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- Which one of the following statements from Chapter 8 and 18 is FALSE? O For a compound to be classified as aromatic, it must have an odd number of pairs of n-electrons and must be fully conjugated, cyclic and planar. O Inclusion of heteroatoms as part of the conjugated ring system renders the molecule to be considered non-aromatic. O Benzene is a six-membered ring where the n-electrons are equally shared across all six carbons in the ring and thus it possesses 36 kcal/mol of resonance stabilization energy. O The key reaction in Chapter 18 is the EAS reaction, which stands for electrophilic aromatic substitution. O All EAS reactions follow the same three mechanistic steps: (1) generate the electrophile, (2) capture the electrophile to give a carbocation intermediate, and (3) loss of a proton to regain aromaticity.Assuming the rings are planar, label attached ion as aromatic, antiaromatic, or not aromatic.is this molecule aromatic ,anti aromoatic,or non aromatic??
- I need help figuring out the number of electrons in a cyclic conjugated system and determining if the compound is aromatic, anti-aromatic, or neither.Build a model of methylcyclohexane, and use the model to complete the following Newmanprojections of methylcyclohexane in the chair conformation: a. When the methyl group is in an axial or equatorial (circle one) position, the molecule is inits lowest potential energy conformation. b. Label one Newman projection above anti and the other gauche to describe the relationshipbetween the methyl group and C3 of the ring. c. In general, which is a lower PE conformation, anti or gauche? d. Explain how your answer to b and c provide an explanation for why it is more favorable fora large group to be in an equatorial than an axial position.I know the main chain is cyclononane but the numbering for the substituents is where I have trouble
- Categorize the following molecules as aromatic, anti-aromatic, or non-aromatic by adding the assigned letters to the corresponding category. Assume each molecule is planar.Would the following be aromatic, antiaromatic, or non-aromatic? Explain the reason.Q4. Draw the orbitals of thiophene to show that is aromatic.
- give an energy diagram for the cyclopropenyl MOs. (The polygon rule is helpful.)Label each MO as bonding, nonbonding, or antibonding, and add the nonbonding line.Notice that it goes through the approximate average of the MOs.(c) Add electrons to your energy diagram to show the configuration of the cyclopropenylcation and the cyclopropenyl anion. Which is aromatic and which is antiaromatic?Select all that is true for cycloheptatriene and the ions it can form. The 6 pi electrons in cycloheptatriene anion can be delocalized over the ring, which decreases the electronic energy of the molecule. Delocalization of the pi electrons in cycloheptatriene anion increases the electronic energy of the molecule. The cycloheptatriene contains 6 pi electrons, which makes it an aromatic compound. The pi electrons in cycloheptatriene cannot be delocalized over the ring. The pi electrons in cycloheptatriene cation can be delocalized over the ring. The 6 pi electrons in cycloheptatriene cation can be delocalized over the ring, which decreases the electronic energy of the molecule. The cycloheptatriene anion contains 6 pi electrons, which makes it an aromatic compound.Assuming the rings are planar, label each ion as aromatic, antiaromatic, or not aromatic.