What is the hybridization state of the carbon atoms in diamond, graphite, and fullerenes respectivel — p Block Elements Chemistry Question

💡 Solution & Explanation

In diamond, each carbon is $sp^3$ hybridized, forming a tetrahedral 3D network. In graphite, carbon atoms are $sp^2$ hybridized in planar hexagonal sheets. In fullerenes, carbon atoms are also $sp^2$ hybridized, forming a curved, closed-cage structure.