Figure EC-Ö:] :NEC A < 1 of 1 > [EN-C=O: 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) O Structure A is more favored. O Structure B is more favored. O The structures are equally favored. Submit Provide Feedback Next >
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
![Figure
[EN=C-03]
A
< 1 of 1 >
EN-C=O:]
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)
▶
O Structure A is more favored.
O Structure B is more favored.
O The structures are equally favored.
Submit
Provide Feedback
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![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:
TC
▼
Part A
FC=
valence e in
free atom
nonbonding e
shown
Formal Charge for H, O, F, O =
+
1
2
bonding e
shown
[)]
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 al
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.
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