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Compare the electron dot structures of the carbonate (CO32−) and borate (BO33−) ions.

  1. Are these ions isoelectronic?
  2. How many resonance structures does each ion have?
  3. What are the formal charges of each atom in these ions?
  4. If an H+ ion attaches to CO32− to form the bicarbonate ion, HCO3−, does it attach to an O atom or to the C atom?

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Robert Kubara
Robert KubaraLv10
18 Dec 2020

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Related questions

Draw resonance structures for the bicarbonate ion, HCO3-. 

(a) Does HCO3- have the same number of resonance structures as the CO32- ion? Are any less likely than others?

(b) What are the formal charges on the O and C atoms in HCO3-? What is the average formal charge on the O atoms? Compare this with the O atoms in CO32-.

(c) Protonation of HCO3- gives H2CO3. How do formal charges predict where the H+ ion will be attached? 

Draw the resonance structures for the bicarbonate ion, HCO3-.

  1. Does HCO3- have the same number of resonance structure as the CO32- ion? Are any less likely than others?
  2. What are the formal charges on the O and C atoms in HCO3-? What is the average formal charge on the O atoms? Compare this with the O atoms in CO32-.
  3. Protonation of HCO3- gives H2CO3. How do formal charges predict whether H+ ion will be attached?

Compare the electron dot structures of the hydrogen carbonate ion and nitric acid.

(a) Are these species isoelectronic?

(b) How many resonance structures does each species have?

(c) What are the formal charges of each atom in these species?

(d) Compare the two species with respect to their acid-base behavior. (Can either or both species behave as a base and form a bond to H+?)

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