Question 1 Report
Which of the following statements is correct about ionization energy? It
The correct statement about ionization energy is that it decreases down the group. Ionization energy is defined as the energy required to remove an electron from an atom or a positive ion in the gaseous state. The ionization energy of an atom depends on the nuclear charge, the distance between the nucleus and the outermost electron, and the shielding effect of inner electrons. As we move down a group in the periodic table, the number of electron shells increases, and the shielding effect of inner electrons also increases. This means that the outermost electrons are held less tightly by the nucleus and are easier to remove. Therefore, the ionization energy decreases down the group. Conversely, as we move across a period, the number of electron shells remains the same, but the nuclear charge increases. This means that the outermost electrons are held more tightly by the nucleus and require more energy to remove. Therefore, the ionization energy increases across the period. The other options in the question are incorrect. Ionization energy does not result in the formation of an anion, nor does it cause metallic nuclei to disintegrate.