Answered: 13a-c Use the following picture for the… | bartleby

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 45CTQ

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Chemistry
this is organic chem. i got these questions
wrong
13a-c Use the following picture for the next few questions.
R
NH2
How many nitrogen atoms have:
Delocalized electron pairs
Localized electron pairs
H-
-N
A.
Which nitrogen is the strongest Lewis base? Place either A, B, or C in the box
B.

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Several acids and their respective equilibrium constants are: Which is the strongest acid? Which is the weakest acid? Which acid has the weakest conjugate base? Which acid has the strongest conjugate base?
Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize-excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid—base pairs.
Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4
5. Given the general equation illustrating the reaction of the acid HA in water, HA(aq)+H2O(l)H3O+(aq)+A(aq)explain why water is considered a base in the Brønsted-Lowry model.
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: NaHSO3, NaHSeO3, NaHSO4. (b) basicity: BrO2-, ClO2-,IO2-. (c) acidity: HOCI, HOBr, HOI. (d) acidity: HOCl, HOClO, HOClO2, HOClO3. (e) basicity: NH2-, HS-, HTe-, PH2-. (f) basicity: BrO-, BrO2-, Bro3-, BrO4-
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
The following reactions illustrate Brnsted acid-base behavior. Complete each equation. a.HI(aq)+?H3O+(aq)+I(aq) b.NH3(l)+?NH4++NH2 c.H2C2O4(aq)+H2O(l)?+HC2O4(aq) d.H2N2O2(aq)+H2O(l)H3O+(aq)+? e.?+H2O(l)H3O+(aq)+CO32(aq)
Of the hydrogen halides, only HF is a weak acid. Give a possible explanation.
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.
Rank the following acids (M=0.10)in order of decreasing[ H+ ]: HFHCl HCN HCIO

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