Drawing the Lewis structure for Coordination Compounds

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Brandon Fujii 1K
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Drawing the Lewis structure for Coordination Compounds

Postby Brandon Fujii 1K » Wed Dec 06, 2017 10:14 am

If we are given a coordination compound, i.e. [HgF2(OH2))2]1+, do we use the total charge of the compound (1+) to find the formal charge of the lewis structure in addition to finding the oxidation state of the metal atom?

Zane Mills 1E
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Re: Drawing the Lewis structure for Coordination Compounds

Postby Zane Mills 1E » Wed Dec 06, 2017 10:16 am

Yes, the formal charges actually refer to the individual atoms and their electrons though, so you would use this number to find the overall charge on the molecule given the individual formal charges.

Austin Ho 1E
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Re: Drawing the Lewis structure for Coordination Compounds

Postby Austin Ho 1E » Wed Dec 06, 2017 10:19 am

In short: yes, I think so. The charge on the outside lets you know the overall charge of the whole molecule, thus it should be kept into account when drawing a Lewis structure. For your example for instance, [HgF2(OH2))2]1+, I believe the oxidation number of Hg would be (V) since there are 4 negative charges (2 from F- and 2 from OH-) but an overall +1 charge on the molecule.

Ammar Amjad 1L
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Re: Drawing the Lewis structure for Coordination Compounds

Postby Ammar Amjad 1L » Wed Dec 06, 2017 10:35 am

Austin Ho 1E wrote:In short: yes, I think so. The charge on the outside lets you know the overall charge of the whole molecule, thus it should be kept into account when drawing a Lewis structure. For your example for instance, [HgF2(OH2))2]1+, I believe the oxidation number of Hg would be (V) since there are 4 negative charges (2 from F- and 2 from OH-) but an overall +1 charge on the molecule.


The OH2 is neutral; therefore it doesn't have a charge. There would be a -2 charge from F2; therefore, the oxidation number of mercury would be (III).


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