Write the full electron configuration of the Period 3 element with the following successive IEs (in kJ/mol):
IE₁ = 738
IE₂ = 1450
IE₃ = 7732
IE₄ = 10,539
IE₅ = 13,628

It is the amount of energy required to remove valance shell electron of an atom in gaseous phase. The more the electron is closer to the nucleus the more energy is required to remove the electron.

Trend:

Increases from left to right in period.

Decreases generally from top to bottom in group.

In our case the data is:

IE₁ = 738

IE₂ = 1450

IE₃ = 7732

IE₄ = 10,539

IE₅ = 13,628

This data matches the Ionization energies of Magnesium (Mg). Magnesium has 12 electrons with 2 electrons in valance shell. It has 12 Ionization energies.

Electronic Configuration of Magnesium (Mg): [tex]1s^22s^22p^63s^2[/tex]

adioabiola adioabiola · Answer 2 · 2021-12-03T15:09:38+01:00

adioabiola adioabiola

03-12-2021

The electron configuration of the Period 3 element with the given successive IEs is;

1s² 2s² 2p⁶ 3s²

The ionization energy data given is in synchrony with that of Magnesium, Mg.

In essence, the element in question is Magnesium, Mg.

The electronic configuration of Magnesium is therefore;

1s² 2s² 2p⁶ 3s².

Write the full electron configuration of the Period 3 element with the following successive IEs (in kJ/mol): IE₁ = 738 IE₂ = 1450 IE₃ = 7732 IE₄ = 10,539 IE₅ = 13,628

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Write the full electron configuration of the Period 3 element with the following successive IEs (in kJ/mol):
IE₁ = 738
IE₂ = 1450
IE₃ = 7732
IE₄ = 10,539
IE₅ = 13,628