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01.08.2019 •
Chemistry
Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. for a molecule of fluorous acid, the atoms are arranged as hofo. (note: in this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.) what is the formal charge on each of the atoms? enter the formal charges in the same order as the atoms are listed.
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Ответ:
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H - O - F - O:
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We can calculate the formal charge of an atom using the following formula:
Formal charge = [# of valence electrons] - [# of non-bonded electrons + # of bonds]
H: Formal charge = [1]-[0+1] = 0
O: Formal charge = [6]-[4+2] = 0
F: Formal charge = [7]-[4+2] = +1
O: Formal charge = [6]-[6+1] = -1
As we can see the overall charge of the molecule is neutral since the fluorine as a +1 charge and the oxygen a -1 charge.
Ответ:
The chances of the offspting being pink is 50%