Anti-periplanar
In organic chemistry, anti-periplanar, or antiperiplanar, describes the bond angle in a molecule. In this conformer, the dihedral angle of the bond and the bond is greater than +150° or less than −150° (Figures 1 and ). Anti-periplanar is often used in textbooks to mean strictly anti-coplanar, with an 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 and between +30° and −30° (see Figure 2). 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, and the C–Cl anti-bonding orbital, σ*, 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 into σ*, but both C–H and C–Cl bonds are weakened. A molecular orbital diagram shows that the mixing of σ and σ* in 2-chloro-2,3-dimethylbutane lowers the energy of both the orbitals (Figure 7). Examples of anti-periplanar geometry in mechanisms. E mechanism. A bimolecular elimination reaction will occur in a molecule where the breaking carbon-hydrogen bond and the leaving group are anti-periplanar (Figure 8). This geometry is preferred because it aligns σ and σ* orbitals. Figure 9 shows the  σ orbital and the σ* orbital parallel to each other, allowing the σ orbital to donate into the σ* anti-bonding orbital through hyperconjugation. This serves to weaken C-H and C-X bond, both of which are broken in an E reaction. It also sets up the molecule to more easily move its σ electrons into a π orbital (Figure 10). Pinacol rearrangement. In the pinacol rearrangement, a methyl group is found anti-periplanar to an activated alcohol functional group. This places the σ orbital of the methyl group parallel with the σ* orbital of the activated alcohol. Before  the activated alcohol leaves as HO 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. ‘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”. 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.