within ui 10.35 It is important to understand the origins of stabilization of li
ID: 1043501 • Letter: W
Question
within ui 10.35 It is important to understand the origins of stabilization of linear conjugated molecules because they play important biological roles in plants and animals (see Case study 9.1). According to Hückel theory, the energies of the bonding ? molecular orbitals of butadiene, CH,-CH,-CH, CH 2, are E ? + 1.62ß and ? + 0.62ß The energies of the antibonding ?* molecular orbitals are E-?-1.6B and ?-062a The total n-electron binding energy, E, is the sum of the energies of each ? electron. Recalling that there are four electrons to accommodate in the ? molecular orbitals, calculate the ?-electron and benzen in a 2p orbit for the ener (a) Calcula cyclooctat energy lev of benzens 10.36) W compare binding energies of ethene (see Section 10.7) and butadiene. Is thera energy of the butadiene molecule lower or higher than the sum of two individual n bonds?Explanation / Answer
? electron binding energy for Ethene = 2(?+?) = 2? + 2?
? electron binding energy for butadiene = 2(?+1.62?) + 2(?+0.62?) = 4? + 4.48?
Binding Energy for two individual ? bonds = 2(2? + 2?) = 4? + 4?
Therefore, difference in energy between butadiene and two individual ? bonds = (4? + 4.48?) - (4? + 4?) = 0.48?
Hence, butadiene is more stable by 0.48?
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