Timeline for What causes ionisation in redox reactions?
Current License: CC BY-SA 4.0
5 events
| when toggle format | what | by | license | comment | |
|---|---|---|---|---|---|
| Nov 7, 2023 at 0:56 | vote | accept | John O'brien | ||
| Nov 6, 2023 at 15:39 | comment | added | anon | Yes, reducing temperature slows reactions. The atoms can only bond if they collide with enough energy to overcome the activation energy. This becomes less likely at low temperatures. Eventually it will essentially stop. I don't know how cold you have to make magnesium before oxidation becomes negligible... probably pretty cold. | |
| Nov 6, 2023 at 15:04 | comment | added | Mithoron | @JohnO'brien Electrons don't ever "break free" in chemistry, unless it's plasma chemistry. Your atoms just bump into each other creating highly polarised bond that is called "ionic". That does not mean there are separate ions in a molecule, just that ionic component of bonding is greater than covalent. | |
| Nov 6, 2023 at 13:25 | comment | added | John O'brien | Thanks for this! So just to be clear, the heat at room temperature is what allows for the two valence electrons to break free from the Mg, but only when they're in close proximity to the O atom? So if we attempted the reaction in an environment with a much lower temperature, nothing would happen? | |
| Nov 6, 2023 at 12:50 | history | answered | anon | CC BY-SA 4.0 |