Question

Which has the highest carbon bond length among graphite diamond fullerene

Answer 1

Answer:

Explanation:

Carbon atoms are unique in that they are able to form many different kinds of bonds with other carbon atoms. Graphite is layered. Within each layer, carbon atoms form strong covalent bonds in a hexagonal pattern (planar). A covalent bond is one in which one or more pairs of bonding electrons (valence) are shared. Carbon forms a double covalent bond, which means that two pairs of bonding electrons are shared. This type of bond is very strong. The bond length is 0.142 nm. The bonds between atoms of carbon in the layers of graphite may be strong, but the bonds that are formed by carbon atoms between layers are quite weak. These atoms are held together by Van Der Waal's forces. This kind of attraction is caused by shifts in the cloud of electrons surrounding carbon nuclei. When the electron cloud shifts in a certain way, the carbon atom may become slightly negatively charged on one side and slightly positively charged on the other. The carbon atom becomes a dipole and induces other carbon atoms to become dipoles, as well. Since the layers are only weakly attracted to each other, they can easily slide past one another. This is why graphite is used in pencil lead. The distance between layers is 0.335 nm.

Carbon atoms in diamond are covalently bonded and are arranged in a three-dimensional tetrahedral structure. All bonds are of the same length, 0.154 nm. In this rigid network, none of the carbon atoms can move. This accounts for the fact that diamonds are so hard and have such a high melting point.

Answer 2

The highest carbon bond length among graphite, diamond, and fullerene is acquired by fullerene.

Explanation:

Graphite, diamond, fullerene are all allotropes of carbon. In graphite carbon atoms are arranged in layers attached to each other in a hexagonal arrangement. Bond length of carbon atoms in graphite is $1.421^{o}A$.

In diamond, four carbon atoms are covalently bonded to each other forming a ring structure. Bond length of carbon atoms in diamond is 1.545.

In fullerene, carbon atoms are also covalently attached with a bond length of $1.86^{o}A$.

Learn more about allotropes of carbon:

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