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1 Introductory article Water: Structure and Article Contents Properties . Introduction Kim A Sharp, E. R. Johnson Research Foundation, University of Pennsylvania, Molecular Structure and Polarity . Philadelphia, Pennsylvania, USA Dielectric Constant . . Ionization . Hydrogen Bonding Water is a major component of all living things. It is anomalous in many of its physical Hydrophobic and Hydrophilic Interactions: Water as a . and chemical properties. Some are essential for life while others have profound effects on Solvent the size and shape of living organisms, how they work, and the constraints within which they must operate. Many of water’s basic physical properties can now be explained, at least semiquantitatively, in molecular and structural terms, although in spite of intense study it remains incompletely understood. Introduction bonds, or H-bonds) between the oxygen and hydrogen atoms. This is reflected in its high boiling point, the large ). bc Water is the material cause of all things (Thales, 624–546 amount of heat needed to vaporize it, and its high surface Water is a unique, ubiquitous substance that is a major tension. Replacement of one or both of the hydrogens component of all living things. Its nature and properties dramatically weakens these intermolecular interactions, have intrigued philosophers, naturalists and scientists since reducing the magnitude of these quantities. The strong antiquity. Water continues to engage the attention of cohesive interactions in water also result in: scientists today as it remains incompletely understood in spite of intense study over many years. This is primarily (1) a high viscosity, since for a liquid to flow interactions because water is anomolous in many of its physical and between neighbouring molecules must constantly be chemical properties. Some of water’s unique properties are broken; and literally essential for life, while others have profound (2) a high specific heat capacity – the ability to store a large effects on the size and shape of living organisms, how they amount of potential energy for a given increment in work, and the physical limits or constraints within which kinetic energy (temperature). they must operate. This was recognized by Lawrence Henderson in 1913 in his classic and still very readable In part water’s high specific heat and heat of vaporization The Fitness of the Environment: An Inquiry into the book, relative to other liquids results from its small size. More . Since Biological Significance of the Properties of Matter intermolecular interactions are contained in a given then more has been learned about the structure and volume of water than comparable liquids. When this is properties of water at the molecular level, much of it taken into account by expressing the specific heat and heat through spectroscopic and thermodynamic experiments. of vaporization on a molar basis, methanol and water are The more recent discipline of computer simulation has also comparable. The surface tension of water, however, is still played a role, having achieved a level of sophistication in anomolously large after accounting for differences in size. the study of water in which it can be used to interpret Water has one of the highest dielectric constants of any experiments and simulate properties not directly accessible nonmetallic liquid. It also has the remarkable properties of by experiment. Many of water’s basic physical properties 8 C to its freezing point, expanding when it is cooled from 4 can now be explained, at least semiquantitatively, in and again when it freezes. Both the expansion of water and molecular and structural terms. its high dielectric constant reflect subtle structural features of liquid water at the molecular level. Basic physical properties Table 1 . Selected physical properties of water are given in Biological relevance of water’s physical To put these in context, comparison is made to the organic properties solvents methanol and dimethyl ether, where one and two Water, owing to its high boiling point, exists predomi- of the hydrogen atoms are replaced by a methyl group, nantly in its liquid form in the range of environments where respectively. Water is a small solvent, occupying about 3 per molecule in the liquid state at room life flourishes, although the other two phases, ice and 0.03 nm temperature and pressure, yet it is highly cohesive because vapour, play an essential role in shaping the environment. of the strong intermolecular interactions (hydrogen The high specific heat and heat of vaporization of water ENCYCLOPEDIA OF LIFE SCIENCES © 2001, John Wiley & Sons, Ltd. www.els.net 1

2 Water: Structure and Properties Selected physical properties of water Table 1 Property Water Methanol Dimethyl ether Formula H (CH OH OCH ) O 2 3 3 2 –1 )183246 Molecular weight (g mol –1 ) 0.998 0.7914 0.713 Density (kg L 338 248 Boiling point (K) 373 3 0.0299 ) 0.0420 0.107 Molecular volume (nm 3 ) 0.0027 Negative Negative Volume of fusion (nm Liquid density maximum (K) 277 None None –1 –1 g ) 4.182.532.37 Specific heat (J K –1 –1 mol 109.0 ) 75.2 81.0 (J K –1 ) 2.3 1.16 0.40 Heat of vaporization (kJ g –1 37.1 18.4 41.4 ) (kJ mol –1 ) 72.8 22.6 16.4 Surface tension (mN m 550 Viscosity ( Pa s) 1002 233 μ 5.0 33.6 Dielectric constant 78.6 30 a ) 6.01 5.68 4.34 Dipole moment (Cm × 10 Values at 293 K unless indicated. a In the gas phase. have important consequences for organisms at the cellular such as ocean and lake freezing, the formation of the and physiological level, in particular for the efficiency polar ice cap, and in weathering by freeze–thaw cycles. of processes involving heat transfer, temperature regula- tion, cooling, etc. Viscosity is the major parameter of Molecular Structure and Polarity water that determines how fast molecules and ions can be transported and how rapidly they diffuse in aqueous The geometry of the water molecule is illustrated in solution. It thus provides a physical upper limit to the . It consists of two O–H bonds of length 0.096 nm Figure 1a rates of many molecular level events, within which 8 at an angle of 104.5 . Other basic properties of water are its organisms must live and evolve. These include the rates size, shape and polarity. Atoms that are not bonded will of ion channel conductance, association of substrates repel each other strongly if brought close enough that their with enzymes, binding rates, and rates of macromolecular electron orbitals overlap. At larger distances two atoms assembly. It also sets an upper bound to the length scale attract each other weakly due to an induced dipole-induced over which biological processes can occur purely by dipole (London dispersion) force. The combination of diffusion. In many cases, for example in enzyme–substrate repulsive and attractive interactions is termed the van der reactions, evolution has pushed the components of Waals interaction. The point at which the repulsive and living systems to the limits set by water’s viscosity. attractive forces balance is commonly used to define the The high surface tension of water is relevant at two diameter of an atom, which for oxygen and hydrogen are levels. First, below a length scale of about 1 mm surface 0.32 nm and 0.16 nm, respectively. The water molecule is tension forces dominate gravitational and viscous forces, thus approximately spherical. Water is electrically neutral, and the air–water interface becomes an effectively but because the electronegativity of oxygen is much greater impenetrable barrier. This becomes a major factor in the than that of hydrogen the electron distribution is environment and life style of small insects, bacteria concentrated more around the former, i.e. water is and other microorganisms. Second, at the molecular electrically polarized, having a permanent dipole moment (0.1–100 nm) scale the surface tension plays a key role 2 30 C m in the gas phase. The dipole moment is  10 of 6 in water’s solvent properties. The high dielectric constant 2 30 C m) in liquid and ice because  even larger ( c .8 10 of water also plays an important role in its action as a neighbouring water dipoles mutually polarize each other. solvent. The biological significance of the expansion of A useful way to represent the polarity of a molecule is to C and upon freezing, though 8 water upon cooling below 4 assign a partial charge to each atom, so as to reproduce the crucial, is largely indirect through geophysical aspects molecule’s net charge, dipole moment, and possibly ). The magnitude Figure 1b higher-order electrical moments ( 2

3 Water: Structure and Properties vacuum, and it is an order of magnitude more polarizable H-bond length than most organic solvents. The dielectric constant of a O H Angle O 0.096 nm polar liquid such as water depends on four major factors: O HH HH the permanent dipole moment of the molecule, the density ° 104.5 H (a) of dipoles, how easily they can reorient in response to a 109.5 ° 0.32 nm field, and how cooperative this reorientation is. Water has 0.275 nm O O a high dipole moment, it is small so there are a large H H H number of dipoles per unit volume, and in the liquid state O H O –1 they are easily and rapidly (within 10 ps) reoriented. In 0.45 nm H H H addition, because water is extensively H bonded, the O +0.5 +0.5 Ice I polarization response is cooperative: water molecules H (c) (b) cannot simply reorient independently of their neighbours. They effectively reorient in groups of about three. Finally, Tetrahedral waters there is a small contribution to the dielectric constant H . 2–3) from the polarizability and flexibility of water. All c ( H H Hydrophobic H O O these factors explain the very high dielectric constant of solute H O H H H water. Decreasing the temperature increases the dielectric H O O Polar constant since it reduces the randomizing thermal fluctua- H O O H θ solute H tions that oppose dipole alignment by an electrostatic field. θ HH O H Interestingly, the static dielectric constant of water O O H O H continues to increase through the freezing point. The high HH HH H Table 2 ) demonstrates the dielectric constant of ice ( Tetrahedral waters (d) (e) importance of the cooperative effect of dipole reorienta- tion, although the time scale of reorientation is six orders of Structure of water. (a) Definition of key lengths and angles. (b) Figure 1 magnitude longer. Model of water. (c) Structure of Ice I. (d) Schematic of H bonding structure in liquid water, and in presence of an apolar solute. (e) Schematic of H bonding structure around a positively charged ion of polar atom. Ionization of an atom’s partial charge is a measure of its polarity. For Because the O–H bond of water is strongly polarized, the water there is about 1 0.5 on each hydrogen, and a charge electron density around the hydrogen atom is very low and of opposite sign and twice this magnitude on the oxygen. In the O–H bond is rather weak compared with most covalent contrast, the hydrogens of an apolar molecule such as m s bonds. Thermal fluctuations in the liquid often (every 20 methane have a partial charge of  0.1, and methane’s or so) result in sufficient further polarization of the O–H dipole moment is zero. Thus water is a very polar molecule bond that the hydrogen nucleus can dissociate as a proton, with the ability to make strong electrostatic interactions 1 ion. Water being an excellent solvent for ions, it can or H with itself, other molecules and ions. 2 1 solvate the resulting OH ions, the latter and H Putting all this together, one can picture a water 1 O . As a consequence dissociated water primarily as H 3 molecule as a slightly sticky sphere of radius 0.32 nm in has a relatively long lifetime of about 100 s in pure water m which two positive charges of 1 1/2 and a negative charge before recombination. The spontaneous ionization of of 2 1 are embedded at the hydrogen and oxygen atomic water is characterized by a dissociation constant, derived ). Many of liquid water’s Figure 1b centres respectively ( using eqn [1]. properties, including its cohesiveness, its high heat of vaporization, dielectric constant and surface tension can be  þ Š OH Š½ H ½  1 16   10 1 ¼ : 82 Š ½ mol L 1 explained with this simple molecular model. Other proper- H ½ O Š 2 ties such as the temperature dependence of the density need 1 2 With a water concentration of 55.6 mol L , the concen- a more sophisticated model that includes water’s flexibility, 1 7 2 tration of H 8 mol -  10 at 25 C in pure water is 1.0 polarizability and quantum mechanical effects. 1 L 2 1 and thus it has a pH of log10([H ]) 5 7. The 2 hydrogen ion is highly mobile in liquid water, diffusing ). Dielectric Constant Table 2 about five times more rapidly than water itself ( Remarkably, the mobility of a proton in ice is higher still, The dielectric constant is a measure of how easily a material clearly demonstrating that proton transport occurs not so is polarized by an electric field relative to vacuum. It is much by movement of a single proton, but by a hopping defined by the magnitude of the dielectric polarization mechanism between H-bonded waters, whereby a water (dipole moment per unit volume) induced by a unit field. molecule accepts a proton on one side, and releases a Water has nearly 80 times the dielectric constant of proton on the other side. Since the lifetime of an individual 3

4 Water: Structure and Properties Selected physical proteins of liquid water and ice Table 2 Liquid (293 K) Ice I (269 K) 4.7 4 Coordination number 30 10 Dipole moment (Cm – – 9.4 8.7 8.7 )8.0 × Polarizability (nm) 0.144 0.144 Static dielectric constant 78.6 93 – 16 22 – 1 – 3.8 10 )1.82 10 Ionization constant (mol L × × – 1 9 – 5 – 10 Dissociation rate (s )2.5 3 10 × × Dielectric relaxation time 9.5 ps 10 s μ s 10 10 ps Molecular reorientation time μ 10 20 ps s Molecular translation time μ + O lifetime 1 ps 0.1 ps H 3 H – bond lifetime 1 ps – 2 1 – s ) Diffusion constant (m 9 – – 15 3.9 O2 10 10 H × × 2 9 + – 8 – 2 10 10 H 9 × × Coordination water exchange time – 1 ps Around water 10 ns – – Around a typical ion 1 1 O H ion is  1 ps, about five orders of magnitude shorter both are dominated by the hydrogen-bonding interaction. 3 than the lifetime of dissociated water, many hopping events The hydrogen bond (H-bond) is a strong bond formed occur before recombination. This lifetime is also shorter between a polar hydrogen and another heavy atom, usually than the molecular translation time, again indicating that carbon, nitrogen, oxygen or sulfur in biological molecules. 1 O cannot account for the high direct diffusion of the H In the gas phase the strength of an H bond between two 3 1 2 proton mobility. The ionization constant of water is orders , although in liquids and solids its waters is 22.7 kJ mole of magnitude higher than that of most organic solvents. strength is greatly dependent on geometry and the 2 Water’s unique ability to ionize easily and to solvate OH surrounding molecules. It is sometimes characterized as 1 2 1 and H ions allows it to partake in OH and H intermediate between ionic and covalent bonds in char- exchange with many polar solutes. Water can donate its acter, although its energy as a function of the length and 1 1 H from an acid. Acid– to a base, or accept (solvate) H angle can be quite accurately described by a Coulombic base and proton exchange reactions are pervasive in interaction between the partial atomic charges on the biology, occurring in protein folding, protein binding, hydrogen, the heavy atom it is covalently attached to, and enzyme catalysis, ion pumping, ion channel reactions, the oxygen, nitrogen, carbon or sulfur atom with which it is bioenergetic pathways, synthesis of ATP, and in the making the H-bond. chemiosmotic mechanisms of energy transduction, to Ice I is a tetrahedral lattice where each water makes name a few. Communication of a biological signal or H-bonds to four other waters, which lie equidistant from transmission of energy via protons is also extremely rapid each other at the vertices of a regular tetrahedron with edge ). The H-bonds are 0.275 nm Figure 1c due to the facile ionization of water and the high proton lengths of 0.45 nm ( H- 8 long measured from oxygen to oxygen, and linear (0 mobility. Figure 1a ). The H-bonding pattern of ice is bond angle; symmetrical: each water makes two donor H bonds with its Hydrogen Bonding hydrogen atoms, and two acceptor H-bonds with the hydrogen atoms of neighbouring waters. The 2–2 Water structure H-bonding symmetry is an important feature of water. Combined with an H–O–H bond angle very close to the Water exists in three phases: vapour, liquid and ice, the last , and with the tendency for 8 ideal tetrahedral angle of 109.5 of which has at least nine known forms. For biological the four neighbouring waters to repel each other electro- phenomena, the most important is the liquid phase. It is statically, it is sufficient to explain the tetrahedral H- useful, however, when describing its structure to use the simplest form of ice, Ice I, as a reference. The structures of 4

5 Water: Structure and Properties bonding pattern of Ice I and the persistence of the second layer seen in the Ice I structure. The area under the tetrahedral pattern in liquid water. first peak gives the coordination number of water at 25 8 C A different way of describing the structure of Ice I is to as 4.7. This is somewhat higher than for Ice I, indicating count up the number of neighbours each water has as a that the lattice structure has partially collapsed, and each function of distance. Starting at the central water depicted water on average makes an H bond to more than four in Figure 1c and moving out, the first four neighbours are waters. Organic solvents typically have coordination found at a distance of 0.275 nm. The next set is encountered numbers of 6 or higher, so by comparison water has an at 0.45 nm: 12 waters that are H-bonded to the first four ‘open’ structure. Experiments and computer simulations neighbours. Continuing out, shells of water are encoun- show that the open structure results from the high degree Figure 3 shows the tered at discrete distances. The resulting radial distribution of angular ordering in liquid water. probability distribution of H-bond angles made by each function (rdf) is characteristic of a crystalline solid, and Figure 2 ). The number of waters water to its 4.7 neighbours. It is bimodal, and should be consists of discrete peaks ( in the first peak defines the ‘coordination’ number, which in contrasted with the H-bond angle distribution for Ice Ice I is four. Liquids do not have a single structure since the . In liquid four of the H bonds 8 I, which is a single peak at 0 molecules are in constant motion but the rdf is an extremely ), and are approximately linear (mean angle of about 12 8 Figure 2 useful way to describe their average structure. very close to their length in Ice I. This indicates that shows the rdf for liquid water obtained either from X-ray much of the tetrahedral structure of Ice I persists in liquid Figure 1d ). The H-bond to scattering experiments or computer simulations using water, albeit in a distorted form ( the additional neighbour(s) is more distorted, with an Figure 1b . The rdf for liquids is the water model in average angle of about 52 , since these neighbours have to 8 normalized to one so that the value at any point is the sit in a face of the tetrahedron formed by the primary average number of waters found at that distance relative hydration waters. to the number expected if the distribution of water The open tetrahedral structure is also responsible for molecules were completely random, i.e. if there were no the anomalous temperature dependence of water density. structure. Water contracts upon melting, and continues to contract The broad overlapping peaks decaying away to a constant 8 C, above which it until it reaches a temperature of 4 value of one at large distances is characteristic of a liquid. expands like most liquids. In the contraction phase the The first peak or hydration shell indicates that there collapse of the open tetrahedral structure due to increas- is a high probability that two waters will be separated ingly bent H-bonds outweighs the normal tendency for by about 0.25–0.30 nm, the range of H-bonding distances. materials to expand because the molecules become further Beyond 0.3 nm there is a dip since waters at this distance apart. are likely to overlap with those in the first shell, then there is a smaller peak at 0.45 nm, which is the remains of the Ice I Water with hydrophobic solute Pure 1 0.7 H bonds of water length 0.31 nm 4 H bonds of Water: length 0.276 nm 0.0 X-ray scattering simulation Water near 1 apolar group Relative probability Radial distribution function (rdf) Water near Ice I polar group 0.4 0 0.2 0.6 0.8 0.0 90 70 10 50 10 – 30 R (nm) H-bond angle ( ° ) Figure 2 Radial distribution functions (rdf) of Ice I (bottom), pure water (middle), and water around a hydrophobic solute (top). Lines, measured; Hydrogen bond angle probability distribution for Ice I and pure Figure 3 circles, computer simulation. water (top), and for water around solutes (bottom). 5

6 Water: Structure and Properties amino acids such as arginine, and aspartic acid. These Effect of solutes solutes are hydrophilic (water-loving). This category also Solutes perturb the structure of water, primarily in the includes some other neutral amino acids such as aspar- solute’s first hydration shell (the layer of water in contact agine, the peptide backbone of proteins, the phosphate- with the solvent), with a lesser effect on more distant sugar backbone of nucleic acids, sugars and lipid head- Figure 2 shows the rdf for liquid water around the waters. groups. At the low solubility end are aliphatic amino acids hydrophobic (water-avoiding) solute tetramethyl ammo- such as leucine, the aromatic amino acids such as nium. There is a slight sharpening of the distribution phenylalanine, and the hydrocarbon ‘tails’ of lipids. These caused by an increase in the first peak height and a decrease solutes are hydrophobic. Other solutes such as nucleic acid in the first dip. This is indicative of increased ordering of bases and the amino acid tryptophan have intermediate water in the first hydration shell, but the effect is not large. solubility, and cannot be simply classified as hydrophobic The rdf of liquid water is dominated by the size and packing or hydrophilic. of the water, i.e. by the van der Waals interactions, and these are relatively insensitive to the presence of the solute. In contrast, solutes have a large effect on the angular Physical basis of solvation ). Apolar solutes and groups Figure 3 structure of water ( shift the bimodal distribution of water–water H-bond The logarithm of the solubility of a solute is proportional angles towards the more ice-like, linear form, effectively to the thermodynamic work, or hydration free energy hyd increasing the ordering of water by decreasing the less ) necessary to transfer it into water from a reference D G ( ordered population of H-bonds. These solutes lack the solvent (here cyclohexane). High water solubility corre- hyd ability to make strong electrostatic interactions with water, , low solubility to a sponds to a negative (favourable) D G hyd and they interact primarily through the van der Waals (work must be performed to dissolve the D G positive hyd potential. Their effect is essentially geometric: they tend to solute). G D is directly related to the properties of the displace the more weakly H-bonded facial water in the solute, the water, and the strength of interactions between Figure 1d ), thus reducing the population coordination shell ( water and solvent. It is here that the high surface tension of more bent H-bonds. Ions and polar solutes and groups and dielectric constant of water are crucial. The surface have the opposite effect. They shift the distribution of tension is the work necessary to create a unit area of water– water–water H-bond angles towards the more bent form. vacuum interface (units of force per unit length are This is a consequence of the strong electrostatic interac- equivalent to energy per unit area). Work is necessary tions they can make with water. Water dipoles tend to align since interactions must be broken to bring water from the towards or away from the atoms with large atomic partial interior to the surface. Hydrating a solute can be divided charges, consequently distorting the water–water H-bond into two steps: ). Figure 1e ( . creation of a solute-shaped cavity in water, which requires work to be done against the surface tension of Hydrophobic and Hydrophilic water; placing the solute in the cavity, which involves interac- . Interactions: Water as a Solvent tions of the solute with water molecules and restructur- ing of the water. Perhaps water’s most important biological role is as a solvent. It can dissolve a remarkable variety of important molecules, ranging from simple salts through small The first step always opposes dissolution of any solutes. If molecules such as sugars and metabolites to very large the interactions between the solute and water are weak, as molecules such as proteins and nucleic acids. In fact water they are for apolar solutes and groups, the cavity term is sometimes called the universal solvent. Practically all the dominates and the solubility will be low. The cavity term molecular processes essential to life – chemical reactions, drives aggregation of apolar molecules to reduce the association and binding of molecules, diffusion-driven surface area in contact with solvent. This is known as the encounters, ion conduction – will only take place at hydrophobic effect. In contrast, when a polar or ionic significant rates in solution, hence the importance of solute is dissolved in water the electric field from the water’s solvent properties. Equally important as water’s solute’s partial atomic charges induces a large polarization abilities as a good solvent is its differential effect as a (reorientation) of the water dipoles resulting in an solvent – the fact that it dissolves some molecules much attractive electrostatic field (the reaction field) back at better than others. Figure 4 shows the relative solubilities in the solute. This results in a high solubility – a consequence water of a selection of solutes that are of biological of water’s high dielectric constant, and the reason it can importance or are building blocks of biologically impor- dissolve a wide range of ionic and polar solutes. tant macromolecules. The solubilities range over 50 orders In summary, the solubility is determined by two major of magnitude! The high end includes ions and charged contributions: 6

7 Water: Structure and Properties Phosphate + Na – Cl N -Propyl-guanidine (arg side-chain) Acetic acid (asp side-chain) Glucose Propionic acid (glu side-chain) Acetamide (asn side-chain/peptide) Butyl-amine (lys side-chain) Propionamide (gln side-chain) Guanine (nucleic acid base) 4-Methyl imidazole (his side-chain) Cytosine (nucleic acid base) Methanol (ser side-chain) Ethanol (thr side-chain) Uracil (nucleic acid base) Adenine (nucleic acid base) Thymine (nucleic acid base) -Cresol (tyr side-chain) P Hydrogen (gly side-chain) Methanethiol (cys side-chain) Methane (ala side-chain) 3-Methyl-indole (trp side-chain) Ethyl, methyl sulfide (met side-chain) Toluene (phe side-chain) Propane (val side-chain) Isobutane (leu side-chain) Butane (ile side-chain) Hexadecane (lipid tail) 20 40 – 10 030 10 50 (relative solubility) Log 10 of the solubility ratio between water and the apolar solvent cyclohexane. Figure 4 Solubilities of selected solutes in water, expressed as log 10 . formation of macromolecular complexes such as multi- . The cavity contribution, which is unfavourable and meric proteins, protein–nucleic acid assemblies and approximately proportional to area of the solute or membrane protein–lipid assemblies; solute group(s) exposed to water. . specific binding and recognition of molecules with . The electrostatic contribution, which depends on the complementary apolar surface groups. strength of the reaction field induced in water. This in turn depends on the magnitude of the partial atomic Solvation of polar groups acts in a reverse fashion to the charge, the dielectric constant of water, and how near hydrophobic effect in the above processes: there is a strong the atomic charge is to the water (i.e. the atom’s radius, driving force to keep the ionic and polar portions of and whether it is buried or exposed to solvent). proteins, lipids and nucleic acids on the surface in contact with water. This is also the reason that the low dielectric lipid tail region of membranes is impervious to ions, a key Role of solvation property of biological membranes. The delicate balance between polar and apolar solvation Many biological macromolecules, such as proteins, forces contributes to a remarkable fidelity and accuracy of nucleic acids and lipids, contain both hydrophilic and self-assembly. For example, related proteins of different hydrophobic groups. Water’s differential ability to solvate sequence but with conserved patterns of amino acid the different groups produces a driving force for them to hydrophobicity/hydrophilicity can adopt structures that adopt structures or self-assemble in ways where the are similar to 0.1 nm or better tolerance. hydrophilic groups are exposed to water and the hydro- phobic groups are sequestered from water. This is a major Further Reading factor in the folding, assembly and maintainence of precise, complex three-dimensional structures of proteins, mem- Eisenberg D and Kauzmann W (1969) The Structure an dProperties of branes, nucleic acids and protein–nucleic acid assemblies. . Oxford: Oxford University Press. Water For example, the hydrophobic effect promotes: Gerstein M and Levitt M (1998) Simulating water and the molecules of life. Scientific American 279 : 100–105. . formation of a buried apolar core of amino acids in Henderson LJ (1913) The Fitness of the Environment: An Inquiry in to the protein folding; Biological Significance of the Properties of Matter . New York: . helix formation in nucleic acids through base stacking; Macmillan. . formation of lipid membranes with an apolar lipid tail Rahman A and Stillinger F (1971) Molecular dynamics study of liquid 55 water. : 3336–3359. Journal of Chemical Physics region; 7

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