Histidine–Serine Models
FULL PAPER
that the Ser–His dyad is less sequestered to solvent than the His–
Asp counterpart. In the solid phase, NMR spectroscopic studies (see
reference [6]) recently confirmed what X-ray snapshots (see refer-
ence [7]) seemed to point out: the Ser–His intramolecularly bonded
microscopic state does not seem to be sufficiently populated to be
macroscopically observed. For NMR spectroscopic studies, see:
b) K. Coffman Haddad, J. L. Sudmeier, D. A. Bachovchin, W. W.
Bachovchin, Proc. Natl. Acad. Sci. USA 2005, 102, 1006–1011; for
X-ray studies, see: c) E. S. Radisky, J. M. Lee, C.-J. K. Lu, D. E., Jr.
tꢆnez, P. N. Romasanta, G. Y. Buldain, A. K. Chattah, J. Org. Chem.
2010, 75, 3208–3213; d) X, Sun, J. Qiu, S. A. Strong, L. S. Green,
J. W. F. Wasley, J. P. Blonder, D. B. Colagiovanni, S. C. Mutka, A. M.
Stout, J. P. Richards, G. J. Rosenthal, Bioorg. Med. Chem. Lett. 2011,
21, 5849–5853; e) direct synthesis between imidazole and formalde-
hyde activated by microwave: S. Lupsor, F. Aonofriesei, M. Iovu,
[13] I. M. McDonald, I. M. Buck, D. J. Dunstone, I. D. Linney, M. J.
Pether, J. Spencer, K. I. M. Steel, P. Tisselli, P. T. Wright, R. A. D.
Hull, C. Austin, E. A. Harper, E. Griffin, S. B. Kalindjian, C. M. R.
Low PCT Int. Appl. 2006, WO 2006-GB2042 20060602.
[14] a) D. J. Chadwick, R. I. Ngochindo, J. Chem. Soc. Perkin Trans. 1
1984, 3, 481–486; b) A. J. Carpenter, D. J. Chadwick, Tetrahedron
midazole: R. J. Sundberg, P. V. Nguyen, Med. Chem. Res. 1997, 7,
123–136.
[4] In 1982, Steitz and Shulman reviewed the X-ray crystal structures
and NMR spectroscopic data on serine proteases and confirmed
early conclusions: the His–Ser hydrogen bond does not seem to
exist in resting enzymes but must form upon complexation with sub-
strates. Bachovchin recently addressed this question by carrying out
equivalent 15N NMR spectroscopic studies on enzyme crystals and
found that there was no His–Ser hydrogen bond in the crystal (see
reference [3]). In fact, as crystals were routinely made in high
Li2SO4 solutions, a sulfate ion was bound in the active site between
His and Ser, thereby raising the pKa of His such that it is protonated
even at high pH in crystals and therefore unable to hydrogen bond
to Ser195. This result was recently confirmed by ultra-high resolu-
tion X-ray studies (see reference [3c]).
[6] Such as reducing the effective molarity by displaying various resi-
dues in optimal positions on a macromolecular flexible scaffold, ac-
tivating the reactive partners through general acid–base catalysis,
stabilizing various transition states with the help of an oxyanion
hole, desolvating the reactive entities, and so on.
[7] Qualitatively, the fundamental mechanism of enhancing the nucleo-
philic power of any given oxygen atom is to enhance the electron
density of the nucleophilic lone pair. This leads to two molecular
strategies of generating increased electron density in the reactant
state by altering the coordination and/or bonding of the nucleophile.
The first one is desolvation, or more precisely the stripping of hy-
drogen-bond donors to the nucleophilic lone pair. The second one
consists of coordinating the alcohol proton (i.e., hydrogen bonding
to a general base that might ultimately lead to its ionization). In ad-
dition to these two mechanisms, an electric field generated at the
active site can polarize a bond to the nucleophile, thereby enhancing
its nucleophilicity. Consequently, the physical properties of the
active site (dielectric constant, dipolar moment, permeability toward
water, and so forth) are of crucial importance to the activation of
the reactive partners. For an extensive review on this topic, see:
[8] V. T. DꢄSouza, M. L. Bender, Acc. Chem. Res. 1987, 20, 146–152.
[9] In particular, intramolecularly activated acylation reactions were ob-
served and monitored on 2- and 4-hydroxymethylimidazoles that
bear various substituents on the heterocycle, whereas the corre-
sponding analogues that lack the alcohol moiety failed to intermo-
lecularly induce the acyl transfer on water or ethanol. For more de-
tails, see: a) V. Somayaji, K. I. Skorey, R. S. Brown, R. G. Ball, J.
[16] a) The reactive medium was subsequently neutralized at low temper-
ature to avoid the formation of the aldehyde (resulting from double-
bond migration) as the major product; b) G. Bridger, A. Kaller, C.
Harwig, R. Skerlj, D. Bogucki, T. R. Wilson, J. Crawford, E. J.
McEachern, B. Atsma, S. Nan, Y. Zhou, D. Schols, C. D. Smith,
M. R. Di Fluri, US Patent US2004/19058A1, 2004.
[17] a) O. Thillaye du Boullay, E. Marchal, B. Martin-Vaca, F. P. Cossio,
have also been shown to promote efficiently the ROP of lacOCA:
duelle, B. Martin-Vaca, F. P. Cossio, D. Bourissou, Chem. Eur. J.
[18] The unsaturation of the side chain is expected to alter the nucleo-
philicity of the alcohol moiety. In fact, measurements on primary
amines have revealed the following order of nucleophilicity:
ꢀ
MeNH2 >H2C=CH CH2NH2 ꢁEtNH2 >CH CCH2NH2. For more
[19] The remaining 20% correspond to higher oligomers. On the basis of
k values, the theoretical ratio is 36:44.
[20] Whereas the intermolecular constant can be roughly evaluated by
using Hunterꢄs model detailed in reference [10a], the ratio of intra-
molecular binding constants was deduced from the calculations of
the Gibbs enthalpy of the corresponding bonded states (see below
and the Supporting Information).
[21] For the trimolecular scenario 4+MeOH+7: d[LacOMe]/c0dt=
kM[ImOH]/c0[MeOH]/c0[LacOCA]/c0, whereas the bimolecular sce-
nario 4+7 follows: d[ImOMe]/c0dt=kI[ImOH]/c0[LacOCA]/c0, with
[MeOH] being approximately constant and roughly equal to
90c7(t=0), the resulting rate gives: d[LacOMe]/d[LacOMe]=kM/
kI [MeOH]ꢂ90c7(t=0)/c0 =k’c7(t=0). For more details, see the Sup-
porting Information.
3836; b) S. Anderson, H. L. Anderson, J. K. M. Sanders, J. Chem.
[23] H. Adams, E. Chekmeneva, C. A. Hunter, M. C. Misuraca, C. Nav-
theless, such an evolution was reported to be a general trend for
ortho, meta, or para-hydroxyalkyl structures, whereas for the latter,
IMHB is clearly geometrically inaccessible. Such a tendency could
therefore not be directly attributed exclusively to the IMHB
strength because it is subjected to electronic parameters such as a
through-bond inductive effect of the OH group.
which translates into Kinter =0.088m.
,
[11] V. M. Krishnamurthy, V. Semetey, P. J. Bracher, N. Shen, G. M.
[12] a) S. Sahli, B. B. Stump, T. Welti, W. B. Schweizer, F. Diederich, D.
707–730; b) M. L. Quan, P. Y. S. Lam, Q. Han, D. J. P. Pinto, M. Y.
He, R. Li, C. D. Ellis, C. G. Clark, C. A. Teleha, J.-H. Sun, R. S.
[25] A linear relationship was actually found between log(kmax) (with
kmax being the kinetic constant for ring opening of a strained tricyclic
anilide) and pKa value. See reference [30d,e].
Chem. Eur. J. 2013, 00, 0 – 0
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