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- 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)3. Rank the hydrogens in bold in the following molecules in order of their acidity. Rank the most acidic first down to the least acidic. I > ty > IV > 161 I H II H H III IV HIndicate which is the weaker base and explain why. Be specific! NH3 or NF3
- Which of the following bases has a conjugate acid with the smallest pKa? Select one: O (CH_CH,CH),N O NH, O CH,CH,CH,NH, O (CH,CH,CH,), NHWithout reference to a pKa table, decide which compound in each pair is the stronger acid. (see attachment)Which of the following has the lowest pka value? Hint: a methyl group is an electron donating group which can destabilize the negative charge of the conjugate base. * I CH,COOH I HCOOH 1 (CH),CH – COOH II CH,CH,COH IV
- 5. Which of these compounds would you expect to be a stronger base, and why? Hint: draw resonance structures to explain. O₂N NH₂ NH₂ O₂NWhich site do you think is the most acidic? Note that this is not a complete Lewis structure-you need to think about where the electrons are and how positive the hydrogens are. -H HWhich is the least stable base? (F-, Cl-, Br-, and I-)
- Rank the following in order of decreasing basicity. You may use analogous structures in a table of acidity constants to guide your reasoning. Be sure to answer all parts. Drag each item to the correct box. Most basic ☐ ? de Least basicFigine CH3 too CH₂ CH3 A 5-6 to NI H₂ No B CH3 CH₂ с CH3 O=C OHow to determine which molecule is a stronger base?
