Question

h has a higher ionization energy: chlorine (Cl) or magnesium (Mg)? Why? Select the best answer.(1 point) Responses Cl; it takes less energy to add an electron to a valence shell that is nearly full. Cl; it takes less energy to add an electron to a valence shell that is nearly full. Mg; it takes more energy to pull two electrons away from magnesium(Mg) than it does to take them from chlorine(Cl). Mg; it takes more energy to pull two electrons away from magnesium(Mg) than it does to take them from chlorine(Cl). Cl; it takes much more energy to pull an electron away from a valence shell that is nearly full. Cl; it takes much more energy to pull an electron away from a valence shell that is nearly full. Mg; magnesium has more valence electrons than chlorine. Mg; magnesium has more valence electrons than chlorine.

Answer 1

The correct answer is: Cl; it takes much more energy to pull an electron away from a valence shell that is nearly full.

Explanation:

Chlorine (Cl) has a higher ionization energy than magnesium (Mg) because it is close to having a complete outer shell with 7 valence electrons. Removing an electron from chlorine, which would result in a less stable electronic configuration, requires significantly more energy compared to removing electrons from magnesium, which has 2 valence electrons and can lose them more easily to achieve a stable noble gas configuration. In general, nonmetals like chlorine have higher ionization energies than metals like magnesium due to their more stable electron configurations when they have a nearly full outer shell.