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  Web Book Home Page | Chemogenesis Main Index Foreword:  Chemogenesis & Chemical Education Part I   Atoms | Elements | Periodic Tables 1.1  Introduction to Chemogenesis 1.2  Nucleosynthesis of The Elements 1.3  The Segrè Chart 1.4  Quantum Numbers to Periodic Tables 1.5  The Periodic Table: What Is It Showing? 1.6  The INTERNET Database of Periodic Tables 1.7  Periodicity Part II   Structure | Bonding | Material Type 2.1  Mono-Bond Typed Binary Compounds 2.2  Binary Compound Synthlet 2.3  Electronegativity 2.4  van Arkel-Ketelaar Triangles of Bonding 2.5  Tetrahedra of Structure, Bonding & Material Type 2.6  Structure, Bonding & Material Synthlet 2.7  The Classification of Matter: Chemical Stuff Part III   Interactions | Reactions | Mechanisms 3.1  The Chemogenesis Analysis: An Overview 3.2  Lewis and Brønsted Models of Acidity 3.3  The Hard Soft [Lewis] Acid Base Principle 3.4  Main Group Elemental Hydrides 3.5  Five Hydrogen Probe Experiments 3.6  Congeneric Dots, Series & Planars 3.7  Quantifying Congeneric Behaviour 3.8  Ligand Replacement Congeneric Series 3.9  Congeneric Array Interactions 3.10  Emergence of Organic Chemistry 3.11  Congeneric Array Database 3.12  The Five Reaction Chemistries 3.13  Lewis Acids & Lewis Bases: A New Analysis 3.14  The Lewis Acid/Base Interaction Matrix 3.15  Patterns in Reaction Chemistry Poster 3.16  Lewis Acid/Base Interaction Matrix Database 3.17  Nucleophiles, Bases & The Fluoride Ion 3.18  Redox Chemistry 3.19  Redox Chemistry Synthlet 3.20  Radical Chemistry 3.21  Diradical Chemistry 3.22  Photochemistry 3.23  Species/Species Interactions 3.24  The Simplest Mechanistic Step: STAD 3.25  Unit & Compound Mechanistic Steps 3.26  The Mechanism Matrix 3.27  Addition To A Double Bond Synthlet 3.28  Pericyclic Reaction Chemistry Part IV   Chemical Theory 4.1  Why Do Chemical Reactions Occur? 4.2a  Thermochemistry: List Reactions Synthlet 4.2b  Thermochemistry: Play With Reaction Synthlet 4.2c  Thermochemistry: Bulid A Reaction Synthlet 4.3  Timeline of Structural Theory 4.4  Modern Lewis Theory 4.5  Valence Shell Electron Pair Repulsion: VSEPR 4.6  Diatomic Species by Molecular Orbital Theory 4.7  Polyatomic Species: Molecular Orbitals 4.8  Organic π-Systems 4.9  Functional Group Database Part V   Complexity & Emergence 5.1  Chemistry & Complexity: Systems 5.2  Linear Chemistry Systems 5.3  Chemical Systems Prone to Complexity Part VI   Extras 6.1  Chemogenesis Videos 6.2  Chemical Thesaurus Reaction Chemistry Database 6.3  Paper: Chemogenesis 6.4  Paper: Electronegativity as a Basic Elemental Property (FoC) 6.5  Workshop: What is Chemistry? 6.6  Paper: Scientific laws, Dalton’s postulates, chemical reactions
          and Wolfram’s NKS (FoC) 6.7  Literature References & Further Reading

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The INTERNET Database of Periodic Tables

There are thousands of periodic tables in web space, but this is the only comprehensive database of periodic tables & periodic system formulations. If you know of an interesting periodic table that is missing, please contact the database curator: Mark R. Leach Ph.D. The database holds information on periodic tables, the discovery of the elements, the elucidation of atomic weights and the discovery of atomic structure (and much, much more).

Periodic Tables from the year 1918 :

Hackh's Classification of the Elements

From Quam & Quam's 1934 review paper.pdf

Meyer's Periodisches System der Elemente

Periodic Table of Meyer (1918) with an intraperiodic accommodation of the rare earths. Reproduced from Meyer, S., 1918. Phys. Z. 19, 178.

Philip Stewart has provided a bit more detail:

Stefan Meyer (1872-1949) was an Austrian physicist, no relation of Julius Lothar Meyer. He had a special interest in 'rare earth' and radioactive elements. He published several versions of the periodic table. In this definitive version of 1918, note elements 69-72. Tu I is 'thulium I', Ad is Aldeberanium (Yb), Cp is Cassiopeium (Lu) and Tu II is 'thulium II' (Hf).:

Cherkesov: Two Periodic Tables

von Bichowsky FR, The place of manganese in the periodic system, J. Am. Chem. Soc. 1918, 40, 7, 1040–1046 Publication Date: July 1, 1918 https://doi.org/10.1021/ja02240a008 

René Vernon writes:

"In this curious article, von Bichowsky, a physical chemist (1889-1951), mounted an argument for regarding Mn as belonging to group 8 (see table 1 below) rather than group 7 (table 2). His article has effectively been assigned to the dustbin of history, having apparently gathered zero citations over the past 103 years.

"Items of note in his 24-column table:

• While Mn, 43 and 75 are assigned to group 8 they remain in alignment with group 7. Se is shown as Sc
• 14 lanthanides, from Ce to Yb, make up group 3a; If La and Lu are included, there are 16 Ln
• Gd is shown as Cd
• Positions of Dy and Ho have been reversed
• Tm and Tm2
• Po shown as "RaF"
• Ra shown as "RaEm"
• Pa shown as Ux2

von Bichowsky made his argument for Mn in group 8, on the following grounds:

• by removing the Ln from the main body of the table all of the gaps denoted by the dashes (in table 2) were removed
• the eighth group links Cr with Cu; Mo with Ag; and W with Au
• the symmetry of the table is greatly increased
• the triads are replaced by tetrads and a group of 16 Ln which accords better with "the preference of the periodic system for powers of two"
• about eight chemistry-based differences between Ti-V-Cr and Mn, including where Mn shows more similarities to Fe-Co-Ni, for example:
  • divalent Ti, V, Cr cations are all powerful reducing agents, Cr being one of the most powerful known; divalent Mn, Fe, Co, Ni are either very mild reducing agents as divalent Mn or Fe, or have almost no reducing power in the case of divalent Co or Ni;
  • metal titanates, vanadates and chromates are stable in alkaline solution and are unstable in the presence of acid whereas permanganates are more stable in acid than alkali; their oxidizing power is also widely different.

I can further add:

• Mn, Fe, and Co, and to some extent Ni, occupy the "hydrogen gap" among the 3d metals, having no or little proclivity for binary hydride formation
• the +2 and +3 oxidation states predominate among the Mn-Fe-Co-Ni tetrad (+3 not so much for Mn)
• in old chemistry, Mn, Fe, Co, and Ni represented the "iron group" whereas Cr, Mo, W, and U belonged to the "chromium group": Struthers J 1893, Chemistry and physics: A manual for students and practitioners, Lea Brothers & Co., Philadelphia, pp. 79, 123
• Tc forms a continuous series of solid solutions with Re, Ru, and Os

Moving forward precisely 100 years, Rayner-Canham (2018) made the following observations:

• Conventional classification systems for the transition metals each have one flaw: "They organise the TM largely according to one strategy and they define the trends according to that organisation. Thus, linkages, relationships, patterns, or similarities outside of that framework are ignored."
• There are two oxide series of the form MnO and Mn3O4 which encompass Mn through Ni. Here the division is not clear cut since there are also the series Mn2O3 for Ti-Cr and Fe; and MnO2 for Ti to Cr.
• Under normal condition of aqueous chemistry, Mn favours the +2 state and its species match well with those of the following 3d member, Fe.

  Rayner-Canham G 2018, "Organizing the transition metals" [a chapter in] in E Scerri & G Restrepo, Mendeleev to Oganesson: A multidisciplinary perspective on the periodic table, Oxford University Press, Oxford, pp. 195–205

I've also attached a modern interpretation of von Bichowsky’s table. It's curious how there are eight metals (Fe aside) capable of, or thought to be capable of, achieving +8. I am not sure that a table of this kind with Lu in group 3 is possible, without upsetting its symmetry."

One of Mendelejeff's Tables, Modified

From Smith A 1918, General Chemistry for Colleges, 2nd ed., The Century Co., New York, p. 299

René Vernon writes:

• H is missing, as are the noble gases.
• Consequently, the period numbers are out by one apiece.
• Seven groups are on the left and seven are on the right (the ever present allure of symmetry).
• After La, Ce is placed under Zr, and Nd is placed under columbium/technetium.
• According to Smith the rest of the lanthanide elements do not fit into any series, because their valences and other chemical properties do not permit most of them to be distributed over so many different groups.
• Po is expected to be a metal which is what it turned out to be Smith has anticipated that astatine will be a metal. Nine decades later, Hermann, Hoffmann & Ashcroft (2013) predicted the same thing: Hermann, A.; Hoffmann, R.; Ashcroft, N. W. (2013). Condensed astatine: Monatomic and metallic. Physical Review Letters, 111 (11), 116404-1–116404-5
• While he does not discuss it, Smith appears to have allowed for missing elements between Li and Gl and between Na and Mg.
• The three elements inside square brackets are those predicted by Mendeleev.

© Mark R. Leach Ph.D. 1999 –

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