Anti-periplanar

In organic chemistry, anti-periplanar, or antiperiplanar, describes the A−B−C−D bond angle in a molecule. In this conformer, the dihedral angle of the A−B bond and the C−D bond is greater than +150° or less than −150°^[1] (Figures 1 and 2). Anti-periplanar is often used in textbooks to mean strictly anti-coplanar,^[2] with an A−B C−D dihedral angle of 180° (Figure 3). In a Newman projection, the molecule will be in a staggered arrangement with the anti-periplanar functional groups pointing up and down, 180° away from each other (see Figure 4). Figure 5 shows 2-chloro-2,3-dimethylbutane in a sawhorse projection with chlorine and a hydrogen anti-periplanar to each other.

Syn-periplanar or synperiplanar is similar to anti-periplanar. In the syn-periplanar conformer, the A and D are on the same side of the plane of the bond, with the dihedral angle of A−B and C−D between +30° and −30° (see Figure 2).

Figure 2: Functional groups are considered periplanar if they have a dihedral angle less than −150° or greater than +150° or −30° to +30°. Adapted from a figure by Dreamtheater published on Wikimedia Commons.^[3]

Figure 3: Representation of a strictly anti-coplanar conformation. A, B, C, and D are in the same plane and the dihedral angle between A–B and C–D is 180°.

Figure 4: Newman projection showing A and D anti-periplanar.

Figure 5: Sawhorse projection of 2-chloro-2,3-dimethylbutane showing Cl and H anti-periplanar.

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Molecular orbitals

An important factor in the antiperiplanar conformer is the interaction between molecular orbitals. Anti-periplanar geometry will put a bonding orbital and an anti-bonding orbital approximately parallel to each other, or syn-periplanar. Figure 6 is another representation of 2-chloro-2,3-dimethylbutane (Figure 5), showing the C–H bonding orbital, σ_C–H, and the C–Cl anti-bonding orbital, σ*_C–Cl, syn-periplanar. The parallel orbitals can overlap and become involved in hyperconjugation. If the bonding orbital is an electron donor and the anti-bonding orbital is an electron acceptor, then the bonding orbital will be able to donate electronegativity into the anti-bonding orbital. This filled-to-unfilled donor-acceptor interaction has an overall stabilizing effect on the molecule. However, donation from a bonding orbital into an anti-bonding orbital will also result in the weakening of both of those bonds. In Figure 6, 2-chloro-2,3-dimethylbutane is stabilized through hyperconjugation from electron donation from σ_C-H into σ*_C-Cl, but both C–H and C–Cl bonds are weakened. A molecular orbital diagram shows that the mixing of σ_C–H and σ*_C–Cl in 2-chloro-2,3-dimethylbutane lowers the energy of both the orbitals (Figure 7).

Examples of anti-periplanar geometry in mechanisms

E₂ mechanism

A bimolecular elimination reaction will occur in a molecule where the breaking carbon-hydrogen bond and the leaving group are anti-periplanar^[4]^[5]^[6]^[7] (Figure 8). This geometry is preferred because it aligns σ_C-H and σ*_C-X orbitals.^[8]^[9] Figure 9 shows the σ_C-H orbital and the σ*_C-X orbital parallel to each other, allowing the σ_C-H orbital to donate into the σ*_C-X anti-bonding orbital through hyperconjugation. This serves to weaken C-H and C-X bond, both of which are broken in an E₂ reaction. It also sets up the molecule to more easily move its σ_C-H electrons into a π_C-C orbital (Figure 10).

Pinacol rearrangement

Figure 11: Mechanism of a pinacol rearrangement. The C–C bonding orbital is aligned with the C–O anti-bonding orbital, which facilitates the methyl shift. H–A is a generic acid.

In the pinacol rearrangement, a methyl group is found anti-periplanar to an activated alcohol functional group.^[10]^[11] This places the σ_C–C orbital of the methyl group parallel with the σ*_C–O orbital of the activated alcohol. Before the activated alcohol leaves as H₂O the methyl bonding orbital donates into the C–O antibonding orbital, weakening both bonds. This hyperconjugation facilitates the 1,2-methyl shift that occurs to remove water. See Figure 11 for the mechanism.

History, etymology, and misuse

The term anti-periplanar was first coined by Klyne and Prelog in their work entitled "Description of steric relationships across single bonds", published in 1960.^[12] ‘Anti’ refers to the two functional groups lying on opposite sides of the plane of the bond. ‘Peri’ comes from the Greek word for ‘near’ and so periplanar means “approximately planar”.^[13] In their article “Periplanar or Coplanar?” Kane and Hersh point out that many organic textbooks use anti-periplanar to mean completely anti-planar, or anti-coplanar, which is technically incorrect.^[14]

References

^ Eliel, Ernest; Wilen, Samuel; Mander, Lewis (September 1994). Stereochemistry of Organic Compounds. New York: Wiley-Scientific. ISBN 978-0-471-01670-0.
^ Kane, Saul; Hersh, William (1 October 2000). "Periplanar or Coplanar?". Journal of Chemical Education. 77 (10): 1366. Bibcode:2000JChEd..77.1366K. doi:10.1021/ed077p1366.
^ Wikipedia, Dreamtheater at English (9 August 2012), English: An illustration of the syn/anti peri/clinal nomenclature of molecular torsional conformations. To be used on the page Alkane stereochemistry., retrieved 17 March 2017
^ Wade, Leroy (6 January 2012). Organic Chemistry (8th ed.). Pearson. pp. 267–268. ISBN 978-0321768414.
^ Carey, Francis; Sundberg, Richard (27 May 2008). Advanced Organic Chemistry: Part A: Structure and Mechanisms (5th ed.). Springer. pp. 558–563. ISBN 978-0387683461.
^ Deslongchamps, Ghislain; Deslongchamps, Pierre (12 May 2011). "Bent bonds, the antiperiplanar hypothesis and the theory of resonance. A simple model to understand reactivity in organic chemistry". Organic & Biomolecular Chemistry. 9 (15): 5321–5333. doi:10.1039/C1OB05393K. PMID 21687842.
^ Hunt, Ian; Spinney, Rick. "Chapter 5: Structure and Preparation of Alkenes. Elimination Reactions". Retrieved 13 March 2017.
^ Anslyn, Eric; Dougherty, Dennis (15 July 2005). Modern Physical Organic Chemistry. University Science. pp. 590–592. ISBN 978-1891389313.
^ Rzepa, Henry (4 February 2012). "An orbtial analysis of the stereochemistry of the E2 elimination reaction". Retrieved 13 March 2017.
^ Anslyn, Eric; Dougherty, Dennis (15 July 2005). Modern Physical Organic Chemistry. University Science. pp. 676–677. ISBN 978-1891389313.
^ Carey, Francis; Sundberg, Richard (30 December 2010). Advanced Organic Chemistry: Part B: Reactions and Synthesis (5th ed.). Springer. pp. 883–886. ISBN 978-0387683546.
^ Klyne, William; Prelog, Vladimir (1 December 1960). "Description of steric relationships across single bonds". Experientia. 16 (12): 521–523. doi:10.1007/BF02158433. S2CID 48829.
^ Kane, Saul; Hersh, William (1 October 2000). "Periplanar or Coplanar?". Journal of Chemical Education. 77 (10): 1366. Bibcode:2000JChEd..77.1366K. doi:10.1021/ed077p1366.
^ Kane, Saul; Hersh, William (1 October 2000). "Periplanar or Coplanar?". Journal of Chemical Education. 77 (10): 1366. Bibcode:2000JChEd..77.1366K. doi:10.1021/ed077p1366.

This page was last edited on 9 August 2023, at 12:52

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