Ionisation energy

What is the first ionisation energy

The energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

What is nuclear attraction affected by?

Atomic radius, nuclear charge, electron shielding

Atomic radius

The closer the electron is to the positively charged nucleus, the greater the force of attraction between the electron and nucleus. As atomic radios increases, nuclear attraction decreases.

Nuclear charge

The more protons an atom has, the greater the positive charge in the nucleus. A greater positive charge will result in a stronger attraction between the nucleus and electrons. So as nuclear charge increase, nuclear attraction increases

Electron shielding

Between the outermost electron shell and the nucleus, there could be other electron shells

Negative electrons in these shells block some of the attractive force between the nucleus and outermost electrons

Increase in electron shielding will result in a decrease of nuclear attraction

What is the conclusion statement for how nuclear attraction is affected

The means the increased atomic radius and sheiding must outweigh the increased nuclear charge

What is the difference in successive ionisation between S and P orbitals (group 2 vs group 3)

P orbitals at a higher energy than the s orbitals in the same shell. Electrons easier to remove from a p orbital than the corresponding s-orbital.

What is the difference with successive ionisation between group 5 and 6?

Outermost electrons both removed from p-orbitals. Electrons group 3,4,5 is an unpaired electron alone in its orbital. In group 6 now 4 elements alone in the p sub shell, so the outermost electron is paired. The two paired electrons repel each other, making it easier to remove one of the electrons