Timeline for Why is the formation of NaCl an exothermic process?
Current License: CC BY-SA 3.0
3 events
| when toggle format | what | by | license | comment | |
|---|---|---|---|---|---|
| Sep 15, 2016 at 18:35 | comment | added | Jan | @AaryanDewan That’s not exactly the question you asked, but here is the answer: Electron and nucleus attract each other. To strip away the electron, you need to overcome the attraction. That costs energy. Note that calling metal cations ‘stable states’ is typically wrong: If something lost an electron by ionisation (as metals do if they become cations) that will always cost energy and thus metal cations are never more stable than the pure metal. | |
| Sep 15, 2016 at 14:55 | comment | added | Aaryan Dewan | "Note most importantly, that it is not merely the generation of sodium cations (that process is endothermic) or the generation of chloride anions (that process is only weakly exothermic) that causes the overall exothermicity of the entire reaction" . This is exactly , what my question is. I want to know that what causes the sodium conversion to sodium anion to loose energy? I know it's getting stable, but what really is causing it to loose energy? | |
| Sep 15, 2016 at 9:46 | history | answered | Jan | CC BY-SA 3.0 |