Organic ChemistryMain MenuLecture 1: Introduction to Molecular OrbitalsLecture 10: Intermolecular Forces and Intro to ReactivityLecture 11: Alkenes as Nucleophiles ILectures 12 and 13: Alkenes II & IIILecture 14: Benzenes as Nucleophiles ILecture 15 objectives and skillsLecture 2: Molecular Orbitals in Organic StructuresLecture 3: Molecular Orbitals and ResonanceLecture 4: Molecular Orbitals and AromaticityLecture 5: Nomenclature and IR SpectroscopyLecture 6: Stereochemistry ILecture 7: Stereochemistry IILecture 8: Newman and Fisher ProjectionsLecture 9: Conformations and Cyclohexane RingsJulio Terra2fb22914f73f9e5a767bf7fb83987dca0e153e4a
SOLUTION E10.3c
12020-03-01T15:42:03-08:00Julio Terra2fb22914f73f9e5a767bf7fb83987dca0e153e4a359922plain2020-03-01T15:43:06-08:00Julio Terra2fb22914f73f9e5a767bf7fb83987dca0e153e4aBoth protonated amines with double bonds have resonance stabilization of their conjugate bases (the neutral amine species), which makes them stronger acids than the other two. The species with two double bonds would be aromatic as the neutral amine (conjugate base), which makes it the weakest of the bases, and thus, its protonated amine is the strongest acid. The weakest acid is the neutral amine, as its conjugate base would be an anion, relative to the rest which have neutral amines as conjugate bases.
Identify the conjugate acid and conjugate base in each of the following pairs of compounds. Draw the Lewis structures of each species and add necessary formal charges. SOLUTION
(CH3)2CHNH2 and [(CH3)2CHNH]-
CH3CO2H and [CH3CO2]-
[CH3]- and CH4
Identify each of the following as Lewis acid or Lewis base: (CH3)3COH, NH3, [CH2COCH3]-, and H2O. SOLUTION
Rank the following from least acidic to most acidic. SOLUTION
