Which statement best explains why graphite conducts electricity whereas diamond does not?
CHEMISTRY · Single correct · AP · Chemistry · Compound Structure and Properties · Compound Structure and Properties
Problem
Which statement best explains why graphite conducts electricity whereas diamond does not?
(a) In graphite, each carbon atom is sp3-hybridized, generating four equivalent overlapping orbitals that allow electrons to flow; in diamond, the sp2-hybridized carbons confine electrons to π 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 sp2-hybridized, leaving delocalized π electrons that can move throughout the layers; in diamond, all valence electrons are localized in σ bonds.
(d) In graphite, mobile C+ and C− ions migrate within the layers, enabling conduction; in diamond, the absence of ions prevents conductivity.