4 posts • Page 1 of 1
Electron shielding is just the concept that electrons closer to the nucleus act as a shield to those further from the nucleus, making the outermost electrons have less of a pull toward the positive nucleus because the magnetic pull is basically being blocked by the closer electrons.
Basically the electrons that are closer to the nucleus (in smaller sublevels s<p<d<f) are better at shielding. For example, electrons in the s orbital are better at shielding than the p orbital since they are closer to the nucleus and experience a greater nuclear charge in addition to the fact that the p electrons are repelled to the s electrons. The same goes for higher orbitals. In terms of quantum numbers, the lower ones are better at shielding because the n number corresponds to which energy level n=1,2,3.. and l number corresponds to whether it belongs to l= 0,1,2.. s, p, or d. The smaller the quantum numbers, the closer it is to the nucleus (generally speaking).
Electron shielding refers to the blocking of valence shell electron attraction by the nucleus due to the presence of inner-shell electrons. Penetration describes the proximity to which an electron can approach to the nucleus. The principal quantum number gives you an idea of how close the electron is to the nucleus (n=1 is closer than n=3). The closer an electron is to the nucleus, the greater its penetration.
Who is online
Users browsing this forum: No registered users and 2 guests