Why does en decrease down a group?

So, as you move down a group on the periodic table, the electronegativity of an element decreases because the increased number of energy levels puts the outer electrons very far away from the pull of the nucleus.

Why does ionization energy generally decrease going down a group or family?

On the periodic table, first ionization energy generally decreases as you move down a group. This is because the outermost electron is, on average, farther from the nucleus, meaning it is held less tightly and requires less energy to remove.

Why does electron shielding increase?

Electrons in higher energy levels experience a greater shielding effect than electrons in lower energy levels. This is due to the fact that while they are attracted to the positively charged nucleus, they are repelled by the negatively charged electrons in lower energy levels. Remember that like charges will repel.

Does shielding increase or decrease energy?

The shielding effect is shown by the interior electron cloud (light blue) shielding the outer electron of interest from the full attractive force of the nucleus. A larger shielding effect results in a decrease in ionization energy.

Why does ionization energy decrease down Group 2?

Going down group 2: there are more filled shells between the nucleus and the outer electrons … therefore the force of attraction between the nucleus and outer electrons is reduced … so less energy is needed to remove an outer electron.

Why do ionization energies decrease from the top to the bottom of a group on the periodic table of elements?

The ionization energy of the elements within a period generally increases from left to right. This is due to valence shell stability. The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding.

Why does ionic radius decrease down a group?

As you move down a column or group, the ionic radius increases. Ionic radius decreases moving from left to right across a row or period. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly.

Does electron shielding increase going down the periodic table?

Shielding increases as you go down a group.