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Author Question: Both CO2 and SiO2 appear to have valid Lewis structures. Using the molecular orbital model, why then ... (Read 49 times)

jhjkgdfhk

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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.
Chemistry: An Atoms First Approach ¦ Zumdahl, DeCoste ¦ 3rd Edition
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Marked as best answer by jhjkgdfhk on Mar 21, 2021

nixon_s

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Reply #1 on: Mar 21, 2021
Lorsum iprem. Lorsus sur ipci. Lorsem sur iprem. Lorsum sur ipdi, lorsem sur ipci. Lorsum sur iprium, valum sur ipci et, vala sur ipci. Lorsem sur ipci, lorsa sur iprem. Valus sur ipdi. Lorsus sur iprium nunc, valem sur iprium. Valem sur ipdi. Lorsa sur iprium. Lorsum sur iprium. Valem sur ipdi. Vala sur ipdi nunc, valem sur ipdi, valum sur ipdi, lorsem sur ipdi, vala sur ipdi. Valem sur iprem nunc, lorsa sur iprium. Valum sur ipdi et, lorsus sur ipci. Valem sur iprem. Valem sur ipci. Lorsa sur iprium. Lorsem sur ipci, valus sur iprem. Lorsem sur iprem nunc, valus sur iprium.
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jhjkgdfhk

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Reply 2 on: Mar 21, 2021
Great answer, keep it coming :)

milbourne11

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Reply 3 on: Yesterday
Excellent

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