Pls help ASAP. Pls do all asked questions I BEG Part BTwo possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude abouthow favorable the structures are?► View Available Hint(s)Structure A is more favored.Structure B is more favored.The structures are equally favored.Submit A bonded atom is considered to "own" all its nonbonding electrons but only half of the bonding electrons because these areshared with another atom. Therefore, the formal charge formula can be rewritten as follows:FC =(valence e infree atomin) - [(nonbonding eshown-) + ² ((bonding e)]Part ADue to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less commonand less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures forthese acids and use formal charges for the evaluation of these structures. For a molecule of fluorous acid, the atoms arearranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the moreelectronegative 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.Express your answers as charges separated by comma. For example, a positive one charge would be written as+1.View Available Hint(s)Formal Charge for H, O, F, O =

Answered: Image /qna-images/answer/f7709bdc-416f-4704-9439-30978c6813d5.jpg

Part B Two possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude about how favorable the structures are? ► View Available Hint(s) Structure A is more favored. Structure B is more favored. The structures are equally favored. Submit

Part B Two possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude about how favorable the structures are? ► View Available Hint(s) Structure A is more favored. Structure B is more favored. The structures are equally favored. Submit

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Pls help ASAP. Pls do all asked questions I BEG

Part B
Two possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude about
how favorable the structures are?
► View Available Hint(s)
Structure A is more favored.
Structure B is more favored.
The structures are equally favored.
Submit

A bonded atom is considered to "own" all its nonbonding electrons but only half of the bonding electrons because these are
shared with another atom. Therefore, the formal charge formula can be rewritten as follows:
FC =
(
valence e in
free atom
in) - [(
nonbonding e
shown
-) + ² (
(bonding e
)]
Part A
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.
Express your answers as charges separated by comma. For example, a positive one charge would be written as
+1.
View Available Hint(s)
Formal Charge for H, O, F, O =

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