Something to do with the free electron it has, that can carry a charge, and also it can ibrate/move
all C-C bond length in graphite is 1.415 angstrom which agree with the assumption that the bond order in graphite is nearly 1.33
covalent
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
Network solid
Covalent Bonding ...these two elements are non metals with a relativelly small difference in electronegativity. The compound is boron nitride, BN which has a structure like graphite, however it is colorless and does not conduct electricity.
all C-C bond length in graphite is 1.415 angstrom which agree with the assumption that the bond order in graphite is nearly 1.33
covalent
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
graphite
Pencil lead (aka graphite) DOES conduct electricity. It does this thanks to electron delocalization within the carbon layers. Since the valence electrons are free to move, they are able to conduct electricity.
Only eighteen elements in the periodic table are generally considered nonmetals, compared to over eighty metals. Although nonmetals are generally poor conductors of heat and electricity when compared to metals, many of them still can conduct electricity. The metalloid elements (such as Silicon and Germanium) can conduct electricity and are used as semiconductors in electronics. Many generally nonmetal compounds (composed of nonmetals) can also conduct electricity, with gallium arsenide, and silicon carbide being popular components in semiconductors as well.
seeing how it has a CRYSTAL STRUCTURE I would say ionic bond.
Network solid
Yes, it can bond with other cabons . For example, a diamond, graphite (in pencils) and charcoal.
Covalent Bonding ...these two elements are non metals with a relativelly small difference in electronegativity. The compound is boron nitride, BN which has a structure like graphite, however it is colorless and does not conduct electricity.
In graphite which consists of fused hexagons of carbon atoms arranged in sheets there is considerable delocalisation of electrons. In diamond the structure is "3 dimensional" with each atom of carbon tetrahedrally surronded by 4 other carbon atoms. The bonding is covalent and the electrons in each bond are localised.