Beryllium is the group 3A element with the highest ionization energy.
Boron, since ionization energy increases from bottom to top.
The element with the highest first ionization energy in group 14 is carbon.
Helium (He) has the highest first ionization energy. Ionization energy increase as you go across the periodic table from left to right
Beacause of electronic configuration (M.O.T)
In a group the ionization energy decrease when the atomic radius increase; in a period this relation is not generally valid.
the ionization energy is increased because of electronegativity when we move down the group the electronegativity is decrees who hold all electrons hardly to gather that's why the electrons loose easily and become an ion.
The element with the highest first ionization energy in group 14 is carbon.
It takes more energy to knock off two electrons
Helium (He) has the highest ionization energy, then Neon (Ne) Ionization energy increases as you go across a period from left to right. Ionization energy decreases as you go down a group. Therefore, elements in the upper right of the periodic table have the highest ionization energy.
the nobles gases are the greatest ionization group
Beryllium will have the highest. Down a group ionization energy decreases.
Ionization energy increases as you go across a period, but as you go down a group it decreases.
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.
Helium (He) has the highest first ionization energy. Ionization energy increase as you go across the periodic table from left to right
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.
Beacause of electronic configuration (M.O.T)
Alkali metals (group 1 elements) have one valence electron. Hence have one ionization energy Alkaline earth metals (group 2 elements) have two valence electron. Hence have two ionization energy
Sodium has the greatest ionization energy of the four elements listed from column 1 of a wide form periodic table. Among this group of metals that readily form cations, the largest always has the lowest ionization energy and the smallest has the most. This is generally ascribed to the fact that the valence shell electron is further from the nucleus in the largest element and nearest in the smallest element.