Gilbert lewis atomic model

The subject of chemical bonding is at the heart of chemistry. In 1916 Gilbert Newton Lewis (1875–1946) published his seminal paper suggesting that a chemical bond is a pair of electrons shared by two atoms.

Once physicists studying the structure of the atom began to realize that the electrons surrounding the nucleus had a special arrangement, chemists began to investigate how these theories corresponded to the known chemistry of the elements and their bonding abilities. Lewis was instrumental in developing a bonding theory based on the number of electrons in the outermost “valence” shell of the atom.

Shared Electrons and Chemical Bonds

In 1902, while Lewis was trying to explain valence to his students, he depicted atoms as constructed of a concentric series of cubes with electrons at each corner. This “cubic atom” explained the eight groups in the periodic table and represented his idea that chemical bonds are formed by electron transference to give each atom a complete set o

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Gilbert Lewis

Gilbert Newton Lewis, one of the most influential and admired scientists of the twentieth century, was a pioneer in both chemistry and physics.

Born in Weymouth Landing, Massachusetts in 1875, Lewis was able to read by the age of 3. He entered college at age 15, and then transferred to Harvard University, where he earned a BS (1896) and a PhD (1899). His research concentrated on thermodynamics and valence theory (on the behavior of electrons when atoms combine). From this early work on valence, Lewis developed the concept of the covalent bond and invented the "Lewis symbols," which are still used to describe ways in which atoms bond.

Lewis taught at Harvard and the Massachusetts Institute of Technology before becoming a Professor and Dean at the University of California at Berkeley. He single-handedly transformed the then-languishing College of Chemistry at UC Berkeley into one of the nation's best. Lewis became the mentor to 290 PhD recipients and 20 Nobel Pr

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Lewis structure

Diagrams for the bonding between atoms of a molecule and lone pairs of electrons

Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.^[1][2][3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molekyl, as well as coordination compounds. ^[4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a kemikalie bond.

Lewis structures show each atom and its position in the structure of the molecule using its kemikalie symbol. Lines are drawn between atoms that are bonded to one another (pairs of dots can be used i