I'm a high school student and I'm learning about ionization energy and atomic radius of elements. I want to compare the ionization energy of lithium and magnesium.
Here is the information provided in my textbook:
In periodic table, the atomic radius of elements gradually decreases from left to right of a period and increases from up to down of a group.
If the atomic radius of an element is greater than the atomic radius of another element, then the ionization energy of the first element is less than the ionization energy of the second element.
So according to my book, magnesium has a greater atomic radius than lithium which means magnesium has less ionization energy than lithium. But when I checked on the internet, the result was completely opposite. Is there an explanation for this exceptionality?
Please share an explanation that is suitable for a high school student.