1. Figure Number: 08-00CO
Title: Protonated 1,3-Butadiene
Caption: Electrostatic potential map for carbocation formed by protonating 1,3-butadiene.
Notes: 1,3-Butadiene protonated at carbon 1 is an allylic cation. Protonation removes carbon 1 from the pi system. Note that the positive charge is delocalized between carbons 2 and 4. Carbons 1 and 3 are more greenish in color than carbons 2 and 4, indicating that little positive charge resides on carbons 1 and 3. Nucleophiles are attracted to positive charge on either carbon 2 or carbon 4, depending on reaction conditions.

2. Figure Number: UN
Title: Naming Alkenynes
Caption: Three named examples of alkenynes.
Notes: When naming a compound with both a double bond and a triple bond, the longest chain has to flow through both pi systems, and the carbons have to be numbered so that either the alkene or the alkyne has the lowest possible number regardless of which functional group gets the lower number. The alkene function precedes the alkyne function in the name.

3. Figure Number: T01
Title: Table 8.1 Priorities of Functional Group Suffixes
Caption:
Notes:

4. Figure Number: T02
Title: Table 8.2 Carbon-carbon single bond on hybridization of orbitals
Caption:
Notes:

5. Figure Number: 08-01
Title: Figure 8.1
Caption: Bonding MOs in allene and structures of the two enantiomers of 2,3-pentadiene (separated by mirror), which is an allenic system.
Notes: The pi MOs in allenic systems are perpendicular to one another. They therefore do not overlap one another, and allenic systems have MOs like two isolated double bonds. Since the MOs are perpendicular to one another, allenic systems are not planar, and functional groups attached to their outer carbons do not lie cis and trans to one another, but are oriented in perpendicular planes. This situation gives rise to enantiomers in molecules like 2,3-pentadiene.

6. Figure Number: UN
Title: Protonated 1,3-Butadiene
Caption: Electrostatic potential map for carbocation formed by protonating 1,3-butadiene.
Notes: 1,3-Butadiene protonated at carbon 1 is an allylic cation. Protonation removes carbon 1 from the pi system. Note that the positive charge is delocalized between carbons 2 and 4. Carbons 1 and 3 are more greenish in color than carbons 2 and 4, indicating that little positive charge resides on carbons 1 and 3. Nucleophiles are attracted to positive charge on either carbon 2 or carbon 4, depending on reaction conditions.

7. Figure Number: 08-02
Title: Figure 8.2
Caption: Reaction coordinate diagram for the addition of HBr to 1,3-butadiene.
Notes: Addition in a 1,4 manner is thermodynamically controlled, since the 1,4-addition product is more stable than the 1,2-addition product. Internal alkenes are more stable than terminal alkenes. Addition in a 1,2 manner is kinetically controlled, since the 1,2-addition product is formed from the carbocation intermediate faster than the 1,4-addition product. Reaction conditions which allow the reverse reaction to occur allow the system to come to equilibrium, favoring 1,4 addition. Conditions which inhibit the reverse reaction favor 1,2 addition because this product is initially formed in greater amounts.

8. Figure Number: 08-03
Title: Figure 8.3
Caption: Structures and electrostatic potential maps of ethene, propenal, and propenenitrile.
Notes: Electron-withdrawing groups attached to double bonds decrease the electron density in the double bond, shifting its color in a potential map from yellowish to greenish to bluish.

9. Figure Number: 08-04
Title: Figure 8.4
Caption: The Diels–Alder reaction results from in-phase overlap of the HOMO of the diene with the LUMO of the diene or vice-versa. Initially, electrons are absorbed from the HOMO of one partner into the LUMO of the other.
Notes: In Diels–Alder reactions of dienes and dienophiles which do not have strongly electron-withdrawing or electron-donating groups attached, the Diels–Alder reaction prefers to transfer electrons from the HOMO of the diene to the LUMO of the dienophile, since these are closer in energy to one another than the LUMO of the diene and the HOMO of the dienophile. Substituting strongly electron-withdrawing groups on the diene lowers the energy of its HOMO, and substituting strongly electron-donating groups on the dienophile raises the energy of its LUMO. Doing both of these substitutions increases the energy difference between the HOMO of the diene and the LUMO of the dienophile, resulting in reactions involving the LUMO of the diene and the HOMO of the dienophile.

10. Figure Number: 08-05
Title: Figure 8.5
Caption: Relative energies of bonding and antibonding sigma and pi orbitals, and nonbonding (n) orbitals.
Notes: Electronic transitions are named according to the kinds of orbitals involved in these transitions (e.g., n --> p*, or p --> p*).

11. Figure Number: 08-06
Title: Figure 8.6
Caption: The UV spectrum of acetone.
Notes: The pi bond between carbon and oxygen in acetone and the presence of nonbonding electrons on the oxygen atom of this species makes n --> p* (274 nm) and p --> p* (195 nm) electronic transitions observable in the UV spectrum.

12. Figure Number: T03
Title: Table 8.3 Ethylene and conjugated dienes
Caption:
Notes:

13. Figure Number: 08-08
Title: Figure 8.8
Caption: Nitroethane anion formation can be monitored by UV at 240 nm.
Notes: The rate of proton removal from nitroethane can be measured by monitoring the nitroethane anion formed by the reaction.

14. Figure Number: 08-09
Title: Figure 8.9
Caption: Pyruvate concentration can be monitored by UV at 340 nm.
Notes: The rate of reduction of pyruvate by NADH can be measured by monitoring pyruvate disappearance at 340 nm.

15. Figure Number: 08-10
Title: Figure 8.10
Caption: The absorbance of an aqueous solution of phenol at 287 nm as a function of pH.
Notes: The absorption at 287 nm is due to the presence of phenoxide ion (the conjugate base of phenol). When half of the phenol has been converted into phenoxide, the concentrations of phenol and phenoxide are equal. At this point, pH = pKa.

16. Figure Number: 08-11
Title: Figure 8.11
Caption: The absorbance of a solution of DNA at 260 nm as a function of the temperature of the solution.
Notes: Single-stranded DNA absorbs at 260 nm because nonbonding electrons on nitrogen atoms, which are normally tied up in hydrogen bonding together complementary strands of DNA, are free to undergo n --> p* transitions in single-stranded DNA. When the temperature has risen to the point that half of the DNA is single-stranded, DNA is said to be at its "melting" temperature, Tm.

17. Figure Number:
Title: Table 8.4  Dependence of the Color Observed on the Wavelength
of Light Absorbed
Caption:
Notes:

18. Figure Number: T01
Title: Table 8.1 Priorities of Functional Group Suffixes
Caption:
Notes:

19. Figure Number: T02
Title: Table 8.2 Carbon-carbon single bond on hybridization of orbitals
Caption:
Notes:

20. Figure Number: T03
Title: Table 8.3 Ethylene and conjugated dienes
Caption:
Notes: