Lewis dot structures of CO│Electron dot structure of CO
A simple method for writing Lewis Electron Dot Structures (Dot Electron Structures) was given in a previous article entitled “Lewis Structures and the Octet Rule”. Several worked examples relevant to this procedure were given in previous posts please see the Sitemap – Table of Contents (Lewis Electron Dot Structures).
Let us consider the case of the Lewis electron dot structures of carbon monoxide CO.
Carbon monoxide (CO) is a colorless, odorless, and tasteless flammable gas that is slightly less dense than air. It is toxic to animals that use hemoglobin as an oxygen carrier (both Invertebrate and vertebrate) when encountered in concentrations above about 35 ppm, although it is also produced in normal animal metabolism in low quantities, and is thought to have some normal biological functions. In the atmosphere, it is spatially variable and short lived, having a role in the formation of ground-level ozone.
Carbon monoxide consists of one carbon atom and one oxygen atom, connected by a triple bond that consists of two covalent bonds as well as one dative covalent bond.
Draw Lewis structures of CO step by step:
2.Total valence electron is 4+6 = 10
3.Connect the atoms with single bonds.
4.P=6n+2 -V =6×2 +2 -10 = 14-10 = 4 ; 4 electron which must be shared through pi bonding i.e; there must be to pi bond.
5.Distribution of other electron
6. Complete the octet shells
7. Calculare the formal charege….
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- NIOSH Pocket Guide to Chemical Hazards. “#0105“. National Institute for Occupational Safety and Health (NIOSH).
- “Molecular orbitals in Carbon Monoxide CO“. University of Liverpool. Retrieved May 10, 2016.
- G.N. Lewis, J.A.C.S, 38, 762-785, (1916)