Timeline for How are the hybrid orbitals of sulfur hexafluoride shaped?
Current License: CC BY-SA 3.0
9 events
| when toggle format | what | by | license | comment | |
|---|---|---|---|---|---|
| Apr 13, 2017 at 12:57 | history | edited | CommunityBot |
replaced http://chemistry.stackexchange.com/ with https://chemistry.stackexchange.com/
|
|
| Jul 15, 2016 at 8:28 | history | edited | bon | CC BY-SA 3.0 |
added 92 characters in body
|
| Jul 14, 2016 at 19:50 | comment | added | permeakra | @bon Apologies. This work dx.doi.org/10.1071/CH04113 suggests that there is some pi-interaction involved and it has to do with d-orbitals. | |
| Jul 14, 2016 at 19:26 | comment | added | bon | @permeakra No it says that they mostly participate in sigma bonding. Read the section on the fourth page about $d_{\sigma}$ and $d_{\pi}$ contributions. pubs.acs.org/doi/pdf/10.1021/ja00273a006 | |
| Jul 14, 2016 at 18:24 | comment | added | permeakra | @bon But the article points that sulphur d-orbitals are mostly participating in pi-bonding ! | |
| Jul 14, 2016 at 9:21 | history | edited | bon | CC BY-SA 3.0 |
added 597 characters in body
|
| Jul 14, 2016 at 9:11 | comment | added | bon | @StevenStewart-Gallus More or less. I read the paper provided by DavePhD and added some more detail in my answer. What do you mean by 'does it have empty spots in it'? | |
| Jul 13, 2016 at 20:52 | comment | added | Ms. Molly Stewart-Gallus | So, the sulfur atom is more like a +3 ion and has a valence electron configuration like: $[\ce{Ne}] \underset{(3s)^{0.97}(3p)^{1.82}(3d)^{0.24}}{[\uparrow \vert \uparrow \vert \uparrow ]}$? Is this set of hybridized orbitals completely symmetrical or does it have empty spots in it? | |
| Jul 13, 2016 at 19:57 | history | answered | bon | CC BY-SA 3.0 |