namely: -3 -2, -1, 0, +1, +2, +3
<h3>Further explanation</h3>In an atom, there are energy levels in the shell and subshell.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
ml value: between -l to + l
ms value: +1/2 or -1/2
Determination of electron configurations based on principles:
- 1. Aufbau: Electrons occupy orbitals of the lowest energy level
- 2 Hund: electron fills orbitals with the same energy level
- 3. Pauli: there are no electrons that have 4 equal quantum numbers
So for 5f orbitals, the value of a possible quantum number is
n = 5;
l = 3 (f = 3);
m = -3 -2, -1, 0, +1, +2, +3;
s = + - 1/2
<h3>Learn more</h3>the locations and properties of two electrons
It's sublevel
a possible full set of quantum numbers
Keywords: orbitals, subshells, quantum numbers
