Silicon dioxide (SiO2SiO_2SiO2) is a solid with a high melting point (1713∘C1713^\circ\text{C}1713∘C), whereas carbon dioxide (CO2CO_2CO2) is a gas at room temperature that sublimes at −78.5∘C-78.5^\circ\text{C}−78.5∘C. Which statement correctly explains this difference in physical properties?
Silicon dioxide (SiO2SiO_2SiO2) has a giant covalent structure where strong covalent bonds must be broken to melt it, whereas carbon dioxide (CO2CO_2CO2) has a simple molecular structure where only weak intermolecular forces must be overcome.
Silicon dioxide (SiO2SiO_2SiO2) has a giant ionic structure with strong electrostatic attractions, whereas carbon dioxide (CO2CO_2CO2) has a simple molecular structure with weak covalent bonds between its molecules.
Silicon dioxide (SiO2SiO_2SiO2) has a simple molecular structure with strong intermolecular forces, whereas carbon dioxide (CO2CO_2CO2) has a giant covalent structure with weak covalent bonds.
Silicon dioxide (SiO2SiO_2SiO2) has a giant covalent structure where weak intermolecular forces must be broken to melt it, whereas carbon dioxide (CO2CO_2CO2) has a simple molecular structure where strong covalent bonds must be broken.