Both CO₂ and SiO₂ appear to have valid Lewis structures.Using the molecular orbital model,why then are CO₂ molecules stable and SiO₂ molecules not stable? A)CO₂ is able to form sigma bonds and SiO₂ is not. B)The silicon 3p valence orbitals do not overlap very effectively with the smaller oxygen 2p orbitals. C)The carbon atom is larger than the silicon atom,giving carbon a higher electron density and thus better pi bonding. D)Silicon prefers to bond to other silicon atoms over oxygen atoms. E)At least two of the above are correct.

Question

Quizplus · Accepted Answer

The stability of a molecule is determined by the overlap of its atomic orbitals to form molecular orbitals. In SiO₂, the overlap between the larger silicon 3p orbitals and smaller oxygen 2p orbitals is not effective enough to form stable bonds. On the other hand, in CO₂, the carbon atom is smaller, making it easier for its 2p orbitals to overlap with the sulfur and oxygen atoms, resulting in stable molecular orbitals. Choices A, C, and D are not correct as they do not accurately explain the differences in stability between the two molecules.

Both CO2 and SiO2 Appear to Have Valid Lewis Structures

Both CO₂ and SiO₂ Appear to Have Valid Lewis Structures