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For each compound below, identify all lone pairs and

Chapter 2, Problem 2.36

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QUESTION:

For each compound below, identify all lone pairs and indicate whether each lone pair is localized or delocalized. Then, use that information to determine the hybridization state and geometry for each atom that exhibits a lone pair. (a) H2N NH2 (b) O N O (c) O OH H2N NH2 (d) N (e) N H (f) O O O

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QUESTION:

For each compound below, identify all lone pairs and indicate whether each lone pair is localized or delocalized. Then, use that information to determine the hybridization state and geometry for each atom that exhibits a lone pair. (a) H2N NH2 (b) O N O (c) O OH H2N NH2 (d) N (e) N H (f) O O O

ANSWER:

Step 1 of 15

(a)

The molecule is as follows:

     

Each nitrogen atom exhibits a lone pair. Consider the Nitrogen atom on the left side of the molecule.

The lone pair of the left nitrogen can form a resonance structure, so it is delocalized. The lone pair occupies the p orbital. This means the nitrogen is sp2 hybridized and trigonal planar.

     

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