Answer :
Answer:
The bond is planar. There is free rotation about the carbonyl carbon and nitrogen bond.
Explanation:
The peptide bond is planar and for this reason there is free rotation about the carbonyl carbon and nitrogen bond. Peptide bonds don't have double-bonds or delocalized electrons in their structure. Both oxygen and nitrogen have a net negative charge on the peptide bonds.
Final answer:
A peptide bond is planar, does not allow free rotation due to its double-bond character, and has no net charge under physiological conditions.
Explanation:
The characteristics of a typical peptide (amide) bond are as follows:
- The bond is planar. This is because of the resonance or delocalization of the peptide bond.
- There is not free rotation about the carbonyl carbon and nitrogen bond. This is due to the double-bond character of the peptide bond caused by the resonance.
- A peptide bond has a double bond character which gives it its planar structure.
- There is no net charge on either the nitrogen or the oxygen in a peptide bond under physiological circumstances i.e. pH 7.4. So, the last statement that nitrogen has a net negative charge and oxygen has a positive charge is not correct.
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