The electron configuration for sodium ion Na⁺ : <u>(2) 2-8</u>
<h3>Further explanation
</h3>
In an atom there are levels of energy in the shell and sub shell
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-shells in the shell of an atom, namely s, p, d and f. The maximum number of electrons for each sub shell is
- s: 2 electrons
- p: 6 electrons
- d: 10 electrons and
- f: 14 electrons
Charging electrons in the sub shell uses the following sequence:
<em>1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.
</em>
Determination of electron configurations based on principles:
• 1. Aufbau: Electrons occupy orbitals of the lowest energy level
• 2 Hund: electrons fill orbitals with the same energy level
• 3. Pauli: no electrons have the same 4 quantum numbers
The alkali metal Na will release electrons to form Na + so that the electron configuration is stable as the noble gas element Ne
electron configuration Ne: [He] 2s² 2p⁶
Na electron configuration: [Ne] 3s¹
electron configuration Na + = [Ne] = [He] 2s² 2p⁶
The maximum number of electrons in the shell K, L, M, N
According to Bohr, the maximum number of electrons that can occupy each atomic shell can be calculated by the formula 2n²
- K shell (n = 1): 2.1² = 2 electrons
- L shell (n = 2): 2. 2² = 8 electrons
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M shell (n = 3): 2. 3² = 18 electrons
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N shell (n = 4): 2. 4² = 32 electrons
If we look at the configuration of the Na⁺ ion:
1s² 2s² 2p⁶ then
on the shell n=1 (1s) there are 2 electrons
on the shells n=2 (2s and 2p) there are 8 electrons
So that the configuration
Na⁺ = 2-8
<h3>Learn more
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