The Dependence of Hydrophobic Interactions on the Shape of Solute Surface

According to our recent studies on hydrophobicity, this work is aimed at understanding the dependence of hydrophobic interactions on the shape of a solute’s surface. It has been observed that dissolved solutes primarily affect the structure of interfacial water, which refers to the top layer of water at the interface between the solute and water. As solutes aggregate in a solution, hydrophobic interactions become closely related to the transition of water molecules from the interfacial region to the bulk water. It is inferred that hydrophobic interactions may depend on the shape of the solute surface. To enhance the strength of hydrophobic interactions, the solutes tend to aggregate, thereby minimizing their surface area-to-volume ratio. This also suggests that hydrophobic interactions may exhibit directional characteristics. Moreover, this phenomenon can be supported by calculated potential mean forces (PMFs) using molecular dynamics (MD) simulations, where different surfaces, such as convex, flat, or concave, are associated with a sphere. Furthermore, this concept can be extended to comprehend the molecular packing parameter, commonly utilized in studying the self-assembly behavior of amphiphilic molecules in aqueous solutions.


Introduction
The term "hydrophobic" stems from the Greek words "hydros", meaning water, and "phobos", signifying fear.Hydrophobic effects denote the inclination of nonpolar molecules or segments thereof to cluster in aqueous environments (or to be expelled from water, forming specific complexes in solutions).They are widespread and are considered the primary driving force behind numerous biological and biochemical phenomena, including the spontaneous organization of molecules with both hydrophilic and hydrophobic regions in water [1][2][3].It is well-established that dissolved molecules aggregate to form structures with diverse geometric configurations, such as spherical, globular, rod-like, or bilayers [1][2][3].As a result, self-assembly processes are increasingly exploited to design and produce highly organized materials with functional or physical properties distinct from those of their individual components.Therefore, hydrophobic effects have attracted considerable attention, and numerous works [4][5][6][7][8][9][10][11][12][13][14][15][16][17][18] have been carried out.
In the early 1940s, Frank and Evans [4] introduced the renowned "iceberg" model of hydrophobic effects, suggesting that water molecules assemble into an ordered "cage" structure around small hydrophobic solutes like argon or methane.However, dissolving large solutes in water can disrupt the hydrogen bonds of water molecules [5], leading to an enthalpic penalty.To explore the relationship between hydrophobic interactions and solute size, Lum, Chandler, and Weeks (LCW) [6][7][8][9] developed a theoretical framework.In the LCW theory, Gaussian density fluctuations for small solutes and the physics of interface formation for large solutes reflect the dependence of hydrophobic hydration on solute size.Additionally, a crossover between small and large solutes is anticipated at the nanometer length scale [8].In our recent works [16][17][18], we derived hydration free Molecules 2024, 29, 2601 2 of 15 energy to investigate the mechanism of hydrophobic effects.As solute size increases, it is reasonably partitioned into initial and hydrophobic solvation processes [16,18].Moreover, distinct behaviors of solutes in water can be anticipated during the initial and hydrophobic solvation processes, leading to dispersed or aggregated distributions in solutions [16][17][18].
Mathematically, solute curvature can broadly be categorized as positive curvature (convex), zero curvature (flat surface), and negative curvature (concave).Experimental and computational studies [19,20] have revealed differences in the solvation of convex, flat, and concave surfaces.This differentiation is ascribed to the influence of external surfaces on water hydrogen bonding.On a concave surface, water molecules are unable to form as many connections with other water molecules as they can on more exposed surfaces, such as flat and convex surfaces [19,20].
This study is aimed at investigating the dependence of hydrophobic interactions on the geometric shape of the solute surface.Owing to hydrophobic interactions, the solutes tend to be aggregated in a specific direction to minimize the ratio of the surface area to the volume of solutes [16,18].Therefore, hydrophobic interactions may be closely related to the shape of the solute surface.This relationship can be elucidated through the PMF calculations obtained via MD simulations, where a sphere is associated with various surfaces, including convex, flat, or concave.Moreover, this can be extended to elucidate the molecular packing parameter, a metric commonly employed to investigate the self-assembly dynamics of amphiphilic molecules in aqueous solutions.

Thermodynamic Analysis
In thermodynamics, Gibbs free energy (∆G) serves as a useful tool for determining whether a process is favored (∆G < 0) or disfavored (∆G > 0).When solutes are dissolved in water, the total thermodynamic functions can be expressed as follows, ∆G Total = ∆G Solute-solute + ∆G Solute-water + ∆G Water-water (1) Before the solutes are affected by the direct solute-solute interactions, they must approach each other in solution.This process is undoubtedly related to the changes in ∆G associated with water-water (∆G Water-water ) and solute-water (∆G Solute-water ) interactions.To understand the mechanisms underlying hydrophobic effects, it is essential to investigate the structure of liquid water, and the effects of solutes on water structure.
OH vibrations are sensitive to the hydrogen bonding network of water, and are widely used to investigate the structure of liquid water [21,22].Water molecular clusters, denoted as (H 2 O) n , offer insights into the relationship between OH vibrations and hydrogen-bonded networks.Based on our recent studies [23], when the three-dimensional hydrogen bonds appear (≥6), distinct OH vibrational frequencies correspond to various hydrogen-bonded networks within the first shell of a water molecule (local hydrogen bonding), while the effects of hydrogen bonding beyond the first shell on OH vibrations are weak.
To understand the structure of water, various structural models have been proposed, and these can be roughly categorized into two groups: mixture and continuum models [24][25][26][27][28][29][30][31].In Raman spectroscopic studies [23] on liquid water, the local statistical model (LSM) has been proposed.This model suggests that a water molecule interacts with neighboring water molecules (in the first shell) through various local hydrogen-bonded networks, such as DDAA (double donor-double acceptor, tetrahedral hydrogen bonding), DDA (double donor-single acceptor), DAA (single donor-double acceptor), DA (single donor-single acceptor), and free OH vibrations [23].
As a solute is embedded into water, a solute-water interface is expected to appear, which may affect the structure of water.When the three-dimensional hydrogen bonds occur in water, the OH vibrations may be closely related to the local hydrogen bonds of a water molecule [23].Consequently, the solute predominantly affects the topmost water layer at the solute-water interface, referred to as interfacial water.Hence, during the time in which a solute is dissolved in water, it can be divided into interfacial and bulk water.
Therefore, the effects of the solute on the water structure (∆G Solute-water ) may be closely associated with the solute-water interface.
Based on a vibrational sum frequency generation (SFG) study [32] on the air-water interface, no tetrahedral (DDAA) hydrogen bonding is expected to be present in the interfacial water.Once the ratio of the interfacial water layer to volume is determined, it is used to determine the Gibbs free energy between the solute and water (∆G Solute-water ).
Here, ∆G DDAA represents the Gibbs free energy of DDAA (tetrahedral) hydrogen bonding, R Interfacial water/volume denotes the molecular number ratio of the interfacial water layer to volume, and n HB represents the average number of hydrogen bonds per molecule.At 293 K and 0.1 MPa, ∆G DDAA is calculated to be −2.66 kJ/mol.
The hydration free energy represents the change in Gibbs free energy as an ion or molecule is transferred from a vacuum or gas phase to a solvent.For a spherical solute, the ratio of interfacial water layer to volume (R Interfacial water/volume ) can be expressed as 4•r H2O /R, where R is the radius of the solute [16].Consequently, when the spherical solute is immersed in water, the hydration free energy can be expressed as follows (Figure 1): where ∆G Water-water represents the Gibbs free energy of water.At 293 K and 0.1 MPa, ∆G Water-water is −1500 cal/mol [33].Under ambient conditions, the average volume of a water molecule is approximately 3 × 10 −29 m 3 .Assuming it is a sphere, r H2O is 1.9 Å.
Based on a vibrational sum frequency generation (SFG) study [32] on the air-wate interface, no tetrahedral (DDAA) hydrogen bonding is expected to be present in the inter facial water.Once the ratio of the interfacial water layer to volume is determined, it is used to determine the Gibbs free energy between the solute and water (ΔGSolute-water).The hydration free energy represents the change in Gibbs free energy as an ion o molecule is transferred from a vacuum or gas phase to a solvent.For a spherical solute the ratio of interfacial water layer to volume (RInterfacial water/volume) can be expressed as 4•rH2O/R, where R is the radius of the solute [16].Consequently, when the spherical solute is immersed in water, the hydration free energy can be expressed as follows (Figure 1 where ∆GWater-water represents the Gibbs free energy of water.At 293 K and 0.1 MPa, ∆GWater water is −1500 cal/mol [33].Under ambient conditions, the average volume of a water mole cule is approximately 3 × 10 −29 m 3 .Assuming it is a sphere, rH2O is 1.9 Å.
In thermodynamics, the stability of a system is inversely related to its hydration free energy: the lower the hydration free energy, the more stable the system.The hydration free energy comprises the sum of ΔGWater-water and ΔGSolute-water.It may be dominated by either ΔGWater-water or ΔGSolute-water, depending on the size of the dissolved solute.Thus, a structural transition is anticipated to occur when ΔGWater-water equals ΔGSolute-water.In thermodynamics, the stability of a system is inversely related to its hydration free energy: the lower the hydration free energy, the more stable the system.The hydration free energy comprises the sum of ∆G Water-water and ∆G Solute-water .It may be dominated by either ∆G Water-water or ∆G Solute-water , depending on the size of the dissolved solute.Thus, a structural transition is anticipated to occur when ∆G Water-water equals ∆G Solute-water .
where Rc represents the critical radius of the solute [16].At 293 K and 0.1 MPa, Rc is 6.5 Å for a sphere hydrophobic solute (Figure 1).As the size of the solute increases, it undergoes initial and hydrophobic solvation processes.Furthermore, ∆G Solute-water is proportional to the ratio of the surface area to the volume of solute (1/R).Consequently, various solute dissolution behaviors in water may be expected during the initial and hydrophobic solvation processes.
In the initial solvation process, where ∆G Solute-water is less than ∆G Water-water , hydration free energy is primarily governed by ∆G Solute-water [16,17].To achieve thermodynamic stability, maximizing the absolute value of ∆G Solute-water is crucial.Consequently, dissolved solutes tend to disperse in aqueous solutions, with water molecules expected to exist between the solutes.However, during the hydrophobic solvation process, the Gibbs free energy of interfacial water exceeds that of bulk water (∆G Solute-water > ∆G Water-water ).To achieve more thermodynamic stability, maximizing the magnitude of ∆G Water-water becomes crucial.This is accompanied by the minimization of the Gibbs free energy of interfacial water (|∆G Solute-water |).Consequently, dissolved solutes tend to aggregate in solutions to minimize their surface area-to-volume ratio [16,17].
Due to hydrophobic interactions, the solutes are attracted and aggregated in aqueous solutions to maximize the hydrogen bonds of water.As solute surfaces come into contact, the available surface area for interfacial water inevitably decreases.Consequently, as solutes accumulate in water, the Gibbs free energy associated with interfacial water can be expressed as follows: ∆G Interfacial water = γ•∆G Solute-water (5) in which γ represents the geometric factor [17].It is introduced to reflect the changes in solute surfaces available for interfacial water as solutes aggregate in solutions.In fact, during the time in which solutes associate in water, changes in solute volume may also occur.Consequently, γ can be given as follows: in which r Separation denotes the distance between the solutes.When solute surfaces come into contact, the corresponding distance between them is termed the hydrophobic radius (R H ) [17].With reference to R H (or γ), the hydrophobic solvation process can be reasonably divided into H1w and H2s hydrophobic solvation processes.
In the H1w hydrophobic process, the separation between solutes exceeds R H (>R H ), or γ equals 1 [11], and no molecular surface aggregation is anticipated.As the distance between solutes decreases, water molecules within the inter-solute region are expelled into bulk water.Consequently, energy barriers may arise in the H1w process, likely due to the expulsion of water molecules.As a result, dissolved solutes are expected to approach each other in the direction with the lowest energy barrier, where fewer water molecules are expelled [34].However, in the H2s hydrophobic process, the surfaces of dissolved solutes come into contact, resulting in γ being less than 1 (γ < 1).The aggregation of solute surfaces inevitably reduces the available surface area for interfacial water.To achieve greater thermodynamic stability, the solutes may aggregate to minimize their surface areato-volume ratio.Thus, in the H2s solvation process, the directional nature of hydrophobic interactions is also expected.Consequently, different directional tendencies are found in the H1w and H2s processes [34].
During the aggregation of solutes in water, a phenomenon akin to the liquid-gas phase transition, known as the dewetting transition, may be observed [35,36].To date, dewetting has been observed in numerous theoretical simulations involving nanotubes, plates in water [37,38], water-protein interfaces [39], and collapsing polymers [40].From our recent study [17,18], dewetting may be closely associated with H2s hydrophobic processes, wherein a single water layer between solutes is expelled, leading to solutes making contact in solutions.
As solutes associate in solutions, interfacial water molecules within the region between solutes may be expelled into bulk water, which may be closely associated with hydrophobic interactions.Therefore, the strength of hydrophobic interactions may be dependent on the number of water molecules transitioning from interfacial to bulk water, which can be expressed as follows: Here, the first (second) term represents the Gibbs energy of interfacial water after (before) solutes are aggregated in aqueous solutions.Additionally, n Interfacial→bulk water represents the number of water molecules transitioning from interfacial to bulk water during the association of solutes in solutions.
Owing to hydrophobic interactions, dissolved solutes tend to aggregate in aqueous solutions.Maximizing hydrophobic interactions may lead to the minimization of the surface area-to-volume ratio of solutes.To achieve greater thermodynamic stability, more interfacial water is expected to transition into bulk water as solutes aggregate in water.Because the solutes primarily affect the structure of interfacial water, the strength of hydrophobic interactions is closely linked to the geometric characteristics of the solute, such as its shape and size.For instance, when a sphere is associated with solutes having various surfaces, it tends to aggregate preferentially with convex surfaces compared to flat or concave surfaces.
When solutes are immersed in water, they must first approach each other before they can experience direct solute-solute interactions, such as van der Waals forces.Undoubtedly, hydrophobic interactions play a pivotal role as fundamental driving forces when solutes aggregate in solutions.Additionally, hydrophobic interactions may be related to the geometric characteristics of the solute, including its size and shape.Therefore, manipulating the geometric characteristics of solutes, such as their size and surface shape, can be applied to engineer "designed materials".
Hydrophobic interactions are the most important nonspecific interactions and are regarded to play an important role in the self-assembly process of amphiphilic molecules in water [41][42][43][44].This work may be applied to understand the concept of molecular packing parameters.The parameter was proposed by Israelachvili, Mitchell, and Ninham [2], which is defined as v 0 /aI 0 , where v 0 and I 0 are the volume and the length of the surfactant tail and a is the surface area of the hydrophobic core of the aggregate expressed per molecule in the aggregate.It is well known that the following connection exists between the molecular packing parameter and the aggregate shape: 0 ≤ v 0 /aI 0 ≤ 1/3 for sphere, 1/3 ≤ v 0 /aI 0 ≤ 1/2 for cylinder, and 1/2 ≤ v 0 /aI 0 ≤ 1 for bilayer [3].Thus, upon determining the molecu- lar packing parameter, the shape and size of the equilibrium aggregate become readily discernible.This underscores the relationship between hydrophobic interactions and the geometric shape of interacting particles.
In the hydrophobic solvation process, the Gibbs energy of bulk water (∆G Water-water ) is lower than that of interfacial water (∆G Solute-water ), indicating a thermodynamically favorable state for solute aggregation in solutions.It seems that "attractive" forces exist between them.During the time in which the solutes are accumulated in solutions, a transition from interfacial to bulk water occurs.To maximize the hydrogen bonding of water, the solutes tend to aggregate to minimize their surface area-to-volume ratio.Therefore, hydrophobic interactions may be dependent on the geometric shape of the solute.

MD Simulations
In mathematics, the curvature of a solute surface can be roughly categorized as convex, flat, and concave.Moreover, the minimum ratio of surface area to volume is expected when the sphere aggregates with the concave surface of the solute.From the discussion on the dependence of hydrophobic interactions on the surface shape of solute, different hydrophobic interactions may be expected, as a sphere is associated with the various surfaces mentioned above.This variation may be related to the transformation of water molecules from interfacial to bulk water as the sphere is accumulated with the solute surface.
In this work, to understand the dependence of hydrophobic interactions on the solute shape, a test solute is constrained to move to various surfaces of a target solute.The test solute is a C 60 fullerene, and the target solute is graphite composed of different surfaces, such as concave, flat, and convex surfaces (Figure 2).In this study, during the time in which C 60 fullerene is associated with various surfaces of the target solute, PMFs are calculated through umbrella sampling (US) [45][46][47] combined with the Weighted Histogram Analysis Method (WHAM) [48][49][50].Based on the calculated PMFs, these may be utilized to understand the effects of surface shape on hydrophobic interactions.faces mentioned above.This variation may be related to the transformation of water molecules from interfacial to bulk water as the sphere is accumulated with the solute surface.
In this work, to understand the dependence of hydrophobic interactions on the solute shape, a test solute is constrained to move to various surfaces of a target solute.The test solute is a C60 fullerene, and the target solute is graphite composed of different surfaces, such as concave, flat, and convex surfaces (Figure 2).In this study, during the time in which C60 fullerene is associated with various surfaces of the target solute, PMFs are calculated through umbrella sampling (US) [45][46][47] combined with the Weighted Histogram Analysis Method (WHAM) [48][49][50].Based on the calculated PMFs, these may be utilized to understand the effects of surface shape on hydrophobic interactions.
According to the US calculations, the PMF profiles can be determined for the association of C60 fullerene with various surfaces of graphite in water (Figure 3).Upon decreasing the separation between C60 and graphite, three minima are observed in the calculated PMFs.The first minimum represents the contact minimum, with respective distances of 1.75 Å, 15.45 Å, and 19.75 Å for the C60-concave, C60-flat, and C60-convex surfaces.The second minimum corresponds to the solvent-separated PMF, indicating that only one water molecular layer can enter the space between the C60 fullerenes and graphite (Figure 3).These minima are located at 6.25 Å, 18.65 Å, and 23.05 Å, respectively.Additionally, a third minimum, positioned at 10.65 Å, 21.65 Å, and 23.05 Å, is also found in the calculated PMF curves, indicating the presence of a double water molecular layer between the test and target solutes (Figure 3).Furthermore, these are in accordance with other MD simulations [17,[51][52][53][54] regarding the calculated PMFs of C60-C60 in water, and CH4-CH4 in water.According to the US calculations, the PMF profiles can be determined for the association of C 60 fullerene with various surfaces of graphite in water (Figure 3).Upon decreasing the separation between C 60 and graphite, three minima are observed in the calculated PMFs.The first minimum represents the contact minimum, with respective distances of 1.75 Å, 15.45 Å, and 19.75 Å for the C 60 -concave, C 60 -flat, and C 60 -convex surfaces.The second minimum corresponds to the solvent-separated PMF, indicating that only one water molecular layer can enter the space between the C 60 fullerenes and graphite (Figure 3).These minima are located at 6.25 Å, 18.65 Å, and 23.05 Å, respectively.Additionally, a third minimum, positioned at 10.65 Å, 21.65 Å, and 23.05 Å, is also found in the calculated PMF curves, indicating the presence of a double water molecular layer between the test and target solutes (Figure 3).Furthermore, these are in accordance with other MD simulations [17,[51][52][53][54]    From Figure 3, energy barriers are observed between neighboring minima in the calculated PMFs.These barriers may arise from the expulsion of a single water layer within the confined volume as the solutes move closer together.This suggests that the water molecules between the solutes are progressively expelled into the bulk water, layer by layer, as the solutes approach each other.Consequently, the energy barrier is closely associated with the expulsion of water molecules during the association of solutes in solutions.
In addition, during the time in which the C60 is associated with various surfaces of graphite, obvious differences can be found in the calculated PMFs, especially at the first minimum, and the first energy barrier.Based on the calculated PMFs (Figure 3), the first minimum is ranked as follows: (first minimum)C60-concave < (first minimum)C60-flat < (first minimum)C60-convex.Additionally, the first energy barrier is listed as, (first energy barrier)C60concave > (first energy barrier)C60-flat > (first energy barrier)C60-convex.Therefore, as C60 is associated with graphite, PMFs are dependent on the shape of solute surfaces.
To understand the water-induced contributions (ΔGWater-induced) as C60 is associated with different surfaces of graphite in water, the PMFs between solutes in a vacuum are also calculated using the US method (Figure 3).From the calculated PMFs, the water-induced contributions can be determined as follows: Based on the calculated water-induced contributions (ΔGWater-induced) (Figure 3), these can be utilized to investigate the dependence of hydrophobic interactions on the solute shape during their association in solutions.
According to the calculated water-induced contributions (ΔGWater-induced), in combination with our recent studies on hydrophobic interactions [16,17], "attractive" hydrophobic interactions may be expected between the fullerene and graphite.Additionally, different ΔGWater-induced values can be found as the C60 is associated with various surfaces of graphite.Therefore, the water-induced PMFs are dependent on the geometric shape of the solute surface.From Figure 3, they may be listed as follows: (ΔGWater-induced)C60-concave > (ΔGWater- From Figure 3, energy barriers are observed between neighboring minima in the calculated PMFs.These barriers may arise from the expulsion of a single water layer within the confined volume as the solutes move closer together.This suggests that the water molecules between the solutes are progressively expelled into the bulk water, layer by layer, as the solutes approach each other.Consequently, the energy barrier is closely associated with the expulsion of water molecules during the association of solutes in solutions. In addition, during the time in which the C 60 is associated with various surfaces of graphite, obvious differences can be found in the calculated PMFs, especially at the first minimum, and the first energy barrier.Based on the calculated PMFs (Figure 3), the first minimum is ranked as follows: (first minimum) C60-concave < (first minimum) C60-flat < (first minimum) C60-convex .Additionally, the first energy barrier is listed as, (first energy barrier) C60-concave > (first energy barrier) C60-flat > (first energy barrier) C60-convex .Therefore, as C 60 is associated with graphite, PMFs are dependent on the shape of solute surfaces.
To understand the water-induced contributions (∆G Water-induced ) as C 60 is associated with different surfaces of graphite in water, the PMFs between solutes in a vacuum are also calculated using the US method (Figure 3).From the calculated PMFs, the water-induced contributions can be determined as follows: Based on the calculated water-induced contributions (∆G Water-induced ) (Figure 3), these can be utilized to investigate the dependence of hydrophobic interactions on the solute shape during their association in solutions.
According to the calculated water-induced contributions (∆G Water-induced ), in combination with our recent studies on hydrophobic interactions [16,17], "attractive" hydrophobic interactions may be expected between the fullerene and graphite.Additionally, different ∆G Water-induced values can be found as the C 60 is associated with various surfaces of graphite.Therefore, the water-induced PMFs are dependent on the geometric shape of the solute surface.From Figure 3, they may be listed as follows: (∆G Water-induced ) C60-concave > (∆G Water-induced ) C60-flat > (∆G Water-induced ) C60-convex .The strongest hydrophobic interactions are expected as C 60 is aggregated with the concave surface of the target solute, which is also in accordance with the minimization of the surface area-to-volume ratio of solutes.
From the above discussion, when C 60 associates with graphite, the hydrophobic interactions may depend on the separation between them.During the time in which C 60 associates with the concave surface of graphite, hydrophobic interactions can be fit as a function of the distance (r) between fullerene and graphite (Figure 4): where r 0 is the solute-solute distance at the first minimum of the PMFs when solutes are aggregated in a vacuum, and r − r 0 means the separation between them.Additionally, the coefficients a and b are fitted to be −21.01 and 27.62, respectively.
aggregated in a vacuum, and r − r0 means the separation between them.Additionally, the coefficients a and b are fitted to be −21.01 and 27.62, respectively.
In the works of Ball [55,56], water is recognized as an active participant in cell biology.It is widely acknowledged that water plays a crucial role in mediating hydrophobic interactions.During the hydrophobic solvation process, dissolved solutes are attracted and tend to aggregate within the water.As the distance between solute molecules decreases, water molecules within the region between them may be forced out into the bulk water.To understand the dependence of hydrophobic interactions on the geometric shape of the solute surface, it is essential to investigate the rearrangement of water molecules when fullerene associates with various surfaces of graphite in aqueous solutions.
As a solute becomes immersed in water, an interface emerges between the solute and water, inevitably influencing the structure of water.Recently, numerous experimental studies [57][58][59][60][61] have been conducted to investigate the effects of dissolved solutes on water structure.These studies suggest that the effects of ions on water are primarily confined to the first solvation shell.Indeed, this observation can also be elucidated through the dependence of OH vibrations on the hydrogen bonding network of water [23].Consequently, the dissolved solute mainly affects the structure of interfacial water at the solutewater interface [23].From the MD simulations, decreasing the distance between the C60 and the solute surface leads to a decrease in the amount of interfacial water, but an increase in that of In the works of Ball [55,56], water is recognized as an active participant in cell biology.It is widely acknowledged that water plays a crucial role in mediating hydrophobic interactions.During the hydrophobic solvation process, dissolved solutes are attracted and tend to aggregate within the water.As the distance between solute molecules decreases, water molecules within the region between them may be forced out into the bulk water.To understand the dependence of hydrophobic interactions on the geometric shape of the solute surface, it is essential to investigate the rearrangement of water molecules when fullerene associates with various surfaces of graphite in aqueous solutions.
As a solute becomes immersed in water, an interface emerges between the solute and water, inevitably influencing the structure of water.Recently, numerous experimental studies [57][58][59][60][61] have been conducted to investigate the effects of dissolved solutes on water structure.These studies suggest that the effects of ions on water are primarily confined to the first solvation shell.Indeed, this observation can also be elucidated through the dependence of OH vibrations on the hydrogen bonding network of water [23].Consequently, the dissolved solute mainly affects the structure of interfacial water at the solute-water interface [23].
From the MD simulations, decreasing the distance between the C 60 and the solute surface leads to a decrease in the amount of interfacial water, but an increase in that of bulk water (Figure 5).Therefore, as solutes are aggregated in water, the interfacial water may be expected to change into bulk water.In other words, regarding the hydrophobic interactions, they may be closely related to the transition from interfacial to bulk water.In addition, the obvious changes from interfacial to bulk water, dewetting, is found as the separation between solutes, R H (Figure 5).With a decreasing solute-solute distance, this is divided into H1w and H2s hydrophobic processes.
Molecules 2024, 29, x FOR PEER REVIEW 9 of 15 bulk water (Figure 5).Therefore, as solutes are aggregated in water, the interfacial water may be expected to change into bulk water.In other words, regarding the hydrophobic interactions, they may be closely related to the transition from interfacial to bulk water.In addition, the obvious changes from interfacial to bulk water, dewetting, is found as the separation between solutes, RH (Figure 5).With a decreasing solute-solute distance, this is divided into H1w and H2s hydrophobic processes.In the H1w hydrophobic process, water molecules may be found between solutes.When decreasing the amount of separation between solutes, the water molecules in the region between them may be expelled into bulk water.Therefore, this relates to the molecular reorganization between interfacial and bulk water during the H1w process.However, the solute surfaces begin to become a contact in the H2s process.In combination with our recent studies [17,18], dewetting may be closely related to H2s hydrophobic processes, in which a single water layer between solutes is expelled, and solutes come into contact in aqueous solutions.
Additionally, in our recent study [34], various directional natures are found in the H1w and H2s processes.In the H1w process, dissolved solutes are expected to approach each other in a specific direction characterized by the lowest energy barrier, resulting in fewer expelled water molecules.In the H2s process, to maximize the hydrogen bonding of water (or bulk water), the dissolved solutes are expected to aggregate in order to minimize the surface area-to-volume ratio.It is inferred that C60 tends to pass through the corners (or edges) of graphite and to be aggregated with the concave surface of graphite.This is supported by free MD simulations conducted during their accumulation in water (Supplementary Materials).
Various hydrophobic interactions may be found as C60 associates with different surfaces of graphite (Figure 4).Consequently, hydrophobic interactions exhibit dependency on the geometric shape of the solute surface.Additionally, based on MD simulations, as the sphere aggregates with various surfaces of graphite, the number of water molecules transformed from interfacial to bulk water (H2OInterfacial→bulk water) can be determined.It is evident that the ΔGWater-induced is proportional to the H2OInterfacial→bulk water (Figure 6).This is in agreement with the theoretical analysis of the effects of the geometric shape of the solute surface on hydrophobic interactions, as discussed above.In the H1w hydrophobic process, water molecules may be found between solutes.When decreasing the amount of separation between solutes, the water molecules in the region between them may be expelled into bulk water.Therefore, this relates to the molecular reorganization between interfacial and bulk water during the H1w process.However, the solute surfaces begin to become a contact in the H2s process.In combination with our recent studies [17,18], dewetting may be closely related to H2s hydrophobic processes, in which a single water layer between solutes is expelled, and solutes come into contact in aqueous solutions.
Additionally, in our recent study [34], various directional natures are found in the H1w and H2s processes.In the H1w process, dissolved solutes are expected to approach each other in a specific direction characterized by the lowest energy barrier, resulting in fewer expelled water molecules.In the H2s process, to maximize the hydrogen bonding of water (or bulk water), the dissolved solutes are expected to aggregate in order to minimize the surface area-to-volume ratio.It is inferred that C 60 tends to pass through the corners (or edges) of graphite and to be aggregated with the concave surface of graphite.This is supported by free MD simulations conducted during their accumulation in water (Supplementary Materials).
Various hydrophobic interactions may be found as C 60 associates with different surfaces of graphite (Figure 4).Consequently, hydrophobic interactions exhibit dependency on the geometric shape of the solute surface.Additionally, based on MD simulations, as the sphere aggregates with various surfaces of graphite, the number of water molecules transformed from interfacial to bulk water (H 2 O Interfacial→bulk water ) can be determined.It is evident that the ∆G Water-induced is proportional to the H 2 O Interfacial→bulk water (Figure 6).This is in agreement with the theoretical analysis of the effects of the geometric shape of the solute surface on hydrophobic interactions, as discussed above.Due to hydrophobic interactions, dissolved solutes tend to be aggregated in aqueous environments, resulting in the transition from interfacial to bulk water.This transition highlights the relationship between hydrophobic interactions and the transformation of water molecules from interfacial to bulk water during solute aggregation.Because the solutes mainly affect the structure of interfacial water, the expulsion of water molecules during the transition from interfacial to bulk water may depend on the geometric shape of the solute surface.From the simulations, compared to flat and convex graphite, more water molecules are transformed from interfacial to bulk water when C60 is associated with the concave surface of graphite (Figure 5).Therefore, the strongest hydrophobic interactions are expected between the fullerene and the concave surface of graphite.
To maximize the hydrogen bonding of water (or bulk water), the dissolved solutes are expected to aggregate in order to minimize the surface area-to-volume ratio.This strategy corresponds to a specific orientation where more interfacial water molecules can be transformed into bulk water during the accumulation of solutes in aqueous solutions.In fact, the directional nature observed in the H2s process can be attributed to the maximization of hydrophobic interaction strength as solutes aggregate in aqueous solutions.
Due to the formation of hydrogen bonds between water molecules, water is generally regarded as an anomalous liquid.To date, various definitions of hydrogen bonds have been proposed.In this work, the geometrical definition of hydrogen bonding is employed to determine whether a hydrogen bond is formed or not [62].Specifically, a hydrogen bond is considered to exist between two neighboring water molecules when the oxygenoxygen distance (ROO) is less than 3.5 Å, and the ∠OOH angle between the two water molecules is less than 30°.In this study, the hydrogen bonding of water is calculated using the Visual Molecular Dynamics program [63].
From the MD simulations, the average number of hydrogen bonds per water molecule (nHB) can be determined during the association of C60 with the concave surface of the target solute (Figure 7).Compared to bulk water, a lower number of hydrogen bonds are observed in interfacial water.This is due to the truncation of hydrogen bonds at the solute-water interface.Regarding the origin of hydrophobic interactions, it is ascribed to the hydrogen bonds of bulk water being stronger than those of interfacial water.To maximize the hydrogen bonding of water, the dissolved solutes tend to aggregate in solutions.From a thermodynamic perspective, this aggregation process can be reasonably considered as an enthalpic process.Due to hydrophobic interactions, dissolved solutes tend to be aggregated in aqueous environments, resulting in the transition from interfacial to bulk water.This transition highlights the relationship between hydrophobic interactions and the transformation of water molecules from interfacial to bulk water during solute aggregation.Because the solutes mainly affect the structure of interfacial water, the expulsion of water molecules during the transition from interfacial to bulk water may depend on the geometric shape of the solute surface.From the simulations, compared to flat and convex graphite, more water molecules are transformed from interfacial to bulk water when C 60 is associated with the concave surface of graphite (Figure 5).Therefore, the strongest hydrophobic interactions are expected between the fullerene and the concave surface of graphite.
To maximize the hydrogen bonding of water (or bulk water), the dissolved solutes are expected to aggregate in order to minimize the surface area-to-volume ratio.This strategy corresponds to a specific orientation where more interfacial water molecules can be transformed into bulk water during the accumulation of solutes in aqueous solutions.In fact, the directional nature observed in the H2s process can be attributed to the maximization of hydrophobic interaction strength as solutes aggregate in aqueous solutions.
Due to the formation of hydrogen bonds between water molecules, water is generally regarded as an anomalous liquid.To date, various definitions of hydrogen bonds have been proposed.In this work, the geometrical definition of hydrogen bonding is employed to determine whether a hydrogen bond is formed or not [62].Specifically, a hydrogen bond is considered to exist between two neighboring water molecules when the oxygen-oxygen distance (R OO ) is less than 3.5 Å, and the ∠OOH angle between the two water molecules is less than 30 • .In this study, the hydrogen bonding of water is calculated using the Visual Molecular Dynamics program [63].
From the MD simulations, the average number of hydrogen bonds per water molecule (n HB ) can be determined during the association of C 60 with the concave surface of the target solute (Figure 7).Compared to bulk water, a lower number of hydrogen bonds are observed in interfacial water.This is due to the truncation of hydrogen bonds at the solute-water interface.Regarding the origin of hydrophobic interactions, it is ascribed to the hydrogen bonds of bulk water being stronger than those of interfacial water.To maximize the hydrogen bonding of water, the dissolved solutes tend to aggregate in solutions.From a thermodynamic perspective, this aggregation process can be reasonably considered as an enthalpic process.Due to hydrophobic interactions, the solutes are attracted to form the aggregate in water (Figure 8).While the solutes are aggregated in water, the interfacial water molecules between solutes may be expelled into bulk water, which may be related to the strength of hydrophobic interactions.To maximize the hydrogen bonding of water, the solutes may be aggregated to minimize their surface area-to-volume ratio.The dissolved solutes mainly affect the hydrogen bonding of interfacial water.Therefore, hydrophobic interactions are dependent on the geometric shape of the solute (Figure 8).Due to hydrophobic interactions, the solutes are attracted to form the aggregate in water (Figure 8).While the solutes are aggregated in water, the interfacial water molecules between solutes may be expelled into bulk water, which may be related to the strength of hydrophobic interactions.To maximize the hydrogen bonding of water, the solutes may be aggregated to minimize their surface area-to-volume ratio.The dissolved solutes mainly affect the hydrogen bonding of interfacial water.Therefore, hydrophobic interactions are dependent on the geometric shape of the solute (Figure 8).Due to hydrophobic interactions, the solutes are attracted to form the aggregate in water (Figure 8).While the solutes are aggregated in water, the interfacial water molecules between solutes may be expelled into bulk water, which may be related to the strength of hydrophobic interactions.To maximize the hydrogen bonding of water, the solutes may be aggregated to minimize their surface area-to-volume ratio.The dissolved solutes mainly affect the hydrogen bonding of interfacial water.Therefore, hydrophobic interactions are dependent on the geometric shape of the solute (Figure 8).

Figure 1 .
Figure 1.Hydration free energy at 293 K and 0.1 MPa.It is the sum of the Gibbs energies of the bulk (∆GWater-water) and interfacial (∆GSolute-water) water.With reference to Rc, it is divided into initial and hydrophobic solvation processes, respectively.

Figure 1 .
Figure 1.Hydration free energy at 293 K and 0.1 MPa.It is the sum of the Gibbs energies of the bulk (∆G Water-water ) and interfacial (∆G Solute-water ) water.With reference to Rc, it is divided into initial and hydrophobic solvation processes, respectively.

Figure 2 .
Figure 2. Simulated systems used to investigate the dependence of hydrophobic interaction on the geometric shape of the solute surface.A C 60 is constrained to move to the concave (a,b), flat (c,d), and convex (e,f) surfaces of the target solute.Both initial and final configurations are shown.
regarding the calculated PMFs of C 60 -C 60 in water, and CH 4 -CH 4 in water.

Figure 2 .
Figure 2. Simulated systems used to investigate the dependence of hydrophobic interaction on the geometric shape of the solute surface.A C60 is constrained to move to the concave (a,b), flat (c,d), and convex (e,f) surfaces of the target solute.Both initial and final configurations are shown.

Figure 3 .
Figure 3. (a,c,e) The PMFs as the fullerene are associated with various surfaces of graphite in water and under vacuum at 300 K and 0.1 MPa.(b,d,f) The corresponding water-induced PMFs as solutes are aggregated in water.

Figure 3 .
Figure 3. (a,c,e) The PMFs as the fullerene are associated with various surfaces of graphite in water and under vacuum at 300 K and 0.1 MPa.(b,d,f) The corresponding water-induced PMFs as solutes are aggregated in water.

Figure 4 .
Figure 4.The water-induced PMFs as the C60 is aggregated with the concave surface of graphite at 300 K and 0.1 MPa.It is fitted as ΔGWater−induced = a + b/(r − 1.75).In reference to RH (hydrophobic radius), the hydrophobic interactions are divided into H1w and H2s hydrophobic processes.During the H1w process, γ = 1.During the H2s process, solute surfaces begin contact in water, and γ < 1.

Figure 4 .
Figure 4.The water-induced PMFs as the C 60 is aggregated with the concave surface of graphite at 300 K and 0.1 MPa.It is fitted as ∆G Water−induced = a + b/(r − 1.75).In reference to R H (hydrophobic radius), the hydrophobic interactions are divided into H1w and H2s hydrophobic processes.During the H1w process, γ = 1.During the H2s process, solute surfaces begin contact in water, and γ < 1.

Figure 5 .
Figure 5.The changes in the interfacial and bulk water as C60 is associated with the concave (a,b), flat (c,d), and convex (e,f) surfaces of graphite in water at 300 K and 1 bar.The dashed line represents the corresponding time of RH.

Figure 5 .
Figure 5.The changes in the interfacial and bulk water as C 60 is associated with the concave (a,b), flat (c,d), and convex (e,f) surfaces of graphite in water at 300 K and 1 bar.The dashed line represents the corresponding time of R H .

Figure 6 .
Figure 6.The relationship between water-induced PMFs and expelled water molecules from interfacial to bulk water as C60 is associated with various surfaces of graphite.

Figure 6 .
Figure 6.The relationship between water-induced PMFs and expelled water molecules from interfacial to bulk water as C 60 is associated with various surfaces of graphite.

Figure 7 .
Figure 7. Hydrogen bonding number per water molecule in interfacial and bulk water (a) and total water (b) as the fullerene is aggregated with the concave surface of graphite at 300 K and 0.1 MPa.

Figure 8 .
Figure 8.(a) Owing to hydrophobic interactions, the solutes are aggregated to minimize their surface area-to-volume ratio.(b) Hydrophobic interactions, related to the water molecules transformed from interfacial to bulk water, may be dependent on the solute shape.

Figure 7 .
Figure 7. Hydrogen bonding number per water molecule in interfacial and bulk water (a) and total water (b) as the fullerene is aggregated with the concave surface of graphite at 300 K and 0.1 MPa.

Molecules 2024 , 15 Figure 7 .
Figure 7. Hydrogen bonding number per water molecule in interfacial and bulk water (a) and total water (b) as the fullerene is aggregated with the concave surface of graphite at 300 K and 0.1 MPa.

Figure 8 .
Figure 8.(a) Owing to hydrophobic interactions, the solutes are aggregated to minimize their surface area-to-volume ratio.(b) Hydrophobic interactions, related to the water molecules transformed from interfacial to bulk water, may be dependent on the solute shape.

Figure 8 .
Figure 8.(a) Owing to hydrophobic interactions, the solutes are aggregated to minimize their surface area-to-volume ratio.(b) Hydrophobic interactions, related to the water molecules transformed from interfacial to bulk water, may be dependent on the solute shape.
∆GDDAA represents the Gibbs free energy of DDAA (tetrahedral) hydrogen bonding, RInterfacial water/volume denotes the molecular number ratio of the interfacial wate layer to volume, and nHB represents the average number of hydrogen bonds per molecule At 293 K and 0.1 MPa, ∆GDDAA is calculated to be −2.66 kJ/mol.