![]() ![]() This is very important for the reactivity of chloro-benzene because in the presence of an electrophile it will react and the formation of another bond will be directed and determine by resonance. The Hybrid Resonance forms show the different Lewis structures with the electron been delocalized. A carbon with a negative charge is the least favorable conformation for the molecule to exist, so the last resonance form contributes very little for the stability of the Ion. The nitrogen is more electronegative than carbon so, it can handle the negative charge more than carbon. For example, if we look at the above rules for estimating the stability of a molecule, we see that for the third molecule the first and second forms are the major contributors for the overall stability of the molecule. Some structural resonance conformations are the major contributor or the dominant forms that the molecule exists. Molecules and ions with more than one resonance form The delocalized electrons in the benzene ring make the molecule very stable and with its characteristics of a nucleophile, it will react with a strong electrophile only and after the first reactivity, the substituted benzene will depend on its resonance to direct the next position for the reaction to add a second substituent.Įxample 2.5.1: Multiple Resonance of other Molecules The extra electron that created the negative charge one terminal oxygen can be delocalized by resonance through the other terminal oxygen.īenzene is an extremely stable molecule due to its geometry and molecular orbital interactions, but most importantly, due to its resonance structures. Ozone with both of its opposite formal charges creates a neutral molecule and through resonance it is a stable molecule. The above resonance structures show that the electrons are delocalized within the molecule and through this process the molecule gains extra stability. Resonance forms that are equivalent have no difference in stability and contribute equally.Positive charges on the least electronegative atom (most electropositive) is more stable.A structure with a negative charge on the more electronegative atom will be more stable. ![]() The structure with the least separation of formal charges is more stable.The structure with the least number of formal charges is more stable.The greater the number of covalent bonds, the greater the stability since more atoms will have complete octets.Rules for estimating stability of resonance structures This particular ion is discussed in further detail in Section 2.6. \)Īfter completing this section, you should be able to use the concept of resonance to explain structural features of certain species for example, why all of the carbon-oxygen bonds in the carbonate ion are the same length. ![]()
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