ORGANIC CHEMISTRY I PRACTICE PROBLEMS FOR BRONSTED-LOWRY ACID-BASE CHEMISTRY

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Cody Bond
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1 RGANIC CHEMISTRY I PRACTICE PRBLEMS FR BRNSTED-LWRY ACID-BASE CHEMISTRY 1. For each of the species below, identify the most acidic proton and provide the structure of the corresponding conjugate base. You might want to draw detailed Lewis formulas in some cases. HF CH 3 CH 3 CH 3 CH 2 H CH 3 CN H 3 HC CH H 2 H 2 RNH 3 CH 3 H 2 2. For each of the species below, identify the basic atom and provide the structure of the corresponding conjugate acid. You might want to draw detailed Lewis formulas in some cases. S 4 CN _ 2 CH 3 CH 2 H CH 3 CH 2 H PhC H 2 Br NH 2

You might want to draw detailed Lewis formulas in some cases. HF CH 3 CH 3 CH 3 CH 2 H CH 3 CN H 3 HC CH H 2 H 2 RNH 3 CH 3 H 2 2.

2 3. Fill in the reactants or products for the following acid-base reactions. Keep in mind that in line-angle formulas hydrogens are not shown. When in doubt, write complete Lewis structures. Abbreviations used: Ph=phenyl (a benzene ring attached to a carbon chain) HN 3 + H 2 F + H 3 H 3 C CH 3 + H PhC + HCl H 2 C 3 + H + H 2 NH 3 + HC C H + H 4. Arrange the substances by order of acidity or basicity as indicated. You may use pka tables, periodic tables, or any other tools available to you (except for your cell phone). H 2 Se H 2 H 2 S Br F I Cl strongest base weakest base CH 4 HI PH 3 H 2 Se F H NH 2 CH 3 CH 2 CH 2 CH 2 weakest basse strongest base CH 3 CH 2 H CH 3 CH HF Benzene

Abbreviations used: Ph=phenyl (a benzene ring attached to a carbon chain) HN 3 + H 2 F + H 3 H 3 C CH 3 + H PhC + HCl H 2 C 3 + H + H 2 NH 3 + HC C H + H 4.

3 5. Circle the side favored by equilibrium in the following acid-base reactions. CN + NH 3 HCN + NH 2 H + H3 C CH 2 + H3 C CH 3 H 2 + NH 3 H 3 + NH 2 H 2 C 3 + H 2 HC 3 + H 3 CH 3 CH 2 CH 2 CH 3 + CH 2 CH 3 CH 2 CH 2 CH 2 + CH 3 6. The conjugate acid of ammonia, NH 3, is: A) NH 4 + B) NH 2 H C) NH 2 - D) none of the above 7. Methanesulfonic acid, CH 3 S 3 H, has a pk a of -7 while ethanol, CH 3 CH 2 H, has a pk a of Which is the stronger acid and what accounts for this large difference in relative acidity? 8. Would you predict trifluoromethanesulfonic acid, CF 3 S 3 H, to be a stronger or weaker acid than methanesulfonic acid, CH 3 S 3 H? Explain your reasoning. 9. Consider the species CH 3 -, NH 2 -, and CH 3 C-. Rank these ions in order of increasing basicity, and explain your rationale. 10. The K a of formic acid is 1.7 x The pk a of formic acid is. A) 1.7 B) 10.3 C) 4.0 D) 3.8 E) Provide the structure of the conjugate base of phenol (shown below) and all its resonance forms. H 12. Rank the following in order of increasing acidity: CH 3 H, HCl, NH 3, and CH Rank the following in order of increasing basicity: CH 3 -, H 2 N -, H 2, and NH 3.

The conjugate acid of ammonia, NH 3, is: A) NH 4 + B) NH 2 H C) NH 2 - D) none of the above 7. Methanesulfonic acid, CH 3 S 3 H, has a pk a of -7 while ethanol, CH 3 CH 2 H, has a pk a of 15.9.

4 14. When methanol (CH 3 H) acts as a base, its conjugate acid is. A) CH 4 H B) CH 3 H + 2 C) CH 4 + D) CH 3 - E) - CH 2 H 15. Which of the following pairs of bases lists the stronger base first? A) H 2 > H - B) H 2 N - > CH 3 C - C) CH 3 C - > H - D) I - > Cl - E) H - > H 2 N Draw the structure of the conjugate acid of acetone (CH 3 CCH 3 ).

Which of the following pairs of bases lists the stronger base first?

5 ANSWERS 1. HF F CH 3 CH 3 CH 3 CH 2 CH 3 CH 2 H CH 3 CH 3 CH 3 CN CH 2 CN H 3 H 2 HC CH HC C H 2 H H 2 H RNH 3 RNH 2 CH 3 H 2 CH 3 H 2. CN HCN CH 3 CH 3 CH 3 CH 2 H S 4 _ 2 HS 4 H H 2 CH 3 CH 2 H CH 3 CH 2 H 2 PhC PhCH H 2 H 3 Br HBr NH 2 NH 3

6 3. HN 3 + H 2 H 3 + N 3 HF + H 2 F + H 3 + H + H 2 H 3 C CH 3 H 3 C CH 2 PhCH + Cl PhC + HCl H 2 C 3 + H HC 3 + H 2 + H 2 + H NH 2 + HC CH NH 3 + HC C H + H + H 2 4. Periodic trend H 2 < H 2 S < H 2 Se Periodic trend F strongest base > Cl > Br > I weakest base Periodic trend HI > H 2 Se > PH 3 > CH 4 Periodic trend F < H < NH 2 < CH 3 CH 2 CH 2 CH 2 weakest basse strongest base pk a trend Benzene < CH 3 CH 2 H < CH 3 CH < HF

Periodic trend H 2 < H 2 S < H 2 Se Periodic trend F strongest base > Cl > Br > I weakest base Periodic

7 5. The numbers represent approximate pk a values for the substances acting as acids. CN + NH 3 HCN + NH H + H3 C CH 2 + H3 C CH H 2 + NH 3 H 3 + NH H 2 C 3 + H 2 HC 3 + H CH 3 CH 2 CH 2 CH 3 + CH 2 CH 3 CH 2 CH 2 CH 2 + CH A 7. Methanesulfonic acid is the stronger acid. The lower the pka, the stronger the acid. A lower pka is associated with a larger Ka which signifies greater dissociation. The large relative difference in acidity in this case can be most easily seen by gauging the relative basicities of the conjugate bases. The weaker the base, the stronger the corresponding conjugate acid. Methanesulfonate, CH 3 S 3 -, is considerably stabilized by resonance delocalization which is not found in ethoxide, CH 3 CH 2 -. This effect greatly reduces the basicity of methanesulfonate relative to ethoxide. Draw the Lewis formula for methanesulfonate and the resonance forms for practice. 8. Trifluoromethanesulfonic acid is a stronger acid. Compare the strengths of the conjugate bases and remember that the weaker the base, the stronger the conjugate acid. Both bases are stabilized by resonance, but in the case of the trifluoro derivative, the presence of the highly electronegative fluorine atoms serves to delocalize the negative charge to an even greater extent by the inductive effect of fluorine. This additional delocalization makes trifluoromethanesulfonate a weaker base. 9. CH 3 C- < CH 3 - < NH 2 - first factor to consider is the nature of the atom which bears the negative charge. The more electronegative the atom that bears the negative charge, the more stable the

A lower pka is associated with a larger Ka which signifies greater dissociation.

8 anion. Stable anions are less reactive and are hence weaker bases. Since is more electronegative than N, the NH 2 - is the strongest base in the set. In the remaining two species, the negative charge is on the, but in the case of CH 3 C-, the negative charge is also delocalized by resonance. 10. D 11. See class notes, or p. 417 of the Wade textbook, for all the resonance structures of the phenoxide ion shown below. (see p. 429 for 4 more resonance resonance structures) structures 12. CH 4 < NH 3 < CH 3 H < HCl (periodic trend) 13. H 2 < NH 3 < CH 3 - < H 2 N - Negatively charged ions are stronger bases than neutral counterparts. A table of pk a values will further aid in deciding the final order of basicity. 14. B 15. B 16. H H 3 C CH 3

417 of the Wade textbook, for all the resonance structures of the phenoxide ion shown below. (see p. 429 for 4 more resonance resonance structures) structures 12.

Chapter 2 - Polar Covalent Bonds; Acids and Bases

Chapter 2 - Polar Covalent Bonds; Acids and Bases For questions 1-10 give the letter of the term that best matches the given definition. a. Brønsted-Lowry Acid f. Ionic Bond b. Brønsted-Lowry Base g. Covalent