Show the Lewis structure of CPo2. Be sure to show lone pairs.
The correct answer and explanation is:
The correct Lewis structure for CPo₂ (carbon dipolonide) follows these steps:
- Count Valence Electrons:
- Carbon (C) has 4 valence electrons.
- Polonium (Po) belongs to Group 16 (like oxygen) and has 6 valence electrons. Since there are two Po atoms, their total contribution is 6 × 2 = 12 electrons.
- The total number of valence electrons is 4 + 12 = 16.
- Determine the Central Atom:
- Carbon is the least electronegative, so it is the central atom. The two polonium atoms will be terminal atoms.
- Connect Atoms with Single Bonds:
- Draw single bonds between C and each Po, using 2 electrons per bond. This initially uses up 4 electrons, leaving 12 electrons.
- Distribute Lone Pairs:
- Each polonium atom gets three lone pairs (6 electrons each) to satisfy the octet rule.
- Check Octets:
- Carbon only has 4 electrons (from two single bonds), which is not a full octet.
- To satisfy the octet rule for carbon, one lone pair from each Po must be shared to form double bonds with carbon.
- Final Structure:
- Carbon forms two double bonds with polonium (C=Po=C), and each polonium still retains two lone pairs.
Explanation
- Octet Rule: Carbon now has 8 electrons (two double bonds). Each polonium also has 8 electrons (two bonds + two lone pairs).
- Formal Charge Calculation:
- Carbon: (4 – (4/2) – 0 = 0)
- Polonium: (6 – (4/2) – 4 = 0)
- Since all atoms have formal charges of zero, this is the most stable structure.
Now, here’s the Lewis structure representation:
I’ll generate the image now.
Here is the Lewis structure of CPo₂ (carbon dipolonide) with lone pairs clearly shown. Let me know if you need any modifications or further explanation!