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There is no relation ship. They have the lowest ionization energies.
Noble gases
Ionisation energy determines the ability to loose electron. It tells the amount of energy changes in the process.
This quantities have the same magnitude but opposite sign.
It tends to become negative ions, it has a high electronegativity and ionization energy. Also, it gains electrons.
In the alkali metals column (Group 1), atomic radius increases down the group and reactivity increases. There are more shells preventing the attraction between the positive nucleus and negatively charged outer electron. (All Group 1 elements have 1 electron in their outer shell). Also, because they contain more shells down the group, the distance between the nucleus and electrons is increased. Therefore the electrostatic force is lessened between them. Both of these allow the outer electron to be lost easier to other elements, thus increasing reactivity.
Barium has more energy levels. So it has lesser ionization energy.
The relationship between atomic numbers and first ionization energies is that within the same period, as atomic number increases so does first ionization because as nuclear charge increases and atomic radius decreases, electrons become harder to remove. However, within the same group, the first ionization energy decreases as atomic number increases because of the added energy level, the electrons are farther from the nucleus and easier to remove.
ionization potential energy. but remember the atom must be neutral .
Helium (He) has the highest ionization energy.
No fire is not an ionization energy
ionization energy