The stability of NH 4 + ion in the given solvent is to be explained. The ability of the solvent to solvate cation and anion is to be explained. Concept introduction: A protic solvent can solvate both cation and anion, but an aprotic solvent can solvate only cation and not anions. The protic solvent is a compound containing at least one hydrogen atom bonded to an electronegative atom of oxygen, nitrogen, or fluorine and capable of forming a hydrogen bond. The aprotic solvent is a compound which cannot form a hydrogen bond due to the lack of hydrogen atom bonded to an electronegative atom of oxygen, nitrogen, or fluorine. The polar solvent molecule has a partial negative and partial positive charge. The negative ends of the solvent’s dipole solvate the cation strongly, and the positive end of the solvent’s dipole solvate the anion strongly. When two positively charged species are present in the solution, the stronger acid is the one that is less stable.

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Chapter 6, Problem 6.86P

Interpretation Introduction

Interpretation:

The stability of NH4+ ion in the given solvent is to be explained. The ability of the solvent to solvate cation and anion is to be explained.

Concept introduction:

A protic solvent can solvate both cation and anion, but an aprotic solvent can solvate only cation and not anions. The protic solvent is a compound containing at least one hydrogen atom bonded to an electronegative atom of oxygen, nitrogen, or fluorine and capable of forming a hydrogen bond. The aprotic solvent is a compound which cannot form a hydrogen bond due to the lack of hydrogen atom bonded to an electronegative atom of oxygen, nitrogen, or fluorine. The polar solvent molecule has a partial negative and partial positive charge. The negative ends of the solvent’s dipole solvate the cation strongly, and the positive end of the solvent’s dipole solvate the anion strongly. When two positively charged species are present in the solution, the stronger acid is the one that is less stable.

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Part V. Label ad match the carbons in compounds Jane and Diane w/ the corresponding peak no. in the Spectra (Note: use the given peak no. To label the carbons, other peak no are intentionally omitted) 7 4 2 -0.13 -0.12 -0.11 -0.10 -0.08 8 CI Jane 1 -0.09 5 210 200 190 180 170 160 150 140 130 120 110 100 -8 90 f1 (ppm) 11 8 172.4 172.0 f1 (ppr HO CI NH Diane 7 3 11 80 80 -80 -R 70 60 60 2 5 -8 50 40 8. 170 160 150 140 130 120 110 100 90 -0 80 70 20 f1 (ppm) 15 30 -20 20 -60 60 -0.07 -0.06 -0.05 -0.04 -0.03 -0.02 -0.01 -0.00 -0.01 10 -0.17 16 15 56 16 -0.16 -0.15 -0.14 -0.13 -0.12 -0.11 -0.10 -0.09 -0.08 -0.07 -0.06 -0.05 -0.04 17.8 17.6 17.4 17.2 17.0 f1 (ppm) -0.03 -0.02 550 106 40 30 20 20 -0.01 -0.00 F-0.01 10 0