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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Identify the Lewis Structure
- In the carbonate ion $$CO_{3}^{2-}$$, carbon is bonded to three oxygen atoms
- One oxygen has a double bond, two have single bonds with negative charge distribution
Step 3:: Determine Electron Configuration
- In $$CO_{3}^{2-}$$, carbon forms 3 bonds
- Carbon has 4 valence electrons - Total electron count: 4 (carbon) + 3(12 from oxygens) + 2 (additional electrons from negative charge) - This suggests an expanded octet
Step 4:: Analyze Bonding Geometry
- Angles between bonds are approximately $$120^{\circ}
- The carbon is surrounded by three oxygen atoms - The geometry is trigonal planar
Step 5:: Determine Hybridization
- One $$p$$ orbital remains unhybridized for $$\pi$$ bonding
- Three sp^{2} hybrid orbitals are formed
Final Answer
The hybridization of carbon in CO_{3}^{2 -} is sp^{2}.
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