Timeline for Why does chlorine have a higher electron affinity than fluorine?
Current License: CC BY-SA 3.0
11 events
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| Sep 29, 2017 at 8:52 | comment | added | Jan | @ashu There is absolutely no reason to consider vacant d orbitals in partly filled electron shells. You don’t consider f orbitals for bromine either. In fact, while this answer does start off well I have to give it a $-1$ for invoking a concept that does not help and is introduced incorrectly. | |
| Nov 7, 2016 at 1:56 | comment | added | ashu | We're considering vacant orbitals in partially filled electron shells, not empty electron shells. | |
| Nov 6, 2016 at 18:10 | comment | added | user3932000 | @ashu But if we're considering vacant orbitals, all atoms have an infinite number of vacant orbitals, with energy levels from 1≤n<∞? | |
| Nov 6, 2016 at 17:45 | comment | added | ashu | @user3932000 Fluorine doesn't have a 3rd (M) electron shell hence no d-orbitals. | |
| Nov 6, 2016 at 17:39 | comment | added | user3932000 | @ashu You could say the same for fluorine and say fluorine also has vacant d-orbitals, since its configuration would then be 1s2 2s2 2p5 3s0 3p0 4s0 3d0. | |
| Nov 6, 2016 at 14:42 | comment | added | ashu | @user3932000 Chlorine have vacant d-orbitals. Since empty orbitals are omitted when writing electronic configuration, it is written as $1s^2 2s^2 2p^6 3s^2 3p^5$. Complete electronic configuration would be $1s^2 2s^2 2p^6 3s^2 3p^5 3d^0$. | |
| Oct 29, 2016 at 16:49 | comment | added | user3932000 | ....but chlorine doesn't have any d-orbitals either? | |
| Sep 2, 2014 at 13:57 | history | edited | ashu | CC BY-SA 3.0 |
added 22 characters in body
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| Nov 12, 2013 at 19:11 | vote | accept | abhishek | ||
| Nov 12, 2013 at 11:22 | comment | added | Nicolau Saker Neto | I don't think d orbitals contribute to atomic size, since they're always only populated in an internal shell. Calculated atomic radii decrease continuously across a period, and they decrease a little slower in the d-block because the inner d orbitals shield the valence s/p electrons from the nuclear charge better than adding electrons to the outer shell. If anything, the presence of a populated d subshell actually helps contract the atom, allowing it to reach a higher effective nuclear charge than expected in a period with no d subshell. | |
| Nov 12, 2013 at 5:11 | history | answered | ashu | CC BY-SA 3.0 |