Chemistry

Problem

Which statement best explains why graphite conducts electricity whereas diamond does not? a) In graphite, each carbon atom is

sp^{3}

-hybridized, generating four equivalent overlapping orbitals that allow electrons to flow; in diamond, the

sp^{2}

-hybridized carbons confine electrons to

\pi

bonds. b) The weak London forces between graphite's layers permit electrons to slip and carry charge, whereas diamond's three-dimensional network prevents electron movement. c) In graphite, each carbon atom is

sp^{2}

-hybridized, leaving delocalized

\pi

electrons that can move throughout the layers; in diamond, all valence electrons are localized in

\sigma

bonds. d) In graphite, mobile

\mathrm{C^{+}}

and

\mathrm{C^{-}}

ions migrate within the layers, enabling conduction; in diamond, the absence of ions prevents conductivity.

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