In the case of benzene, the hybrid structure is the one below (the one you learn at school): When resonance theory was first applied to understanding the structure of benzene, the key feature seemed to be a resonance hybrid of ring structures containing alternating single and double bonds. Two of the hybrid orbitals are used to form σ bonds with the carbon atom neighbours, and one is used to form a σ bond with a hydrogen atom. Benzene is commonly regarded as a resonance hybrid of the two Kekule structures, but other possible structures can also contribute. When resonance theory was first applied to understanding the structure of benzene, the key feature seemed to be a resonance hybrid of ring structures containing alternating single and double bonds. Actual molecule of benzene is usually represented by this structure. To be reasonable, all structures in a set representing a resonance hybrid must have exactly the same locations of the atoms in space. An orbital model for the benzene structure. Benzene has a moderate boiling point and a high melting point. The perfectly symmetrical structure of benzene, however, indicates that it exists as a resonance hybrid: The actual bond length (1.395 Å ) is the intermediate between the sp 2 – sp 2 single bonds (1.46 Å) and double bonds (1.33 Å). Each of the six carbon atoms is taken to be sp2 hybridized. The resonance structure with the Formal Charge closest to zero is the most accepted structure, however, the correct Lewis structure is actually a combination of all the resonance structures and is not solely describe as one. New X-ray studies reveal that the distance between the carbon atoms in benzene is 1.39 Angstroms. Benzene is built from hydrogen atoms (1s 1) and carbon atoms (1s 2 2s 2 2p x 1 2p y 1). e) All of these contribute. The oscillating double bonds in the benzene ring are explained with the help of resonance structures as per valence bond theory. The resonance hybrid is Structure #3 below. The actual structure of benzene lies somewhere in between A and B and may be represented as C, referred to as resonance hybrid. In Kekule's structure, the carbon atoms in benzene are arranged in a hexagonal ring with each carbon atom is attached to two other carbon atoms.The ring contains alternate single and double bond.These double bonds are due to the π electrons present in benzene.These π electrons can delocalize and form two structures with different position of a double bond.These are the resonance … The classical example of resonance is benzene, C 6 H 6. The two structures of benzene which have been mentioned above are called resonance structures of benzene. Benzene is a unique molecule when it comes to resonance structures.

9) Which of the following structures does not contribute to the resonance hybrid of the intermediate formed when nitrobenzene undergoes meta-chlorination? Each Lewis structure that contributes to the resonance hybrid is a resonance structure. Because it is a bit tedious to draw all the dots, the structure of the benzene molecule is often written as shown in Structure #4, with the dotted lines represented by a circle. Benzene has 2 resonance structures but taken individually none show the delocalisation of electrons and they can exist at the same time as electrons are delocalised. Modern descriptions of the benzene structure combine resonance theory with molecular orbital theory. Chemical bonding - Chemical bonding - Resonant structures: The description of the planar hexagonal benzene molecule, C6H6, illustrates another aspect of VB theory. It is highly inflammable and burns with a sooty flame. The actual structure of benzene is a hybrid of these two resonance structures. Chemical bonding - Chemical bonding - Resonant structures: The description of the planar hexagonal benzene molecule, C6H6, illustrates another aspect of VB theory. Resonance of Benzene. 43.2. Resonance hybrid of benzene. Two of the hybrid orbitals are used to form σ bonds with the carbon atom neighbours, and one is used to form a σ bond with a hydrogen atom.