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Unformatted text preview: For compounds 'A' and 'B' that carbocation is secondary; for compound 'C' it's tertiary. The tertiary carbocation will be lower in energy than a secondary, and so the transition state leading to it will be lower in energy as well, so that the activation energy leading to that carbocation should be lower than that generated from 'A' or 'B'. Protonation of both 'A' and 'B' gives the same carbocation; however, since 'B' is less stable than 'A' ( cis relative to trans alkene), 'B' will be closer in energy to the transition state leading to that carbocation. Thus 'B' will have a lower activation energy than 'A' in hydration - it will react faster...
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- Fall '08