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Because elements in the first row (second period) form multiple bonds much more readily than elements in the second row (third period).

N2 is a gas, with the molecule triple-bonded. But P4 is a solid, with each atom at a corner of a tetrahedron, and single bonds to the other three atoms.

Similarly O2 is a gas with double-bonded molecules, but S8 is a solid with sulfur atoms in 8-membered rings. And most dramatically of all, carbon dioxide is a gas with double-bonded atoms: O=C=O , while silicon dioxide is quartz -- a network structure with only single bonds. Each silicon atom is surrounded by and single-bonded to four oxygen atoms; each oxygen atom is single-bonded to two silicon atoms.

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