QQuestionChemistry
QuestionChemistry
"Determine the molecular geometry of the carbonate ion, CO^2−3."
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Identify the Central Atom
The central atom in the carbonate ion is carbon (C). This is the atom to which all other atoms are bonded.
Step 3:: Determine the Number of Valence Electrons
Total valence electrons: $$4 + 18 + 2 = 24
- Carbon (C): 4 valence electrons - Oxygen (O): 6 valence electrons × 3 = 18 valence electrons - Charge of ion: - 2
Step 4:: Draw the Lewis Structure
- Use $$\frac{24}{2} = 12$$ electron pairs to construct the structure
- Carbon is the central atom - Three oxygen atoms are bonded to carbon - One oxygen has a full negative charge - Resonance structure shows equal electron distribution among oxygen atoms
Step 5:: Determine Electron Geometry
- Total electron domains around carbon: 3 - Bonding domains: 3 - Lone pair domains: 0 Electron geometry: Trigonal planar
Step 6:: Determine Molecular Geometry
- Since all electron domains are bonding domains - Molecular geometry is also trigonal planar
Step 7:: Confirm Structural Characteristics
- Bond angles: $$120°
- Symmetric arrangement - Planar structure
Final Answer
The carbonate ion CO_{3}^{2 -} has a trigonal planar molecular geometry with 120° bond angles.
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