Based on charge stability, rank species A-G from weakest base to strongest base.HO.F ÉAВF

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Answered: Based on charge stability, rank species…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter5: Resonance

Section: Chapter Questions

Problem 24CTQ

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Consider the following bases: a. For each base above, circle the atom/atoms with the highest PE (will release the most P.E.when a lone pair on this atom combines with an H+ ) b. Rank the bases 1 (highest P.E./strongest base) to 7 (lowest PE/weakest base), and explainyour reasoning.
For each molecule below, draw the conjugate acid or conjugate base or both if the molecule hasboth a conjugate acid and a conjugate base (e.g., water).
Based on the charge stability, rank species A-G from the weakest base to the strongest base.
Using the data in the table, which of the conjugate bases below is the strongest base? A) OAc- B) C7H5O2- C) NO2- D) F- E) OAc- and C7H5O2-
For each pair of bases, identify the stronger base.
Indicate which is the weaker base and explain why. Be specific! NH3 or NF3
The following are equivalent ways of asking about the acidity of an H atom: • What is the most acidic H on the molecule? • Which H is associated with the published pKa value? • Which H on the molecule is easiest to remove? • Which H on the molecule takes the least energy to remove? • Which bond to an H is most polarized? • For which H atom is removal least uphill in energy? • Which bond to an H atom, when broken, results in the lowest PE conjugate base? We will often find the last of these questions is easiest to answer. To do this, find all the different Hatoms on the molecule, and draw all possible conjugate bases.Only the lowest-energy one is the “real” conjugate base. Identify this structure, and you have found the most acidic H. Use this strategy to find the most acidic H on each of the following molecules. Note: Each structure hasat least three different kinds of H’s, so draw at least three unique conjugate bases for each.
Complete the equation for the reaction between each Lewis acid-base pair. In each equation, label which starting material is the Lewis acid and which is the Lewis base; use curved arrows to show the flow of electrons in each reaction. In doing this problem, it is essential that you show valence electrons for all atoms participating in each reaction. (a) (b) (c) (d)
Construct an explanation for why sulfuric acid is such a strong acid. (Note that sulfur is in thethird row of the periodic table and can have more than eight electrons.)
For the previous four questions, label each molecule that appears in the question or your answer asstrong acid, strong base, weak acid, or weak base.
Summarize the relationship between pKa and acid strength by completing the following sentences: a. The higher the pKa of an acid, the stronger or weaker the acid. b. The lower the pKa of an acid, the stronger or weaker the acid.
Which is a stronger base, S2 - or Se2 -? Explain.

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Based on charge stability, rank species A-G from weakest base to strongest base. HO. F É A В F