Answer
See the explanation
Work Step by Step
To draw the Lewis structure for the vile-smelling orange liquid with the formula S2Cl2, we need to follow these steps:
1. Determine the total number of valence electrons:
- Sulfur (S) has 6 valence electrons
- Chlorine (Cl) has 7 valence electrons
- Total valence electrons = 2 × 6 + 2 × 7 = 26
2. Arrange the atoms in the molecule:
- The central atoms are the sulfur atoms, and the chlorine atoms are bonded to them.
- The structure can be represented as Cl-S-S-Cl.
3. Draw the skeletal structure:
- The skeletal structure is Cl-S-S-Cl.
4. Determine the number of bonds:
- There are two single bonds between the sulfur atoms and the chlorine atoms.
- The total number of bonds is 2.
5. Distribute the remaining valence electrons:
- The total number of valence electrons is 26.
- The number of bonds is 2, which accounts for 4 electrons.
- The remaining 26 - 4 = 22 electrons are distributed as lone pairs on the atoms.
- Each sulfur atom has 3 lone pairs, and each chlorine atom has 3 lone pairs.
6. Verify the formal charges:
- The formal charge on each atom is zero, as the number of valence electrons is equal to the number of bonds plus the number of lone pairs.
The complete Lewis structure for the vile-smelling orange liquid with the formula S2Cl2 is:
Cl-S=S-Cl
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This structure satisfies the requirement of having a formal charge of zero on all elements in the compound.
