R. Centore et al. / Inorganica Chimica Acta 358 (2005) 2112–2116
2115
˚
H22ꢁ ꢁ ꢁBr2 = 3.03 A) and in the range reported in the lit-
erature [12c,13], so it is reasonable to think that this
interaction could play a role in stabilizing II with respect
to I. A further experimental finding, not in contrast with
this picture, consists in the observation that in all five-
coordinated Pt(II) olefin complexes reported in the liter-
ature, which give this type of stereoisomerism and have
one halogen as axial ligand, and for which both rota-
mers have been observed in solution, the most abundant
rotamer is the one having more olefin hydrogens from
the side of the halogen ligand [2d,2e,2f].
Finally, we think that the possible implications that
the interaction Calkene–Hꢁ ꢁ ꢁX (X = halogen) could play
in some important catalytic processes, whose key step
involves coordination of an olefin molecule to alkyl-hal-
ogen complexes of low valence transition elements, are
worth of being investigated.
Fig. 3. X-ray molecular structure of II. Thermal ellipsoids are drawn
at 30% probability level. The chloroform solvent molecule is not
˚
shown for clarity. Selected bond lengths (A), bond angles (°) and
torsion angles (°): Pt–N1 2.190(7), Pt–N2 2.189(7), Pt–Se 2.461(3), Pt–
Br 2.518(3), C21–C22 1.48(1), C21–C23 1.49(1), C22–C25 1.46(1), N1–
Pt–N2 75.5(3), Se–Pt–N1 88.4(2), Se–Pt–N2 91.0(2), Se–Pt–Br
177.17(4), Pt–Se–C15 106.8(3), C20–C15–Se–Pt ꢀ99.9(9), N2–Pt–Se–
C15 ꢀ9.6(4), C22–C21–C23–O1 86(1), C21–C22–C25–O3 2(2).
Acknowledgements
at the X-ray molecular structure of the rotamers (Figs. 2
and 3), no relevant difference is found in the pattern of
bond lengths and angles, as well as in the coordination
sphere of the metal, as already noted, so the different
stability should probably derive from secondary, non-
bonded interactions. In particular, we have noted above
that the relative position of the p conjugated systems of
the phenyl and of the heteroaromatic chelate ligand is
almost the same in the two rotamers and no feature of
steric encumbrance is evident in the two compounds
so as to allow for their different stability. In this respect,
we observe that any different effect of steric crowding be-
tween I and II should necessarily involve contacts
among olefin substituents and the axial ligands; how-
ever, van der Waals radii of Br and Se are very close
Financial support of MIUR of Italy is acknowledged.
We thank the CIMCF of the University of Naples
‘‘Federico II’’ for the Nonius X-ray equipment.
References
[1] (a) V. De Felice, M. Funicello, A. Panunzi, F. Ruffo, J. Organomet.
Chem. 403 (1991) 243;
(b) V.G. Albano, G. Natile, A. Panunzi, Coord. Chem. Rev. 133
(1994) 67.
[2] (a) H. van der Poel, G. van Koten, Inorg. Chem. 20 (1981) 2950;
(b) M.E. Cucciolito, V. De Felice, A. Panunzi, A. Vitagliano,
Organometallics 8 (1989) 1180;
˚
(1.85 and 1.90 A [11]).
(c) V.G. Albano, C. Castellari, M.E. Cucciolito, A. Panunzi, A.
Vitagliano, Organometallics 9 (1990) 1269;
Actually, a possibly relevant feature is that in the
most stable rotamer the two olefin hydrogens are from
the same side of the bromine atom with respect to the
equatorial plane.
(d) S. Bartolucci, P. Carpinelli, V. De Felice, B. Giovannitti, A.
De Renzi, Inorg. Chim. Acta 197 (1992) 51;
(e) M.L. Ferrara, I. Orabona, F. Ruffo, V. De Felice, J.
Organomet. Chem. 519 (1996) 75;
Recently, it has been recognized that metal bound
halogens (M–X with M transition metal) are very good
hydrogen bonding acceptors [12], while C–H hydrogens
are considered as weak hydrogen bonding donors [12c].
Several cases of ‘‘weak’’ C–Hꢁ ꢁ ꢁX (X = halogen) hydro-
gen bonding have been recently reported [13]. This inter-
action has been found to play roles in crystal
engineering [13a–b] and in stereoselective synthesis
[13c–e]. In the present case, although the angles
(f) F. Giordano, F. Ruffo, A. Saporito, A. Panunzi, Inorg. Chim.
Acta 264 (1997) 231.
[3] (a) V.G. Albano, M. Monari, I. Orabona, A. Panunzi, F. Ruffo,
J. Am. Chem. Soc. 123 (2001) 4352;
(b) A. Panunzi, G. Roviello, F. Ruffo, Organometallics 21 (2002)
3503.
[4] V.G. Albano, M. Monari, V. De Felice, G. Roviello, F. Ruffo,
Eur. J. Inorg. Chem. (2005), in press.
`
[5] R. Centore, CELLFIT, Universita di Napoli ’’Federico II’’,
Napoli, Italy, 2002.
[6] G.M. Sheldrick, SHELX-97, University of Go¨ttingen, Go¨ttingen,
Germany, 1997.
C
alkene–Hꢁ ꢁ ꢁBr (97° and 101°) and Pt–Brꢁ ꢁ ꢁH (55° and
57°) are smaller as compared with the values reported
in the literature for intermolecular bonding [12c]
(we note, however, that these angles are somewhat
constrained by the intramolecular nature of the con-
tact), nevertheless the distances Brꢁ ꢁ ꢁH are close to the
[7] (a) J. Chatt, L.A. Duncanson, J. Chem. Soc. (1953) 2959;
(b) P. Corradini, C. Pedone, A. Sirigu, Chem. Commun. (1966)
341;
(c) F.R. Hartley, Angew. Chem., Int. Ed. Engl. 11 (1972) 596;
(d) F.R. Hartley, J. Organomet. Chem. 216 (1981) 277.
[8] Z. Urbanczyk-Lipkowska, P. Gluzinsky, Supramol. Chem. 7
(1996) 113.
˚
sum of van der Waals radii (H21ꢁ ꢁ ꢁBr1 = 2.88 A,