What is the relationship between the electron configuration for an atom and the atomic radius of the atom?
2007-01-26 02:00:50 · 4 answers · asked by Robert d 1 in Science & Mathematics ➔ Chemistry
The more electron shells an atom has, like 1s, 2s, 2p, 3s, 3p, etc., the larger the atomic radius.
2007-01-26 02:23:05 · answer #1 · answered by JJ 7 · 0⤊ 0⤋
As the shell # increases (n), the atom will become larger, but as electrons are added to a subshell, the atom will become smaller.
n is the principal quantum # and relates to the row #s on the periodic table. As n gets larger, an entire new shell of electrons is added to the atom. It is kind of like adding a skin level to an onion. Now, as electrons are added to each subshell within the new shell, they are actually pulled closer and closer to the nucleus. This seems odd, but it is due to the fact that the nucleus is being populated with protons at the same time and the electrons which are in the same shell do not shield the pull of the nucleus very effectively. In your chemistry class, you will call this the Z effective. It is the effective atomic # that an electron sees. The inner shells are able to shield some of the pull of the protons.
2007-01-26 11:05:04 · answer #2 · answered by serf_tide 4 · 0⤊ 0⤋
More you have electrons , more the atom should be large since many shells are occupied. But it is not sufficient .
In a row of periodic table, the size of the atoms decrease fom the
left to the right. so alkaline elements have always a greater size tha halogens since the single electron on the valence shell is less attracted
2007-01-26 11:11:07 · answer #3 · answered by maussy 7 · 0⤊ 0⤋
is this Mr. Beiber's homework?
2007-01-28 12:52:55 · answer #4 · answered by Onyx M 1 · 0⤊ 1⤋