Chapter 3 - Exercises - Page 150d: 81

See the explanation

Here are the Lewis structures for the given molecules: a. $CCl_{4}$: The central atom is carbon (C), and it is surrounded by four chlorine (Cl) atoms. To obey the octet rule, the carbon atom needs to have 8 valence electrons around it. \[ \begin{array}{ccc} & \mathrm{Cl} & \\ & \mathrm{|} & \\ \mathrm{Cl} & -\mathrm{C}- & \mathrm{Cl} \\ & \mathrm{|} & \\ & \mathrm{Cl} & \end{array} \] In this structure, the carbon atom has 4 covalent bonds, each sharing 2 electrons, resulting in a total of 8 valence electrons around the carbon atom. b. $NCl_{3}$: The central atom is nitrogen (N), and it is surrounded by three chlorine (Cl) atoms. To obey the octet rule, the nitrogen atom needs to have 8 valence electrons around it. Lewis structure: \[ \begin{array}{ccc} \mathrm{Cl} & -\mathrm{N}- & \mathrm{Cl} \\ & \mathrm{|} & \\ & \mathrm{Cl} & \end{array} \] In this structure, the nitrogen atom has 3 covalent bonds, each sharing 2 electrons, resulting in a total of 6 valence electrons around the nitrogen atom. The remaining 2 valence electrons are in the form of a lone pair on the nitrogen atom. c. $SeCl_{2}$: The central atom is selenium (Se), and it is surrounded by two chlorine (Cl) atoms. To obey the octet rule, the selenium atom needs to have 8 valence electrons around it. Lewis structure: Cl-Se-Cl In this structure, the selenium atom has 2 covalent bonds, each sharing 2 electrons, resulting in a total of 4 valence electrons around the selenium atom. The remaining 4 valence electrons are in the form of two lone pairs on the selenium atom. d. ICl: The central atom is iodine (I), and it is surrounded by one chlorine (Cl) atom. To obey the octet rule, the iodine atom needs to have 8 valence electrons around it. Lewis structure: I-Cl In this structure, the iodine atom has 1 covalent bond, sharing 2 electrons, resulting in a total of 7 valence electrons around the iodine atom. The remaining 1 valence electron is in the form of a lone pair on the iodine atom.