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Graphite is another form of carbon. The difference in properties between graphite and diamond is a great example of the incredible versatility of carbon bonding. Carbon's ability to exist in such diverse forms (as the pure element) really stands as a "testament" to the existence of carbon-containing compounds numbering well into the thousands. Indeed, if it were not for carbon's flexibility in bonding, life, as we know it, would not exist! In fact, the wide range of carbon-compound molecular structures provides the "raw materials" necessary for the complex chemical processes of life. Consequently, the scientific study of carbon and numerous carbon-containing compounds is, fittingly, called Organic Chemistry. Many years ago it was a commonly-held belief that carbon-containing compounds could only be produced by way of life processes.
Graphite is a conglomeration of stacked planar massive fused-hexagonal-ring layers loosely connected together. The sp2 hybridized bonding within the fused-ring layers leaves a single p-atomic orbital for each carbon atom. The p orbitals extend above and below at right angles to the fused ring plane. Sigma bonding (end-to-end overlap) between p-orbitals holds the layers together, but only very weakly. The result is that fused ring layers can easily be sloughed off, which provides the familiar "broken pencil lead" chipped appearance. Pencil "lead" actually contains no lead whatsoever - Pencils contain varying compositions of clay+graphite mixtures, depending on hardness rating. This is important for graphite-drawing artists, so that multiple variations in line thickness and darkness may be obtained.
Graphite also exhibits metallic properties of luster and conductivity. The optical and electrical characteristics are both a result of freely roaming electrons (delocalized across pi-bonded (side-to -side overlap)) throughout the fused ring layers. The following diagram is a pictorial representation of carbon-graphite.
That's all for now. Thank you for reading!
A Publication of http://ExcellenceInLearning.biz
Graphite is another form of carbon. The difference in properties between graphite and diamond is a great example of the incredible versatility of carbon bonding. Carbon's ability to exist in such diverse forms (as the pure element) really stands as a "testament" to the existence of carbon-containing compounds numbering well into the thousands. Indeed, if it were not for carbon's flexibility in bonding, life, as we know it, would not exist! In fact, the wide range of carbon-compound molecular structures provides the "raw materials" necessary for the complex chemical processes of life. Consequently, the scientific study of carbon and numerous carbon-containing compounds is, fittingly, called Organic Chemistry. Many years ago it was a commonly-held belief that carbon-containing compounds could only be produced by way of life processes.
Graphite is a conglomeration of stacked planar massive fused-hexagonal-ring layers loosely connected together. The sp2 hybridized bonding within the fused-ring layers leaves a single p-atomic orbital for each carbon atom. The p orbitals extend above and below at right angles to the fused ring plane. Sigma bonding (end-to-end overlap) between p-orbitals holds the layers together, but only very weakly. The result is that fused ring layers can easily be sloughed off, which provides the familiar "broken pencil lead" chipped appearance. Pencil "lead" actually contains no lead whatsoever - Pencils contain varying compositions of clay+graphite mixtures, depending on hardness rating. This is important for graphite-drawing artists, so that multiple variations in line thickness and darkness may be obtained.
Graphite also exhibits metallic properties of luster and conductivity. The optical and electrical characteristics are both a result of freely roaming electrons (delocalized across pi-bonded (side-to -side overlap)) throughout the fused ring layers. The following diagram is a pictorial representation of carbon-graphite.
That's all for now. Thank you for reading!
A Publication of http://ExcellenceInLearning.biz