AS chemistry help

it’s 3 because in the first two options, the outermost electron is in the s sub shell which means it’s closer to the nucleus and there’s a stronger attraction and therefore larger ionization energy is needed. now between 3, and 4 it’s its 3 because 4 has more electrons and therefore a stronger attraction and more energy is needed to remove that electron. this is my best guess, i’m not entirely sure.

it’s 3 because in the first two options, the outermost electron is in the s sub shell which means it’s closer to the nucleus and there’s a stronger attraction and therefore larger ionization energy is needed. now between 3, and 4 it’s its 3 because 4 has more electrons and therefore a stronger attraction and more energy is needed to remove that electron. this is my best guess, i’m not entirely sure.

also theres a greater shielding effect in 3 and 4

The difference between 3 and 4 is not accounted for by stronger attraction, attraction to what?

You would expect 4 to have more electron shielding than 3 but that does not account for the fact 3 has lower ionisation energy than 4. Its about completed electron shells.

not really since both 3 and 4 have the same number of shells so the shielding effect is the same. however, it is larger than in 1 and 2.

as the number of electrons increases, the number of protons (positive charge) increases as well making the attraction between the electrons and the positive charge stronger (again, im not sure so please correct me if im mistaken)

If you look at the actual first ionisation energy of 3 which is boron and 4 which is carbon, you will see why you are incorrect.

i’m award that boron has a lower ionization energy than carbon which is why my answer was 3, which is boron. however this is not due to the shielding the effect. it is due to other factors

The attraction between protons and electrons decrease rapidly with atomic number so the first ionisation energy of potassium is less than sodium. If you are right sodium would be more reactive than potassium but the reverse is true.

i’m award that boron has a lower ionization energy than carbon which is why my answer was 3, which is boron. however this is not due to the shielding the effect. it is due to other factors

That is incorrect. The reason why sodium has a higher ionization energy than potassium is the increased shielding effect (K has 4 principal shells, Na has 3)which overcomes the increased positive charge. Otherwise, the attraction between protons and electrons increases as the atomic number increases, which is why the ionization energy increases across a period.

What other factors?

The shielding between 3 and 4 is the same, why are the ionisation energies different?

the increased attraction between the positive charge and the electrons (due to the increased numbers of electrons present)

How would attraction between electrons and protons account for the high first ionisation energy of noble gases?