Ionization energy

Ionization Energy is the amount of energy required to remove an electron from a neutral atom in its gaseous phase. Conceptually, ionization energy is considered the opposite of electronegativity. The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikely the atom becomes a cation. Generally, elements on the right side of the periodic table have a higher ionization energy because their valence shell is nearly filled. Elements on the left side of the periodic table have low ionization energies because of their willingness to lose electrons and become cations. Thus, ionization energy increases from left to right on the periodic table

❤️The ionization energy of the elements within a period generally increases from left to right. This is due to valence shell stability.
❤️The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding.
❤️The noble gases possess very high ionization energies because of their full valence shell as indicated in the graph. 📌Note that Helium has the highest ionization energy of all the elements.