Timeline for Why does ozone have an electrostatic potential map similar to that of SO2?
Current License: CC BY-SA 3.0
16 events
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| Apr 6, 2016 at 15:33 | history | edited | hBy2Py | CC BY-SA 3.0 |
Replaced SO2 image with non-transparent version; restructured for clarity
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| Jan 22, 2015 at 21:09 | vote | accept | Caters | ||
| Dec 23, 2014 at 18:10 | answer | added | bon | timeline score: 5 | |
| Oct 10, 2014 at 16:40 | comment | added | tschoppi | @permeakra Sounds like you could write that up into a good answer! :) | |
| Aug 10, 2014 at 7:25 | history | tweeted | twitter.com/#!/StackChemistry/status/498369475914510336 | ||
| Aug 9, 2014 at 23:02 | comment | added | Caters | Let us continue this discussion in chat. | |
| Aug 9, 2014 at 21:54 | comment | added | permeakra | @caters in fact dipole moment is a function of charge distribution. Electronegativity considerations allow to some extent predict some aspects of charge distribution in case of simple compounds with ordinary bonds. However, in case of molecules with dative bonds ($\ce{CO}$, $\ce{O3}$, $\ce{SO2}$ and many more), conjugated $\pi$-systems and other compounds with nontrivial electronic structures electronegativity alone does not work. | |
| Aug 9, 2014 at 21:35 | comment | added | permeakra | @caters Nope. Dipole moment is completely attributed to electron distribution in the molecule, and electron donation may go against electronegativity to some extent. | |
| Aug 9, 2014 at 21:25 | comment | added | Caters | but the 3 Os all have the same electronegativity and isn't it electronegativity difference that determines dipole moment and thus polarity regardless of whether it is charged or not? | |
| Aug 9, 2014 at 21:22 | comment | added | permeakra | @caters Ozone has dipole moment of ~ 0.5 D. It is three times smaller than for sulfur dioxide, but still high enough. And I repeat, both have roughly same electron structure. | |
| Aug 9, 2014 at 21:07 | comment | added | Caters | charged molecule does not automatically mean polar. All it means is that it is an ion. You also have to take into consideration dipole moment(and thus electronegativity) to know whether it is a nonpolar ion(such as in the case of ozone), a polar ion(such as methoxide), or will participate in an ionic bond with another ion(as long as you know what that other ion is and its electronegativity). | |
| Aug 9, 2014 at 20:56 | comment | added | Caters | there is 0 dipole moment because all atoms in ozone have the same electronegativity. 0 dipole moment means nonpolar. However it is an ion to some degree because of the positively charged oxygen in the center. | |
| Aug 9, 2014 at 20:50 | comment | added | Dissenter | Ozone is non-polar? You might want to rethink that. | |
| Aug 9, 2014 at 20:40 | comment | added | Caters | yeah but 1 is polar(the sulfur dioxide) and the other is nonpolar with a positive charge(the ozone). I would expect that the positive charge of ozone would make the central oxygen pull harder in the bond(because of the positive charge it has) and thus the electrons spend less time around the terminal oxygens thus making the MEP more like the one of H2O | |
| Aug 9, 2014 at 20:27 | comment | added | permeakra | Because their outer orbitals are very similar. The bonding nature in these to molecules is exactly the same with slightly more electronic structure moved from central atom in $\ce{SO2}$. | |
| Aug 9, 2014 at 18:59 | history | asked | Caters | CC BY-SA 3.0 |