QQuestionChemistry
QuestionChemistry
Is the carbonate ion, CO^32−, a polar or non-polar molecule?
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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:: Understand the Molecular Structure
The carbonate ion $$CO_{3}^{2-}$$ has a trigonal planar geometry.
This means the carbon atom is at the center, with three oxygen atoms arranged symmetrically around it at 120° angles.
Step 3:: Analyze Electronegativity
- Carbon has an electronegativity of 2.55 - Oxygen has an electronegativity of 3.44 - There is a significant difference in electronegativity between carbon and oxygen
Step 4:: Examine Electron Distribution
- The three oxygen atoms are arranged symmetrically - Two oxygen atoms have single bonds - One oxygen atom has a double bond to carbon - The negative charge is distributed equally among the three oxygen atoms
Step 5:: Evaluate Molecular Symmetry
- The three $$C-O$$ bonds create equal but opposing dipole moments
- Due to the symmetric arrangement, the individual bond dipoles cancel each other out
Step 6:: Determine Polarity
- This means the $$CO_{3}^{2-}$$ ion is non-polar
- The symmetric arrangement results in a net dipole moment of zero
Final Answer
The carbonate ion CO_{3}^{2 -} is a non-polar molecule due to its symmetric trigonal planar structure that cancels out individual bond dipoles.
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