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The difference in electrical conductivity between diamond and graphite arises because:
Graphite has delocalized electrons; diamond does not
Diamond has metallic bonding, graphite does not
Diamond has tightly packed ions
Both have free electrons, but in different numbers
Graphite has delocalized electrons; diamond does not
Graphite is a conductor because each carbon atom is bonded to three others, leaving one delocalized electron per atom to move freely throughout the structure. In contrast, diamond features a rigid tetrahedral network where all four valence electrons of carbon are tied in strong covalent bonds, leaving no free electrons for conduction.
Graphite is a conductor because each carbon atom is bonded to three others, leaving one delocalized electron per atom to move freely throughout the structure. In contrast, diamond features a rigid tetrahedral network where all four valence electrons of carbon are tied in strong covalent bonds, leaving no free electrons for conduction.
This concept relates to the chemistry of Allotropes, a fundamental topic in Physical Science under the General Science section of the UPSC and SSC CGL syllabus.
Graphite has a two-dimensional hexagonal layered structure.
Diamond is the hardest natural substance known on Earth.
Both diamond and graphite are allotropes of carbon.
Delocalized electrons in graphite allow it to conduct electricity, making it useful for electrodes in batteries and electrolysis.
Diamond acts as an electrical insulator but is an excellent thermal conductor due to its stiff lattice vibrations.
Option B is incorrect because neither diamond nor graphite possess metallic bonding; both are covalently bonded structures.
Option C is incorrect because diamond is a covalent network solid, not an ionic crystal.
A is correct тАФ Graphite contains free delocalized electrons, whereas diamond's structure utilizes all valence electrons in covalent bonds.
When studying Chemistry for competitive exams, link carbon allotropes with their hybridisation states: Diamond is sp3 hybridized (tetrahedral), while Graphite is sp2 hybridized (trigonal planar).
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