For which of the following pure solids is it necessary to break covalent bonds to make a liquid or gas: C(graphite),CO₂(s),C₆₀(s),and C(diamond)? A) C(graphite)only B) CO₂(s)only C) CO₂(s)and C₆₀(s) D) C(graphite),C₆₀(s)and C(diamond) E) C(graphite)and C(diamond)

Question

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Both C(graphite) and C(diamond) are pure covalent solids composed entirely of carbon atoms bonded together in a network of covalent bonds. Breaking these bonds is necessary to transition from a solid to a liquid or gas. CO₂(s) and C₆₀(s) are both molecular solids held together by intermolecular forces such as London dispersion forces and dipole-dipole interactions. These forces can be overcome by increasing temperature and/or decreasing pressure to convert the substance to liquid or gas without breaking covalent bonds.

For Which of the Following Pure Solids Is It Necessary