Properties of Solids

AP Chemistry· difficulty 4/5

The chart compares melting points: NaCl (801°C), SiO2 (1713°C), and CO2 (-78°C). The vertical bar height represents melting point.

The very low melting point of CO2 (a molecular solid) is best explained by:

A
$Lack of nuclei in CO2$
B
$Weak ionic bonds in CO2$
C
$Weak C=O double bonds$
D
$Only weak intermolecular forces (London dispersion) hold CO2 molecules together$
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Explanation

Within each CO2 molecule, the C=O bonds are strong, but only weak London dispersion forces hold molecules to one another, so CO2 melts at very low temperature.

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