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OH O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over multiple atoms, including an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over multiple atoms, including two electronegative oxygen atoms.

OH O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over multiple atoms, including an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over multiple atoms, including two electronegative oxygen atoms.

Organic Chemistry: A Guided Inquiry
Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Andrei Straumanis
Chapter4: Polar Bonds, Polar Reactions
Section: Chapter Questions
Problem 28E: The following are equivalent ways of asking about the acidity of an H atom: • What is the most...
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OH O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over multiple atoms, including an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over multiple atoms, including two electronegative oxygen atoms.
Transcribed Image Text:OH O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge associated with an sp? hybrid orbital. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance. O The blue proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized over a carbon atom and an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over multiple atoms, including an electronegative oxygen atom. O The red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over multiple atoms, including two electronegative oxygen atoms.
NH2 но O he red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over two electronegative oxygen atoms. O The blue proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over two less electronegative nitrogen atoms. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over two less electronegative nitrogen atoms. O The red proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over two electronegative oxygen atoms.
Transcribed Image Text:NH2 но O he red proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over two electronegative oxygen atoms. O The blue proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over two less electronegative nitrogen atoms. O The blue proton is more acidic because its conjugate base is more stable, with a negative charge that is delocalized by resonance over two less electronegative nitrogen atoms. O The red proton is more acidic because its conjugate base is less stable, with a negative charge that is delocalized by resonance over two electronegative oxygen atoms.
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