Across the periodic table, there are predictable variations in the initial ionization energy. The ionization energy grows from left to right during the course of a period and drops from top to bottom in groups. As a result, helium has the highest initial ionization energy while francium has one of the lowest.
<h3>What do you understand by ionization energy?</h3>
The least amount of energy needed to free the most loosely bound electron from an isolated gaseous atom, positive ion, or molecule is known as the "ionization energy". the first ionization energy is
"X(g) + energy" →X(g) + e−
Where X is any atom or compound, X+ is the ion formed when the original atom loses one electron, e- is the lost electron, and X is the starting atom or compound.
The process of ionization is endothermic because the ionization energy is positive for neutral atoms. The ionization energy of an atom is roughly proportional to how far its outermost electrons are from its nucleus.
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