Answer:
The correct answers are: Each oxygen of carbonate ion has -2/3 or -0.67 charge.
Bond order of each carbon‑oxygen bond in the carbonate ion = 1.33
Explanation:
The carbonate ion (CO₃²⁻) is an organic compound, in which a carbon atom is covalently bonded to three oxygen atoms. The net formal charge on a carbonate ion is −2.
The carbonate ion is resonance stabilized and has three equivalent resonating structures, which exhibits that all the three carbon-oxygen bonds in a carbonate ion are equivalent.
In the resonance hybrid of carbonate ion, the negative charge is equally delocalized on all the three oxygen atoms.
Thus, each bonded oxygen has -2/3 or -0.67 charge.
In a carbonate ion there is one double bond oxygen (C=O) and two single bonded oxygen (C-O). Bond order of 1 C=O is 2 and bond order of C-O is 1.
∴ Bond order = sum of all bond orders ÷ number of bonding groups = (2+1+1) ÷ 3 = 1.33
Each of the single bonded oxygen atoms in the carbonate ion has a bond order of 1.5 and a formal charge of -1 each.
In some compounds or ions, it is impossible to fully describe the bonding in terms of one structure. In such cases, we must assume that a number of structures contribute to the actual bonding in the molecule.
In the carbonate ion, resonance structure can be shown for the molecule. The formal charges on each of the oxygen atoms are calculated below;
For the oxygen atom that has a double bond;
Formal charge = 6 - 4 - 4/2 = 0
Formal charge on the two single bonded oxygen atoms = 6 - 6 - 2/2 = -1
The bond order of the carbon oxygen double bond is 2 while the bond order for the C - O single bonds is 1.5.
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