Ionisation energy of Mg??

Bit stuck on a question n wondering If someone can help pls:

explain why the second ionisation energy of magnesium is greater than the first ionisation energy of magnesium

thankyouu

In the positive ion, there are more protons than electrons. So the electrons are pulled in more strongly (by nucleus) to the positive charge. They are therefore more hard to remove so more energy is needed to remove that electron from an atom.
This is why successive ionisation energies increase. So the third ionisation energy would be greater than the second.

Hope this helps

The answer would be similar for every element.
The first ionisation energy is the energy required to remove an electron from a NEUTRAL atom.
The second ionisation energy is the energy to remove an electron from an ion with a POSITIVE charge. There is a stronger attraction between this electron and a positive ion than between the first electron and an uncharged atom.

The answer would be similar for every element.
The first ionisation energy is the energy required to remove an electron from a NEUTRAL atom.
The second ionisation energy is the energy to remove an electron from an ion with a POSITIVE charge. There is a stronger attraction between this electron and a positive ion than between the first electron and an uncharged atom.

Although this IS the accepted answer, it is not correct.

The stability of any electron is a function of the electrostatic attraction from the nucleus and the electrostatic repulsion from the other electrons.

Once an ion is formed there is less repulsion as there is 1 less electronand the electrostatic attraction from the nucleus remains the same (in the case of Mg and any other element in which we are dealing with the same energy level)

The net attraction is much greater than the repulsion, so more energy is required for ionisation.

Are you recommending that answer to a student doing their AS / A level exams?

No. As I explained the answer you wrote is the accepted answer.

But it is not correct.

No. As I explained the answer you wrote is the accepted answer.

But it is not correct.

Understood, and I'm not suggesting you're incorrect.

I humbly would say that this is a students chemistry forum, mostly high school students needing answers appropriate to their syllabus. Persuit of clarifying the very latest understanding and the model/ theories understood by academics to be closest to their observations could esily "muddy the waters" for the OP and other users.
I'm not trying to be argumentative nor to disagree with what you have said. It's perhaps not something for a forum serving mostly GCSE / A Level (and their equivalents) and some undergraduates.

Although this IS the accepted answer, it is not correct.

The stability of any electron is a function of the electrostatic attraction from the nucleus and the electrostatic repulsion from the other electrons.

Once an ion is formed there is less repulsion as there is 1 less electronand the electrostatic attraction from the nucleus remains the same (in the case of Mg and any other element in which we are dealing with the same energy level)

The net attraction is much greater than the repulsion, so more energy is required for ionisation.

Good students should be given good explanations.