From owner-metabolic-reg@net.bio.net Thu Jun 13 23:00:00 1996 Path: biosci!rutgers!uwm.edu!math.ohio-state.edu!jussieu.fr!news.belnet.be!news.be.innet.net!INbe.net!news.nl.innet.net!INnl.net!hunter.premier.net!news.mathworks.com!newsfeed.internetmci.com!in1.uu.net!earth.superlink.net!news From: Eric Lucas Newsgroups: bionet.molbio.proteins,de.sci.biologie,de.sci.chemie,sci.bio.misc,sci.chem,bionet.metabolic-reg,bionet.molbio.methds-reagnts,bionet.biophysics Subject: Re: Why is solubility phe > tyr ? Date: Thu, 13 Jun 1996 21:32:14 -0500 Organization: SuperNet Inc. (908) 828-8988 Lines: 33 Message-ID: <31C0CF2D.1A50@peabody.sct.ucarb.com> References: <31B735A3.30D8@ibex.ca> <31C097E6.6008@uconnvm.uconn.edu> Reply-To: lucas@superlink.net NNTP-Posting-Host: p6.superlink.net Mime-Version: 1.0 Content-Type: text/plain; charset=us-ascii Content-Transfer-Encoding: 7bit X-Mailer: Mozilla 3.0b2 (Macintosh; I; 68K) Xref: biosci bionet.molbio.proteins:8129 sci.bio.misc:3485 sci.chem:58418 bionet.metabolic-reg:769 bionet.molbio.methds-reagnts:45712 bionet.biophysics:2113 Davy Kalonia wrote: > The free energy of solubilization (del G) depends on three factors. ... > The energy of crystallization for Tyr is much larger than that of Phe, > ie. the O..H--O interaction and stacking of the hydrophobic rings > results in stronger interaction in the solid state. Thus more energy > must be provided to move the molecules from a solid_solid state to a > solvent_solid state. Thus poor solubility for tyr. Quite correct, but it's not just hydroxy groups that have this effect; methoxy groups can have the same effect. There are several synthetic tricks that structural chemists can use to make compounds that are easier to crystallize for X-ray structural analysis. One of the tricks is to use phenyl rings; they stack beautifully. In this case, both phe and tyr have benzene rings, so that isn't it. However, beyond this, another common trick is to attach hydroxy or methoxy groups to the phenyl ring. Very often they really make for excellent crystallization, because they really increase the lattice energy. In grad school, I tried to get two rather different reactions to give crystals for quite some time. When I changed the ligands in both (very different ligands) from having a phenyl to a having a dimethoxyphenyl, I got x-ray quality, analytically pure crystals in the NMR tubes I did the reactions in. Without any effort at all. Just left em there and came in the next day, and handed the tubes to the crystallographer. The argument about hydroxy groups and hydrogen bonding makes a lot of sense. However, methoxy groups obviously don't have the same option. It's also hard for me to believe it's simple polarity--typical crystal stacking with phenyl rings is in a direction orthogonal to the benzene ring, and the dipole of a methoxyphenyl is in the plane of the ring. Any crystallographers out there have a good explanation as to why methoxy groups seem unique in making phenyl-containing compounds much more crystalline? Eric .