| Author | Message | ||
     Andrew Username: 951129 Registered: 04-2003 |
Excuse me, I want to ask sth abt ionization energy... Here's the question Place the following ions or atom in the order of increasing ionization energy. (S+ , S , S-) My question is which approach should we use to determine the order of ionization energy? a. full/half filled subshell b. radius of the atom (the distance between the electron and the nucleus) c. the charge of the atom or ion thx much !!! | ||
| Inamoto5 Username: admin Registered: 04-2003 |
2nd ionization ethalpy must be higher than the 1st one......so S+>S....the problem is s-, how do u think? | ||
| Andrew Username: 951129 Registered: 04-2003 |
In my points of view, i think that the IE of S is lower than S-. Because after losing an electron, S will become S+ and thus obtain a more stable state (half filled sub shell). However, the answer stated that the IE of S- is lower than S. So i feel confused about that. | ||
| Inamoto5 Username: admin Registered: 04-2003 |
then 1st ionization enthalpy of S is 999.6 kJmol^-1 but the 1st electron affinity is about -200 kJmol^-1....so it means that the ionization enthalpy of S^1- is about +200 KJmol^-1......sometimes thinking quantitatively is more useful than qualitative one | ||
| Andrew Username: 951129 Registered: 04-2003 |
Why the IE of S- is lower than S? | ||
| Andrew Username: 951129 Registered: 04-2003 |
I still dun know the answer... | ||
| Inamoto5 Username: admin Registered: 04-2003 |
There are several ways to explain it qualitatively. One of the possible explanation is about the electrostatic attraction between the nucleus and the outmost shell (=o.m.s.) electrons. Which one is larger? o.m.s. electrons in S- or in S? (Hints: you should consider about the electronic repulsion of the electrons in the shell and also the ionic/atomic radius) |