Question 1 Which of the following is the correct Lewis Dot Structure for \( \mathrm{SCl}_{4} \) ? ..

To determine the correct Lewis Dot Structure for \( \mathrm{SCl}_{4} \), we need to follow these steps: 1. **Count the total valence electrons**: - Sulfur (S) has 6 valence electrons. - Each chlorine (Cl) has 7 valence electrons, and there are 4 chlorine atoms. - Total valence electrons = \( 6 + (4 \times 7) = 6 + 28 = 34 \) electrons. 2. **Determine the central atom**: - Sulfur is less electronegative than chlorine, so it will be the central atom. 3. **Arrange the atoms**: - Place sulfur in the center and surround it with the four chlorine atoms. 4. **Form bonds**: - Connect each chlorine atom to the sulfur atom with a single bond. This uses 8 electrons (4 bonds). 5. **Distribute remaining electrons**: - After forming the bonds, we have \( 34 - 8 = 26 \) electrons left. - Each chlorine atom needs 6 more electrons to complete its octet (3 lone pairs), which uses \( 4 \times 6 = 24 \) electrons. - This leaves us with \( 26 - 24 = 2 \) electrons. 6. **Place remaining electrons on the central atom**: - The 2 remaining electrons will be placed as a lone pair on the sulfur atom. 7. **Check the octet rule**: - Each chlorine has 8 electrons (6 from lone pairs and 2 from the bond with sulfur). - Sulfur has 8 electrons (4 from the bonds with chlorine and 2 from the lone pair). The final Lewis structure for \( \mathrm{SCl}_{4} \) will have sulfur in the center with four single bonds to chlorine atoms and one lone pair on sulfur. If you have options to choose from, look for the structure that matches this description. If you need a visual representation, it would look something like this: ``` Cl | Cl - S - Cl | Cl ``` With a lone pair of dots on the sulfur atom.