Journal articles: 'Periodic table of elements'

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Zolotov, Yu A. "Periodic table of elements." Journal of Analytical Chemistry 62, no. 9 (September 2007): 811–12. http://dx.doi.org/10.1134/s1061934807090018.

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Mary Peelen. "Periodic Table of the Elements." Antioch Review 75, no. 2 (2017): 169. http://dx.doi.org/10.7723/antiochreview.75.2.0169.

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Eaborn, Colin. "Periodic Table of the Elements." Journal of Organometallic Chemistry 326, no. 1 (May 1987): C54. http://dx.doi.org/10.1016/0022-328x(87)80148-1.

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Birch, Gordon. "Periodic table of the elements." Food Chemistry 23, no. 1 (January 1987): 79. http://dx.doi.org/10.1016/0308-8146(87)90029-x.

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Hoffman, D. C. "Role of the periodic table in discovery of new elements." Proceedings in Radiochemistry 1, no. 1 (September 1, 2011): 1–5. http://dx.doi.org/10.1524/rcpr.2011.0000.

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AbstractThis year (2009) marks the 140th Anniversary of Mendeleev's original 1869 periodic table of the elements based on atomic weights. It also marks the 175th anniversary of his birth in Tolbosk, Siberia. The history of the development of periodic tables of the chemical elements is briefly reviewed beginning with the presentation by Dmitri Mendeleev and his associate Nikolai Menshutkin of their original 1869 table based on atomic weights. The value, as well as the sometimes negative effects, of periodic tables in guiding the discovery of new elements based on their predicted chemical properties is assessed. It is noteworthy that the element with Z=101 (mendelevium) was identified in 1955 using chemical techniques. The discoverers proposed the name mendelevium to honor the predictive power of the Mendeleev Periodic Table. Mendelevium still remains the heaviest element to have been identified first by chemical rather than nuclear or physical techniques. The question concerning whether there will be a future role for the current form of the periodic table in predicting chemical properties and aid in the identification of elements beyond those currently known is considered.

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Shiga, David. "Heaviest elements yet join periodic table." New Scientist 210, no. 2816 (June 2011): 11. http://dx.doi.org/10.1016/s0262-4079(11)61357-2.

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BAUM, RUDY M. "THE PERIODIC TABLE Of The Elements." Chemical & Engineering News 81, no. 36 (September 8, 2003): 27–29. http://dx.doi.org/10.1021/cen-v081n036.p027.

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Jonasson, Ralph G. "Elsevier's periodic table of the elements." Geochimica et Cosmochimica Acta 52, no. 5 (May 1988): 1320. http://dx.doi.org/10.1016/0016-7037(88)90289-x.

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Semenova, Anna A., Alexey B. Tarasov, and Eugene A. Goodilin. "Periodic table of elements and nanotechnology." Mendeleev Communications 29, no. 5 (September 2019): 479–85. http://dx.doi.org/10.1016/j.mencom.2019.09.001.

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Nelson, P. G. "Elsevier's periodic table of the elements." Analytica Chimica Acta 212 (1988): 361–62. http://dx.doi.org/10.1016/s0003-2670(00)84168-9.

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Chun-Xuan, Jiang. "The Jiang Periodic Table of Elements." Journal of Middle East and North Africa Sciences 2, no. 6 (2016): 5–12. http://dx.doi.org/10.12816/0032677.

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Seddon, Kenneth R. "The Periodic Table of the Elements." Journal of Organometallic Chemistry 326, no. 2 (June 1987): C88—C89. http://dx.doi.org/10.1016/0022-328x(87)80173-0.

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Chattopadhyay, Dhrubajyoti. "Endangered elements of the periodic table." Resonance 22, no. 1 (January 2017): 79–87. http://dx.doi.org/10.1007/s12045-017-0434-9.

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Clarke, J. R. P. "Elsevier's periodic table of the elements." TrAC Trends in Analytical Chemistry 7, no. 7 (August 1988): 272. http://dx.doi.org/10.1016/0165-9936(88)85080-5.

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Steen, Paul H., Chun-Ti Chang, and Joshua B. Bostwick. "Droplet motions fill a periodic table." Proceedings of the National Academy of Sciences 116, no. 11 (February 21, 2019): 4849–54. http://dx.doi.org/10.1073/pnas.1817065116.

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Drawing parallels to the symmetry breaking of atomic orbitals used to explain the periodic table of chemical elements; here we introduce a periodic table of droplet motions, also based on symmetry breaking but guided by a recent droplet spectral theory. By this theory, higher droplet mode shapes are discovered and a wettability spectrometer is invented. Motions of a partially wetting liquid on a support have natural mode shapes, motions ordered by kinetic energy into the periodic table, each table characteristic of the spherical-cap drop volume and material parameters. For water on a support having a contact angle of about 60°, the first 35 predicted elements of the periodic table are discovered. Periodic tables are related one to another through symmetry breaking into a two-parameter family tree.

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Atkins, Peter. "Elements of Education." Chemistry International 41, no. 4 (October 1, 2019): 4–7. http://dx.doi.org/10.1515/ci-2019-0404.

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Abstract The periodic table was born in chemical education and thrives there still. Mendeleev was inspired to create his primitive but pregnant table in order to provide a framework for the textbook of chemistry that he was planning, and it has remained at the heart of chemical education ever since. It could be argued that the education of a chemist would be almost impossible without the table; at least, chemistry would remain a disorganized heap of disconnected facts. Thanks to Mendeleev and his successors, by virtue of the periodic table, chemical education became a rational discussion of the properties and transformations of matter. I suspect that the educational role of the periodic table is its most important role, for few research chemists begin their day (I suspect) by gazing at the table and hoping for inspiration, but just about every chemistry educator uses it as a pivot for their presentation.

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Cao, Chang-Su, Han-Shi Hu, Jun Li, and W. H. Eugen Schwarz. "Physical origin of chemical periodicities in the system of elements." Pure and Applied Chemistry 91, no. 12 (December 18, 2019): 1969–99. http://dx.doi.org/10.1515/pac-2019-0901.

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AbstractThe Periodic Law, one of the great discoveries in human history, is magnificent in the art of chemistry. Different arrangements of chemical elements in differently shaped Periodic Tables serve for different purposes. “Can this Periodic Table be derived from quantum chemistry or physics?” can only be answered positively, if theinternalstructure of the Periodic Table is explicitly connected to facts and data from chemistry. Quantum chemical rationalization of such a Periodic Tables is achieved by explaining the details ofenergies and radiiof atomiccore and valenceorbitals in theleadingelectron configurations of chemicallybondedatoms. The coarse horizontal pseudo-periodicity in seven rows of 2, 8, 8, 18, 18, 32, 32 members is triggered by the low energy of and large gap above the 1s andnsp valence shells (2 ≤ n ≤ 6 !). The pseudo-periodicity, in particular the wavy variation of the elemental properties in the four longer rows, is due to the different behaviors of the s and p vs. d and f pairs of atomic valence shells along the ordered array of elements. The so-called secondary or vertical periodicity is related to pseudo-periodic changes of the atomic core shells. The Periodic Law of the naturally given System of Elements describes the trends of the many chemical properties displayedinsidethe Chemical Periodic Tables. While the general physical laws of quantum mechanics form a simple network, their application to the unlimited field of chemical materials under ambient ‘human’ conditions results in a complex and somewhat accidental structureinsidethe Table that fits to some more or less symmetricoutershape. Periodic Tables designed after some creative concept for the overall appearance are of interest in non-chemical fields of wisdom and art.

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Pyper, N. C. "Relativity and the periodic table." Philosophical Transactions of the Royal Society A: Mathematical, Physical and Engineering Sciences 378, no. 2180 (August 17, 2020): 20190305. http://dx.doi.org/10.1098/rsta.2019.0305.

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The periodic table provides a deep unifying principle for understanding chemical behaviour by relating the properties of different elements. For those belonging to the fifth and earlier rows, the observations concerning these properties and their interrelationships acquired a sound theoretical basis by the understanding of electronic behaviour provided by non-relativistic quantum mechanics. However, for elements of high nuclear charge, such as occur in the sixth and higher rows of the periodic table, the systematic behaviour explained by non-relativistic quantum mechanics begins to fail. These problems are resolved by realizing that relativistic quantum mechanics is required in heavy elements where electrons velocities can reach significant fractions of the velocity of light. An essentially non-mathematical description of relativistic quantum mechanics explains how relativity modifies valence electron behaviour in heavy elements. The direct relativistic effect, arising from the relativistic increase of the electron mass with velocity, contracts orbitals of low angular momentum, increasing their binding energies. The indirect relativistic effect causes valence orbitals of high angular momentum to be more effectively screened as a result of the relativistic contraction of the core orbitals. In the alkali and alkaline earths, the s orbital contractions reverse the chemical trends on descending these groups, with heavy elements becoming less reactive. For valence d and f electrons, the indirect relativistic effect enhances the reductions in their binding energies on descending the periodic table. The d electrons in the heavier coinage metals thus become more chemically active, which causes these elements to exhibit higher oxidation states. The indirect effect on d orbitals causes the chemistries of the sixth-row transition elements to differ significantly from the very similar behaviours of the fourth and fifth-row transition series. The relativistic destabilization of f orbitals causes lanthanides to be chemically similar, forming mainly ionic compounds in oxidation state three, while allowing the earlier actinides to show a richer range of chemical behaviour with several higher oxidation states. For the 7p series of elements, relativity divides the non-relativistic p shell of three degenerate orbitals into one of much lower energy with the energies of the remaining two being substantially increased. These orbitals have angular shapes and spin distributions so different from those of the non-relativistic ones that the ability of the 7p elements to form covalent bonds is greatly inhibited. This article is part of the theme issue ‘Mendeleev and the periodic table’.

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Reedijk, Jan. "Elements of IYPT2019." Chemistry International 41, no. 4 (October 1, 2019): ii. http://dx.doi.org/10.1515/ci-2019-0401.

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Abstract The Periodic Table of Chemical Elements has without any doubt developed to one of the most significant achievements in natural sciences. The Table (or System, as called in some languages) is capturing the essence, not only of chemistry, but also of other science areas, like physics, geology, astronomy and biology. The Periodic Table is to be seen as a very special and unique tool, which allows chemists and other scientists to predict the appearance and properties of matter on earth and even in other parts of our the universe.

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Meija, Juris, Javier Garcia-Martinez, and Jan Apotheker. "IUPAC Periodic Table Challenge." Chemistry International 42, no. 2 (April 1, 2020): 18–21. http://dx.doi.org/10.1515/ci-2020-0204.

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AbstractIn 2019, the world celebrated the International Year of the Periodic Table of Chemical Elements (IYPT2019) and the IUPAC centenary. This happy coincidence offered a unique opportunity to reflect on the value and work that is carried out by IUPAC in a range of activities, including chemistry awareness, appreciation, and education. Although IUPAC curates the Periodic Table and oversees regular additions and changes, this icon of science belongs to the world. With this in mind, we wanted to create an opportunity for students and the general public to participate in this global celebration. The objective was to create an online global competition centered on the Periodic Table and IUPAC to raise awareness of the importance of chemistry in our daily lives, the richness of the chemical elements, and the key role of IUPAC in promoting chemistry worldwide. The Periodic Table Challenge was the result of this effort.

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BORMAN, STUART A. "Three-Dimensional Periodic Table Of Elements Proposed." Chemical & Engineering News 68, no. 1 (January 1990): 18–21. http://dx.doi.org/10.1021/cen-v068n001.p018.

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22

Bush, Elizabeth. "The Periodic Table: Elements with Style! (review)." Bulletin of the Center for Children's Books 60, no. 10 (2007): 411–12. http://dx.doi.org/10.1353/bcc.2007.0346.

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Gumiński, Cezary. "Solubility and the periodic table of elements." Pure and Applied Chemistry 87, no. 5 (May 1, 2015): 477–85. http://dx.doi.org/10.1515/pac-2014-0935.

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AbstractInteresting general tendencies of changes of solubilities of elements and groups of compounds may be observed when the corresponding solubility data are arrayed according to the increasing atomic number of the elements. Such trends are exemplified with the data of various systems (metallic and salt-water type) evaluated in several volumes of the IUPAC-NIST Solubility Data Series. The solubilities of elements in mercury as well as in liquid alkali metals, when ordered according their atomic numbers, change roughly in a corresponding way as the temperatures and energies of melting or boiling points of the elements. However, majority of transition metals dissolved in alkali metals are subject to some side reactions with nonmetallic impurities that may drastically elevate their concentration levels. The solubilities of intermetallic compounds in mercury depend primarily on the energies of formation of these intermetallics in the binary alloys and then on the dissolution energies of the component metals in mercury. It has been observed that the experimental solubilities of metal halates in water show quite well defined periodical changes. The arrayed solubility data of rare earth metal fluorides and chlorides in water display quite smooth changes with the increasing atomic numbers if the solutes are isomorphic. Some exceptions from the smooth changes for rare earth metal bromides and iodides are explained. These general observations are useful in evaluating and predicting solubilities in experimentally unknown systems.

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TONELLI, R., and F. MELONI. "CHUA'S PERIODIC TABLE." International Journal of Bifurcation and Chaos 12, no. 07 (July 2002): 1451–64. http://dx.doi.org/10.1142/s0218127402005406.

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An interdisciplinary analysis is presented in this paper on the relationship between the bifurcation behavior of chaotic systems, specifically Chua's circuit, and the quantized energy level of atoms. We show that it is possible to associate special capacitance values in Chua's circuits with the electronic energy levels Enof atoms calculated from Bohr's Law. In particular, these particular capacitance values correspond to the bifurcation points αnof Chua's circuits. We found a functional relation associating a specific Chua's circuit to the Hydrogen atom and obtained a map of "Atom" to " Chua's Circuit". This map can be extended to other elements in the Periodic Table, thereby demonstrating an almost universal relation between the two different physical systems. With this map we can calculate the energy levels of different atoms from bifurcation diagrams (or vice-versa) and express the analytical relations in terms of the two variables αnand En.

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Poliakoff, Martyn, and Samantha Tang. "The periodic table: icon and inspiration." Philosophical Transactions of the Royal Society A: Mathematical, Physical and Engineering Sciences 373, no. 2037 (March 13, 2015): 20140211. http://dx.doi.org/10.1098/rsta.2014.0211.

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To start this discussion meeting on the new chemistry of the elements held on 12 May 2014, Martyn Poliakoff, Foreign Secretary of the Royal Society, was invited to give the opening remarks. As a chemist and a presenter of the popular online video channel ‘The periodic table of videos’, Martyn communicates his personal and professional interest in the elements to the public, who in turn use these videos both as an educational resource and for entertainment purposes. Ever since Mendeleev’s first ideas for the periodic table were published in 1869, the table has continued to grow as new elements have been discovered, and it serves as both icon and inspiration; its form is now so well established that it is recognized the world over as a symbol for science. This paper highlights but a few of the varied forms that the table can take, such as an infographic, which can convey the shortage of certain elements with great impact.

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"Herald of the RAS", Board of the journal. "150th anniversary of periodic table of chemical elements." Вестник Российской академии наук 89, no. 6 (June 21, 2019): 561–62. http://dx.doi.org/10.31857/s0869-5873896561-562.

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The United Nations declared 2019 the International Year of the Periodic Table of Chemical Elements, coinciding with the 150th anniversary of the Periodic Law, opened in 1869 by the great Russian scientist-encyclopedist Dmitry Ivanovich Mendeleev (1834–1907).

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H. M. Al-Ossmi, Laith. "A Simplified Method for Estimating Atomic Number and Neutrons Numbers of Elements Based on Period and Group Numbers in the Periodic Table." Oriental Journal of Chemistry 35, no. 1 (February 20, 2019): 39–48. http://dx.doi.org/10.13005/ojc/350104.

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This research has proposed formulas, in which the atomic number and neutron numbers to any element in the periodic table are determined according to element position in the periodic table. These formulas have been arranged to fit with periodic system of elements in the IUPAC's Periodic Table. The main outcome is to introduce layout regularity, which may reflect the regularity of the periodic law more faithfully. In this research, atomic number to any element in the periodic table is predictably calculated by the group and period numbers which were displayed into 7 Periods horizontally, and 18 Groups vertically, determining and dispensing altogether the elements positions at the periodic system. Application of these proposed formulas showed linearity from has good agreement with these separated elements of Lanthanum in the f-block elements (Lanthanides and Actinides), which were in no interruptions in the sequence of increasing atomic numbers. In addition, the relationship of the f-block to the other blocks of the periodic table also becomes easier to see. In addition, the formulas are extensible to expanding future table and allowed determining the atomic number of the future elements starting from 119 till the element of 136, at the main body of the periodic table, and can be used as a simple and alternative method for determine the numbers of atomic and neutron in the IUPAC's Periodic Table.

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Stonik, Valentin A., and Tatyana N. Makarieva. "Mendeleev’s Periodic Table and Marine Biomolecules." Vestnik RFFI, no. 1 (April 24, 2019): 105–19. http://dx.doi.org/10.22204/2410-4639-2019-101-01-105-119.

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The mini-review highlights the involvement of some elements of Mendeleev Periodic Table into marine biogenic compounds and these elements participation in the marine organisms’ metabolism. Some metals accumulation by marine invertebrates and the metal complexation by highly structurally diverse secondary metabolites are discussed. In addition, examples of the covalent bonds formation in marine bioorganic molecules with a number of non-metals are considered.

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Christy, Andrew G. "Causes of anomalous mineralogical diversity in the Periodic Table." Mineralogical Magazine 79, no. 1 (February 2015): 33–49. http://dx.doi.org/10.1180/minmag.2015.079.1.04.

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AbstractWhen crustal abundance (A, measured in atomic parts per million) of a chemical element is plotted vs. number of mineral species in which that element is an essential constituent (S), a significantly positive correlation is obtained, but with considerable scatter. Repeated exclusion of outliers at the 90% confidence level and re-fitting leads, after the sixth iteration, to a steady state in which 40 of the 70 elements initially considered define a trend with log S = 1.828 + 0.255 log a (r = 0.96), significantly steeper than the original. Three other methods for reducing the effect of outliers independently reproduce this steeper trend. The 'diversity index' D of an element is defined as the ratio of observed mineral species to those predicted from this trend. D separates elements into three groups. More than half of the elements (40 of 70) have D = 0.5–2.0. Apart from these 'typical' elements, a group of 15 elements (Sc, Cr, Ga, Br, Rb, In, Cs, La, Nd, Sm, Gd, Yb, Hf, Re and Th) form few species of their own due to being dispersed as minor solid solution constituents, and a hitherto unrecognized group of 15 elements are essential components in unusually large numbers of minerals. The anomalously diverse group consists of H, S, Cu, As, Se, Pd, Ag, Sb, Te, Pt, Au, Hg, Pb, Bi and U, with Te and Bi by far the most mineralogically diverse elements (D = 22 and 19, respectively). Possible causes and inhibitors of diversity are discussed, with reference to atomic size, electronegativity and Pearson softness, and particularly outer electronic configurations that result in distinctive stereochemistry. The principal factors encouraging mineral diversity are: (1) Particular outer electronic configurations that lead to a preference for unique coordination geometries, enhancing an element's ability to form distinctive chemical compounds and decreasing its ability to participate in solid solutions. This is particularly noteworthy for elements possessing geometrically flexible 'lone-pair cations' with an s2 outer electronic configuration. (2) Siderophilic or chalcophilic geochemical behaviour and intermediate electronegativity, allowing elements to form minerals that are not oxycompounds or halides. (3) Access to a wide range of oxidation states. The most diverse elements can occur as anions, native elements and in more than one cationic valence state.

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Cotton, Simon. "The periodic table of the elements, 2nd edition." Polyhedron 6, no. 3 (January 1987): 659. http://dx.doi.org/10.1016/s0277-5387(00)81042-6.

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31

Bouma, J. "An application-oriented periodic table of the elements." Journal of Chemical Education 66, no. 9 (September 1989): 741. http://dx.doi.org/10.1021/ed066p741.

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Goodilin, Eugene A., Paul S. Weiss, and Yury Gogotsi. "Nanotechnology Facets of the Periodic Table of Elements." ACS Nano 13, no. 10 (September 23, 2019): 10879–86. http://dx.doi.org/10.1021/acsnano.9b06998.

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Wang, Frank Z. "A Triangular Periodic Table of Elementary Circuit Elements." IEEE Transactions on Circuits and Systems I: Regular Papers 60, no. 3 (March 2013): 616–23. http://dx.doi.org/10.1109/tcsi.2012.2209734.

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Oganessian, Yury Ts, and Sergey N. Dmitriev. "Superheavy elements in D I Mendeleev's Periodic Table." Russian Chemical Reviews 78, no. 12 (December 31, 2009): 1077–87. http://dx.doi.org/10.1070/rc2009v078n12abeh004096.

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Castleman, A. W. "From Elements to Clusters: The Periodic Table Revisited." Journal of Physical Chemistry Letters 2, no. 9 (April 15, 2011): 1062–69. http://dx.doi.org/10.1021/jz200215s.

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Johnson, Jennifer A. "Populating the periodic table: Nucleosynthesis of the elements." Science 363, no. 6426 (January 31, 2019): 474–78. http://dx.doi.org/10.1126/science.aau9540.

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Elements heavier than helium are produced in the lives and deaths of stars. This Review discusses when and how the process of nucleosynthesis made elements. High-mass stars fuse elements much faster, fuse heavier nuclei, and die more catastrophically than low-mass stars. The explosions of high-mass stars as supernovae release elements into their surroundings. Supernovae can leave behind neutron stars, which may later merge to produce additional heavy elements. Dying low-mass stars throw off their enriched outer layers, leaving behind white dwarfs. These white dwarfs may also later merge and synthesize elements as well. Because these processes occur on different time scales and produce a different pattern of elements, the composition of the Universe changes over time as stars populate the periodic table.

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Eichler, Robert. "The Periodic Table of Elements: Superheavy in Chemistry." Nuclear Physics News 29, no. 1 (January 2, 2019): 11–15. http://dx.doi.org/10.1080/10619127.2019.1571803.

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Supanchaiyamat, Nontipa, and Andrew J. Hunt. "Conservation of Critical Elements of the Periodic Table." ChemSusChem 12, no. 2 (January 2, 2019): 397–403. http://dx.doi.org/10.1002/cssc.201802556.

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Rouvray, Dennis H. "Elements in the history of the Periodic Table." Endeavour 28, no. 2 (June 2004): 69–74. http://dx.doi.org/10.1016/j.endeavour.2004.04.006.

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Abel, E. W. "Elsevier's periodic table of the elements (wall chart)." Endeavour 13, no. 1 (January 1989): 43. http://dx.doi.org/10.1016/0160-9327(89)90064-1.

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Poliakof, Martyn. "The Periodic Table: Icon and Inspiration." Vestnik RFFI, no. 1 (April 24, 2019): 25–38. http://dx.doi.org/10.22204/2410-4639-2019-101-01-25-38.

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Since Dmitry Mendeleev published the initial concept of the Periodic Law in 1869, the Table has been continuously updated with newly discovered elements, and figuratively speaking, today it serves both as an icon and as an inspiration for modern chemists. Its image is so easily recognizable all around the world that it has become a symbol for science. This paper highlights just a few of the varied forms that the Table can take, such as an infographic, which can convey the shortage of certain elements with great impact.

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Ferrins, Lori, Christine Dunne, João Borges, and Fun Man Fung. "Reflecting on a Year of Elements." Chemistry International 42, no. 3 (July 1, 2020): 3–5. http://dx.doi.org/10.1515/ci-2020-0302.

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AbstractThe Periodic Table of Younger Chemists (PTYC) arose from a group of aspiring scientists in attendance at the 2017 World Chemistry Leadership Meeting in Sao Paulo, Brazil. This project was a celebration of the 100th anniversary of IUPAC and the International Year of the Periodic Table. IUPAC and the International Younger Chemists Network (IYCN) joined forces to create the PTYC and honor rising stars in chemistry from around the world. Beginning in July 2018 and ending in July 2019 at the World Chemistry Congress, we unveiled and honored a diverse group of 118 outstanding younger chemists who embody the mission and core values of IUPAC. The resulting Periodic Table highlights the diversity of careers, outreach participation, and dedication to the chemistry community of those leading us into the next century of IUPAC.

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LI, Shuni, Quanguo ZHAI, Yucheng JIANG, Mancheng HU, Zhihong LIU, and Shengli GAO. "Periodic Table of Elements and Chemistry Education: Commemorating the 150th Anniversary of the Publication of Mendeleev's Periodic Table of Elements." University Chemistry 34, no. 12 (2019): 2–7. http://dx.doi.org/10.3866/pku.dxhx201909024.

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Boeyens, Jan C. A. "The Periodic Electronegativity Table." Zeitschrift für Naturforschung B 63, no. 2 (February 1, 2008): 199–209. http://dx.doi.org/10.1515/znb-2008-0214.

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The origins and development of the electronegativity concept as an empirical construct are briefly examined, emphasizing the confusion that exists over the appropriate units in which to express this quantity. It is shown how to relate the most reliable of the empirical scales to the theoretical definition of electronegativity in terms of the quantum potential and ionization radius of the atomic valence state. The theory reflects not only the periodicity of the empirical scales, but also accounts for the related thermochemical data and serves as a basis for the calculation of interatomic interaction within molecules. The intuitive theory that relates electronegativity to the average of ionization energy and electron affinity is elucidated for the first time and used to estimate the electron affinities of those elements for which no experimental measurement is possible

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Rath, M. C. "Periodic Table of Elements Revisited for Accommodating Elements of Future Years." Current Science 115, no. 9 (November 10, 2018): 1644. http://dx.doi.org/10.18520/cs/v115/i9/1644-1647.

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Kurushkin, Mikhail. "Viatscheslaw Romanoff: unknown genius of the periodic system." Pure and Applied Chemistry 91, no. 12 (December 18, 2019): 1921–28. http://dx.doi.org/10.1515/pac-2019-0803.

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Abstract The history of chemistry has not once seen representations of the periodic system that have not received proper attention or recognition. The present paper is dedicated to a nearly unknown version of the periodic table published on the occasion of the centenary celebration of Mendeleev’s birth (1934) by V. Romanoff. His periodic table visually merges Werner’s and Janet’s periodic tables and it is essentially the spiral periodic system on a plane. In his 1934 paper, Romanoff was the first one to introduce the idea of the actinide series, a decade before Glenn T. Seaborg, the renowned creator of the actinide concept. As a consequence, another most outstanding thing about Romanoff’s paper occurs towards its very end: he essentially predicted the discovery of elements #106, #111 and #118. He theorized that, had uranium not been the “creative limit”, we would have met element #106, a “legal” member of group 6, element #111, a precious metal, “super-gold” and element #118, a noble gas. In 2019, we take it for granted that elements #106, #111 and #118 indeed exist and they are best known as seaborgium, roentgenium and oganesson. It is fair to say that Romanoff’s success with the prediction of correct placement and chemical properties of seaborgium, roentgenium and oganesson was only made possible due to the introduction of an early version of the actinide series that only had four elements at that time. Sadly, while Professor Romanoff was imprisoned (1938–1943), two new elements, neptunium (element #93) and plutonium (element #94) were discovered. While Professor Romanoff was in exile in Ufa (1943–1953), six further elements were added to the periodic table: americium (element #95), curium (element #96), berkelium (element #97), californium (element #98), einsteinium (element #99) and fermium (element #100). The next year after his death, in 1955, mendelevium (element #101), was discovered. Romanoff’s version of the periodic table is an unparalleled precursor to the contemporary periodic table, and is an example of extraordinary anticipation of the discovery of new chemical elements.

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Karpov, Yuri A., Mikhail F. Churbanov, Vasilisa B. Baranovskaya, Olga P. Lazukina, and Ksenia V. Petrova. "High purity substances – prototypes of elements of Periodic Table." Pure and Applied Chemistry 92, no. 8 (September 25, 2020): 1357–66. http://dx.doi.org/10.1515/pac-2019-1205.

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AbstractThe Mendeleev Periodic Table of Chemical Elements delivered a strong impetus to the development of fundamental and applied chemistry, chemical technology, analytical chemistry, and material sciences. Each element under the Periodic Table is an idealized substance with a certain structure and properties as defined by existing theoretical frameworks. In the real world, we deal with substances that are close in composition to the element of Periodic Table under study but differ in the presence of different elements in them – impurities that distort (sometimes radically) the structure and properties of the target research object. For many centuries, humanity has sought to obtain pure substances in order to achieve desired properties. In the second half of the 20th century, a unique collection of high purity substances was created, which includes samples representing material artifacts, prototypes of elements of Periodic Table that contain record low contents of impurity elements. With ongoing scientific and technological progress, the achieved purity of substances continuously increases and, therefore, their approximation to idealized elements of Periodic Table. This is facilitated by: new technological processes for the production and storage of high purity substances with a constant decrease in the level of impurities; the creation of isotope-friendly substances; complexes of more highly sensitive multi-element analysis methods; identification of the unique properties of high purity substances, bringing them closer to the capabilities of analog elements of Periodic Table and much more. This article is devoted to progress in these areas. Special attention is also paid to the problems in modern analytical chemistry of high purity substances and the use of the latter in the metrology of chemical analysis as the standards of comparison.

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Tsivadze, Aslan Yu. "Periodic Law, Mendeleev Society and Mendeleev Congresses." Vestnik RFFI, no. 1 (April 24, 2019): 17–24. http://dx.doi.org/10.22204/2410-4639-2019-101-01-17-24.

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In November 1868, the Ministry of Enlightenment of Russia approved the Charter of the Russian Chemical Society (RCS), one of the Founding Members of which had been Dmitri Mendeleev. The first report on Mendeleev Periodic Table of Chemical Elements was delivered during a meeting of the RCS in March 1869. Therefore 1869 is considered by the world science as the year of discovery of the Periodic Law and formulation of the Periodic Table of Chemical Elements. Year 2019 is the 150th anniversary since Dmitry Mendeleev discovered the Periodic System, and the United Nations proclaimed this year to be the International Year of the Periodic Table of Chemical Elements (IYPT2019). After a series of transformations, in 1992 the RCS became the Mendeleev Russian Chemical Society. In 2019, the RCS is holding anniversary events. The extraordinary Mendeleev Congress on General and Applied Chemistry is one of them. It will be held in Saint Petersburg in September 2019 and will host approximately 3,000 foreign and Russian participants. English-speaking symposia, conferences and round tables on current issues of strategic development of science and technology are planned as a part of the Congress.

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Tarasova, Natalia P. "International Year of the Periodic Table of Chemical Elements." Vestnik RFFI, no. 1 (April 24, 2019): 39–42. http://dx.doi.org/10.22204/2410-4639-2019-101-01-39-42.

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Year 2019, the International Year of the Periodic Table of Chemical Elements, is of special value for our country. 150 years ago, in 1869, the outstanding Russian scientist D.I. Mendeleev published the first scheme of the Periodic table of chemical elements. The International Year of the Periodic Table of Chemical Elements draws the world community attention to the development of fundamental sciences, to deepening and expansion of education for sustainable development, to global problems that cannot be solved without active use of achievements of modern green chemistry. The quality of everyday life of present and future generations is directly connected with the progress and achievements of chemical science and technology. In 2019, the large-scale events dedicated to D.I. Mendeleev and his scientific heritage will take place both in Russia and throughout the world The International Year of the Periodic Table once again emphasizes the importance of the systematicity in our chaotic world. The System gives an opportunity to understand the idea of regularity and thus arms human beings with the ability to predict.

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Chapman, Kit. "Elements of the Future." Chemistry International 41, no. 4 (October 1, 2019): 12–15. http://dx.doi.org/10.1515/ci-2019-0406.

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Abstract When Dimitri Mendeleev assembled his periodic table in 1869, the heaviest known element was uranium, element 92. As the table filled, it soon became clear that this was the heaviest element that existed in large quantities on Earth. But it was far from the limit of the building blocks of matter.

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Journal articles on the topic 'Periodic table of elements'

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