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Chapter 3: Problem 52

Indicate the oxidation state of \(S\) in \(\left(\text { a) } \mathrm{SO}_{3}^{2-}\right.\) (b) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-} ;\) (c) \(\mathrm{S}_{2} \mathrm{O}_{8}^{2-} ;\) (d) \(\mathrm{HSO}_{4}^{-} ;\) (e) \(\mathrm{S}_{4} \mathrm{O}_{6}^{2-}\)

Short Answer

Expert verified
The oxidation states of Sulfur (S) in the compounds are: (a) +4, (b) +2, (c) +7, (d) +6, (e) +2.

Step by step solution

01

Understand the rules for Oxidation States

First, it's necessary to know the rules of oxidation states. The oxidation state of a pure element is always zero. The oxidation state of a monoatomic ion is equal to the charge of that ion. Hydrogen usually has an oxidation state of +1 and Oxygen usually has an oxidation state of -2.
02

Calculate the oxidation state for SO3^2-

For SO3^2-, we know the oxidation state of Oxygen(O) is usually -2 and there are 3 of them, so the total oxidation state for O is -6. Since the overall charge of the molecule is -2, the oxidation state of S must be +4 to balance it.
03

Calculate the oxidation state for S2O3^2-

For S2O3^2-, the total oxidation state for 3 Oxygens is -6. To balance the compound with a charge of -2, the total oxidation state for 2 Sulfur atoms must be +4, so the oxidation state for one Sulfur is +2.
04

Calculate the oxidation state for S2O8^2-

For S2O8^2-, the total oxidation state for 8 Oxygens is -16. To balance the compound with a charge of -2, the total oxidation state for 2 Sulfur atoms should be +14, so the oxidation state for one Sulfur is +7.
05

Calculate the oxidation state for HSO4^-

In HSO4^-, the hydrogen and oxygen contribute +1 and -8 respectively to the total oxidation number due to their usual states. The total must equal -1 to balance the compound, which means the oxidation state of S is +6.
06

Calculate the oxidation state for S4O6^2-

In S4O6^2-, the total oxidation state for 6 Oxygens is -12. To balance the compound with a charge of -2, the total oxidation state for 4 Sulfur atoms is +10, so the oxidation state for one Sulfur is +2.

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Most popular questions from this chapter

What is the molecular formula of a hydrocarbon containing \(n\) carbon atoms and only one double bond? Can such a hydrocarbon yield a greater mass of \(\mathrm{H}_{2} \mathrm{O}\) than \(\mathrm{CO}_{2}\) when burned in an excess of oxygen?

Selenium, an element used in the manufacture of photoelectric cells and solar energy devices, forms two oxides. One has \(28.8 \%\) O, by mass, and the other, 37.8\% O. What are the formulas of these oxides? Propose acceptable names for them.

The formula for calcium chlorite is (a) \(\mathrm{CaClO}_{2}\) (b) \(\mathrm{Ca}\left(\mathrm{ClO}_{2}\right)_{2} ;(\mathrm{c}) \mathrm{CaClO}_{3} ;(\mathrm{d}) \mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}\)

Write formulas for the compounds: (a) magnesium perchlorate; (b) lead(II) acetate; (c) tin(IV) oxide; (d) hydroiodic acid; (e) chlorous acid; (f) sodium hydrogen sulfite; (g) calcium dihydrogen phosphate; (h) aluminum phosphate; (i) dinitrogen tetroxide; (j) disulfur dichloride.

Para-cresol ( \(p\) -cresol) is used as a disinfectant and in the manufacture of herbicides. A 0.4039 g sample of this carbon-hydrogen-oxygen compound yields \(1.1518 \mathrm{g} \mathrm{CO}_{2}\) and \(0.2694 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\) in combustion analysis. Its molecular mass is 108.1 u. For \(p\) -cresol, determine its (a) mass percent composition; (b) empirical formula; (c) molecular formula.
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