Write the Lewis structures for the following molecules and polyatomic ions. In each case, the first atom is the central atom. (a) \(\mathrm{CCl}_{4}\) (b) \(\mathrm{NCl}_{3}\) (c) \(\mathrm{COCl}_{2}\) (d) \(\mathrm{SO}_{3}^{2-}\)

1. Determine the valence electrons: Carbon (C) has 4 valence electrons and Chlorine (Cl) has 7 valence electrons. Since there are 4 Cl atoms, the total valence electrons are \(4+4\times 7=32\). 2. Arrange the atoms: Place the Carbon atom in the center and surround it with the 4 Chlorine atoms. 3. Distribute the electrons: Assign 2 electrons to each of the C-Cl bonds (8 electrons). Assign the remaining 24 electrons to the Chlorine atoms, with each Cl atom getting 6 more electrons to complete its octet. 4. Stability check: Carbon has 8 electrons in its outer shell and each Chlorine atom has 8 electrons in its outer shell. The Lewis structure for \(\mathrm{CCl}_{4}\) is stable.

1. Determine the valence electrons: Nitrogen (N) has 5 valence electrons and Chlorine (Cl) has 7 valence electrons. Since there are 3 Cl atoms, the total valence electrons are \(5+3\times 7=26\). 2. Arrange the atoms: Place the Nitrogen atom in the center and surround it with the 3 Chlorine atoms. 3. Distribute the electrons: Assign 2 electrons to each of the N-Cl bonds (6 electrons). Assign the remaining 20 electrons to the Chlorine atoms, with each Cl atom getting 6 more electrons to complete its octet. 4. Stability check: Nitrogen has 8 electrons in its outer shell and each Chlorine atom has 8 electrons in its outer shell. The Lewis structure for \(\mathrm{NCl}_{3}\) is stable.

1. Determine the valence electrons: Carbon (C) has 4 valence electrons, Oxygen (O) has 6 valence electrons, and Chlorine (Cl) has 7 valence electrons. Since there are 2 Cl atoms, the total valence electrons are \(4+6+2\times 7=24\). 2. Arrange the atoms: Place the Carbon atom in the center, with Oxygen on one side and the two Chlorine atoms on the other side. 3. Distribute the electrons: Assign 2 electrons to each of the C-O and C-Cl bonds (8 electrons). Assign the remaining 16 electrons to the Oxygen and Chlorine atoms, with Oxygen getting 4 more electrons and each Cl atom getting 6 more electrons to complete their octet. 4. Stability check: Carbon has 8 electrons in its outer shell, Oxygen has 8 electrons, and each Chlorine atom has 8 electrons. The Lewis structure for \(\mathrm{COCl}_{2}\) is stable.

1. Determine the valence electrons: Sulfur (S) has 6 valence electrons and Oxygen (O) has 6 valence electrons. Since there are 3 O atoms and there is a 2- charge, the total valence electrons are \(6+3\times 6+2=26\). 2. Arrange the atoms: Place the Sulfur atom in the center and surround it with the 3 Oxygen atoms. 3. Distribute the electrons: Assign 2 electrons to each of the S-O bonds (6 electrons). Assign the remaining 20 electrons to the Oxygen atoms, with each O atom getting 6 more electrons to complete its octet. 4. Stability check: Sulfur has 8 electrons in its outer shell and each Oxygen atom has 8 electrons in its outer shell. The Lewis structure for \(\mathrm{SO}_{3}^{2-}\) is stable.