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Chapter 4: Problem 45

Give oxidation numbers for the underlined atoms in the following molecules and ions: (a) \(\underline{\mathrm{Cs}_{2} \mathrm{O}},\) (b) \(\mathrm{Ca} \underline{\mathrm{I}}_{2}\), (c) \(\underline{\mathrm{Al}_{2} \mathrm{O}_{3}}\) (d) \(\mathrm{H}_{3} \mathrm{As} \mathrm{O}_{3},\) (e) \(\underline{\mathrm{Ti} \mathrm{O}_{2}},\) (f) \(\underline{\mathrm{Mo}} \mathrm{O}_{4}^{2-}\), (g) \(\underline{\mathrm{Pt} \mathrm{Cl}_{4}^{2-}}\) (h) \(\underline{\mathrm{Pt}} \mathrm{Cl}_{6}^{2-}\) (i) \(\underline{\operatorname{Sn} F}_{2}\) (j) \(\underline{\mathrm{ClF}_{3},}\) (k) \(\underline{\mathrm{Sb}} \mathrm{F}_{6}^{-}\)

Short Answer

Expert verified
(a) +1, (b) -1, (c) +3, (d) +5, (e) +4, (f) +6, (g) +2, (h) +4, (i) +2, (j) +3, (k) +5

Step by step solution

01

Recall the rules of assigning oxidation numbers

The key rules to remember are: 1) The oxidation number of an atom in an element is zero. 2) The oxidation number of an atom in a monatomic ion is the charge of that ion. 3) Hydrogen is +1 when combined with nonmetals and -1 when combined with metals. 4) Oxygen is typically -2. 5) Fluorine is always -1. 6) For other halogens (Cl, Br, I), they are -1 when they are the most electronegative element in a compound, and positive when they are with oxygen or group 1 & 2 elements. 7) The sum of oxidation states in a compound is zero, while in an ion it is equal to the charge of the ion.
02

Assign oxidation numbers

(a) Cs in Cs₂O: As a group 1 element, Cs is +1. (b) I in CaI₂: Group 2 elements like Ca always exhibit +2, therefore I is -1. (c) Al in Al₂O₃: With oxygen as -2, Al is +3. (d) As in H₃AsO₃: With H as +1 and O as -2, As is +5. (e) Ti in TiO₂: Oxygen is -2, so Ti is +4. (f) Mo in MoO₄²⁻: Oxygen is -2, so Mo is +6. (g) Pt in PtCl₄²⁻: Chlorine is -1, so Pt is +2. (h) Pt in PtCl₆²⁻: Chlorine is -1, so Pt is +4. (i) Sn in SnF₂: Fluorine is -1, so Sn is +2. (j) Cl in ClF₃: Fluorine is -1, so Cl is +3. (k) Sb in SbF₆⁻: Fluorine is -1, so Sb is +5.

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