When you go down the periodic table what happens to the ionization energy and why?

Answer 1

As you go across a period, ionization energy tends to increase. The reason for this is that as you move across a period, the outer shell of the atom becomes more complete. Consequently, there is a larger "Z" effect (attraction between the valence electrons and the nucleus) which leads to an increased difficulty in removing electrons.

It is important to note that while this trend is generally valid, there are certain exceptions.

Answer 2

The first ionization energy decreases down a column (group) and increases across a row (period). The first ionization energy decreases when going down a group because with increasing period, the number of electron shells also increase, and therefore the electrons in the valence shells of larger elements are further away from the nucleus and experience more 'shielding' from electrons in inner shells. This means that the nucleus of larger elements would not be able to exert its full attraction force on its outer most electrons compared to smaller elements in the same group and these outer electrons can therefore leave the larger elements easier. The ionization energy increases when going across a period (from left to right) because the number of protons, and therefore the attraction force exerted by the nucleus, increases but the energy level of the valence shell is constant. Therefore elements on the right hand side is able to hold onto its electrons more tightly.

Answer 3

Ionization energy will increase as you go left to right across a row on the Periodic Table.

Answer 4

Ionization energy increases across the period table left to right, and increases bottom to top (down to up). The higher up and more right an element, the higher its ionization energy.

Answer 5

Moving from left to right, the ionization energy decreases.

Answer 6

The ionization energy increase from left to right.

Answer 7

it will decrease it will decrease

Answer 8

Both decreases down a group.