This structure is called the " resonance hybrid " of that molecule.
2.
Therefore, the resonance hybrid cannot be represented by a combination of isomers.
3.
When comparing resonance structures for the same molecule, usually those with the fewest formal charges contribute more to the overall resonance hybrid.
4.
The molecule cannot be represented by one structure, but rather a resonance hybrid of different structures, such as with the two resonance structures of benzene.
5.
When this situation occurs, the molecule's Lewis structure is said to be a resonance structure, and the molecule exists as a resonance hybrid.
6.
The resonance hybrid is the approximate intermediate of the contributing structures, but the overall energy is lower than each of the contributors, due to the resonance energy.
7.
Equivalent contributors contribute equally to the actual structure; those with low potential energy ( the major contributors ) contribute more to the resonance hybrid than the less stable minor contributors.
8.
The resulting resonance hybrid, now possessing ? + charges in the ortho-and para-positions repels approaching electrophiles increasing the relative success of attack in the meta position.
9.
According to one model, an iron dioxygen complex is initially formed and stabilized as a resonance hybrid of Fe 2 + O 2 and Fe 3 + O 2 ".
10.
Several Lewis structures are used collectively to describe the actual molecular structure, which is an approximate intermediate between the canonical forms called a "'resonance hybrid " '.
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