Name the following compounds and assign oxidation states to the halogens in them: (a) \(\mathrm{Co}\left(1 \mathrm{O}_{3}\right)_{3},\) (b) \(\mathrm{Ca}\left(1 \mathrm{O}_{4}\right)_{2}\), (c) \(\mathrm{PF}_{6}^{-},(\mathbf{d}) \mathrm{ICl}_{4}^{-}\), (e) \(\mathrm{HBrO},\) (f) AtH.

(a) \(\mathrm{Co}\left(1 \mathrm{O}_{3}\right)_{3}\): This compound contains Cobalt (Co) and the polyatomic ion IO₃⁻ which is Iodate. So, the name of the compound is Cobalt(III) Iodate. (b) \(\mathrm{Ca}\left(1 \mathrm{O}_{4}\right)_{2}\): This compound contains Calcium (Ca) and the polyatomic ion IO₄⁻ which is Periodate. So, the name of the compound is Calcium Periodate. (c) \(\mathrm{PF}_{6}^{-}\): This compound contains Phosphorus (P) and Fluorine (F) with a -1 charge. The name of this compound is Hexafluorophosphate ion. (d) \(\mathrm{ICl}_{4}^{-}\): This compound contains Iodine (I) and Chlorine (Cl) with a -1 charge. The name of this compound is Tetrachloroiodate ion. (e) \(\mathrm{HBrO}\): This compound contains Hydrogen (H), Bromine (Br), and Oxygen (O). The name of this compound is Hypobromous acid. (f) AtH: This compound contains Hydrogen (H) and Astatine (At). The name of this compound is Astatine Hydride.

(a) \(\mathrm{Co}\left(1 \mathrm{O}_{3}\right)_{3}\): Here, the halogen is Iodine (I). To determine its oxidation state, we use some of the rules for oxidation states: 1. The sum of the oxidation states in a neutral compound is 0. 2. The oxidation state of oxygen in most compounds is -2. IO₃⁻ oxidation states: I + 3(-2) = -1 I = +5, so the oxidation state of Iodine in this compound is +5. (b) \(\mathrm{Ca}\left(1 \mathrm{O}_{4}\right)_{2}\): In this compound, the halogen is again Iodine (I). IO₄⁻ oxidation states: I + 4(-2) = -1 I = +7, so the oxidation state of Iodine in this compound is +7. (c) \(\mathrm{PF}_{6}^{-}\): In this compound, the halogen is Fluorine (F). PF₆⁻ oxidation states: P + 6(F) = -1 Since the oxidation state of F in compounds is always -1: P + 6(-1) = -1 P = +5, thus the oxidation state of Fluorine in this compound is -1. (d) \(\mathrm{ICl}_{4}^{-}\): Here, the halogens are Iodine (I) and Chlorine (Cl). ICl₄⁻ oxidation states: I + 4(Cl) = -1 Since the oxidation state of Cl in compounds is usually -1: I + 4(-1) = -1 I = +3, so the oxidation state of Iodine in this compound is +3, and the oxidation state of Chlorine is -1. (e) \(\mathrm{HBrO}\): In this compound, the halogen is Bromine (Br). HBrO oxidation states: H + Br + O = 0 Using standard oxidation states for H (+1) and O (-2), +1 + Br - 2 = 0 Br = +1, thus the oxidation state of Bromine in this compound is +1. (f) AtH: In this compound, the halogen is Astatine (At). AtH oxidation states: At + H = 0 Using standard oxidation states for H (+1), At + 1 = 0 At = -1, so the oxidation state of Astatine in this compound is -1.