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The question appears to be asking about the molecular structure of a C-O-C molecule, where the central carbon (C) atom in a C-C-C chain is replaced with an oxygen (O) atom. Below is a breakdown of how to fill in the table for the C-O-C structure:

1. **Lone pairs of electrons (central atom)**: 
   - Oxygen typically has **2 lone pairs** of electrons. 

2. **Bonding groups (central atom)**: 
   - In the C-O-C structure, oxygen forms two single bonds, one with each carbon atom, so the bonding groups are **2**.

3. **Total valence electrons**: 
   - Oxygen has 6 valence electrons, and each carbon has 4 valence electrons. For the C-O-C molecule:
     - Carbon (C): 2 atoms × 4 valence electrons = 8 electrons
     - Oxygen (O): 1 atom × 6 valence electrons = 6 electrons
     - Total = **14 valence electrons**.

4. **VSEPR molecular shape (central atom)**: 
   - With 2 bonding groups and 2 lone pairs on the oxygen atom, the molecular geometry according to VSEPR theory is **bent** (similar to the structure of water).

Would you like more details on any of these points, or do you have any additional questions?

Here are 5 related questions:
1. How does the replacement of a central carbon atom with oxygen affect bond angles in a molecule?
2. What are the electron-pair geometries of oxygen in different molecular contexts?
3. How do lone pairs of electrons influence the shape of a molecule?
4. What is the difference between bonding groups and lone pairs in determining molecular geometry?
5. How does the VSEPR theory predict molecular shapes for different central atoms?

**Tip:** When drawing Lewis structures, always account for lone pairs and bonding pairs to predict the correct molecular geometry.

Start over with C-C-C then change the central C to an O atom.

Explore how to calculate lone pairs of electrons, bonding groups, and the VSEPR molecular shape of a C-O-C structure by replacing the central C in C-C-C with an oxygen atom. Suitable for high school chemistry students learning molecular geometry.

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