00:01
Problem 25 asks what you consider most when you compare ionic radius to the radius of the uncharged atom.
00:08
So figure 8 .8 can be very helpful here in showing you how ionic size changes across the periodic table.
00:18
So ionic size doesn't really mirror atomic radius perfectly.
00:23
Instead, what you have to do is consider how the number of electrons relates to the number of protons.
00:28
When an atom loses electrons, protons sort of outweigh the electrons, meaning that more positive central charge pulls in electrons more, resulting in a smaller radius.
00:43
So what i mean by that is if you consider this first column over here containing lithium, sodium, potassium, and rubidium, because these are on the far left -hand side of the periodic table, remember that these are most likely to lose electrons to become more like the noble gases.
01:06
So each of these atoms will lose one electron to become a positive ion.
01:11
What this means is that there's one fewer electron to balance out the positive charge of the nucleus here, meaning that each of the remaining electrons is sort of pulled in tighter, to the central nucleus.
01:33
So the radius becomes smaller...
