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The more electrons protect the outer electron shell from the nucleus, the less energy is required to extract the electron from the specified atom. The higher the protective effect, the lower the ionization energy. It is because of the screening effect that the ionization energy decreases from the top down inside the group. In general, the first ionization energy increases as we go from left to right through a series of periodic table. The first ionization energy decreases when we descend on the column of the periodic table. In the group of elements B, with an increase in the atomic mass of the element (with increasing radius), a decrease in the first ionization energy is observed. If we compare the elements B and the elements A in the group, then the elements of B will have a larger radius, hence the value of the ionization energy will be less than the cell in the elements A.