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Resumé Presented thesis is dedicated to specific problems of van Gogh's art. In the first chapters I investigate Heidegger's philosophy of art and his philosophical interpretation of van Gogh's painting Old shoes. Second chapter is dedicated to the critical reaction of distinguished art-historian Meyer Schapiro. Schapiro wrote two short texts, where he attacked Heidegger's way of interpretation of the painting. But Schapiro did not take into account Heidegger's philosophical arguments and completely misunderstood Heidegger's essay. Third chapter is dedicated to the "conclusion" of the conflict of interpretations. In late seventies French philosopher Jacques Derrida published an article (Restitutions), which deals with previous contributions. Derrida seriously attempted to investigate philosophical principals of Heidegger and Schapiro and he suggested, that both authors have the same tendency to appropriate the shoes to some person, in Heidegger's case to peasant woman in that of Schapiro to van Gogh. Derrida tried to leave the "theory of appropriation" by saying that the shoes belong to the painting. I also added two appendices dedicated to specific problems of van Gogh's painting. In first appendix I investigated the role of synthesis of painting and drawing in van Gogh. In second appendix I trace the...

Thesis advisor: Andre Brouillette / Thesis advisor: Brian P. Dunkle / Thesis (STL) — Boston College, 2016. / Submitted to: Boston College. School of Theology and Ministry. / Discipline: Sacred Theology.

The van der Waals forces, which are forces between neutral atoms and molecules, play an important role in physics (e.g. in phase transitions), chemistry (e.g. in chemical reactions) and biology (e.g. in determining properties of DNA). These forces are of quantum nature and it is long being conjectured and experimentally verified that they have universal behaviour at large separations: they are attractive and decay as the inverse sixth power of the pairwise distance between the atoms or molecules. In this thesis we prove the van der Waals law under the technical condition that ionization energies (energies of removing electrons) of atoms are larger than electron affinities (energies released when adding electrons). This condition is well justified experimentally as can be seen from the table, \newline \begin{tabular}{|c|c|c|c|} \hline Atomic number & Element & Ionization energy (kcal/mol)& Electron affinity (kcal/mol) \\ \hline 1 & H & 313.5 & 17.3 \\ \hline 6 & C & 259.6 & 29 \\ \hline 8 & O & 314.0 & 34 \\ \hline 9 & F & 401.8 & 79.5 \\ \hline 16 & S & 238.9 & 47 \\ \hline 17 & Cl & 300.0 & 83.4 \\ \hline \end{tabular} \newline where we give ionization energies and electron affinities for a small sample of atoms, and is obvious from heuristic considerations (the attraction of an electron to a positive ion is much stronger than to a neutral atom), however it is not proved so far rigorously. We verify this condition for systems of hydrogen atoms. With an informal definition of the cohesive energy $W(y),\ y=(y_1,...,y_M)$ between $M$ atoms as the difference between the lowest (ground state) energy, $E(y)$, of the system of the atoms with their nuclei fixed at the positions $y_1,...,y_M$ and the sum, $\sum_{j=1}^M E_j$, of lowest (ground state) energies of the non-interacting atoms, we show that for $|y_i-y_j|,\ i,j \in \{1,...,M\}, i \neq j,$ large enough, $$W(y)=-\sum_{i<j}^{1,M} \frac{\sigma_{ij}}{|y_i-y_j|^6}+O(\sum_{i<j}^{1,M} \frac{1}{|y_i-y_j|^7})$$ where $\sigma_{ij}$ are in principle computable positive constants depending on the nature of the atoms $i$ and $j$.

The van der Waals forces, which are forces between neutral atoms and molecules, play an important role in physics (e.g. in phase transitions), chemistry (e.g. in chemical reactions) and biology (e.g. in determining properties of DNA). These forces are of quantum nature and it is long being conjectured and experimentally verified that they have universal behaviour at large separations: they are attractive and decay as the inverse sixth power of the pairwise distance between the atoms or molecules. In this thesis we prove the van der Waals law under the technical condition that ionization energies (energies of removing electrons) of atoms are larger than electron affinities (energies released when adding electrons). This condition is well justified experimentally as can be seen from the table, \newline \begin{tabular}{|c|c|c|c|} \hline Atomic number & Element & Ionization energy (kcal/mol)& Electron affinity (kcal/mol) \\ \hline 1 & H & 313.5 & 17.3 \\ \hline 6 & C & 259.6 & 29 \\ \hline 8 & O & 314.0 & 34 \\ \hline 9 & F & 401.8 & 79.5 \\ \hline 16 & S & 238.9 & 47 \\ \hline 17 & Cl & 300.0 & 83.4 \\ \hline \end{tabular} \newline where we give ionization energies and electron affinities for a small sample of atoms, and is obvious from heuristic considerations (the attraction of an electron to a positive ion is much stronger than to a neutral atom), however it is not proved so far rigorously. We verify this condition for systems of hydrogen atoms. With an informal definition of the cohesive energy $W(y),\ y=(y_1,...,y_M)$ between $M$ atoms as the difference between the lowest (ground state) energy, $E(y)$, of the system of the atoms with their nuclei fixed at the positions $y_1,...,y_M$ and the sum, $\sum_{j=1}^M E_j$, of lowest (ground state) energies of the non-interacting atoms, we show that for $|y_i-y_j|,\ i,j \in \{1,...,M\}, i \neq j,$ large enough, $$W(y)=-\sum_{i<j}^{1,M} \frac{\sigma_{ij}}{|y_i-y_j|^6}+O(\sum_{i<j}^{1,M} \frac{1}{|y_i-y_j|^7})$$ where $\sigma_{ij}$ are in principle computable positive constants depending on the nature of the atoms $i$ and $j$.

Diss.--Phil.-Fak.--Bonn--Friedrich-Wilhelms-Univ., 1999. / Bibliogr. p. 421-430. Index.

Proefschrift--Faculteit der sociale wetenschapen--universiteit Leiden, 2000. / Bibliogr. p. 292-298.

Proefschrift--Amsterdam--Vrije universiteit, 2005. / Bibliogr. p. 569-580. Résumé en anglais.

Reproduction de : Thèse de doctorat : Lettres et arts : Lyon 2 : 2007. / Titre provenant de l'écran-titre. Bibliogr.

Proefschrift--Groningen.