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Covalent bonds involve the sharing of valence electrons between nonmetals.
The bonding of electrons is a very important factor in chemistry, because it makes up the world around us. [1] Unlike ionic bonding, which bonds nonmetals and metals, covalent bonding bonds nonmetals with themselves. CITATION REQUIRED In some cases a bonding pair does not share electrons properly in that case, one atom is a stronger attractor than the other. [2]
History
Gilbert N. Lewis is the founder of covalent bonding. [3]. In 1916 this American chemist thought of a structure that we know today as the Electron Dot Configuration, Electron Dot Notation, or as Lewis Notation. (www.chemistry daily.com) The diagram shows the bond between different atoms as the one you see on the front page. Through the Lewis Dot Configuration, you see how valence electrons bond. [4] Each pair you see in the diagram shows a single covalent bond, or shared pair of valence electrons.
Gilbert Newton Lewis was born at Weymouth, Massachusetts. [5]. At the age of 14, Lewis attended the University of Nebraska. Three years later, he went to Harvard college. He got out of college and became very successful. He not only invented the Lewis Dot Diagram, but then went on to teach 20 Nobel Prize winners and 220 people who earned Ph.D.'s(www,its.caltech.edu)
Lewis Dot Diagrams
On the periodic table, there are metals, metalloids, and nonmetals, but covalent bonds is the bonding of only nonmetals with nonmetals. [6]. Only nonmetals are able to form covalent bonds because of their electron configuration. When you see elements in the Lewis Dot Diagram, you see pairs and single dots around the element, these are the valence electrons and the single dots are the amount of electrons that are able to bond to the atom.
To know how many valence electrons each element has you look at the group on the periodic table of elements. (www.chem guide. co. uk) group 7A has only one electron that is able to bond and that is why group 7A or 17 can only make single blonds. Carbon that is the only nonmetal in group 4A has four valence electrons so it can bond up with four different atoms and can perform single,double, and triple bonds. In group 5A, the element have five valence electrons and can bond three times and can do triple bonds. In group 5, it has five and can only perform single and double bonds. The noble gases,in group 8A have perfect electron configuration.
Bond Strength
In covalent bonds, there are different kinds, polar covalent bonds is one of them and another is called hydrogen bonds that are weak bonds that hold H2O together that form water and the bond is caused because the electrons are mostly on the oxygen, so the O has a negative charge and hydrogen has a positive charge and helps water stay together. Awkward sentence Covalent bonds have a very strong bond because of valence electrons to reach noble gas configuration. CITATION REQUIRED
Ionic and Covalent Bonding
the difference between ionic and covalent bonding is that ionic bonding you have to have a nonmetal and a metal. a covalent bond has to have two nonmetals. ionic bonds are contracted together by the oppositely ions. covalent bonds are formed if the atoms charged are equally sharing electrons. it is then called polar.
References
- ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company.p. 360
- ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company. pg.361,Pg.A 52
- ↑ LeMaster, N. & McGann, D. (n.d.). Gilbert Newton Lewis: American Chemist. Retrieved January 14, 2009, from http://www.woodrow.org/teachers/ci/1992/Lewis.htm
- ↑ (www.woodrow.org)
- ↑ LeMaster, N. & McGann, D. (n.d.). Gilbert Newton Lewis: American Chemist. Retrieved January 14, 2009, from http://www.woodrow.org/teachers/ci/1992/Lewis.html
- ↑ Nave, R. .Lewis dot diagrams of selected elements. Retrieved January 14, 2009, from http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/perlewis.html
http://chemistry.about.com/od/Chemistrystudent/f/bondtypes.htm, Annie Marie Helmenstine, Ph.D
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