Write Lewis structures that obey the octet rule for each of the following molecules. a. \(\mathrm{CCl}_{4}\) c. \(\mathrm{SeCl}_{2}\) b. \(\mathrm{NCl}_{3}\) d. ICl In each case, the atom listed first is the central atom.

: 1. Identify the central atom and count the total valence electrons. Carbon (C) is the central atom, and there are four Chlorine (Cl) atoms around it. Total valence electrons: Carbon (4) + 4 * Chlorine (7) = 4 + 28 = 32. 2. Place the central atom (C) in the center and arrange the surrounding atoms (Cl) around it. 3. Start by forming a single bond between the central atom and each surrounding atom. This uses up 8 electrons (4 pairs). 4. Distribute the remaining electrons (32 - 8 = 24) to the surrounding atoms (Cl) as lone pairs to complete their octet. 5. Check that the octet rule is obeyed for each atom, including the central atom, Carbon. The Lewis structure for CCl4 is drawn as: Cl | Cl-C-Cl | Cl

: 1. Identify the central atom and count the total valence electrons. Selenium (Se) is the central atom, and there are two Chlorine (Cl) atoms around it. Total valence electrons: Selenium (6) + 2 * Chlorine (7) = 6 + 14 = 20. 2. Place the central atom (Se) in the center and arrange the surrounding atoms (Cl) around it. 3. Start by forming a single bond between the central atom and each surrounding atom. This uses up 4 electrons (2 pairs). 4. Distribute the remaining electrons (20 - 4 = 16) to the surrounding atoms (Cl) as lone pairs to complete their octet and add the rest as lone pairs on the central atom (Se). 5. Check that the octet rule is obeyed for each atom, including the central atom, Selenium. The Lewis structure for SeCl2 is drawn as: Cl-Se-Cl ||

: 1. Identify the central atom and count the total valence electrons. Nitrogen (N) is the central atom, and there are three Chlorine (Cl) atoms around it. Total valence electrons: Nitrogen (5) + 3 * Chlorine (7) = 5 + 21 = 26. 2. Place the central atom (N) in the center and arrange the surrounding atoms (Cl) around it. 3. Start by forming a single bond between the central atom and each surrounding atom. This uses up 6 electrons (3 pairs). 4. Distribute the remaining electrons (26 - 6 = 20) to the surrounding atoms (Cl) as lone pairs to complete their octet. 5. Check that the octet rule is obeyed for each atom, including the central atom, Nitrogen. The Lewis structure for NCl3 is drawn as: Cl | Cl-N-Cl

: 1. Identify the central atom and count the total valence electrons. Iodine (I) is the central atom, and there is one Chlorine (Cl) atom around it. Total valence electrons: Iodine (7) + Chlorine (7) = 14. 2. Place the central atom (I) in the center and arrange the surrounding atom (Cl) around it. 3. Start by forming a single bond between the central atom and the surrounding atom. This uses up 2 electrons (1 pair). 4. Distribute the remaining electrons (14 - 2 = 12) to the surrounding atoms (Cl and I) as lone pairs to complete their octet. 5. Check that the octet rule is obeyed for each atom, including the central atom, Iodine. The Lewis structure for ICl is drawn as: I-Cl ||