Silicon dioxide ( $SiO_2$ ) is a solid with a high melting point ( $1713∘C1713^\circ\text{C}$ ), whereas carbon dioxide ( $CO_2$ ) is a gas at room temperature that sublimes at $−78.5∘C-78.5^\circ\text{C}$ . Which statement correctly explains this difference in physical properties?

Silicon dioxide ( $SiO_2$ ) has a giant covalent structure where strong covalent bonds must be broken to melt it, whereas carbon dioxide ( $CO_2$ ) has a simple molecular structure where only weak intermolecular forces must be overcome.

Silicon dioxide ( $SiO_2$ ) has a giant ionic structure with strong electrostatic attractions, whereas carbon dioxide ( $CO_2$ ) has a simple molecular structure with weak covalent bonds between its molecules.

Silicon dioxide ( $SiO_2$ ) has a simple molecular structure with strong intermolecular forces, whereas carbon dioxide ( $CO_2$ ) has a giant covalent structure with weak covalent bonds.

Silicon dioxide ( $SiO_2$ ) has a giant covalent structure where weak intermolecular forces must be broken to melt it, whereas carbon dioxide ( $CO_2$ ) has a simple molecular structure where strong covalent bonds must be broken.

Silicon dioxide ( $SiO_2$ ) has a simple molecular structure with strong intermolecular forces, whereas carbon dioxide ( $CO_2$ ) has a giant covalent structure with weak covalent bonds.

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