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Relevant bibliographies by topics / Kapustinskii equation

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Academic literature on the topic 'Kapustinskii equation'

Author: Grafiati

Published: 7 June 2025

Last updated: 16 July 2025

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Journal articles on the topic "Kapustinskii equation"

1

Glasser, Leslie. "Lattice Energies of Crystals with Multiple Ions: A Generalized Kapustinskii Equation." Inorganic Chemistry 34, no. 20 (1995): 4935–36. http://dx.doi.org/10.1021/ic00124a003.

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2

Robson, Fernandes de Farias. "On the reliability of volume-based thermodynamics for inorganic-organic salts and coordination compounds with uncharged ligands." Chemistry Research Journal 2, no. 6 (2017): 91–95. https://doi.org/10.5281/zenodo.13936219.

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In the present work, the reliability of the volume-based thermodynamics (VBT) methods in the calculation of lattice energies is investigated by applying the “traditional”  Kapustinskii equation [8], as well as Glasser-Jenkins [3] and Kaya [5] equations to calculate the lattice energies for Na, K and Rb pyruvates [9-11] as well as for the coordination compound [Bi(C<sub>7</sub>H<sub>5</sub>O<sub>3</sub>)<sub>3</sub>C<sub>12</sub>H<sub>8</sub>N<sub>2</sub>] [12] (in which C<sub>12</sub>H<sub>8</sub>N<sub>2</sub> = 1,10 phenathroline and C<sub>7</sub>H<sub>5</sub>O<sub>3</sub><su

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3

Robson, Fernandes de Farias. "Gaseous phase ionic formation enthalpy for 3-cyanopyridinecoordination compounds by modified forms of Kapustinskii equation." Chemistry Research Journal 1, no. 6 (2016): 1–3. https://doi.org/10.5281/zenodo.13957378.

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In the present work, it is shown that modified forms of Kapustinskii equation can be successfully employed to calculate the gaseous phase ionic formation enthalpy for coordination compounds, considering the reaction: M<sub>(g)</sub><sup>2+</sup> + 2Br<sup>-</sup><sub>(g)</sub> + n3-cyanopy<sub>(g)</sub> → [MBr<sub>2</sub>(3-cyanopy)<sub>n</sub>]<sub>(g)</sub>; cyanopy = cyanopyridine<sub>. </sub>The calculated ionic formation enthalpy (Δ<sub>fI</sub>H<sup>θ</sup>) values are compared with experimental (calorimetric) values from literature.  The derived equation is as foll

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4

Robson, F. de Farias. "Thermochemistry of Platinum Fluorides: A Computational Study." Chemistry Research Journal 2, no. 2 (2017): 121–24. https://doi.org/10.5281/zenodo.13956724.

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In the present work, thermochemical parameters for platinum fluorides: PtF<sub>2</sub>, PtF<sub>4</sub>, PtF<sub>5</sub>PtF<sub>6</sub> were calculated by quantum chemical Semi-Emprical (PM6), method and the results compared with (when available) experimental data from literature. Lattice energies are calculated by using Kapustinskii and the generalized Glasser-Jenkins equations. It was concluded that, in gaseous phase, all platinum fluorides are diamagnetic.

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5

Majzlan, Juraj, Marek Tuhý, Edgar Dachs, and Artur Benisek. "Thermodynamics of schafarzikite (FeSb2O$$_4$$) and tripuhyite (FeSbO$$_4$$)." Physics and Chemistry of Minerals 50, no. 3 (2023). http://dx.doi.org/10.1007/s00269-023-01249-2.

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AbstractIn this work, we investigated the thermodynamic properties of synthetic schafarzikite (FeSb2O$$_4$$ 4 ) and tripuhyite (FeSbO$$_4$$ 4 ). Low-temperature heat capacity ($$C_p$$ C p ) was determined by relaxation calorimetry. From these data, third-law entropy was calculated as $$110.7\pm 1.3$$ 110.7 ± 1.3 J mol$$^{-1}$$ - 1 K$$^{-1}$$ - 1 for tripuhyite and $$187.1\pm 2.2$$ 187.1 ± 2.2 J mol$$^{-1}$$ - 1 K$$^{-1}$$ - 1 for schafarzikite. Using previously published $$\Delta _fG^o$$ Δ f G o values for both phases, we calculated their $$\Delta _fH^o$$ Δ f H o as $$-947.8\pm 2.2$$ - 947.8 ±

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Book chapters on the topic "Kapustinskii equation"

1

Keeler, James, and Peter Wothers. "Ionic interactions." In Why chemical reactions happen. Oxford University Press, 2003. http://dx.doi.org/10.1093/hesc/9780199249732.003.0003.

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This chapter discusses ionic interactions. It focuses on the interaction between ions in solid materials. The chapter notes the usage of X–ray diffraction to measure the distance between ions in the lattice while referencing a lattice diagram of NaCl. It explains the force between oppositely charged objects attracted to one another. This is called electrostatic interaction. Additionally, the chapter explains the process and equations used in the formation of ion pairs and lattice. It refers to the Born–Landé equation as an expression for the energy of interaction between the ions in a crystal lattice. The chapter also mentions the Kapustinskii equation before exploring the application of other equations dealt with in the chapter.

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2

Burrows, Andrew, John Holman, Simon Lancaster, et al. "Solids." In Chemistry3. Oxford University Press, 2021. http://dx.doi.org/10.1093/hesc/9780198829980.003.0006.

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This chapter looks closely at covalent, metallic, and ionic bonding in solid state structures, which is important as the properties of solid state materials depend on their structures and bonding. Some of the characteristic/properties of molecular solids, covalent network structures, metals, and ionic solids are summarized. The chapter describes the differences between cubic close packing (ccp) and hexagonal close packing (hcp). It demonstrates how to predict the limiting radius ratio for different geometries and how to use the radius ratio rule to predict the structures of ionic compounds. It also outlines how to calculate packing efficiencies and densities, lattice enthalpies using Born–Haber cycle compounds, and lattice energies using the Born–Landé equation and the Kapustinskii equation.

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3

Almond, Matthew, Mark Spillman, and Elizabeth Page. "Solids." In Workbook in Inorganic Chemistry, edited by Elizabeth Page. Oxford University Press, 2017. http://dx.doi.org/10.1093/hesc/9780198729501.003.0004.

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This chapter focuses on solids. It begins by looking at the packing of spheres to give solid structures, identifying the types of arrangements of atoms. These include hexagonal close packing (hcp), cubic close packing (ccp), and body-centred cubic structure (bcc). The chapter then studies ionic lattices, describing a few of the most common ionic structures that are based on close packing and considering the arrangements of the ions in these structures. It also discusses the radius ratio rule, which predicts the structure that an ionic solid will adopt based upon the ratio of the cation to anion size. Finally, the chapter examines lattice enthalpy and the Born–Haber cycle, as well as the theoretical methods for calculating the lattice enthalpy, including the Born–Landé equation and the Kapustinskii equation.

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