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Chapter 4: Problem 50

Determine the oxidation number for the indicated element in each of the following substances: (a) \(\mathrm{N}\) in \(\mathrm{N}_{2} \mathrm{H}_{4}\), (b) \(\mathrm{Nin} \mathrm{NO}_{2}\), (c) \(\mathrm{Mn}\) in \(\mathrm{MnCl}_{3}\) (d) Fe in \(\mathrm{FeSO}_{4^{\prime}}\) (e) \(\mathrm{Pt}\) in \(\mathrm{PtCl}_{4}\) (f) \(\mathrm{Cl}\) in \(\mathrm{NaClO}_{4}\).

Short Answer

Expert verified
The oxidation numbers for the indicated elements in the following substances are: (a) N in \(\mathrm{N}_{2} \mathrm{H}_{4}\) is -2, (b) N in \(\mathrm{NO}_{2}\) is +4, (c) Mn in \(\mathrm{MnCl}_{3}\) is +3, (d) Fe in \(\mathrm{FeSO}_{4}\) is +2, (e) Pt in \(\mathrm{PtCl}_{4}\) is +4, and (f) Cl in \(\mathrm{NaClO}_{4}\) is +7.

Step by step solution

01

Use rule 2 and the known oxidation numbers of hydrogen

Since hydrogen typically has an oxidation number of +1, and there are four hydrogen atoms in the compound, the sum of the oxidation numbers for hydrogen is +4. Since the compound is neutral, the sum of the oxidation numbers for nitrogen must be -4. There are two nitrogen atoms, so the oxidation number of each nitrogen atom is -2. (b) Determine the oxidation number of N in \(\mathrm{NO}_{2}\)
02

Use rule 2 and the known oxidation numbers of oxygen

Oxygen typically has an oxidation number of -2, and there are two oxygen atoms in the compound, so the sum of the oxidation numbers for oxygen is -4. Since the compound is neutral, the oxidation number of nitrogen must be +4. (c) Determine the oxidation number of Mn in \(\mathrm{MnCl}_{3}\)
03

Use rule 2 and the known oxidation numbers of chlorine

Chlorine typically has an oxidation number of -1, and there are three chlorine atoms in the compound, so the sum of the oxidation numbers for chlorine is -3. Since the compound is neutral, the oxidation number of manganese must be +3. (d) Determine the oxidation number of Fe in \(\mathrm{FeSO}_{4}\)
04

Use rule 3 and the known oxidation numbers of oxygen, sulfur, and the charge of the polyatomic ion

First, note that sulfate ion, \(SO_{4}^{2-}\), is a polyatomic ion with a charge of -2. The oxidation number of oxygen is -2, and there are four of them, contributing an oxidation number of -8. In the sulfate ion, the oxidation number of sulfur must be +6 to make the sum of the oxidation numbers equal to -2. Now, use the neutral compound rule (rule 2) for \(\mathrm{FeSO}_{4}\). The oxidation numbers of all other elements sum to -2, so the oxidation number of iron must be +2. (e) Determine the oxidation number of Pt in \(\mathrm{PtCl}_{4}\)
05

Use rule 2 and the known oxidation numbers of chlorine

Chlorine typically has an oxidation number of -1, and there are four chlorine atoms in the compound, so the sum of the oxidation numbers for chlorine is -4. Since the compound is neutral, the oxidation number of platinum must be +4. (f) Determine the oxidation number of Cl in \(\mathrm{NaClO}_{4}\)
06

Use rule 2 and the known oxidation numbers of sodium, oxygen, and the charge of the polyatomic ion

Sodium, an alkali metal, has an oxidation number of +1. There is an oxygen atom bonded to a more electronegative chlorine atom in the \(\mathrm{ClO}_{4}\) ion, so the oxidation number of oxygen is still -2. The compound is neutral, and the sum of the oxidation numbers for sodium, oxygen, and the other chlorine atoms in the perchlorate ion is -7, so the oxidation number of the central chlorine atom must be +7.

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Most popular questions from this chapter

The labels have fallen off three bottles containing powdered samples of metals; one contains zinc, one lead, and the other platinum. You have three solutions at your disposal: \(1 \mathrm{M}\) sodium nitrate, \(1 \mathrm{M}\) nitric acid, and \(1 \mathrm{M}\) nickel nitrate. How could you use these solutions to determine the identities of each metal powder? [Section 4.4]

Ritalin is the trade name of a drug, methylphenidate, used to treat attention- deficit/hyperactivity disorder in young adults. The chemical structure of methylphenidate is (a) Is Ritalin an acid or a base? An electrolyte or a nonelectrolyte? (b) A tablet contains a \(10.0-\mathrm{mg}\) dose of Ritalin. Assuming all the drug ends up in the bloodstream, and the average man has a total blood volume of \(5.0 \mathrm{~L}\), calculate the initial molarity of Ritalin in a man's bloodstream. (c) Ritalin has a half-life of 3 hours in the blood, which means that after 3 hours the concentration in the blood has decreased by half of its initial value. For the man in part (b), what is the concentration of Ritalin in his blood after 6 hours?

State whether each of the following statements is true or false. Justify your answer in each case. (a) When acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3}\), is dissolved in water, a conducting solution results. (b) When ammonium nitrate, \(\mathrm{NH}_{4} \mathrm{NO}_{3}\), dissolves in water, the solution is weakly conducting and basic in nature.

State whether each of the following statements is true or false. Justify your answer in each case. (a) \(\mathrm{NH}_{3}\) contains no \(\mathrm{OH}^{-}\) ions, and yet its aqueous solutions are basic. (b) HF is a strong acid. (c) Although sulfuric acid is a strong electrolyte, an aqueous solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) contains more \(\mathrm{HSO}_{4}^{-}\) ions than \(\mathrm{SO}_{4}^{2-}\) ions.

A solid sample of \(\mathrm{Fe}(\mathrm{OH})_{3}\) is added to $0.500 \mathrm{~L}\( of \)0.250 \mathrm{M}\( aqueous \)\mathrm{H}_{2} \mathrm{SO}_{4}$. The solution that remains is still acidic. It is then titrated with $0.500 \mathrm{M} \mathrm{NaOH}\( solution, and it takes \)12.5 \mathrm{~mL}$ of the \(\mathrm{NaOH}\) solution to reach the equivalence point. What mass of \(\mathrm{Fe}(\mathrm{OH})_{3}\) was added to the $\mathrm{H}_{2} \mathrm{SO}_{4}$ solution?
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