Timeline for Why do Cu⁺ ions spontaneously form copper metal and Cu²⁺ ions in solution?
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13 events
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| Jun 2, 2022 at 3:27 | history | edited | andselisk♦ | CC BY-SA 4.0 |
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| May 22, 2019 at 11:16 | answer | added | Mayuri Vaish | timeline score: 3 | |
| S May 21, 2019 at 12:36 | history | suggested | Ian Bush |
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| May 21, 2019 at 12:34 | review | Suggested edits | |||
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| May 21, 2019 at 12:09 | comment | added | Mayuri Vaish | @Poutnik I got it!!! Thank you!!! Essentially, both reactions involving Cu+ have the lowest and highest SEPs respectively - so they have to be the strongest oxidizing/reducing agents - thus undergoing disproportionation. :))) | |
| May 21, 2019 at 11:38 | comment | added | Poutnik | Take it as if Cu(I) had been 2 different compounds in one. One as oxidizing agent, the other as reduction agent. Compare potentials for their half reaction. | |
| May 21, 2019 at 11:23 | comment | added | Nilay Ghosh | Strongly related; chemistry.stackexchange.com/questions/42855/… | |
| May 21, 2019 at 11:13 | comment | added | Poutnik | as they are directly related to delta G via nF factor. | |
| May 21, 2019 at 11:04 | comment | added | Poutnik | Did you compare standard potentials of all 3 half reactions ? | |
| May 21, 2019 at 11:02 | comment | added | Mayuri Vaish | @Poutnik - thanks, yes I did. But that does not explain why in terms of the standard electrode potentials involved. I'm having a hard time understanding how you could infer that from the SEPs given. Do you have any idea? Thanks in advance.! | |
| May 21, 2019 at 10:56 | comment | added | Poutnik | See related chemistry.stackexchange.com/questions/115660/… | |
| May 21, 2019 at 10:52 | history | edited | andselisk♦ | CC BY-SA 4.0 |
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| May 21, 2019 at 10:47 | history | asked | Mayuri Vaish | CC BY-SA 4.0 |