Gilbert N. Lewis
Gilbert N. Lewis | |
---|---|
Awards | Fellow of the Royal Society[1] William H. Nichols Medal (1921) Willard Gibbs Award (1924) Davy Medal (1929) |
Scientific career | |
Fields | Physical chemist |
Thesis | A general equation for free energy and physico-chemical equilibrium, and its application (1899) |
Doctoral advisor | Theodore William Richards |
Doctoral students | Michael Kasha Harold Urey Glenn T. Seaborg Joseph Edward Mayer |
Gilbert Newton Lewis
G. N. Lewis was born in 1875 in Weymouth, Massachusetts. After receiving his PhD in chemistry from Harvard University and studying abroad in Germany and the Philippines, Lewis moved to California in 1912 to teach chemistry at the University of California, Berkeley, where he became the dean of the college of chemistry and spent the rest of his life.[3][11] As a professor, he incorporated thermodynamic principles into the chemistry curriculum and reformed chemical thermodynamics in a mathematically rigorous manner accessible to ordinary chemists. He began measuring the free energy values related to several chemical processes, both organic and inorganic. In 1916, he also proposed his theory of bonding and added information about electrons in the periodic table of the chemical elements. In 1933, he started his research on isotope separation. Lewis worked with hydrogen and managed to purify a sample of heavy water. He then came up with his theory of acids and bases, and did work in photochemistry during the last years of his life.
Though he was nominated 41 times, G. N. Lewis never won the
Biography
Early life
Lewis was born in 1875 and raised in Weymouth, Massachusetts, where there exists a street named for him, G.N. Lewis Way, off Summer Street. Additionally, the wing of the new Weymouth High School Chemistry department has been named in his honor. Lewis received his primary education at home from his parents, Frank Wesley Lewis, a lawyer of independent character, and Mary Burr White Lewis. He read at age three and was intellectually precocious. In 1884 his family moved to Lincoln, Nebraska, and in 1889 he received his first formal education at the university preparatory school.
In 1893, after two years at the
Harvard, Manila, and MIT
After his stay in Nernst's lab, Lewis returned to Harvard in 1901 as an instructor for three more years. He was appointed instructor in thermodynamics and electrochemistry. In 1904 Lewis was granted a leave of absence and became Superintendent of Weights and Measures for the Bureau of Science in Manila, Philippines. The next year he returned to Cambridge, Massachusetts when the Massachusetts Institute of Technology (MIT) appointed him to a faculty position, in which he had a chance to join a group of outstanding physical chemists under the direction of Arthur Amos Noyes. He became an assistant professor in 1907, associate professor in 1908, and full professor in 1911.
University of California, Berkeley
G. N. Lewis left MIT in 1912 to become a professor of physical chemistry and dean of the
Lewis' graduate advisees at Berkeley went on to be exceptionally successful with the
While at Berkeley he also refused entry to women, including preventing
Death
On 23 March 1946,[33] a graduate student found Lewis's lifeless body under a laboratory workbench at Berkeley. Lewis had been working on an experiment with liquid hydrogen cyanide, and deadly fumes from a broken line had leaked into the laboratory. The coroner ruled that the cause of death was coronary artery disease, because of a lack of any signs of cyanosis,[34] but some believe that it may have been a suicide. Berkeley Emeritus Professor William Jolly, who reported the various views on Lewis's death in his 1987 history of UC Berkeley's College of Chemistry, From Retorts to Lasers, wrote that a higher-up in the department believed that Lewis had committed suicide.[13]
If Lewis's death was indeed a suicide, a possible explanation was depression brought on by a lunch with
Lewis Hall at Berkeley, built in 1948, is named in his honor.[11]
Scientific achievements
This sect includes a list of general references, but it lacks sufficient corresponding inline citations. (August 2020) |
Thermodynamics
Most of Lewis’ lasting interests originated during his Harvard years. The most important was thermodynamics, a subject in which Richards was very active at that time. Although most of the important thermodynamic relations were known by 1895, they were seen as isolated equations, and had not yet been rationalized as a logical system, from which, given one relation, the rest could be derived. Moreover, these relations were inexact, applying only to ideal chemical systems. These were two outstanding problems of theoretical thermodynamics. In two long and ambitious theoretical papers in 1900 and 1901, Lewis tried to provide a solution. Lewis introduced the thermodynamic concept of
Lewis’ early papers also reveal an unusually advanced awareness of J. W. Gibbs's and P. Duhem's ideas of free energy and thermodynamic potential. These ideas were well known to physicists and mathematicians, but not to most practical chemists, who regarded them as abstruse and inapplicable to chemical systems. Most chemists relied on the familiar thermodynamics of heat (enthalpy) of Berthelot, Ostwald, and Van ’t Hoff, and the calorimetric school. Heat of reaction is not, of course, a measure of the tendency of chemical changes to occur, and Lewis realized that only free energy and entropy could provide an exact chemical thermodynamics. He derived free energy from fugacity; he tried, without success, to obtain an exact expression for the entropy function, which in 1901 had not been defined at low temperatures. Richards too tried and failed, and not until Nernst succeeded in 1907 was it possible to calculate entropies unambiguously. Although Lewis’ fugacity-based system did not last, his early interest in free energy and entropy proved most fruitful, and much of his career was devoted to making these useful concepts accessible to practical chemists.
At Harvard, Lewis also wrote a theoretical paper on the thermodynamics of
Valence theory
About 1902 Lewis started to use unpublished drawings of cubical atoms in his lecture notes, in which the corners of the cube represented possible electron positions. Lewis later cited these notes in his classic 1916 paper on chemical bonding, as being the first expression of his ideas.
A third major interest that originated during Lewis’ Harvard years was his valence theory. In 1902, while trying to explain the laws of valence to his students, Lewis conceived the idea that atoms were built up of a concentric series of cubes with electrons at each corner. This “cubic atom” explained the cycle of eight elements in the periodic table and was in accord with the widely accepted belief that chemical bonds were formed by transfer of electrons to give each atom a complete set of eight. This electrochemical theory of valence found its most elaborate expression in the work of Richard Abegg in 1904,[39] but Lewis’ version of this theory was the only one to be embodied in a concrete atomic model. Again Lewis’ theory did not interest his Harvard mentors, who, like most American chemists of that time, had no taste for such speculation. Lewis did not publish his theory of the cubic atom, but in 1916 it became an important part of his theory of the shared electron pair bond.
In 1916, he published his classic paper on chemical bonding "The Atom and the Molecule"
Acids and bases
In 1923, he formulated the electron-pair theory of acid–base reactions. In this theory of acids and bases, a "Lewis acid" is an electron-pair acceptor and a "Lewis base" is an electron-pair donor.[41] This year he also published a monograph on his theories of the chemical bond.[42]
Based on work by J. Willard Gibbs, it was known that chemical reactions proceeded to an equilibrium determined by the free energy of the substances taking part. Lewis spent 25 years determining free energies of various substances. In 1923 he and Merle Randall published the results of this study,[43] which helped formalize modern chemical thermodynamics.
Heavy water
Lewis was the first to produce a pure sample of deuterium oxide (
O4 Tetraoxygen
In 1924, by studying the magnetic properties of solutions of oxygen in liquid nitrogen, Lewis found that O4 molecules were formed.[48] This was the first evidence for tetratomic oxygen.
Relativity and quantum physics
In 1908 he published the first of several papers on relativity, in which he derived the mass-energy relationship in a different way from Albert Einstein's derivation.[10] In 1909, he and Richard C. Tolman combined his methods with special relativity.[49] In 1912 Lewis and Edwin Bidwell Wilson presented a major work in mathematical physics that not only applied synthetic geometry to the study of spacetime, but also noted the identity of a spacetime squeeze mapping and a Lorentz transformation.[50][51]
In 1926, he coined the term "photon" for the smallest unit of radiant energy (light). Actually, the outcome of his letter to Nature was not what he had intended.[52] In the letter, he proposed a photon being a structural element, not energy. He insisted on the need for a new variable, the number of photons. Although his theory differed from the quantum theory of light introduced by Albert Einstein in 1905, his name was adopted for what Einstein had called a light quantum (Lichtquant in German).
Other achievements
In 1921, Lewis was the first to propose an empirical equation describing the failure of strong electrolytes to obey the law of mass action, a problem that had perplexed physical chemists for twenty years.[53] His empirical equations for what he called ionic strength were later confirmed to be in accord with the Debye–Hückel equation for strong electrolytes, published in 1923.
Over the course of his career, Lewis published on many other subjects besides those mentioned in this entry, ranging from the nature of light quanta to the economics of price stabilization. In the last years of his life, Lewis and graduate student Michael Kasha, his last research associate, established that phosphorescence of organic molecules involves emission of light from one electron in an excited triplet state (a state in which two electrons have their spin vectors oriented in the same direction, but in different orbitals) and measured the paramagnetism of this triplet state.[54]
See also
References
- ^ .
- ^ Jensen, William B. (March 19, 2021). "Gilbert N. Lewis, American chemist". Encyclopedia Britannica.
- ^ a b c "University of California: In Memoriam, 1946". texts.cdlib.org. Retrieved March 9, 2019.
- ^ a b "Gilbert N. Lewis". Atomic Heritage Foundation. Retrieved March 9, 2019.
- Joel H. HildebrandNational Academy of Sciences 1958
- ^ Lewis, Gilbert Newton R. E. Kohler in Complete Dictionary of Scientific Biography (Encyclopedia.com)
- ^ "Gilman Hall University of California, Berkeley - National Historic Chemical Landmark". American Chemical Society. Retrieved March 9, 2019.
- ISSN 1755-4330.
- ^ "December 18, 1926: Gilbert Lewis coins "photon" in letter to Nature". APS News: This Month in Physics History. American Physical Society. December 2012. Retrieved August 4, 2019.
- ^ .
- ^ a b c "Lewis Hall | Campus Access Services". access.berkeley.edu. Retrieved March 9, 2019.
- ^ a b "Nomination Database Gilbert N. Lewis". NobelPrize.org. Retrieved May 10, 2016.
- ^ a b c DelVecchio, Rick; Writer, Chronicle Staff (August 5, 2006). "WHAT KILLED FAMED CAL CHEMIST? / 20th century pioneer who failed to win a Nobel Prize may have succumbed to a broken heart, one admirer theorizes". SFGate. Retrieved March 9, 2019.
- ^ a b "December 18, 1926: Gilbert Lewis coins "photon" in letter to Nature". www.aps.org. Retrieved March 9, 2019.
- .
- ^ a b c d "Gilman Hall University of California, Berkeley - National Historic Chemical Landmark". American Chemical Society. Retrieved March 9, 2019.
- ^ a b "The Nobel Prize in Chemistry 1949". NobelPrize.org. Retrieved March 9, 2019.
- ^ a b "Research Profile - Willard Frank Libby". Lindau Nobel Mediatheque. Retrieved March 9, 2019.
- ^ a b "Gilbert Newton Lewis | Lemelson-MIT Program". lemelson.mit.edu. Archived from the original on April 11, 2020. Retrieved March 9, 2019.
- ISSN 0021-9584.
- ^ Hildebrand, Joel H. (1958). "Gilbert Newton Lewis" (PDF). Biographical Memoirs of the National Academy of Sciences. Vol. 31. Washington, D.C., U.S.A.: National Academy of Sciences. pp. 209–235.; see p. 210. Lewis's Ph.D. thesis was titled "Some electrochemical and thermochemical relations of zinc and cadmium amalgams". He published the results jointly with his supervisor T.W. Richards.
- JSTOR 20020864.
- S2CID 5682498.
- ^ 10 Fierce (But Productive) Rivalries Between Dueling Scientists Radu Alexander. Website of Listverse Ltd. April 7th 2015. Retrieved 2016-03-24.
- ^ Coffey (2008): 195-207.
- ^ "About - Alpha Chi Sigma | Sigma Chapter". axs.berkeley.edu. Retrieved March 9, 2019.
- ^ Physics, American Institute of (September 24, 2021). "Willard Libby - Session I". www.aip.org. Retrieved August 17, 2023.
- ^ Davidson, Keay (September 8, 2006). "Margaret Fuchs -- worked on secret atomic bomb project". SFGATE. Archived from the original on May 13, 2021.
- PMID 10210206.
- ^ "Gilbert N. Lewis". www.nasonline.org. Retrieved October 3, 2023.
- ^ "APS Member History". search.amphilsoc.org. Retrieved October 3, 2023.
- ^ Coffey (2008): 221-22.
- ^ Helmenstine, Todd (March 22, 2018). "Today in Science History - March 23 - Gilbert Lewis". Science Notes and Projects. Retrieved August 6, 2020.
- ^ a b Coffey (2008): 310-15.
- JSTOR 20021635. ; the term "fugacity" is coined on p. 54.
- JSTOR 20022322. ; the term "activity" is defined on p. 262.
- .
- JSTOR 20020988. The term "escaping tendency" is introduced on p. 148, where it is represented by the Greek letter ψ ; ψ is defined for ideal gases on p. 156.
- .
- S2CID 95865413.
- ^ Lewis, Gilbert Newton (1923). Valence and the Structure of Atoms and Molecules. New York: Chemical Catalog Company. p. 142.
We are inclined to think of substances as possessing acid or basic properties, without having a particular solvent in mind. It seems to me that with complete generality we may say that a basic substance is one which has a lone pair of electrons which may be used to complete the stable group of another atom, and that an acid substance is one which can employ a lone pair from another molecule in completing the stable group of one of its own atoms. In other words, the basic substance furnishes a pair of electrons for a chemical bond, the acid substance accepts such a pair.
- ^ Lewis, G. N. (1926) Valence and the Nature of the Chemical Bond. Chemical Catalog Company.
- ^ Lewis, G. N. and Merle Randall (1923) Thermodynamics and the Free Energies of Chemical Substances. McGraw-Hill.
- .
- .
- S2CID 4106325.
- ^ "Deuteron - an overview | ScienceDirect Topics".
- ISSN 0002-7863.
- JSTOR 20022495.
- JSTOR 20022840.
- ^ Synthetic Spacetime, a digest of the axioms used, and theorems proved, by Wilson and Lewis. Archived by WebCite
- ^
Lewis, G.N. (1926). "The conservation of photons". S2CID 4110026.
- . The term "ionic strength" is introduced on p. 1140.
- .
Further reading
- Coffey, Patrick (2008) Cathedrals of Science: The Personalities and Rivalries That Made Modern Chemistry. Oxford University Press. ISBN 978-0-19-532134-0
External links
- Media related to Gilbert Newton Lewis at Wikimedia Commons
- Key Participants: G. N. Lewis - Linus Pauling and the Nature of the Chemical Bond: A Documentary History
- Eric Scerri, The Periodic Table, Its Story and Its Significance, Oxford University Press, 2007, see chapter 8 especially
- National Academy of Sciences Biographical Memoir