Timeline for Which elements can be diatomic?
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20 events
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| Jul 2 at 12:23 | answer | added | Oscar Lanzi | timeline score: 1 | |
| Jul 2 at 11:22 | comment | added | Ali Caglayan | @Harrychink at the time of writing this question the article in question did have such a claim. It has since been updated and mentions diatomic uranium but the bond structure is different. | |
| Jul 2 at 7:04 | comment | converted from answer | Harrychink | chemistry.stackexchange.com/a/140835/148420 Seems to suggest that the sodium, potassium ,caesium, and lithium are all monatomic gases The wiki page linked does not support your statement that uranium and chromium form sextuple bonds | |
| Apr 13, 2017 at 12:57 | history | edited | CommunityBot |
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| Jan 14, 2017 at 2:02 | comment | added | DHMO | I think sodium in the gas phase exists as a dimer, but I could be wrong. | |
| Jan 14, 2017 at 0:33 | history | edited | Melanie Shebel | CC BY-SA 3.0 |
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| Oct 27, 2015 at 17:38 | answer | added | DavePhD | timeline score: 5 | |
| Oct 25, 2015 at 1:48 | comment | added | MaxW | "Stable" is a somewhat nebulous property. In general a chemist would think of stable to mean that the molecule would survive some large ( how big is large??) number of intermolecular collisions. In the cold of deep space where collisions are infrequent I'm sure that any two atoms would form a "molecule." If you increased the partial pressure so that such "molecules" started colliding, then the list would be different. | |
| S Oct 12, 2015 at 3:03 | history | suggested | Melanie Shebel | CC BY-SA 3.0 |
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| Oct 12, 2015 at 1:26 | review | Suggested edits | |||
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| Jun 10, 2015 at 18:39 | history | tweeted | twitter.com/#!/StackChemistry/status/608705116640804864 | ||
| Jun 10, 2015 at 17:55 | comment | added | Mithoron | Depends what you call diatomic - if you count helium vdV dimer than two atoms of any element which will have occasion and time will get bound. | |
| Jun 10, 2015 at 16:28 | comment | added | permeakra | @bon Interesting, it shouldn't. Well, Palladium clasters shouldn't exist to, but they do. | |
| Jun 10, 2015 at 16:07 | history | edited | bon | CC BY-SA 3.0 |
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| Jun 10, 2015 at 16:03 | comment | added | bon | @permeakra Diberyllium exists: 'diberyllium molecule exists (and has been observed in the gas phase). It nevertheless still has a low dissociation energy of only $59~\mathrm{kJ~mol^{-1}}$.' Also see here. | |
| Jun 10, 2015 at 16:01 | comment | added | Ali Caglayan | @permeakra Look at the bottom of further notes for noble gases. | |
| Jun 10, 2015 at 16:00 | history | edited | Ali Caglayan | CC BY-SA 3.0 |
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| Jun 10, 2015 at 15:56 | comment | added | permeakra | Alkali-earth metals and noble gases definitely can't form stable diatomic molecules, Zn/Cd/Hg likely can't too. Homoatomic bonds for most heavy non-transition metals are very weak so detecting diatomic molecules is unlikely. | |
| Jun 10, 2015 at 15:46 | comment | added | Nicolau Saker Neto | I have a feeling almost every element can be found as a diatomic molecule in the right conditions (or at least present as a measurable mole fraction), though high temperatures and low pressures may be needed for many of them. In the majority of cases, any chemical bond will be more stable than no chemical bond. Plus there are some stranger cases, such as bound diatomic noble gas molecules, stable when encapsulated by a fullerene molecule. | |
| Jun 10, 2015 at 15:41 | history | asked | Ali Caglayan | CC BY-SA 3.0 |