Write Lewis structures that obey the octet rule for each of the following molecules. a. \(\mathrm{CCl}_{4}\) b. \(\mathrm{NCl}_{3}\) c. \(\operatorname{Sec} 1_{2}\) d. ICl In each case, the atom listed first is the central atom.

1. Determine the total number of valence electrons: Carbon has 4 valence electrons and each chlorine atom has 7. Since there are 4 chlorine atoms, the total number of valence electrons is 4 + (4 × 7) = 32. 2. Identify the central atom: Carbon is the central atom. 3. Connect the chlorine atoms to the central carbon atom with single bonds: C-Cl. We have used 8 valence electrons so far. 4. Complete the octets of chlorine atoms by adding lone pair electrons to each chlorine atom: Each Cl atom needs 6 more electrons (3 lone pairs) to complete the octet. Thus, the Lewis structure of \(\mathrm{CCl}_{4}\) becomes: Cl | Cl - C - Cl | Cl

1. Determine the total number of valence electrons: Nitrogen has 5 valence electrons and each chlorine atom has 7. Since there are 3 chlorine atoms, the total number of valence electrons is 5 + (3 × 7) = 26. 2. Identify the central atom: Nitrogen is the central atom. 3. Connect the chlorine atoms to the central nitrogen atom with single bonds: N-Cl. We have used 6 valence electrons so far. 4. Complete the octets of chlorine atoms and nitrogen atom by adding lone pair electrons: Each Cl atom needs 6 more electrons (3 lone pairs) to complete the octet. Nitrogen needs 2 more electrons (1 lone pair) to complete the octet. The Lewis structure of \(\mathrm{NCl}_{3}\) becomes: Cl | Cl - N - Cl :

1. Determine the total number of valence electrons: Selenium has 6 valence electrons and each oxygen atom has 6. Since there are 2 oxygen atoms, the total number of valence electrons is 6 + (2 × 6) = 18. 2. Identify the central atom: Selenium is the central atom. 3. Connect the oxygen atoms to the central selenium atom with single bonds: Se-O. We have used 4 valence electrons so far. 4. Complete the octets of oxygen atoms and selenium atom by adding lone pair electrons: Each O atom needs 6 more electrons (3 lone pairs) to complete the octet. Selenium needs 2 more electrons (1 lone pair) to complete the octet. The Lewis structure of \(SeO_{2}\) becomes: O : O - Se - O :

1. Determine the total number of valence electrons: Iodine has 7 valence electrons and chlorine has 7 valence electrons, for a total number of valence electrons of 7 + 7 = 14. 2. Identify the central atom: Iodine is the central atom. 3. Connect the chlorine atom to the central iodine atom with a single bond: I-Cl. We have used 2 valence electrons so far. 4. Complete the octets of iodine and chlorine atoms by adding lone pair electrons: Each atom needs 6 more electrons (3 lone pairs) to complete the octet. The Lewis structure of ICl becomes: I - Cl : : :