10 posts • Page 1 of 1
As there are more valence electrons (aka from left to right on the periodic table), the attraction between the valence electrons and the nucleus grows stronger, so the electrons gravitate closer, making the radius smaller
Within a period or family of elements, all electrons are added to the same shell. At the same time, protons are being added to the nucleus, making it more positively charged, which further indicates greater nuclear attraction. This means that the nucleus attracts the electrons more strongly, pulling the atom's shell closer to the nucleus. The valence electrons are held closer towards the nucleus of the atom, which decreases the atomic radius.
This has to do with the number of valence electrons along with the increasing number of protons in the nucleus as you go from left to right across the periodic table. This trend causes the protons to have a greater pull over the electrons, thus leading to a smaller atomic radius.
Atomic radii is one of the periodic trends. Atomic radius decreases as you move to the right of the period table because electrons are being added to the same shell but also protons are added to the nucleus. This would mean it makes it more positively charged and therefore greater nuclear attraction. Thus, the atom's shell is pulled closer to the nucleus and making the radius smaller.
I think it is important to stress theft that the electrons are being added to the same shell when moving from left to right, therefore the atomic radius does not increase too drastically. At the same time, there are more protons in the nucleus, pulling the electrons in closer, decreasing the atomic radius.
As you move right across a row in the periodic table, the positive charge of the nucleus becomes greater due to the increasing number of protons. This causes the nucleus to have a greater pull on the electrons, thereby decreasing the atomic radius. This is the effect of effective nuclear charge.
Who is online
Users browsing this forum: No registered users and 2 guests