Gibbs Energy Of Complex Formation Research Articles

Room Temperature Gas-Phase Detection and Gibbs Energies of Water Amine Bimolecular Complex Formation.

We have detected the H2O·DMA and H2O·TMA (DMA, dimethylamine; TMA, trimethylamine) bimolecular complexes at room temperature in the gas phase using Fourier transform infrared spectroscopy. For both complexes, five vibrational bands associated with the H2O molecule are observed and assigned. Within a reduced dimensional local mode framework, we set up a six-dimensional model, including the three H2O vibrational modes and three of the six intermolecular modes, all described with internal curvilinear coordinates. The single points on the potential energy surface and Eckart corrected dipole moment surface are calculated with the CCSD(T)-F12a/cc-pVDZ-F12 method. Combining the measured and calculated transition intensities, we determine the Gibbs energy of complex formation of both complexes from each of the observed bands. The multiple determinations give similar Gibbs energies, for each complex, and increase the confidence in the combined experimental and theoretical approach, and improve the accuracy of the determined Gibbs energies. The average Gibbs energies of complex formation are found to be 5.0 ± 0.2 and 3.8 ± 0.2 kJ/mol for H2O·DMA and H2O·TMA, respectively. In addition to the experimental uncertainty, there is a potential error on the calculated intensities corresponding to 0.4 kJ/mol. However, the small spread among the four determinations suggests that this error is even less. The Gibbs energies of these complexes serve as accurate benchmarks for theoretical approaches that are prevalent in hydrogen bonding and nucleation studies.

Thermodynamics of antibiotics: natural cyclodextrin inclusion complex formation and covering of nano-metric calcite with these substances

Isothermal titration calorimetry (ITC) has been used to characterize inclusion complex formation of natural (α-, β-, γ-)cyclodextrins with antibiotics (ampicillin—sodium, penicillin G—sodium, streptomycin sulfate) in aqueous solutions. ITC measurements were taken at 298.15 K on Isothermal Titration Calorimeter Nano ITC. The experimental data were analyzed on the basis of the independent site model. Based on the experimental values of equilibrium constant (K) and enthalpy of complex formation (ΔH), the Gibbs energy of complex formation (ΔG) and the entropy of complex formation (ΔS) have been calculated. The analysis of the obtained inclusion complexes show that independently of the kind of cyclodextrin and antibiotics the obtained equilibrium constants are almost the same, but it is a difference between the changes in enthalpies of complex formation for the investigated systems. The stoichiometry of complexes formed both by ampicillin—sodium and by penicillin G—sodium with all the natural cyclodextrins is the same and equal to 1:1 and the complex formation is entropy driven. Three antibiotics (ampicillin—sodium, penicillin G—sodium and streptomycin sulfate) have been used further for covering of the monodisperse calcium carbonate nanoparticles obtained in the reactor (three-phase reaction) with rotating disks. Three series of experiments have been performed. First was connected with adsorption of the antibiotics on the surface on nano-calcite and two others with intercalation of the drugs into nano-metric CaCO3 structure (aggregates). An intercalation has been performed in two ways: one where the antibiotic was added to the reactor chamber at the beginning of the precipitation reaction and second where it was added just after the end of the reaction. Both pure CaCO3 nanoparticle and antibiotic-coated CaCO3 powders were deeply analyzed by the use of the thermogravimetric and the differential scanning calorimetry method. The performed investigations showed that all the antibiotics used can be both adsorbed and intercalated into the nano-metric CaCO3 obtained in the reactor with rotating disks. The different adsorption obtained by different antibiotics was caused by the different interaction between them and nano-calcite, caused by their different structure. The experimental data have allowed also for distinction between the antibiotics molecules present on calcite surface (adsorption) or antibiotics molecules intercalated into the nano-calcite structure. The conducted research shows that both approaches, i.e., formation of inclusion complexes with natural cyclodextrins and covering (adsorption and intercalation) of nano-metric CaCO3, can be successfully implemented for their pharmaceutical applications.

Attenuated Deuterium Stabilization of Hydrogen-Bound Complexes at Room Temperature.

We have observed nine bimolecular hydrogen- or deuterium-bound complexes at room temperature using Fourier transform infrared (FTIR) spectroscopy. The complexes were formed using methanol or ethanol as hydrogen bond donors, as well as deuterated isotopologues of these, in order to study isotopic effects on hydrogen bonds. The complexes were formed using either a dimethylether- (O) or trimethylamine (N) acceptor, to facilitate comparison of two different types of hydrogen or deuterium bonds, OH(D)·O and OH(D)·N. For each complex, the characteristic OH- or OD-stretching fundamental band in the bimolecular complex was observed. The Gibbs energy of complex formation was determined at room temperature for each complex to compare the relative stability of hydrogen- and deuterium-bound bimolecular complexes. It is well known that deuterium-bound complexes are more stable at low temperatures because of the lower frequency of its intermolecular modes and thus a lower zero point vibrational energy. However, at room temperature, entropic contributions to the stability should also be considered. At room temperature, we find the Gibbs energy of complex formation for each pair of corresponding hydrogen- and deuterium-bound complex to be similar. The similar values of the Gibbs energies at room temperature is explained from a difference in the entropy, upon complexation, which favors the formation of the hydrogen-bound complex more than the deuterium-bound complex at higher temperatures.

Room Temperature Gibbs Energies of Hydrogen-Bonded Alcohol Dimethylselenide Complexes.

A number of hydrogen-bonded complexes, formed between an alcohol donor and dimethylselenide, have been detected experimentally, at room temperature in the gas phase using FTIR spectroscopy. The Gibbs energy of complex formation has been determined from the measured integrated absorbance of the hydrogen-bonded OH stretching band and the calculated oscillator strength of the associated transition. The OH stretching frequency and Gibbs energy of the selenium hydrogen-bonded complexes are compared to those found in complexes with the same donor molecule and either dimethylether (O) or dimethylsulfide (S) as the acceptor molecule. For a given donor, we found a similar OH stretching frequency in the complexes for each of the three acceptors O, S, and Se. However, the Gibbs energies were found to be less positive (i.e., stronger bound) for the dimethylether complexes (OH·O), as compared to the dimethylsulfide (OH·S) and dimethylselenide (OH·Se) complexes, with the latter two having comparable Gibbs energies.

Size makes a difference: Chiral recognition in complexes of fenchone with cyclodextrins studied by means of NMR titration

Gibbs energies of complex formation between enantiomers of bicyclic terpenoid, fenchone, and naturally occurring cyclodextrins, βCD and γCD, were determined by means of 13 C and 1 H nuclear magnetic resonance (NMR) titration data. These results were compared with the corresponding data obtained previously for the diastereomeric fenchone/αCD complexes. The size of the inner cavity of host molecules significantly influences stoichiometry, association constants, and enantiomeric differentiation of the studied complexes. These complementary data allow us to discuss qualitatively the influence of the host size on the guest-host interactions. A method of the simultaneous use of titration data collected for several resonances of different isotopes in the determination of association constants was worked out and thoroughly analyzed. Comparison of the results of global data analyses with weighted means of individual ones revealed that both these approaches are equally trustworthy.

Thermodynamics of β-cyclodextrin–ephedrine inclusion complex formation and covering of nanometric calcite with these substances

Isothermal titration calorimetry (ITC) has been used to characterize inclusion complex formation of β-cyclodextrin (β-CD) with ephedrine in aqueous solutions. ITC measurements were taken at 298.15 K on a MicroCal OMEGA ultrasensitive titration calorimeter (MicroCal Inc.). The experimental data were analyzed on the basis of the model of a single set of identical sites (ITC Tutorial Guide). Based on the experimental values of equilibrium constant (K) and enthalpy of complex formation (ΔH), the Gibbs energy of complex formation (ΔG), and the entropy of complex formation (ΔS), has been calculated. Obtained results showed that β-CD forms inclusion complex of stoichiometry 1:1 with ephedrine and the complex formation is entropy driven. Ephedrine and its complex with β-CD have been further used for covering of the obtained in a controlled way nanometric CaCO3 (calcite), which served as a solid supports for drug depositing. The calcite coating has been analyzed by the use of thermogravimetric method. The size of aggregates of pure calcite particles as well as CaCO3 particles covered by ephedrine and its complex with β-CD have been measured by DLS method. It has been found that pure CaCO3 aggregates are almost monodispersed with the mean diameter equal to 329 nm (±5 nm). Ephedrine and its complex with β-CD layers formed in situ on precipitated calcite surface prevented from crystallites aggregation and decreases particles mean diameter up to 274 nm (±5 nm) for ephedrine and 211 nm (±5 nm) for β-CD complex with ephedrine.

Isothermal titration calorimetry (ITC) study of natural cyclodextrins inclusion complexes with tropane alkaloids

Isothermal titration calorimetry (ITC) has been used to characterize inclusion complex formation of natural cyclodextrins (α- and β-cyclodextrin) with three tropane alkaloids (scopolamine, homatropine hydrobromide and atropine sulfate) in aqueous solutions. ITC measurements were taken at 298.15 K on a MicroCal OMEGA ultrasensitive titration calorimeter (MicroCal Inc.). The experimental data were analyzed on the basis of the model of a single set of identical sites (ITC Tutorial Guide). β-CD forms inclusion complexes of stoichiometry 1:2 with homatropine hydrobromide and 1:1 with scopolamine and atropine sulfate. The smaller molecule of α-CD forms very weak inclusion complexes with the tropane alkaloids. So, only one complex of the same stoichiometry 1:2 with homatropine hydrobromide has been detected by the ITC experiment. Based on the experimental values of equilibrium constant (K) and enthalpy of complex formation (ΔH), the Gibbs energy of complex formation (ΔG) and the entropy of complex formation (ΔS) have been calculated, for all the investigated systems. Obtained results showed that complex formation of both α- and β-CD with all the investigated tropane alkaloids is entropy driven. This indicated that the difference in the cavity dimensions is not reflected in different driving forces of complex formation and binding modes which resulted in the same stoichiometry of the obtained inclusion complexes.

Energy of ligand-RNA complex formation

This work presents an energetic analysis of complex formation of eleven ligands with different structure and charge with RNA aptamers. The most entire set of the components of the total Gibbs energy of complex formation has been first calculated using different physical factors: van der Waals, electrostatic and hydrophobic interactions, hydrogen bonds and specific factors being predominantly of entropic character. The calculated Gibbs energy is found to be in a good agreement with experimental data. Different energy components which stabilize and destabilize complexes are lined up according to the degree of importance. The results obtained provide an understanding of the role of different physical interactions in a ligand-RNA complex formation.

Isothermal titration calorimetry (ITC) study of natural cyclodextrins inclusion complexes with drugs

Isothermal titration calorimetry (ITC) was used to characterize inclusion complex formation of natural cyclodextrins (α- and β-cyclodextrin) with three drugs ((+)brompheniramine, (±)brompheniramine, cyclopentolate) in aqueous solutions. ITC measurements were carried out at 298.15 K on a Microcal OMEGA ultrasensitive titration calorimeter (MicroCal Inc.). The experimental data were analyzed on the basis of the model of a single set of identical sites (ITC tutorial guide). β-CD forms inclusion complexes of stoichiometry 1:1 with the all investigated drugs. In turn, smaller molecule of α-CD forms inclusion complexes of two different stoichiometry: with bigger molecules ((+)brompheniramine and (±)brompheniramine) of a stoichiometry 2:1 and with smaller molecules (cyclopentolate) of a stoichiometry 1:2. Based on the experimental values of equilibrium constant (K) and enthalpy of complex formation (ΔH), the Gibbs energy of complex formation (ΔG), and the entropy of complex formation (ΔS), have been calculated, for all the investigated systems. Obtained results showed that complex formation of β-CD (bigger molecule with wider cavity compared to β-CD) with both (+)brompheniramine, (±)brompheniramine, and cyclopentolate is enthalpy driven while complexes of α-CD with the all investigated drugs are enthalpy-entropy stabilized. This indicated that the difference in the cavity dimensions is reflecting in different driving forces of complex formation and binding modes what resulted in different stoichiometry of the obtained inclusion complexes.

Energetics of complex formation of the dna hairpin structure d(GCGAAGC) with aromatic ligands

The energy contributions of various physical interactions to the total Gibbs energy of complex formation of the biologically important DNA hairpin d(GCGAAGC) with aromatic antitumor antibiotics daunomycin and novantron and the mutagens ethidium and proflavine have been calculated. It has been shown that the relatively small value of the total energy of binding of the ligands to the hairpin is the sum of components great in absolute value and different in sign. The contributions of van der Waals interactions and both intra- and intermolecular hydrogen bonds and bonds with aqueous environment have been studied. According to the calculations, the hydrophobic and van der Waals components are energetically favorable in complex formation of the ligands with the DNA pairpin d(GCGAAGC), whereas the electrostatic (with consideration of hydrogen bonds) and entropic components are unfavorable.

Interpreting protein/DNA interactions: distinguishing specific from non-specific and electrostatic from non-electrostatic components

We discuss the effectiveness of existing methods for understanding the forces driving the formation of specific protein–DNA complexes. Theoretical approaches using the Poisson–Boltzmann (PB) equation to analyse interactions between these highly charged macromolecules to form known structures are contrasted with an empirical approach that analyses the effects of salt on the stability of these complexes and assumes that release of counter-ions associated with the free DNA plays the dominant role in their formation. According to this counter-ion condensation (CC) concept, the salt-dependent part of the Gibbs energy of binding, which is defined as the electrostatic component, is fully entropic and its dependence on the salt concentration represents the number of ionic contacts present in the complex. It is shown that although this electrostatic component provides the majority of the Gibbs energy of complex formation and does not depend on the DNA sequence, the salt-independent part of the Gibbs energy—usually regarded as non-electrostatic—is sequence specific. The CC approach thus has considerable practical value for studying protein/DNA complexes, while practical applications of PB analysis have yet to demonstrate their merit.

Complex Formation of Crown Ethers and Cations in Water–Organic Solvent Mixtures: Part XII. Effect of the Acid–Base Properties of the Mixture on the Thermodynamic Functions of Complex Formation of Benzo-15-Crown-5 with Na+ in Water–Methanol Mixtures at 298.15 K

The enthalpies of solution of benzo-15-crown-5 ether in methanol–water mixtures and methanol–water–sodium iodide systems have been measured at 298.15 K. The values of standard enthalpies of solution of benzo-15-crown-5 ether are positive in the mixtures of water and methanol within the whole range of mixture composition. The equilibrium constants of complex formation of benzo-15-crown-5 ether with the sodium cation have been determined by conductivity measurements at 298.15 K. The thermodynamic functions of the formation of these complexes have been calculated. The Gibbs energy of complex formation depends on the base–acid properties of methanol–water mixture.

Complex Formation of Crown Ethers with Cations in Water–Organic Solvent Mixtures. III. Thermodynamics of Interaction Between Na + Ion with 15-Crown-5 Ether in Water–Acetonitrile Mixtures at 25°C

Enthalpies of solution of 15-crown-5 ether in the acetonitrile–water–sodium iodide system have been measured at 25°C. The equilibrium constants of complex formation of 15C5 with sodium iodide have been determined by molar conductance at various mole ratios 15C5 to sodium iodide in mixtures of water with acetonitrile at 25°C. The thermodynamic functions for complexation of the crown ether with Na+ were calculated. From the result, the standard Gibbs energies of complex formation as a function of the normalized Lewis acidity parameters ENT and enthalpy of solvation of 15C5 in the mixtures of water with acetonitrile have been analyzed. The enthalpies of transfer of the 15C5 complex with sodium iodide from pure acetonitrile to the mixtures studied were calculated and discussed.

Binding of sodium n-dodecyl sulphate and protons to catalase

The binding of sodium n-dodecyl sulphate to catalase has been measured by equilibrium dialysis in the pH range 3.2 to 10.0. On the acid side of the isoelectric point (pH 5.4) the surfactant anions initially bind to cationic sites on the protein and subsequent binding is cooperative. At high pH on the alkaline side of the isoelectric point only cooperative binding is observed. The binding data have been combined with protein titration curves to calculate the Gibbs energies of formation of protein titration curves to calculate the Gibbs energies of formation of protein surfactant proton complexes. Contributions to the Gibbs energies of complex formation by surfactant and protein binding have been estimated. The average Gibbs energies of surfactant binding to specific cationic sites are ca. 28 kJ mol −1 and for cooperative binding ca. 15 kJ mol −1.