The Periodic Table最新文献_第2页

The Periodic Table Exploration Begins! 元素周期表探索开始!

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_0001

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BACK MATTER 回到问题

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_bmatter

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Chemical “Knight’s Move” Relationship 化学“骑士之招”关系

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_0011

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Isodiagonality

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_0012

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Categorizations of the Elements 元素的分类

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_0006

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Lanthanoids, Group 3, and Their Connections 类镧族，族3和它们的联系

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_0013

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Patterns among the Transition Metals 过渡金属中的模式

The Periodic Table Pub Date : 2020-08-04 DOI: 10.1142/9789811218491_0009

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More Chemistry 更多的化学

The Periodic Table Pub Date : 2019-12-12 DOI: 10.1093/oso/9780190914363.003.0019

Eric R. Scerri

{"title":"More Chemistry","authors":"Eric R. Scerri","doi":"10.1093/oso/9780190914363.003.0019","DOIUrl":"https://doi.org/10.1093/oso/9780190914363.003.0019","url":null,"abstract":"The trends within rows and columns of the periodic table are quite well known and are not repeated here. Instead, I concentrate on a number of other chemical trends, some of which challenge the form of reductionism that attempts to provide explanations based on electronic configurations alone. In the case of one particular trend described here, the knight’s move, the chemical behavior defies any theoretical understanding whatsoever, at least at the present time. As is well known to students of inorganic chemistry, a small number of elements display what is termed diagonal behavior where, in apparent violation of group trends, two elements from adjacent groups show greater similarity than is observed between these elements and the members of their own respective groups. Of these three classic examples of diagonal behavior, let us concentrate on the first one to the left in the periodic table, that between lithium and magnesium. The similarities between these two elements are as follows:1. Whereas the alkali metals form peroxides and superoxides, lithium behaves like a typical alkaline earth in forming only a normal oxide with formula Li2O. 2.Unlike the other alkali metals, lithium forms a nitride, Li3N, as do the alkaline earths. 3.Although the salts of most alkali metals are soluble, the carbonate, sulfate, and fluorides of lithium are insoluble, as in the case of the alkaline earth elements. 4.Lithium and magnesium both form organometallic compounds that act as useful reagents in organic chemistry. Lithium typically forms such compounds as Li(CH3)3, while magnesium forms such compounds as CH3MgBr, a typical Grignard reagent that is used in nucleophilic addition reactions. Organolithium and organomagnesium compounds are very strong bases that react with water to form alkanes. 5.Lithium salts display considerable covalent character, unlike their alkali metal homologues but in common with many alkaline earth salts. 6.Whereas the carbonates of the alkali metals do not decompose on heating, that of lithium behaves like the carbonates of the alkaline earths in forming the oxide and carbon dioxide gas. 7.Lithium is a considerably harder metal than other alkali metals and similar in hardness to the alkaline earths.","PeriodicalId":440562,"journal":{"name":"The Periodic Table","volume":"88 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"2019-12-12","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"114492019","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

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Mendeleev

The Periodic Table Pub Date : 2019-12-12 DOI: 10.1093/oso/9780190914363.003.0009

Eric R. Scerri

{"title":"Mendeleev","authors":"Eric R. Scerri","doi":"10.1093/oso/9780190914363.003.0009","DOIUrl":"https://doi.org/10.1093/oso/9780190914363.003.0009","url":null,"abstract":"Dmitri Ivanovich Mendeleev is the undisputed champion of the periodic system in at least two senses. First of all, he is by far the leading discoverer of the system. Although he was not the first to develop a periodic system, his version is the one that created the biggest impact on the scientific community at the time it was introduced and thereafter. His name is invariably and justifiably connected with the periodic system, to the same extent perhaps as Darwin’s name is synonymous with the theory of evolution and Einstein’s with the theory of relativity. Although it may be possible to quibble about certain priority aspects of his contributions, there is no denying that Mendeleev was also the champion of the periodic system in the literal sense of propagating the system, defending its validity, and devoting time to its elaboration. As discussed in chapter 3, there were others who produced significant work on the system, but many of them, such as Alexandre-Émile Béguyer De Chancourtois, William Odling, and Gustavus Hinrichs, moved on to other scientific endeavors. After publishing their initial ideas, these contributors devoted their attention to other fields and never seriously returned to the periodic system to examine its full consequences to the extent that Mendeleev did. This is not to suggest that Mendeleev himself worked only on the periodic system. He is also known for many other scientific contributions, as well as for working in several applied fields, such as the Russian oil industry and as the director of the Russian institute for weights and measures. But the periodic system remained Mendeleev’s pride and joy throughout his adult life. Even toward the end of his life he published an intriguing essay in which he returned to the periodic system and, among other speculations, attempted to place the physicist’s ether within the periodic system as a chemical element. Much has been written on Mendeleev, and it would be impossible to do justice to his contributions in the space of a few pages.","PeriodicalId":440562,"journal":{"name":"The Periodic Table","volume":"53 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"2019-12-12","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"122344836","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

引用次数: 14

Synthetic Elements 人工合成成分

The Periodic Table Pub Date : 2019-12-12 DOI: 10.1093/oso/9780190914363.003.0017

Eric R. Scerri

{"title":"Synthetic Elements","authors":"Eric R. Scerri","doi":"10.1093/oso/9780190914363.003.0017","DOIUrl":"https://doi.org/10.1093/oso/9780190914363.003.0017","url":null,"abstract":"The periodic table consists of about 90 elements that occur naturally ending with element 92 uranium. This lack of precision is deliberate since one or two elements such as technetium were first created artificially and only later found to occur naturally on earth. This kind of occurrence provides a foreshadowing of things to come when we begin to discuss the transuranium elements, meaning those beyond uranium that have been artificially synthesized. Chemists and physicists have succeeded in synthesizing some of the elements that were missing between hydrogen (1) and uranium (92). In addition, they have synthesized a further 25, or so, new elements beyond uranium, although, again, one or two of these elements, like neptunium and plutonium, were later found to exist naturally in exceedingly small amounts. The existence of superheavy elements raises a number of interesting questions that pertain to the field of philosophy of science and also sociology of science. In fact, the very question of whether these superheavy elements actually exist needs to be dissected further, as it will be in the course of this chapter. The synthetic elements are extremely unstable, and only the lightest ones among them have been created in amounts large enough to be observed. Roughly speaking, the heavier the atom, the shorter its lifetime is. For example, the heaviest element for which there is now conclusive evidence is element 118, a few atoms of which have been created in just one single isotope form and with a half-life of less than a millisecond. Laypersons and specialists alike have asked themselves in what sense these elements can really be said to exist. The superheavy elements also have philosophical implications for the study of the periodic system as a whole and the question of whether there is a natural end to chemical periodicity. A related question, which has now become quite pressing, is the possible extension of the periodic table to include a new g-block which in formal terms should begin at element 121.","PeriodicalId":440562,"journal":{"name":"The Periodic Table","volume":"4 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"2019-12-12","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"114290180","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

引用次数: 0