Moving down a group, the atomic radius increases because energy levels are being added with each period. So the outermost electrons are farther away from the positively charged nucleus, so the force of attraction between the nucleus and the outermost electrons is less. So it takes less energy to remove an electron.
The ionization energy decrease moving down in a group.
Beryllium is the group 3A element with the highest ionization energy.
As you go down the group (any group), ionization energy decreases. So in terms of ionization energy, for the alkali metals, Lithium > Sodium > Potassium > Rubidium > Caesium > Francium
the nobles gases are the greatest ionization group
Ionization energy decreases with the rise of atomic number in a group of periodic table.
From left to right on the periodic table, ionization energy increases. From top to bottom in a column (group) the ionization energy decreases.
The element with the highest first ionization energy in group 14 is carbon.
group 1
It takes more energy to knock off two electrons
Imagine that one electron has already been removed from an atom, the energy used to accomplish this is the 1st ionization energy. Now more energy is needed to remove a 2nd electron. That is the 2nd ionization energy.
As one proceeds down the group 7A elements, the first ionization energy decreases. this means that the outermost electron is more readily removed as we go down a group.
sodium because it's the first group and first group are the most