Why is it that the atomic radius decreases as you move across a period?
Unfortunately, I'm aware that this question has been answered before on Yahoo answers, but I can't get rid of the logic that instead, the atomic radius should increase as you go along a period because of the accumulation of electrons. As you add more, and create the shells, should not the radius increase? Shouldn't it get bigger?
Additionally, why does ionization energy decrease from top to bottom of a group? Is it in relation to valence electrons/shells?
Unfortunately, I'm aware that this question has been answered before on Yahoo answers, but I can't get rid of the logic that instead, the atomic radius should increase as you go along a period because of the accumulation of electrons. As you add more, and create the shells, should not the radius increase? Shouldn't it get bigger?
Additionally, why does ionization energy decrease from top to bottom of a group? Is it in relation to valence electrons/shells?
-
For Atomic Radius: As you move across a period, the number of protons increases, so the nucleus is pulling harder on your valence electrons. While VALENCE electrons are increasing, the number of SHIELDING electrons is constant. So the valence electrons will get sucked in.
For IE: As you move down a group, the valence electrons are getting farther and farther away from the positive nucleus. So when a valence electron is a lot farther away from the positive nucleus, it's a lot easier to take one away. So the IE will be lower for bigger atoms.
For IE: As you move down a group, the valence electrons are getting farther and farther away from the positive nucleus. So when a valence electron is a lot farther away from the positive nucleus, it's a lot easier to take one away. So the IE will be lower for bigger atoms.