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- For the aromatic compounds below, draw the p-orbitals for the compound.How do you find the hydridization of the carbon atoms in the resonance hybrid of benzene?The bonding between the carbon and oxygen in a ketone can be described as C(sp2)-0(sp²), o-bond and C(p)-O(p), л-bond. How would you describe the bonding between carbon and oxygen in a ketene? Sketch the orbitals used to make the bonds in the ketene. H a ketene
- Two useful organic compounds that contain Cl atoms are vinyl chloride (CH2 = CHCI) and chloroethane (CH;CH;CI). Vinyl chloride is the starting material used to prepare poly (vinyl chloride), a plastic used in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C- Cl bond of vinyl chloride stronger than the C– CIl bond in chloroethane.3) How many electrons are delocalized in how many p-orbitals? Draw the most and second most stable resonance structures of the following compound. Order the structures by increasing stability. What is the partial charge distribution in the resonance hybrid?The pentadienyl radical, H2C“CH¬CH“CH¬CH2#, has its unpaired electron delocalized over three carbon atoms.(a) Use resonance forms to show which three carbon atoms bear the unpaired electron.(b) How many MOs are there in the molecular orbital picture of the pentadienyl radical?
- Specify whether the two structures are resonance contributors to the same resonance hybrid. Be sure to explain your reasoning. If yes, be sure to specify which is preferred and why. H2C=NH2Sketch the ultraviolet absorption spectrum of 1,3-Butadiene, matching peaks to electronic transitions. show that four isolated p orbital on carbon atoms combine to form pi orbitalHow come the structure labeled as 1 has 8 pi electrons? If the double bond has 2 pi electrons, and you count the lone pairs, wouldn't it have 6 pi electrons? Why does the structure labeled as 2 has aromaticity? If the pi bond has 2 pi electrons and then you coun the lone pairs, wouldn't it only have 5 pi electrons?
- 4. One of the resonance structures of "tropylium ion" (C7H7*) is shown below. It is planar and aromatic with Hückel number of p-n electrons where n=1. Draw all the other contributing resonance structures. (There are more than two.) Based on the “average" of the contributing resonance structures, how close does the average ring carbon get to its "octeť" in tropylium ion?Classify the following structure as either "aromatic", "antiaromatic", or "nonaromatic". How many pi electrons are in the structure? Assume the structure is planar. NH 2-1. What is resonance contributor in which one or more atoms bears a formal change and the most stable resonance form? 2.what is the process of distributing electron pairs in a molecule? 3. Are organic molecules which are less sterically hindered more attractive than those which are more sterically hindered?