Very helpful! Thanks! I learned that atoms on the left side of the periodic table have low ionization energy, and that atoms on the right side have high electron affinity. These properties allow ionic bonds to form between them, as atoms on the right are eager to accept electrons from atoms on the left.
I have a question. You explained electron affinity as the energy released when Be+ gains one electron to be a neutral Be. I think it is equal to ionization energy. I think it is the energy released when NEUTRAL Be gains an electron. right?
Good video. Would be better if it included electronic configuration considerations, such as energy change between 2p3 versus 2p2 and 2p4 and how it fits within the general trend.
why does flourine have less electron affinity than chlorine? i thought electron affinity increases as you go up the group because atomic radii decreases, thus less shielding and more acceptation of electrons
Energy was used from the system of atom. Basically atom or in his scenario cation did work on electron which is outside the system by pulling it to it's orbital. So this work done is the energy called electron affinity.
Yes, that is correct as far as I can understand.The configuration of Fluorine is 1s2 2s2 2p5 and thus it strives to get one more electron in order to complete it's outermost shell.
