University:
Kentucky State University
Course:
CHE 302 | Organic Chemistry II
Academic year:

2022
Views:

342

Pages:

41
Author:

Nicole Wang

14. Conjugated Compounds and Ultraviolet Spectroscopy Conjugated and Nonconjugated Dienes ◼ Compounds can have more than one double or triple bond ◼ If they are separated by only one single bond they are conjugated and their orbitals interact ◼ The conjugated diene 1,3-butadiene has properties that are very different from those of the nonconjugated diene, 1,5-pentadiene Why this Chapter? ◼ Conjugated compounds are common in nature ◼ Extended conjugation leads to absorption of visible light, producing color ◼ Conjugated hydrocarbon with many double bonds are polyenes (lycopene is responsible for red color in tomatoes) ◼ Examine properties of conjugated molecules and reasons for the properties Preparation of conjugated dienes ◼ Typically by elimination in allylic halide ◼ Specific industrial processes for large scale production of commodities by catalytic dehydrogenation and dehydration Simple conjugated dienes used in polymer synthesis include 1,3butadiene, chloroprene (2-chloro-1,3-butadiene), and isoprene (2-methyl1,3-butadiene). Properties of conjugated systems ◼ One of the properties that distinguishes conjugated from nonconjugated dienes is that the central single bond is shorter than might be expected. Measuring Stability ◼ Conjugated dienes are more stable than nonconjugated based on heats of hydrogenation ◼ Hydrogenating 1,3-butadiene produces 16 kJ/mol less heat than 1,4-pentadiene What accounts for the stability of conjugated dienes? ◼ According to valence bond theory the stability is due to orbital hybridization. Thus, the “extra” stability of a conjugated diene results in part from the greater amount of s character in the orbitals forming the C - C single bond. What accounts for the stability of conjugated dienes? According to molecular orbital theory, the stability of a conjugated diene arises because of an interaction between the p orbitals of the two double bonds. What accounts for the stability of conjugated dienes? ◼ In a conjugated diene, the lowest energy π MO (ψ1) has a favorable bonding interaction between C2 and C3 that ◼ is absent in a nonconjugated diene. ◼ As a result, there is a certain amount of ◼ double-bond character to the C2–C3 bond, making that bond both stronger and shorter than a typical single bond. Molecular Orbital Description of 1,3-Butadiene ◼ The single bond between the conjugated double ◼ ◼ ◼ ◼ bonds is shorter and stronger than sp3 The bonding -orbitals are made from 4 p orbitals that provide greater delocalization and lower energy than in isolated C=C The 4 molecular orbitals include fewer total nodes than in the isolated case (See Figures 14-1 and 14-2) In addition, the single bond between the two double bonds is strengthened by overlap of p orbitals In summary, we say electrons in 1,3-butadiene are delocalized over the  bond system ◼ Delocalization leads to stabilization 14.2 Electrophilic Additions to Conjugated Dienes: Allylic Carbocations ◼ Review: addition of electrophile to C=C ◼ Markovnikov regiochemistry via more stable carbocation Carbocations from Conjugated Dienes ◼ Addition of H+ leads to delocalized secondary allylic carbocation Products of Addition to Delocalized Carbocation ◼ Nucleophile can add to either cationic site ◼ The transition states for the two possible products are not equal in energy 14.3 Kinetic vs. Thermodynamic Control of Reactions ◼ At completion, all reactions are at equilibrium and the relative concentrations are controlled by the differences in free energies of reactants and products (Thermodynamic Control) ◼ If a reaction is irreversible or if a reaction is far from equilibrium, then the relative concentrations of products depends on how fast each forms, which is controlled by the relative free energies of the transition states leading to each (Kinetic Control) Kinetic and Thermodynamic Control Example ◼ Addition to a conjugated diene at or below room temperature normally leads to a mixture of products in which the 1,2 adduct predominates over the 1,4 adduct ◼ At higher temperature, product ratio changes and 1,4 adduct predominates 14.4 The Diels-Alder Cycloaddition Reaction ◼ Conjugate dienes can combine with alkenes to form six-membered cyclic compounds ◼ The formation of the ring involves no intermediate (concerted formation of two bonds) ◼ Discovered by Otto Paul Hermann Diels and Kurt Alder in Germany in the 1930’s View of the Diels-Alder Reaction ◼ Woodward and Hoffman showed this shown to be an example of the general class of pericyclic reactions ◼ Involves orbital overlap, change of hybridization and electron delocalization in transition state ◼ The reaction is called a cycloaddition 14.5 Characteristics of the DielsAlder Reaction ◼ The alkene component is called a dienophile ◼ ◼ C=C is conjugated to an electron withdrawing group, such as C=O or CN Alkynes can also be dienophiles Stereospecificity of the Diels-Alder Reaction ◼ The reaction is stereospecific, maintaining relative relationships from reactant to product ◼ There is a one-to-one relationship between stereoisomeric reactants and products Regiochemistry of the Diels-Alder Reaction ◼ Reactants align to produce endo (rather than exo) product ◼ ◼ endo and exo indicate relative stereochemistry in bicyclic structures Substituent on one bridge is exo if it is anti (trans) to the larger of the other two bridges and endo if it is syn (cis) to the larger of the other two bridges Conformations of Dienes in the Diels-Alder Reaction ◼ The relative positions of the two double bonds in the diene are “cis” or “trans” to each other about the single bond (being in a plane maximizes overlap) ◼ These conformations are called s-cis and s-trans (“s” stands for “single bond”) ◼ Dienes react in the s-cis conformation in the DielsAlder reaction ◼ Two examples of dienes that can’t adopt an s-cis conformation, and thus don’t undergo Diels–Alder reactions, are shown in the following Figure Diels-Alder reaction in biosystem 14.6 Diene Polymers: Natural and Synthetic Rubbers ◼ Conjugated dienes can be polymerized ◼ The initiator for the reaction can be a radical, or an acid ◼ Polymerization: 1,4 addition of growing chain to conjugated diene monomer Natural Rubber ◼ A material from latex, in plant sap ◼ In rubber repeating unit has 5 carbons and Z stereochemistry of all C=C ◼ Gutta-Percha is natural material with E in all C=C ◼ Looks as if it is the head-to-tail polymer of isoprene (2-methyl-1,3-butadiene) Synthetic Rubber ◼ Chemical polymerization of isoprene does not produce rubber (stereochemistry is not controlled) ◼ Synthetic alternatives include neoprene, polymer of 2-chloro-1,3-butadiene ◼ This resists weathering better than rubber Vulcanization ◼ Natural and synthetic rubbers are too soft to be used in products ◼ Charles Goodyear discovered heating with small amount of sulfur produces strong material ◼ Sulfur forms bridges between hydrocarbon chains (cross-links) 14.7 Structure Determination in Conjugated Systems: UV Spectroscopy Techniques of structure determination applicable to all organic molecules. 14.7 Structure Determination in Conjugated Systems: UV Spectroscopy 14.7 Structure Determination in Conjugated Systems: UV Spectroscopy ◼ Conjugated compounds can absorb light in the ultraviolet region of the spectrum ◼ The electrons in the highest occupied molecular orbital (HOMO) undergo a transition to the lowest unoccupied molecular orbital (LUMO) ◼ The region from 2 x 10-7m to 4 x 10-7m (200 to 400 nm) is most useful in organic chemistry ◼ A plot of absorbance (log of the ratio of the intensity of light in over light transmitted) against wavelength in this region is an ultraviolet spectrum – see Figure 14-11 Ultraviolet Spectrum of 1,3-Butadiene ◼ Example: 1,3-butadiene has four  molecular orbitals with the lowest two occupied ◼ Electronic transition is from HOMO to LUMO at 217 nm (peak is broad because of combination with stretching, bending) Quantitative Use of UV Spectra ◼ Absorbance for a particular compound in a specific solvent at a specified wavelength is directly proportional to its concentration ◼ You can follow changes in concentration with time by recording absorbance at the wavelength ◼ Beers’ law: absorbance = ecl ◼ “e” is molar absorptivity (extinction coefficient) ◼ “c” is concentration in mol/L ◼ “l” is path of light through sample in cm 14.8 Interpreting UV Spectra: The Effect of Conjugation ◼ max: wavelength where UV absorbance for a compound is greatest ◼ Energy difference between HOMO and LUMO decreases as the extent of conjugation increases ◼ max increases as conjugation increases (lower energy) ◼ 1,3-butadiene: 217 nm, 1,3,5-hexatriene: 258 nm ◼ Substituents on  system increase max ◼ See Table 14-2 14.9 Conjugation, Color and the Chemistry of Vision ◼ Visible region is about 400 to 800 nm ◼ Extended systems of conjugation absorb in visible region ◼ b-Carotene, 11 double bonds in conjugation, max = 455 nm ◼ Visual pigments are responsible for absorbing light in eye and triggering nerves to send signal to brain

14. Conjugated Compoundsand Ultraviolet Spectroscopy

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