The Lewis structure for the molecule SiSO has Si as the central atom and contains explain it.
A. two double bonds.
B. two triple bonds.
C. two single bonds.
D. one double bond and one triple bond.
The correct answer and explanation is :
The correct answer is:
D. One double bond and one triple bond.
Explanation:
The Lewis structure of SiSO (Silicon Oxysulfide) consists of Silicon (Si) as the central atom, with Sulfur (S) and Oxygen (O) bonded to it. To determine the correct bonding, we follow these steps:
- Determine the total number of valence electrons:
- Silicon (Si) has 4 valence electrons.
- Sulfur (S) has 6 valence electrons.
- Oxygen (O) has 6 valence electrons.
- Total valence electrons = 4 + 6 + 6 = 16 electrons.
- Assign the central atom:
- Silicon (Si) is the least electronegative element, so it is placed at the center.
- Form bonds to satisfy the octet rule:
- Silicon forms a double bond with sulfur (S) and a triple bond with oxygen (O).
- This configuration allows all atoms to fulfill the octet rule while minimizing formal charges.
- Verify formal charges:
- The formal charge calculations confirm that this structure is the most stable representation of SiSO.
Bonding in SiSO:
- Si = O (Silicon-Oxygen) → Triple bond
- Si = S (Silicon-Sulfur) → Double bond
Thus, the correct Lewis structure contains one double bond (Si=S) and one triple bond (Si≡O), making the correct answer (D).
Lewis Structure Image:
Here’s a visual representation of the SiSO Lewis structure:
Si=S=O
Here is the Lewis structure diagram of the SiSO molecule, showing the correct bonding: one double bond (Si=S) and one triple bond (Si≡O).