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Title: Both CO2 and SiO2 appear to have valid Lewis structures. Using the molecular orbital model, why then ... Post by: sauceboii on Mar 21, 2021 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? ▸ CO2 is able to form sigma bonds and SiO2 is not. ▸ The silicon 3p valence orbitals do not overlap very effectively with the smaller oxygen 2p orbitals. ▸ The carbon atom is larger than the silicon atom, giving carbon a higher electron density and thus better pi bonding. ▸ Silicon prefers to bond to other silicon atoms over oxygen atoms. ▸ At least two of these are correct. Title: Both CO2 and SiO2 appear to have valid Lewis structures. Using the molecular orbital model, why then ... Post by: knppp000 on Mar 21, 2021 Content hidden
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