Some compounds or chemical preparation methods were thought to be non-existent or impossible. Under such circumstances, misunderstandings of the Periodic Table happen easily, and unexpected chemistry is overlooked. Thus, modern chemistry developed not only along the lines of easily available and practically useful chemicals, but also with effectively blinkered expectations according to the Periodic Table (Keserü et al., 2014 Pye et al., 2017 Llanos et al., 2019 Restrepo, 2019a, b). Then, during the past hundred years, students learned general and inorganic chemistry, and later practiced these through Periodic-Table colored glasses, rationalized by atomic structure theory. Within half a century, with more or less delay depending on the author, Periodic Tables of elements entered most chemistry books and lecture rooms (Kaji et al., 2015 Robinson, 2019).
They addressed this need with the help of two-dimensional tables for groups of elements. Two to one-and-half centuries ago, authors of chemistry books and chemistry teachers such as Leopold Gmelin (Gmelin, 1843), Lothar Meyer (Meyer, 1864), Dmitri Mendeleev (Mendeleev, 1869b) and Viktor von Richter (Von Richter, 1875) felt the need for an ordered arrangement of the increasing number of elements. The combination of experimental data and theoretical insight supports a more nuanced understanding of complex periodic trends and non-periodic phenomena. While it is essential that Periodic Tables display important trends in element chemistry we need to keep our eyes open for unexpected chemical behavior in ambient, near ambient, or unusual conditions.
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Simplified, artistic, or economic tables are relevant to educational and cultural fields, while practicing chemists profit more from “chemical tables of chemical elements.” Such tables should incorporate four aspects: (i) typical valence electron configurations of bonded atoms in chemical compounds (instead of the common but chemically atypical ground states of free atoms in physical vacuum) (ii) at least three basic chemical properties ( valence number, size, and energy of the valence shells), their joint variation across the elements showing principal and secondary periodicity (iii) elements in which the (sp) 8, (d) 10, and (f) 14 valence shells become closed and inert under ambient chemical conditions, thereby determining the “fix-points” of chemical periodicity (iv) peculiar elements at the top and at the bottom of the Periodic Table. Such tables have been designed with the aim of either classifying real chemical substances or emphasizing formal and aesthetic concepts. To this end, a graphical display of the chemical properties of the elements, in the form of a Periodic Table, is the helpful tool.
Comprehensive overviews of the chemistry of the elements and their compounds are needed in chemical science. For a table that shows atomic weight, atomic symbol and atomic number, along with detailed information on how the periodic table is organized, click here.The chemical elements are the “conserved principles” or “kernels” of chemistry that are retained when substances are altered.
We hope you enjoyed the periodic table by name. View our new Interactive Periodic Table! Elements Alphabetically by Periodic Table Name
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