Final answer:
Silicon monoxide and silicon dioxide share the characteristic of silicon forming single bonds with oxygen instead of the double bonds seen in carbon dioxide.
Step-by-step explanation:
The similarity between the results for silicon monoxide and those for silicon dioxide lies in the bonding characteristics of silicon, a group 14 element, with oxygen. Unlike carbon in carbon dioxide, which forms strong è bonds reflected in double bonding to oxygen, silicon does not tend to form such double bonds with oxygen. Instead, silicon dioxide displays a three-dimensional network structure in which each silicon atom forms four Si-O single bonds, leading to a much different set of physical and chemical properties compared to those of CO2.
This difference largely arises from the ability of the second-period elements to form very strong é bonds which are not as easily replicated by elements such as silicon from lower periods. Consequently, the absence of è bonds in compounds like silicon dioxide results in single bonds (ô bonds) that contribute to its covalent network solid structure.