difference the structure of diamond and graphite
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both r natural occuring carbon compounds but there are different
as graphite can conduct electricity due to presence of one free electron
graphite have soft texture while diamond doesnot conduct electicity and have the hardest carbon compound due to its c c intermolecular force of attraction
graphite are used in pencil for writing as a lubricant at high temperature while diamond have high reflective surface after finishing in jewellery shop and to cut mirrors etc are differences
hope it is upto mark
as graphite can conduct electricity due to presence of one free electron
graphite have soft texture while diamond doesnot conduct electicity and have the hardest carbon compound due to its c c intermolecular force of attraction
graphite are used in pencil for writing as a lubricant at high temperature while diamond have high reflective surface after finishing in jewellery shop and to cut mirrors etc are differences
hope it is upto mark
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Hey,
Friend,
● STRUCTURE OF DIAMOND!
Each carbon atom in a linked with four other carbon atoms through strong single convalent bonds. The bond length is 154pm. (Pm means Pico Meter) .The four surroundings atoms lie at the four vertices (Corners) of a rectangular tetrahedron. The bond angle between any two adjacent carbon atoms is of 109° 28'.Because all carbon atoms are linked with four other carbon atoms by strong convalent bonds, the structure of Diamond is very rigid and its Crystal is very hard.
USES : Diamond is used in making jewellery.
● STRUCTURE OF GRAPHITE !
Graphite has a different structure than that of Diamond. A Graphite Crystal consists of layers of carbon atoms or sheets of carbon atoms. In the making of layers or sheets of carbon atoms in graphite ,out of four valence electrons, three electrons are used by each carbon atom through Strong convalent bonds, to form flat hexagonal rings. These hexagonal layers can slide over each other. The various layers of sheets of carbon atoms in hexagonal array are held together through weak Van der Waal forces of attraction. The distance between any two successive layers is 340 pm.
USES: Graphite is used in making lead pencils.
Hope this will help you...
Friend,
● STRUCTURE OF DIAMOND!
Each carbon atom in a linked with four other carbon atoms through strong single convalent bonds. The bond length is 154pm. (Pm means Pico Meter) .The four surroundings atoms lie at the four vertices (Corners) of a rectangular tetrahedron. The bond angle between any two adjacent carbon atoms is of 109° 28'.Because all carbon atoms are linked with four other carbon atoms by strong convalent bonds, the structure of Diamond is very rigid and its Crystal is very hard.
USES : Diamond is used in making jewellery.
● STRUCTURE OF GRAPHITE !
Graphite has a different structure than that of Diamond. A Graphite Crystal consists of layers of carbon atoms or sheets of carbon atoms. In the making of layers or sheets of carbon atoms in graphite ,out of four valence electrons, three electrons are used by each carbon atom through Strong convalent bonds, to form flat hexagonal rings. These hexagonal layers can slide over each other. The various layers of sheets of carbon atoms in hexagonal array are held together through weak Van der Waal forces of attraction. The distance between any two successive layers is 340 pm.
USES: Graphite is used in making lead pencils.
Hope this will help you...
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