Timeline for The bond in coordination complexes
Current License: CC BY-SA 3.0
15 events
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| Aug 28, 2020 at 7:06 | comment | added | Yoda | The case would perhaps not be so simple in TM complexes where the ligands are not all the same? How would the formal charges distribute then? You mention Pauling's guideline presented here is supported by MO calculations; could you perhaps include some results? It would be interesting to look at some of the MOs, and perhaps see what the partial charges look like. | |
| Jun 17, 2017 at 15:54 | comment | added | Philipp |
@TanYongBoon Also, I believe in Para 2 Line 10, the charge of the complex ion is "4-" not "4+". Thanks, I corrected it in my answer.
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| Jun 17, 2017 at 15:53 | comment | added | Philipp | @TanYongBoon Yes, that's why I wrote that this is the only difference between coordinate bonds and covalent bonds that I see. | |
| Jun 17, 2017 at 15:52 | comment | added | Tan Yong Boon | I agree with the "d" orbitals playing a great role but that is only for the case of transition metal ion complexes, not the case of simple covalent substances such as carbon monoxide or the ammonium ion. | |
| Jun 17, 2017 at 15:52 | history | edited | Philipp | CC BY-SA 3.0 |
corrected charge of complex ion
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| Jun 17, 2017 at 15:51 | comment | added | Philipp |
@TanYongBoon Also, you have misunderstood the idea of a "formal charge". To a chemist, "formal charges" are theoretical constructs indicating regions of electron-richness and electron-deficiency in a molecule and are not actual charges. What makes you think that? I never claimed otherwise. But one thing that relates formal and actual charges is that all the formal charges within a molecule have to add up to the actual charge. Apart from that I'm well aware that the two should not be mixed up.
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| Jun 17, 2017 at 15:51 | comment | added | Tan Yong Boon | "Character" refers to the electron distribution and also, the likelihood of it participating in particular reactions. | |
| Jun 17, 2017 at 15:48 | comment | added | Philipp |
@TanYongBoon Are there any differences in terms of the character of the bond from a covalent bond? That depends on what exactly you mean by "character of the bond", so you might get different answers from different people. I don't see much of a conceptual difference between covalent and coordinate bonds but my view is heavily informed by MO theory and there both types of bonds are described on the same footing. It's just that in coordinate bonds d orbitals play a major role.
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| Jun 17, 2017 at 15:27 | comment | added | Tan Yong Boon | Also, I believe in Para 2 Line 10, the charge of the complex ion is "4-" not "4+". | |
| Jun 17, 2017 at 15:24 | comment | added | Tan Yong Boon | Also, you have misunderstood the idea of a "formal charge". To a chemist, "formal charges" are theoretical constructs indicating regions of electron-richness and electron-deficiency in a molecule and are not actual charges. Please take note. | |
| Jun 17, 2017 at 14:54 | comment | added | Tan Yong Boon | So are you suggesting that the coordinate bond is a type of polar covalent bond? Are there any differences in terms of the character of the bond from a covalent bond? ("Covalent bond" here refers to any covalent bond, not necessarily purely covalent) | |
| May 16, 2014 at 19:32 | vote | accept | Keerthana A.K. | ||
| Apr 25, 2014 at 20:04 | vote | accept | Keerthana A.K. | ||
| Apr 25, 2014 at 20:26 | |||||
| Apr 24, 2014 at 20:16 | history | edited | Philipp | CC BY-SA 3.0 |
deleted 3 characters in body
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| Apr 24, 2014 at 20:09 | history | answered | Philipp | CC BY-SA 3.0 |