Low molecular weight compound recognition by a target protein is still rather poorly understood hindering efficient rational design of novel molecules that would tightly and specifically bind selectively to the target protein and could be developed into an efficient and non-toxic drug that does not bind and influence the function of other vital proteins. Protein-compound complexes could be characterized structurally and thermodynamically. Correlations between these approaches is the main focus of this manuscript.
Carbonic anhydrases (CAs, EC 188.8.131.52) are ubiquitous metallo-enzymes which catalyze the hydration reaction of carbon dioxide into bicarbonate. Human CAs belong to the α-family comprised of fifteen isozymes which have different cellular localization, distribution, kinetic properties, expression levels, and oligomerization state (Sly & Hu, 1995; Supuran, 2008; Supuran, 2015; Alterio et al., 2012). CAs are involved in many physiological and pathological processes. Twelve of the isozymes (isoforms) contain Zn(II) metal in the active site coordinated by three histidines, while remaining three CA isozymes do not possess any catalytic activity because they do not have Zn(II) in the active site due to the absence of one or more His residues (Aspatwar et al., 2014) needed for the coordination of the metal.
The 12 human CA isoforms have a high degree of conservative residues between themselves. The amino acids which may form contacts with the inhibitor are nearly identical, especially in the deeper parts of the conical cavity-like active site (Pinard, Mahon & McKenna, 2015). These minor structural differences cause some inhibitors to exhibit million-fold selectivities between isoforms—a phenomenon that is difficult to explain and predict from the inhibitor chemical structure. CAs have been used as models of protein-ligand binding for a long time (Krishnamurthy et al., 2008; Supuran, 2015). There are over 500 CA structures with various bound ligands in the PDB database. However, most structures are available for CA II while other isoforms are represented sparsely, therefore limiting our ability to understand the structural basis of inhibitor selectivity.
A large number of studies have been published where novel series of compounds have been described. Compounds of various seemingly non-related chemical classes appear to be good inhibitors of CAs (Lomelino & McKenna, 2016; Supuran, 2017). Thus, aromatic sulfonamides are not the only available inhibitors, but the oldest group of inhibitors with the largest variation of chemical structures tested towards most CA isoforms. The mechanism of sulfonamide binding is rather well understood. The binding reaction is highly pH-dependent due to the linked protonation-deprotonation reactions of sulfonamide and the water molecule bound to the Zn(II) in the active site (Taylor, King & Burgen, 1970; Pilipuitytė & Matulis, 2015). It is important to dissect those linked reactions and calculate the intrinsic parameters that would be independent of the buffer and pH (Krishnamurthy et al., 2008; Baranauskienė & Matulis, 2012; Jogaitė et al., 2013; Morkūnaitė et al., 2015). Here we correlate the thermodynamics of binding with the structures of a series of fluorinated and chlorinated benzenesulfonamides that have been previously described Kišonaitė et al. (2014), Zubrienė et al. (2015) and Zubrienė et al. (2016).
The thermodynamics of ligand binding depends on many factors, including: (a) classical interaction such as hydrogen bonds, salt bridges, direct Van-der-Waals contacts, and hydrophobic interactions; (b) solvent-related effects (solvation, desolvation, the capture or release of water molecules) before and upon binding process; (c) conformational mobility and conformational changes of the ligand and the protein active site residues upon binding; (d) shape and exposed surface topography of the active site. Much of the thermodynamic data has been determined by isothermal titration calorimetry (ITC) technique that has been extensively reviewed (Pethica, 2015; Falconer, 2016) with the suggestions for the interpretation of ITC data.
The role of non-covalent interactions and reorganization of water molecules around the ligand and in the active site for the application of thermodynamics for drug design has been discussed in Klebe (2015). There is an interesting suggestion that water molecules may have minor impact to the free energy of ligand binding, but relatively large effects to the changes of entropy and enthalpy. In the review by Geschwindner, Ulander & Johansson (2015), the authors also remind that two standard constituents (ΔH and ΔS) of the Gibbs energy of ligand-protein binding comprise in reality a mixture of many contributions which are discussed here.
In the current review on the ligand binding thermodynamics (Claveria-Gimeno et al., 2017) the binding enthalpy change is split into contributions: ΔHobserved = ΔHinteractions + ΔHdesolvation + ΔHconformational + ΔHexchange, where ΔHinteractions is the enthalpy gain associated with formation of non-covalent interactions between binding partners, ΔHconformational is the enthalpy gain associated with the conformational changes of ligand and protein, ΔHdesolvation is the enthalpy gain associated with the desolvation processes of the binding partners, ΔHexchange is the enthalpy gain associated with additional impact from interactions between ligand or protein and another buffer compounds, such as protons, small molecules. The pH influence to the binding process can be determined and removed from ΔHexchange. The ΔHdesolvation, ΔHconformational and ΔHinteractions reflect enthalpies of binding steps: (1) desolvation of binding partners, (2) conformation changes of the partners upon binding, and (3) formation of non-covalent interactions between binding partners. The binding entropy change (multiplied by the absolute temperature) also can be split in a similar way:−TΔSobserved = − TΔSdesolvation − TΔSconformational − TΔSexchange − TΔSroto-translational − TΔSvibrational, where new members TΔSroto-translational and TΔSvibrational are roto-translational (associated with degree of translational and rotational freedom) and vibrational (associated with covalent bonds) entropies. The authors propose to focus on desolvation and conformational entropies. For example, the conformational entropy is usually unfavorable due to reduction in mobility of binding partners.
The changes in enthalpy upon binding could provide an additional information for selecting compounds in the lead discovery and optimization. The enthalpy-driven compounds often have been considered to have better probability to become a drug (Ladbury, Klebe & Freire, 2010). The favorable binding enthalpy can indicate the better geometry of hydrogen bonds, Van-der-Waals, and other interactions between the ligand and the target protein. The enthalpy gain is necessary but not sufficient for an affinity gain due to compensating entropic effects (Freire, 2008).
Whitesides with co-workers provided a comprehensive crystallographic analysis of a series of homologous compounds bound to CA II that was used in several studies of the hydrophobic effect. In the review by Snyder et al. (2013), the authors take note of the influence of water dynamics during ligand binding on the known effect of enthalpy/entropy compensation. Water molecules in the binding pocket and around the ligand are the critical component in the process of protein-ligand binding. Another direction of the research was the use of CA II as a tool for the investigation of Hoffmeister series of ions. The structure of water molecules around the ligand have significant influence to the binding behavior of a molecule to various surfaces. Fox et al. (2015) showed that the binding affinity of anions to the active site of CA II correlates inversely with their affinity for water (free energy of hydration), the poorly hydrated anions associate more effectively with cation (Zn(II)) and non-polar regions of CA II.
In the article by Winquist et al., (2013), the authors showed the complex view of the binding processes by analyzing the binding thermodynamics, kinetics and crystal structures showing that the additional hydrogen bonding is not necessarily reflected in the enthalpic gain. Moreover, the minor changes in the structure of compound can influence in an unpredictable way the kinetic and thermodynamic signatures of the binding reaction due to the small structural rearrangements within the protein binding site and subtle changes in the relative orientation of the compounds.
Davis and colleagues studied the water structural transformation at molecular interfaces using spectroscopic observations. They reported that the properties of water molecules bound in the hydrophobic hydration shell differ from the bulk water in the degree of order in tetrahedrally hydrogen-bonded molecules and in the number of so-called dangling water (defects in water’s tetrahedral H-bond network). The hydration shell has a greater degree of tetrahedral order and reduced population of the weakest hydrogen bonds at low temperatures (Davis et al., 2012). The number of dangling waters, which depends on the temperature, intramolecular charge delocalization, size of hydrophobic domains, also changes near the hydrophobic surface (Davis et al., 2013; Davis et al., 2015).
To better understand the binding and recognition process between a protein and a low-molecular-weight chemical compound, a system of closely related proteins and structurally similar compounds is necessary. Carbonic anhydrase isoforms comprise a nice group of proteins that are recognized by aromatic sulfonamides because the sulfonamide group binds to the active site Zn(II) cation. Because of this recognition, aromatic sulfonamides bind stoichiometrically and specifically to CAs. However, minor differences in the CA isoforms and differences in the tail part of the sulfonamides cause significant difference in the energies of binding. Therefore, the system is highly suitable for the detailed investigation of structure-thermodynamics relationship of the recognition process.
Materials and Methods
Recombinant human carbonic anhydrases isoforms were expressed and purified by affinity chromatography as described previously (CA I in Čapkauskaitė et al. (2013), CA II in Čapkauskaitė et al. (2012), CA XIII in Sūdžius et al. (2010), and CA XII in Jogaitė et al. (2013).
The synthesis, chemical structural characterization, and the purity of 4-substituted-2,3,5,6-tetrafluorobenzenesulfonamides 1–5 and 10 has been described in Dudutienė et al. (2013), chlorinated benzenesulfonamides 6–9 in Čapkauskaitė et al. (2013) and 3,4-disubstituted-2,5,6-trifluorobenzenesulfonamides 11–16 in Dudutienė et al. (2014) and Dudutienė et al. (2015). The purity of all compounds was >95%, as verified by HPLC.
Crystallization conditions of seven crystal structures are listed in Table 1. All crystallization experiments were carried out in Cryschem sitting drop plates (“Hampton Research” Cat. Nr. HR3-160) at 18–20 °C. Crystals of CA II and CA XII were soaked with 0.5 mM solution of the ligand prepared in the crystallization buffer. The quality of the electron density of the compounds is presented in Fig. 1. The crystal structures were solved by molecular replacement using MOLREP software (Vagin & Teplyakov, 1997). Initial models were the following: 3HLJ for CA II, 2NNO for CA XIII, and 1JD0 for CA XII. The 3D models of compounds were generated using AVOGADRO (Hanwell et al., 2012). The library files which contain complete chemical and geometric descriptions of compounds were created using LIBCHECK (Vagin et al., 2004). Model building and refinement were made using COOT (Emsley & Cowtan, 2004) and REFMAC (Murshudov, Vagin & Dodson, 1997) programs, respectively. The graphics were generated using MOLSCRIPT (Kraulis, 1991), BOBSCRIPT (Esnouf, 1999), RASTER3D (Merritt & Bacon, 1997) and PYMOL (Schrödinger, 2010) programs. Coordinates and structure factors have been deposited to the RCSB Protein Data Bank (PDB). PDB access codes are listed in Table 2.
|Isoform-ligand||Crystallization buffer||PDB ID||Sitting drop|
|CA II-4 (VD10-49)||2.03 M sodium malonate (pH 7.5)a||5LLH||6 µL of 20 mg mL−1 CA II protein solution and 6 µL of crystallization buffer|
|CA II-13 (VD11-26)||0.1 M sodium bicine (pH 9) (Roth #9162.3), 0.2 M ammonium sulfate (Sigma-Aldrich #31119) and 2 M sodium malonate (pH 7)||5LLC||5 µL of 40 mg mL−1 CA II protein solution and 5 µL of crystallization buffer|
|CA II-2 (VD10-51)||2.5 M sodium malonate (pH 7.5) and 0.075 M sodium bicine (pH 9)||5LLE||6 µL of 60 mg mL−1 CA II protein solution and 6 µL of crystallization buffer|
|CA II-1 (VD12-10)||0.1 M sodium bicine (pH 9), 0.2 M ammonium sulfate and 2 M sodium malonate (pH 7)||5LLG||4 µL of 50 mg mL−1 CA II protein solution and 4 µL of crystallization buffer|
|CA XII-10 (VD10-35)||0.1 M ammonium citrate (pH 7) (Roth #9488.2), 0.2 M ammonium sulfate and 26% PEG4000 (Roth #0156.1)||5MSB||3 µL of 19.7 mg mL−1 CA XII protein solution and 3 µL of crystallization buffer|
|CA XII-16 (VD12-23)||0.1 M ammonium citrate (pH 7), 0.2 M ammonium sulfate and 26% PEG4000||5LLP||3 µL of 19.7 mg mL−1 CA XII protein solution and 3 µL of crystallization buffer|
|CA XII-12 (VD12-34)||0.1 M ammonium citrate (pH 7), 0.2 M ammonium sulfate and 26% PEG4000||5LLO||3 µL of 24.4 mg mL−1 CA XII protein solution and 3 µL of crystallization buffer|
|Isoform-ligand||CA II-4 (VD10-49)||CA II-13 (VD11-26)||CA II-2 (VD10-51)||CA II-1 (VD12-10)||CA XII-10 (VD10-35)||CA XII-12 (VD12-34)||CA XII-16 (VD12-23)|
|Unit-cell parameters (Å)||
a = 42.2,
b = 41.1,
c = 71.9,
β = 104.4
a = 42.2,
b = 41.1,
c = 72.0,
β = 104.1
a = 42.1,
b = 41.0,
c = 71.6,
β = 104.0
a = 42.1,
b = 41.1,
c = 71.8,
β = 104.2
a = 77.1,
b = 74.1,
c = 91.6,
β = 108.9
a = 77.3,
b = 74.1,
c = 91.6,
β = 109.0
a = 77.5,
b = 74.3,
c = 91.7,
β = 109.0
|Radiation source||Rigaku MicroMax ™-007 HF||EMBL, P13||Rigaku MicroMax ™-007 HF||EMBL, P14||EMBL, P14||EMBL, P13||EMBL, P14|
|Unique reflections number||17,591||95,940||18,840||83,155||237,650||127,546||160,218|
|Rmerge, overall (outer shell)||0.160 (0.211)||0.038 (0.265)||0.109 (0.390)||0.068 (0.400)||0.056 (0.398)||0.049 (0.370)||0.062 (0.256)|
|I/ σ overall (outer shell)||7.0 (3.3)||18.4 (5.7)||17.6 (7.6)||11.2 (3.3)||14.2 (4.2)||18.1 (4.0)||15.7 (7.3)|
|Multiplicity overall (outer shell)||2.1 (2.1)||6.7 (6.5)||3.0 (2.9)||6.6 (5.5)||6.8 (6.7)||6.8 (6.9)||6.9 (6.9)|
|Completeness (%) overall (outer shell)||92.6 (92.6)||98.8 (97.9)||99.6 (100.0)||91.5 (67.0)||99.4 (99.2)||99.0 (99.1)||98.1 (96.6)|
|RMSD bond lengths (Å)||0.019||0.024||0.018||0.024||0.021||0.022||0.024|
|RMSD bond angles (°)||1.976||2.408||1.891||2.307||2.183||2.146||2.339|
|Average B factors (Å2):|
|Number of atoms:|
|Ramachandran statistics (%):|
|Most favored regions||95||96||96||97||97||98||98|
|Additionally allowed regions||5||4||4||3||3||2||2|
The root-mean-square deviations (RMSD) between CA-inhibitor complexes and apo proteins without ligand were calculated by Perl script for protein backbone atoms of chains A of crystal structures. The RMSD of the CA II complexes in comparison with apoCA II was 0.23 ± 0.04 Å (compound 7—0.30 Å, 3—0.22 Å, 4—0.29 Å, 10—0.18 Å, 8—0.19 Å, 12—0.17 Å, 13—0.24 Å, 9—0.25 Å, 2—0.22 Å, 14—0.21 Å, 6—0.26 Å); for CA I complexes vs apoCA I—0.17 ± 0.03 Å (compound 3—0.14 Å and 5—0.20 Å); for CA XII complexes vs apoCA XII—0.27 ± 0.10 Å (compound 10—0.26 Å, 11—0.52 Å, 1—0.18 Å, 15—0.32 Å, 16—0.18 Å and 12—0.17 Å) and for CA XIII complexes vs apoCA XIII—0.51 ± 0.04 Å (compound 9—0.54 Å, 10—0.46 Å and 11—0.53 Å). The differences between main chain atoms between different crystal structures of the same protein have been reported to be around 0.25–0.40 Å (Chothia & Lesk, 1986). RMSD values of peptide backbone between apo proteins and complexes with inhibitor were in range 0.17–0.51 Å and we conclude that no significant conformational changes occur upon ligand binding.
Calculation of molecular surface
The buried surface area (BSA) and accessible surface area (ASA) values were calculated using Voronota (v. 1.10.1544, Olechnovič & Venclovas, 2014) program. Hydrogen atoms were added to models by PERL script. The initial parameters for contacts calculation were set as follows: (1) rolling probe radius was default (1.4 Å); (2) values of Van-der-Waals radii were the following: Cl atom—1.75 Å, C—1.7 Å, F—1.47 Å, N—1.55 Å, O—1.52 Å, S—1.80 Å, Zn—1.39 Å, and H—1.09 Å.
Isothermal titration calorimetry
ITC experiments for the binding of 13–14 and 16 to CA II, CA XII and CA XIII were performed using VP-ITC instrument (Microcal, Inc., Northampton, MA, USA, now part of Malvern Instruments Ltd, UK) with 5–10 µM protein solution in the cell and 50–100 µM compound solution in the syringe. A typical experiment consisted of 25 injections (10 µl each) within 3–4 min intervals. Experiments were carried out at 37 °C in a 50 mM sodium phosphate or TRIS chloride buffer containing 100 mM NaCl at pH 7.0, with a final DMSO concentration of 1%, equal in the cell and syringe. Protein stock solutions were dialyzed against the buffers that were used to prepare the ligand solutions. ITC data were analyzed using MicroCal Origin software. All calorimetric titration data were presented after subtracting the background signal. The first point from the 5 µL injection in the integrated data graph was deleted. The binding constants, enthalpies and entropies of binding were estimated after fitting the data with the single binding site model.
Determination of intrinsic thermodynamics of binding
The observed energies of binding, including the Gibbs energies (observed affinities), enthalpies, and entropies of the protein-ligand pairs were determined by the fluorescent thermal shift assay (Pantoliano et al., 2001; Lo et al., 2004; Matulis et al., 2005; Cimmperman & Matulis, 2011) and isothermal titration calorimetry (Wiseman et al., 1989; Harding & Chowdhry, 2001; Broecker, Vargas & Keller, 2011). The measured observed thermodynamic parameters of binding depend on the assay conditions such as pH and buffer because the binding of sulfonamide to CA is linked to several protonation reactions, the protonation of hydroxide bound to the Zn(II) in the active site of CA, the deprotonation of sulfonamide group of the inhibitor, and the (de)protonation of the buffer (Baker & Murphy, 1996; Krishnamurthy et al., 2008; Baranauskienė & Matulis, 2012; Morkūnaitė et al., 2015). For the structure–activity relationship and correlation of thermodynamic parameters with the X-ray structures, the intrinsic thermodynamic parameters of sulfonamide anion binding to the Zn-bound water form of CA were calculated.
|CA and inhibitor||PDB ID||Kd, nM, FTSA||ΔG, kJ/mol||ΔH, kJ/mol||−TΔS, kJ/mol||References of crystal structures|
|chimeric CA IX-11||4Q07a||n/d||n/d||n/d||n/d||5|
|CA II-15||4QTLa, 5EHEa||4.5||−49.5||−22.1||−27.4||4, 6|
|CA XII –16||5LLP||0.58||−54.8||−29.8||−25||7|
The intrinsic binding thermodynamics of compounds 1–12, and 15 were taken from references given in the Table 3. Isothermal titration calorimetry (ITC) was used to determine the enthalpy of 13–14 and 16 binding to CAII, CA XII, and CA XIII (the intrinsic affinities, determined by the fluorescent thermal shift assay, were taken from Dudutienė et al. (2015). We have shown previously (Smirnovienė, Smirnovas & Matulis, 2017) that the Kb values observed by FTSA and ITC methods were in good agreement and varied up to 3 times. However, the Kb determined by ITC method were not used in this study, because some compounds bound CAs with observed Kd < 10 nM and Wiseman c factor was too large for accurate Kb determination. To avoid discrepancies only the Kb determined by FTSA were used.
The intrinsic thermodynamic parameters for compounds 13–14 and 16 were calculated using Eqs. (1)–(4), where the pKa of sulfonamide protonation was 7.88 and the enthalpy of sulfonamide deprotonation −24.3 kJ/mol.
The intrinsic binding constant Kb_intr is equal to the observed binding constant Kb_obs divided by the fractions of deprotonated inhibitor and protonated Zn-bound water form of CA: (1) The fractions of the deprotonated inhibitor and the Zn bound water form of CA may be calculated: (2) (3) The observed enthalpy (ΔbHobs) is the sum of all protonation events and the intrinsic binding reaction: (4) where ΔbHobs is the observed binding enthalpy, nsulf = fRSO2NH− − 1 is the number of protons uptaken by the inhibitor, Δb_proton_sulf H is the enthalpy of inhibitor protonation, nCA = 1 − fCAZnH2O is the number of protons uptaken by the Zn-hydroxide, Δb_proton_CA H is the enthalpy of CA protonation, nbuf = nsulf + nCA, is the net sum of uptaken or released protons and Δb_proton_buf H is the enthalpy of buffer protonation.
Results and Discussion
A series of 24 crystal structures of complexes between four CA isoforms and 16 aromatic benzenesulfonamides were solved by X-ray crystallography characterizing the structural aspect of the interaction. To characterize the same interactions energetically, the observed affinities of binding (observed dissociation constants, Kd, or observed Gibbs energies of binding) for each protein-ligand pair were determined by the fluorescent thermal shift assay (FTSA), and the observed enthalpies were determined by isothermal titration calorimetry (ITC). The Kd by both methods (FTSA and displacement ITC) agreed nearly perfectly (Zubrienė et al., 2015). The observed entropies (multiplied by the absolute temperature) were obtained by subtracting the Gibbs energies obtained by FTSA from the enthalpies obtained by ITC. However, sulfonamide ligand binding to CA is linked to several protonation reactions and therefore the observed values depend on pH and buffer. To dissect these linked reactions, the intrinsic thermodynamic parameters that are independent of the buffer and pH of deprotonated sulfonamide anion binding to the Zn-bound water form of CA were calculated (see Methods). This analysis of structure–activity relationship and correlations of intrinsic thermodynamic parameters with the X-ray structures characterized each protein-ligand pair both structurally and thermodynamically.
Chemical structures of the 16 benzenesulfonamides used in this study are shown in Fig. 2. Crystal structures of these compounds with CA I, CA II, CA XII, and CA XIII are grouped into pairs combining chemically similar compounds that differ by the hydrophobicity of substituents whose contribution to the binding to CA isoforms is being studied. Fifteen inhibitors were grouped into 13 matched pairs of crystal structures. Six pairs contain crystal structures with CA II, two—with CA XIII, one—with CA I, and four—with CA XII. Two crystal structures of the compound 1 were compared when bound in the active site of CA II and CA XII.
Nine matched pairs of crystal structures exhibited a similar binding mode (pairs S1-9) of the inhibitors in the active site of CA isoforms, i.e., the benzene ring was found in the same orientation while only the positions of substituents may have differed in each pair (Fig. 3). The remaining four matched pairs of complexes exhibited a dissimilar binding mode of the benzenesulfonamide ring in the active site of CA (D1-4) (Figs. 4A–4D).
The sulfonamide-bearing benzene ring was observed in the same orientation for all pairs of “similar binders” (S1-9, Fig. 3). Differences in the binding of ligands within these pairs were observed only in the regions where different substituents were present in the compounds of the pair. The intrinsic thermodynamic parameters of binding are listed in Table 3. Figure 5A shows the energies, including the Gibbs energy, enthalpy, and entropy of binding, for every analyzed pair of similar binders, as a function of the sum of accessible and buried surface areas of the hydrophobic substituents of inhibitors in each matched pair. The accessible and buried surface areas of substituent groups, marked green or magenta in Fig. 3, were calculated by VORONOTA algorithm (Olechnovič & Venclovas, 2014).
The comparison of intrinsic Gibbs energy of binding for each molecular pair in the group S1-9 (Fig. 5A) showed that there was a relatively small increase in affinity with an increase in the accessible and buried surface area. Additional hydrophobic surface seemed to not have a large impact on the binding affinities. However, the intrinsic enthalpies of binding in all pairs of similar binders were significantly less exothermic for compounds bearing larger hydrophobic substituents. Additional contacts between the protein and the ligand did not make the enthalpy more favorable. The entropies of binding mirrored the enthalpies—the enthalpy-entropy compensation was observed (Fig. 5A).
The compounds 2, 3, and 4 are para-substituted fluorinated benzenesulfonamides exhibiting nearly identical binding affinity for CA II (Figs. 3B and 3H, pairs S2 and S8). Fluorinated benzene rings of these compounds bind to the active site of CA II in almost identical mode and their hydrophobic para-substituents interact with the hydrophobic cavity formed by the amino acids Phe131, Val135, Leu198, Pro202, and Leu204. The properties of para-substituents in these compounds are different: propyl of compound 3 is small and flexible and can adopt an optimal conformation for interactions, while 2 and 4 have large and rigid adamantane and aromatic heterocyclic groups, respectively. The hydrophobic area of the para-substituents increases in 4 and 2 as compared to 3 and the entropic gain of the corresponding binding reaction increases too (Fig. 5A and Table 3). The identical binding mode of these compounds allows to propose that ΔHinteractions for these compounds can be similar in the binding to CA II. ΔHconformational gain also can be similar due to (1) identical binding mode to CA II and (2) congeniality between these compounds. As mentioned previously, the pH and buffer influence to ΔHexchange gain is eliminated because we analyze the intrinsic binding parameters. We hypothesize that the enthalpy-entropy differences are caused by the reorganization of the solvent near the hydrophobic surfaces of the compound, but not of compounds themselves. The changes of ΔHdesolvation and −TΔSdesolvation seem as first candidates for explaining the changes between binding thermodynamics of these compounds. The changes of desolvation entropy can be explained by increase of translational and rotational mobility (freedom) of water molecules which were more ordered near the hydrophobic surfaces of compounds before desolvation.
The active site of crystal structure CA II-3 contains more water molecules in comparison with CA II-2 and CA II-4 (Figs. 3B and 3H). However, it is difficult to make accurate analysis of the water molecules because the number of solvent molecules that are visible in crystal structure depend on the resolution. There are more water molecules in the crystal structure CA II–3 with the resolution of 1.06 Å (17 waters by Pymol searching around the ligand within 9 Å distance) as compared to CA II-4 (1.90 Å resolution, six waters) and CA II- 2 (1.90 Å resolution, nine waters). Furthermore, the active site of crystal structure CA II-3 possibly contains more water molecules than it is currently observed in comparison with structures CA II-2 and CA II-4 due to the only one distinct conformation of the flexible His64 (which is important for the rate limiting proton transfer event from the active site). The active sites of crystal structures CA II-2 and CA II-4 contain electron densities of two conformations of His64, one of which disturbs the quality of the electron densities of water molecules in the hydrophilic part of the active site.
Compounds 3 vs 5 in the matched pair S3 are para-substituted fluorinated benzenesulfonamides bound in identical position in the CA I active site (Fig. 3C, pair S3). The binding of 3 by CA I described in Dudutienė et al. (2015) with an unfavorable entropic contribution (Table 3). The extremely high binding affinity was explained by the specific interactions between 3 and CA I where the fluorobenzene ring is fixed between His200 and Leu198 which restricts the mobility of fluorobenzene ring of the ligand from the other side by the aromatic-aliphatic interaction. The minor enlargement of the hydrophobic area (cyclohexane in 5 vs. propyl in 3) resulted in significant changes in the enthalpy-entropy contribution (ΔΔG = − 0.9 ± 1, ΔΔH = 14.7, −ΔTΔS = − 15.6 kJ/mol). The same binding affinities in the pair indicate that compounds interact with the active site in a similar way (similar ΔHinteractions) and the enlargement of the hydrophobic surface is the only factor that influences the difference in thermodynamics.
The unfavorable entropic contribution of 3 binding to CA I seem as uncompensated unfavorable changes of conformational entropy (–TΔSconformational) due to the reduction in mobility of binding partners upon formation of complex.
Compounds 13 and 14 are meta/para-substituted fluorinated benzenesulfonamides that differ by meta-substituents. Both compounds have para-phenyl groups that were found in both crystal structures with CA II “stacked” with the fluorinated benzene ring. In such conformation, the para-phenyl group in both ligands dislocates the water molecules from the hydrophilic part of the active site of CA II (Fig. 3E, S5). The binding of 13 with CA II is enthalpy-driven and the release of water molecules from the active site did not make the entropy more favorable (Table 3, Fig. 5A) due to increase in translational and rotational mobility of waters released from the active site. The additional hydrophobic area of meta-group for the compound 14 induces large changes in enthalpy-entropy terms (ΔΔG = 0.3 ±1, ΔΔH = 26.3, −ΔTΔS = − 26 kJ/mol, Table 3). On the other hand, the overall binding affinity is the same for both compounds.
The structural differences of 10 vs 12 bound in CA II (Fig. 3G, S7) are located in the meta-position of the benzene ring. These compounds have the same position of the fluorinated benzenesulfonamide and of sulfonyl moiety of para-group. The enlargement of the hydrophobic part induces the increase of the binding affinity by −2.3 ± 1 kJ/mol (Table 3) within this pair. The changes of the entropic and enthalpic contributions of the pair S7 (ΔΔG = − 2.3 ± 1, ΔΔH = 10.3, −ΔTΔS = − 12.6 kJ/mol) are more than two times smaller than in the pair S5 (13 and 14 in CA II, Fig. 5A), despite somewhat larger variations in the surface between 10 and 12. The enthalpy-entropy compensation takes place in both cases.
The pair of structures S1, where compounds 10 and 11 (Fig. 3A), that differ by the presence of the bulky cyclooctyl group in the meta-position (Fig. 2) are bound to CA XIII, is an interesting exception between reviewed pairs: the binding affinity is notably increased with the increase of the hydrophobic surface of the meta-group (Fig. 5A). Inhibitor 11 binds to CA XIII 30 times stronger than 10 (Kd 0.29 nM for 11 and 8.9 nM for 10, Table 3). The cyclooctyl group was found in the crystal structure bound to the hydrophilic part of the CA XIII active site displacing water molecules observed in the structure with compound 10 (Fig. 3A, S1). The entropic and enthalpic contributions are large for this pair (ΔΔG = − 8.8 ± 1, ΔΔH = 39.0, −ΔTΔS = − 47.9 kJ/mol). The compound 11 is entropy-driven ligand and large entropic gain seems to be obtained from the changes of desolvation entropy on the hydrophobic surface of ligand and maybe by the release of water molecules from the active site.
Compounds 9 and 8 are para-substituted 2-chlorobenzenesulfonamides, that contain pyrimidine and dimethylpyrimidine groups in the para-position, respectively (Fig. 2). We compared the crystal structures of this pair of inhibitors bound to CA II (Fig. 3I, pair S9) and CA XIII (Fig. 3F, pair S6). The increase of hydrophobic surface between 9 and 8 is small, it is an addition of two methyl groups to the para-pyrimidine. Therefore, for both pairs, the favorable impact to binding affinities is rather small and occurs due to negligible favorable changes of entropies vs changes of enthalpies (Table 3 and Fig. 5A). In CA II (pair S9): ΔΔG = − 0.8 ± 1, ΔΔH = 6.5, −ΔTΔS = − 7.3 kJ/mol and in CA XIII (pair S6): ΔΔG = − 1.4 ± 1, ΔΔH = 3.2, −ΔTΔS = − 4.6 kJ/mol. In CA XIII (pair S6), methylpyrimidine of compound 8 coincides with the pyrimidine ring of 9, whereas in CA II (pair S9), methylpyrimidine of 8 interacts with the other hydrophobic part of the active site than pyrimidine ring of 9 (Figs. 3F and 3I). Methylpyrimidine is larger than pyrimidine and could not occupy the same position as pyrimidine in both CA isoforms. The more spacious hydrophobic part of the CA II active site allowed for the reorientation of the methylpyrimidine along the hydrophobic surface whereas in CA XIII the methylpyrimidine is simply dislocated outwards.
Compounds 7 and 6 are homologous to compounds 9 and 8 respectively (Fig. 2), except that the benzene ring does not contain chlorine. This pair of ligands is represented by the crystal structures of the complexes with CA II (Fig. 3D, pair S4). The binding thermodynamics in S4 exhibits the distinct decrease of the binding affinity towards CA II: ΔΔG = 3.1 ± 1, ΔΔH = 13.6, and −ΔTΔS = − 10.5 kJ/mol due to the uncompensated enthalpic loss and the entropic gain (Fig. 5A and Table 3).
The thermodynamic parameters of the dissimilar inhibitor (Figs. 4A–4D) binding to CA XII are shown in Fig. 5B as a function of the surface of substituent at the benzenesulfonamide group. For the dissimilar binders, there is a significant increase of the intrinsic binding affinity between compounds in matched pairs (e.g., 318 times for the pair D1) when the accessible and buried surface areas increase. The intrinsic enthalpies of binding in all pairs of dissimilar binders were significantly more exothermic for compounds with larger hydrophobic substituents, contrary to the binding thermodynamics of similar binders (pairs S1–S9): pair D1 (ΔΔG = − 14.7 ± 1, ΔΔH = − 16.2, −ΔTΔS = 1.5 kJ/mol), pair D2 (ΔΔG = − 8.7 ± 1, ΔΔH = − 11.5, −ΔTΔS = 2.8 kJ/mol), pair D3 (ΔΔG = − 10.5 ± 1, ΔΔH = − 5.2, −ΔTΔS = − 5.3 kJ/mol), and pair D4 (ΔΔG = − 11.5 ± 1, ΔΔH = − 22.4,−ΔTΔS = 10.9 kJ/mol). Additional contacts between the protein and the ligand made the enthalpy more favorable for this group. The entropy was significantly favorable for the pair D3, significantly unfavorable for D4, and the changes were negligible for D1 and D2. The compounds that are more hydrophobic in these pairs (15, 16, 12, and 11) differ by the meta-substituent from the reference compound 10 and have the same location of the fluorinated benzene ring in the CA XII active site. The meta-substituents are located in the hydrophobic environment and sterically dislocated the remaining part of the compound is bound in the hydrophilic concave of CA XII active site (Figs. 4A–4D). The favorable changes of the binding enthalpies of the dissimilar binders could be explained by the favorable location of the hydrophilic para-group which is sterically dislocate into the hydrophilic part of the active site where the formation of additional hydrogen bonds is more likely. The favorable ΔHinteractions may be the reason for the improved binding affinities.
It is interesting to compare the compounds 12 (pair D4) and 16 (pair D3) that differ by only one bridged methyl group in the meta-substituent. The difference in the binding energy between these compounds (12 vs 16) is significant (ΔΔG = 1.0 ± 1, ΔΔH = 17.2, −ΔTΔS = − 16.2 kJ/mol). Maybe this could be explained by the possibility of only one position of compound 12 para-group when bound in CA XII, where two hydrogen bonds are formed with the residues Asn64 and Pro200. The para-group of 16 was found in the alternate conformation, but in the compound 12 bound to CA XII both substituent groups were found in a single conformation. Another explanation can be the same as for similar binders, where the increase of the hydrophobic surface induces similar behavior of binding thermodynamics. Compound 12 and 16 bind to CA XII in identical mode.
The cases of perfect geometry fit in the interactions between protein and ligand
An extremely high affinity of the compound 1 to CA II and CA XII may be an example of a perfect geometrical fit of the ligand to the CA active site. The compound 1 has a relatively simple structure and its binding is enthalpy-driven (Fig. 4F, Table 3) exhibiting very high intrinsic affinity to both analyzed CA isoforms, 7.4 pM to CA II and 67 pM to CA XII. As seen in both crystal structures shown in Fig. 4F, the ligand is likely to bind so strongly due to the tight aromatic-aliphatic interaction between the benzene ring and a conservative leucine side chain (Leu198 in CA II and Leu197 in CA XII). An important difference between CA II and CA XII is the substitution of Phe131 in CA II with the alanine side chain in CA XII. A loss of the exothermic enthalpy was observed for the binding of 1 to CA XII as compared to CA II due to the possible absence of additional interaction of para-substituent of 1 with Phe131 in CA II.
Compounds of the pair S4 (Fig. 4E) exhibit an identical orientation of the benzenesulfonamide ring as compound 1 (Fig. 4F) bound to CA II and CA XII. The Kd values of 7 and 6 bound to CA II are 25 pM and 80 pM, respectively, and such values are similar to the binding of compound 1 to CA II and CA XII. Moreover, binding of these compounds are enthalpy-driven. The aromatic-aliphatic interaction looks like a possible reason of the favorable enthalpic gain (7: ΔH = − 62.0 kJ/mol and 6: ΔH = − 48.4 kJ/mol) of which a major part is due to ΔHinteractions.
Moreover, analysis of these pairs (1 in CA II and CA XII and matched pair S4) highlights that there are contacts between the para-substituents and the protein. In the crystal structures of 1 in CA II and CA XII, the loss of additional surface (Ala instead of Phe) changes the location of the propyl group which is now directed perpendicularly to the plane of aromatic-aliphatic interaction between Leu198 and benzene ring bound to CA XII (Fig. 4F). The propyl group of the compound 1 bound to CA II (Fig. 4F) is located in the hydrophobic cavity (formed by Phe131 and Pro202) and possibly increases the affinity of the aromatic-aliphatic interaction due to same direction of interactions between (1) propyl group and hydrophobic cavity and (2) benzene ring of compound and leucine side chain.
The matched pair S3 (Fig. 3C) exhibits similar behavior. Atoms of His200 side chain dislocate the fluorinated benzenesulfonamide ring of both compounds 5 and 3 and possibly increases the affinity of the aromatic-aliphatic interaction with Leu198. Compound 5 (of pair S3) binds to CA I with Kd = 1.5pM (Table 3) as previously confirmed both by the thermal shift assay and displacement ITC (Zubrienė et al., 2015).
The water molecules are highly important and poorly understood participants in protein-ligand association (Klebe, 2015; Fox et al., 2017). However, there are a number of difficulties and uncertainties in the analysis of water molecules in active sites of crystal structures. The number of water molecules observed in the active site of crystal structure strongly depends on the resolution and buffer composition resulting in buffer molecules located at the protein surface instead of water molecules, and the assignment of water-like electron densities are often ambiguous. The number of water molecules in the active site cavity is also influenced by the alternative orientation of residues in the structure. In addition, adjacent protein molecules present due to crystal packing often stabilize water molecules at the interface and make them visible in the electron density maps.
Some of the structure-thermodynamics relationships helped us to design compounds that would exhibit selectivities in binding to some CA isoforms. Furthermore, such correlations sometimes help better understand the structural features of the inhibitors that determine the affinity of the compound to CA.
Analysis of binding data showed that most of the similar binders did not exhibit the increase of binding affinities in matched pairs, the additional molecular contacts between the protein and the ligand did not make the binding more favorable. The pair S1 (compounds 10 and 11—CA XIII) is an exception exhibiting 30-fold increase in binding affinity to CA XIII upon the addition of cyclooctyl group to 10. This pair has an interesting feature of binding which is not present in other similar pairs. The access of water molecules to sulfonamide did not change after the increase of hydrophobic surface in pairs S2–S9 (Fig. 3). Only in the pair S1 there are changes in water molecules present near the sulfonamide and Zn(II). Several possibilities to displace water molecules upon compound binding are schematically drawn in Fig. 6. The dissociation of 10 from CA XIII (pair S1) could be described by the mechanism shown in Fig. 6A, while the dissociation of 11—by the mechanism shown in Fig. 6B. The complicated path for water molecule access to displace the sulfonamide is a likely reason for the lowering of the measured by surface plasmon resonance method off-rate koff (koff of SPR: 7.9 ×10−3 (11) (Talibov et al., 2016) vs 1.1 ×10−2 (10)). The hydrophobic substituent creates a temporary barrier against water molecules that must penetrate into the active site during dissociation process. It could be the reason of better affinity for 11.
Among dissimilar binders, the matched pair D1 (Fig. 4A), where compounds 10 and 11 are bound to CA XII is interesting. The inhibitor 10 binds to CA XII 318 times weaker than 11, the values of Kd (Table 3): 35 nM for 10 and 0.11 nM for 11. In the crystal structure compound 10 interacts with the particular part of the active site while the other part is filled with water molecules and the binding mechanism could be schematically shown as in Fig. 6A. The binding kinetics of the compound 11 to CA XII could not be measured by SPR due to an extremely low dissociation rate (Talibov et al., 2016, too slow dissociation, koff <10−3 s−1).
In the crystal structure of the complex CA XII with 11, the para-group is located under the side chains of Asn64 and Lys69 and such binding mode may explain the lower Kd. The bulky hydrophobic group in meta-position dislocates the para-substituent of 11 under the side chains of amino acids in the active site cavity. It is possible that the process of dissociation of compound 11 could begin from the conformational changes of the large flexible hydrophobic group in the meta-position which can induce the escape of the para-group from under protein side chains. The bulky hydrophobic substituent can also serve as a temporary barrier that prevents the entry of water molecules during the process of dissociation. The proposed mechanism explaining the high affinity of 11 towards CA XII is schematically shown in Fig. 6C. Dissimilar binders showed that the hydrophobic group can efficiently press the other part of the compound into small concaves of the active site and restrain the compound mobility. This opportunity may be significant for the design of the isoform-specific compounds that could distinguish between very similar active sites.
The additional molecular contacts did not make the binding affinities more favorable, but caused unfavorable changes in binding enthalpies mirrored by favorable changes in entropies. The position, direction and size of the hydrophobic group seems to play a favorable role for binding affinity only when it moves away water molecules bound deep in the active site cavity and creates a barrier for penetration of water molecules to the ligand (Fig. 6). The complicated dissociation of the ligand away from active site can be a significant reason for higher affinity.
In this manuscript we described cases of correlation between parameters of binding thermodynamics and crystal structures of protein-ligand complexes. Some explanations and correlations could be drawn, but a systematic rational prediction of the binding thermodynamics from structure is still largely an elusive task. The dissociation mechanism of ligand from the binding site is interesting. For compounds discussed in “The cases of perfect geometry fit in the interactions between protein and ligand” we showed that the network of interactions between the ligand and the target strongly fixed the compound in the active site. For dissimilar pairs, another mechanism, where additional hydrophobic surfaces participate in ligand orientation, dislocates so that another part of the ligand is located deep in the active site and possibly complicates penetration of water molecules into the active site upon which the dissociation process has been postulated.
Pairwise comparison of CA ligands enabled determining the correlations between substituent chemical structure of the ligand and the thermodynamics of binding, including Gibbs energies, enthalpies, and entropies. Compounds were allocated to two groups—similar, the ones where the orientation of the main benzene ring is the same in the absence and presence of the substituent, and dissimilar, the ones where the orientation of the main benzene ring changes upon addition of the bulky substituent. The binding of compounds comprising similar pairs was less enthalpy- and more entropy-driven upon addition of the substituent.
However, in the dissimilar pairs, the compounds bearing large substituents were more enthalpy driven than the ones where the substituents were absent. Additional hydrophobic groups enabled the localization of hydrophilic part of more hydrophobic compounds in the hydrophilic part of active site where formation of hydrogen bonds is more likely, and it can explain favorable enthalpic changes of contributions in dissimilar pairs. Moreover, the additional hydrophobic interactions can complicate the dissociation process.