(a) First, add enough electrons as either lone pairs or r bonds to give an overall negative charge. Show all lone pairs in each completed Lewis structure, and show any atomic formal charges that result. (b) Then, for each isomer, consider if other resonance structures can contribute. Since this is an anion, look for a strong electron donor with an adjacent electron acceptor. For each additional resonance structure you draw (some isomers may have more than one additional RS, some may have none), circle the electron pairs in the original Lewis structure which have moved, and draw a curved arrow depicting the motion required to create the new RS. If you have colored pens, color coding your electrons pairs is nice (but not required).
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.
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