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Magazine Chapter 18: Q56E (page 1043)
Carbon forms the \({\rm{CO}}_{\rm{3}}^{{\rm{2 - }}}\)ion, yet silicon does not form an analogous \({\rm{SiO}}_{\rm{3}}^{{\rm{2 - }}}\)ion. Why?
Short Answer
A silicon atom is significantly larger than an oxygen atom, the double bond of oxygen cannot be stable and so silicon does not exist in the form of \({\rm{SiO}}_3^{2 - }.\)
Step by step solution
Lewis structure of carbonate ion
The Lewis structure of a carbonate ion has two single bonds, two negative oxygen atoms, and one short double bond to neutral oxygen.
Lewis structure of carbonate ion
Explanation
A carbon atom is similar in size as compared to an oxygen atom, while a silicon atom is larger.
Since carbon is smaller in size, it can form an ion with three oxygen atoms because of its ability to make a double bond with oxygen. This structure is, however, incompatible with the carbonate ion's observed symmetry, which implies that the three bonds and oxygen atoms are equivalent.
A silicon atom is significantly larger than an oxygen atom, and the double bond of oxygen cannot be stable in this case.
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