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For those of you who have BR, question 1.7 on page 21 asks which carbon-carbon single bond is the MOST stable according to the table of bond dissociation energies provided.
I don't have an issue picking out the correct answer, but one part of the answer explanation seemed odd. Answer choice B, C, and D all include a secondary sp3 hybridized carbon bonded to another carbon (the other carbon is irrelevant to my question). According to the answer explanation and the table provided, a secondary carbon could arise from a group such as ethyl or n-propyl. However, considering that only Et is listed as a substituent in the table, it's the only one we can use. I don't understand how to read this table. How does it account for adding multiple substituents to the carbon we are interested in? For instance, one of the answer choices is an sp2 hybridized carbon (e.g., from a vinyl group) bonded to a secondary sp3 hybridized carbon atom (e.g., which arises from an ethyl group???? how???).
Thanks for the help.
I don't have an issue picking out the correct answer, but one part of the answer explanation seemed odd. Answer choice B, C, and D all include a secondary sp3 hybridized carbon bonded to another carbon (the other carbon is irrelevant to my question). According to the answer explanation and the table provided, a secondary carbon could arise from a group such as ethyl or n-propyl. However, considering that only Et is listed as a substituent in the table, it's the only one we can use. I don't understand how to read this table. How does it account for adding multiple substituents to the carbon we are interested in? For instance, one of the answer choices is an sp2 hybridized carbon (e.g., from a vinyl group) bonded to a secondary sp3 hybridized carbon atom (e.g., which arises from an ethyl group???? how???).
Thanks for the help.