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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

Expert verified

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

01

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

02

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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Most popular questions from this chapter

Draw the Lewis structures and describe the geometry for the following:

(a) \({\rm{P}}{{\rm{F}}_4} + \)

(b) \({\rm{P}}{{\rm{F}}_5}\)

(c) \({\rm{P}}{{\rm{F}}_6}^ - \)

(d) \({\rm{PO}}{{\rm{F}}_3}\)

Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?

Give the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. You may wish to review the chapters on chemical bonding and advanced covalent bonding for relevant examples.

\((a){\rm{Ge}}{{\rm{H}}_4}\)

\((b){\rm{Sb}}{{\rm{F}}_3}\)

\((c){\rm{Te}}{({\rm{OH}})_6}\)

\((d){{\rm{H}}_2}{\rm{Te}}\)

\((e){\rm{Ge}}{{\rm{F}}_2}\)

\((f){\rm{TeC}}{{\rm{l}}_4}\)

\((g){\rm{SiF}}_6^{2 - }\)

\((h){\rm{SbC}}{{\rm{l}}_5}\)

\((i){\rm{Te}}{{\rm{F}}_6}\)

Oxygen forms double bonds in\({{\rm{O}}_2}\), but sulfur forms single bonds in \({{\rm{S}}_8}\). Why?

Which is a stronger acid, sulfurous acid or sulfuric acid? Why?
See all solutions

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