Draw the Lewis structures for each of the following ions or molecules. Identify those in which the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state, for those atoms, how many electrons surround them: $(\mathbf{a}) \mathrm{HCl},(\mathbf{b}) \mathrm{ICl}_{5},\( (c) \)\mathrm{NO}\( (d) \)\mathrm{CF}_{2} \mathrm{Cl}_{2},(\mathbf{e}) \mathrm{I}_{3}^{-}$

The Lewis structures for the given ions/molecules are as follows: a) HCl: H - Cl, obeys octet rule. b) ICl5: Cl | I - Cl - I - Cl | Cl Iodine does not obey octet rule with 12 surrounding electrons. c) NO: N = O (single electron on Nitrogen) Neither Nitrogen nor Oxygen follow the octet rule, with Nitrogen having 7 surrounding electrons and Oxygen having 9 surrounding electrons. d) CF2Cl2: Cl - C - Cl | F | F All atoms obey the octet rule. e) I3-: I | I - I (2 lone pairs on each terminal Iodine) The central Iodine atom does not obey the octet rule, with 10 surrounding electrons.