alkali metals (ia group) have small ionization energies, especially when compared to halogens or vii a group. in addition to the radius (distance between nucleus and the electrons in outermost orbital), the number of electrons between the nucleus and the electron(s) you're looking at in the outermost shell have an effect on the ionization energy as well. this effect, where the full positive charge of the nucleus is not felt by outer electrons due to the negative charges of inner electrons partially canceling out the positive charge, is called shielding. the more electrons shielding the outer electron shell from the nucleus, the less energy required to expel an electron from said atom. the higher the "shielding effect" the lower the ionization energy. it is because of the shielding effect that the ionization energy decreases from top to bottom within a group. from this trend, cesium is said to have the lowest ionization energy and fluorine is said to have the highest ionization energy (with the exception of helium and neon).