Answer
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Step 1:: Identify the central atom and its surrounding atoms or groups of atoms.
In CO3^2 -, the central atom is carbon (C) and it is surrounded by three oxygen (O) atoms.
Step 2:: Determine the number of electron pairs around the central atom.
To find the number of electron pairs, we need to consider both bonding and lone pairs. In this case, there are 3 bonds between the carbon and oxygen atoms. Since each bond contains 2 electrons, there are a total of 3 * 2 = 6 electrons from bonds. Now, let's account for the charge on the ion. The - 2 charge indicates that there are 2 additional electrons in the system. Therefore, the total number of electron pairs around the central atom is 6 (from bonds) + 2 / 2 (from the - 2 charge) = 8 electron pairs.
Step 3:: Apply the valence shell electron pair repulsion (VSEPR) theory to predict the molecular geometry.
According to the VSEPR theory, electron pairs will arrange themselves in such a way that minimizes repulsion between them. When there are 4 electron pairs (including lone pairs) around the central atom, as in our case, the molecular geometry is typically tetrahedral. However, since carbon is bonded to three oxygen atoms, the actual geometry is a distorted tetrahedron, also known as a trigonal planar geometry.
Step 4:: Describe the molecular geometry.
The molecular geometry of CO3^2 - is trigonal planar, with the central carbon atom bonded to three oxygen atoms arranged in a flat, triangular arrangement.
Final Answer
The molecular geometry of CO3^2 - is trigonal planar.
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