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Skip to content. Thinking outside the box - beyond machine learning for quantum chemistry. Journal list menu Journal. International Journal of Quantum Chemistry. Impact factor: 2. On the Cover Skip slideshow. The interaction of successive CO 2 molecules with C 6 Li 6 has been studied using long-range dispersion corrected density functional approach. This interaction leads to the formation of C 6 Li 6 - n CO 2 complexes in which the charge transfer to CO 2 is very close to unity, and adsorption energy per CO 2 is sufficiently large.
In the article e by Ambrish Kumar Srivastava, the calculations suggest that C 6 Li 6 is capable not only in reducing, i. DOI: In the article e, Susi Lehtola reviews fully numerical electronic structure calculations on atoms and diatomic molecules, continuing by discussions of finite element implementations in e and e for atoms and diatomic molecules, respectively. The cover illustrates the use of a real-space basis set to achieve an arbitrary level of accuracy for electronic structure calculations, even though the form of the basis set is not motivated by chemistry. The image also suggests that relatively large numerical basis sets are required to achieve even a qualitative level of accuracy, in agreement with common knowledge.
Magnetically-induced current densities are not exclusive of cyclic molecules. In e, the article from Luis Alvarez-Thon and colleagues investigates the current density patterns of a representative series of open hydrocarbon chains containing two or more C-C double bonds. The cover image showing the current patterns of trans-trans -1,3,5,7-octatetraene and 1,3-butadiene is an example. In e, Oscar Ventura and coworkers describe micro-hydration of 1-chloro and 2-chloroethanol.
leondumoulin.nl/language/mythopoeia/4425-the-end-of.php By the late nineteenth century, virtually all scientists believed that light behaved as a wave. Although some earlier scientists, such as Isaac Newton in the seventeenth century, had thought of light as consisting of particles, the early nineteenth-century experiments of Thomas Young and Augustin Fresnel demonstrated that light has wavelike properties.
In these experiments, light was passed through a pair of slits in a screen, and produced alternating light and dark regions interference patterns on a second screen.
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This phenomenon, known as diffraction, cannot be explained using a particle model for light. In the late nineteenth century, James Clerk Maxwell derived a set of equations based on the wave model for light, which beautifully explained most experimental results.
Despite this apparent certainty that light was a wave, Max Planck and Albert Einstein, at the beginning of the twentieth century, showed that some experiments required the use of a particle model for light, rather than a wave model. Since both models were necessary for an accurate description of all of the properties of light, scientists today use mathematical equations appropriate to both waves and particles in describing the properties of light.
Waves and particles are fundamentally different: a particle exists at a particular point in space, whereas a wave continues on for sometimes a great distance. It defies intuition to think that both of these models might describe the same thing. Nevertheless, an accurate description of light requires the use of both wave and particle ideas. The success of wave-particle duality in describing the properties of light paved the way for using that same idea in describing matter. For hydrogen, the simplest of the atoms, an accurate formula for the possible energies had been experimentally determined but was unexplainable using any particle model for the atom.
The best picture that the particle model could give, consistent with experiments on atoms, put the electron in a sort of "orbit" around the nucleus. Unfortunately, the particle model predicts that the electron should collide with the nucleus, releasing energy in the process.
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Obviously there was a need for a different model for the electron. In Louis de Broglie presented a theory for the hydrogen atom that modeled the electron as a wave. Calculations made for this model give the quantization of energy that is experimentally observed in this atom.