Understand difference between Structure of Diamond and Graphite. Click on the link to Watch the VIDEO explanation: Watch Video
Diamond and Graphite are allotropic forms of carbon widely differing in their physical appearance as can be seen here. Diamond has unmatched brilliance while graphite is dull and lack lustre. The core of pencil is made of graphite. Observe the diagrammatic view of the molecular structure of diamond and graphite. The diamond crystals found in nature are made of tetrahedron units. In diamond carbon atoms are strongly bound to each other. Each carbon atom is bond to four other carbon atom forming a rigid 3D structure. This strong bonding in diamond is the reason for its hardness, resistance to chemical attacks and high density. Diamond is a non conductor of electricity as there are no free electrons to migrate. Graphite on the other hand are cousin hexagonal layer stacked one on the top of the other. In graphite each carbon atom is bound to three other carbon atom. Carbon atoms arrange themselves into layers and between each layer the bonding is very weak. The layers can therefore easily slip over each other. This explains why the surface of graphite is soft and slippery to touch. Click ahead for differences between diamond and graphite.
Diamond and Graphite are allotropic forms of carbon widely differing in their physical appearance as can be seen here. Diamond has unmatched brilliance while graphite is dull and lack lustre. The core of pencil is made of graphite. Observe the diagrammatic view of the molecular structure of diamond and graphite. The diamond crystals found in nature are made of tetrahedron units. In diamond carbon atoms are strongly bound to each other. Each carbon atom is bond to four other carbon atom forming a rigid 3D structure. This strong bonding in diamond is the reason for its hardness, resistance to chemical attacks and high density. Diamond is a non conductor of electricity as there are no free electrons to migrate. Graphite on the other hand are cousin hexagonal layer stacked one on the top of the other. In graphite each carbon atom is bound to three other carbon atom. Carbon atoms arrange themselves into layers and between each layer the bonding is very weak. The layers can therefore easily slip over each other. This explains why the surface of graphite is soft and slippery to touch. Click ahead for differences between diamond and graphite.
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