QQuestionChemistry
QuestionChemistry
Part A: What are the electron and molecular geometries, respectively, for the carbonate ion, CO^2−3
?
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:: Determine the electron geometry using the Valence Shell Electron Pair Repulsion (VSEPR) theory.
In the carbonate ion (CO^2−3), there are 4 regions of electron density around the central carbon atom: 2 from the double bonds to the oxygen atoms and 2 from the lone pairs on the oxygen atoms. According to the VSEPR theory, these electron pairs will arrange themselves in such a way as to minimize repulsion between them.
Step 2:: Place the electron pairs in a tetrahedral arrangement.
Since there are 4 regions of electron density, they will arrange themselves in a tetrahedral shape. However, since there are 2 lone pairs, they will occupy more space than the bonding pairs.
Step 3:: Determine the molecular geometry.
The molecular geometry is based on the arrangement of the atoms, not the electron pairs. In this case, the central carbon atom is bonded to 3 oxygen atoms, forming a trigonal planar shape.
Step 4:: Summarize the electron and molecular geometries.
Electron geometry: Tetrahedral Molecular geometry: Trigonal planar
Final Answer
The electron geometry of the carbonate ion (CO^2−3) is tetrahedral, and the molecular geometry is trigonal planar.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students