Molecular Shapes: What Does CO3^-2 Look Like?

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Discussion Overview

The discussion centers around the molecular structure and shape of the carbonate ion, CO3^-2, including its bonding and geometry. Participants explore how to visualize and represent the molecule based on its valence electrons and bonding arrangements.

Discussion Character

  • Exploratory
  • Technical explanation
  • Conceptual clarification

Main Points Raised

  • One participant asks for a visual representation of the carbonate ion, indicating interest in its molecular shape.
  • Another participant provides clues for determining the structure, emphasizing the importance of valence electrons and the central atom's identity.
  • A different participant describes the bonding in the carbonate ion, stating that carbon is double bonded to one oxygen and single bonded to two others, with the latter carrying a -1 charge each, and identifies the geometry as trigonal planar with sp2 hybridization.
  • One participant expresses understanding after the explanation, suggesting engagement with the material.
  • A participant mistakenly suggests that the original inquiry may refer to CO2 instead of CO3^-2.
  • Another participant clarifies that the discussion is indeed about the carbonate ion, CO3 with a -2 charge.

Areas of Agreement / Disagreement

Participants generally agree on the identity of the molecule as the carbonate ion, but there is some confusion regarding its representation and bonding, with differing interpretations of its structure and bonding details.

Contextual Notes

Some assumptions about the bonding and hybridization are made without detailed justification, and the discussion does not resolve the potential confusion regarding the molecular identity.

decibel
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what does a CO(subscript3)^-2 look like? (as in the drawing and the shape of the molecule?
 
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Clues so you can work this out for yourself:

1.) How many valence electrons are there? (Don't forget to factor in the charge of the molecule!)

2.) It is safe to conclude that carbon is the central atom, given that is typically how the chemical shorthand works.

3.) So if you have a carbon atom at the center and three oxygen atoms, what is the most intuitive way to arrange these three atoms?

4.) Fill the valences with your calculated number of valence electrons for all the atoms, remembering that the final molecule should have a formal charge of -2 at the end.

Good luck!
 
THe central carbon is double bonded to one oxygen and single bonded to two oxygens. The two single bonded oxygens both carry a -1 charge. Trigonal planar, carbon's sp2 hybridized.
 
hmm...ok i think i got it, thanks
 
Originally posted by decibel
what does a CO(subscript3)^-2 look like? (as in the drawing and the shape of the molecule?
You mean [tex]CO_2[/tex]?





-Chris
 
No, he means the carbonate ion. CO3 with a charge of -2.
 

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