Ionization energies decrease moving down a group, because the shielding effect reduces the pull of the nucleus on valence electrons. Making them easier to remove.
1. The ionization energy decrease down in the group.2. The cause is that the distance between the nucleus and the electron shell increase and the needed energy to extract an electron decrease.
Ionization energies go down of course. This is because radii are becoming larger due to addition of electron levels. These farther from the nucleus electrons require less and less energy to liberate from the atom.
Fluorine. Ionization energies are a periodic trend and they generally increase as you go up and to the right in the periodic table.See the chart in the Web Links to the left for a complete chart of the ionization energies of all the elements.
It decreases when going down a group.
It decreases when going down a group.
It decreases when going down a group.
I suppose that this trend is normal.
First ionization energy has a trend similar to that of electronegativity.
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.
The trend for first ionization energy
Electronegativity and first ionization energy both increase as you move up the periodic table
Electronegativity and first ionization energy both increase going up the Periodic Table.