Later, we will show that the contributor with the negative charge on the oxygen is the more stable of the two. The two resonance structures shown below are not equivalent because one show the negative charge on an oxygen while the other shows it on a carbon. Because of this, resonance structures do necessarily contribute equally to the resonance hybrid. In the resonance hybrid, the negative charge is spread out over a larger part of the molecule and is therefore more stable.ģ) Resonance contributors do not have to be equivalent. The resonance hybrid shows the negative charge being shared equally between two oxygens. When looking at the picture above the resonance contributors represent the negative charge as being on one oxygen or the other. The charge is spread out amongst these atoms and therefore more stabilized. Often, resonance structures represent the movement of a charge between two or more atoms. Representations of the formate resonance hybridĢ) The resonance hybrid is more stable than any individual resonance structures. Major resonance contributors of the formate ion ![]() Resonance hybrids are really a single, unchanging structure. When looking at a resonance contributors, we are seeing the exact same molecule or ion depicted in different ways. ![]() This real structure (the resonance hybrid) takes its character from the average of all the individual resonance contributors. When learning to draw and interpret resonance structures, there are a few basic guidelines to help.ġ) There is ONLY ONE REAL STRUCTURE for each molecule or ion. Recognizing, drawing, and evaluating the relative stability of resonance contributors is essential to understanding organic reaction mechanisms. Rules for Drawing and Working with Resonance Contributors
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