Group 1 because across group 1 to 8 nuclear force of attraction increases to a significant extent and as a result greater amount of energy is needed to remove an electron. More specifically Fr has the lowest IE and He has the highest
Group 1 aka Alkali metals have the lowest first ionization energy because its atoms only have 1 valence electron thus requires little energy input to donate the electron to have a complete outershell.
alkali metals have the lowest.
Group 1 elements
Group 1
Francium in group 1 has the lowest first ionization energy.
Beryllium is the group 3A element with the highest ionization energy.
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.
Francium in group 1 has the lowest first ionization energy.
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
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.
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.
All of the elements on the top half of the periodic table belong in upperionizationenergy because the trend is top to bottom. Top being lowest and getting bigger as it goes down.------------------------------------------------------* In a group: the ionization energy decrease from the lighter elements to heavier elements.* In a period: the ionization energy increase from the left elements to the elements of the right.* When the atomic radius decrease the ionization energy increase.
group 1
It takes more energy to knock off two electrons