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Chapter 4: Problem 85

Assign oxidation states for all atoms in each of the following compounds a. \({KMnO}_{4} \quad\quad\quad f. {Fe}_{3} {O}_{4}\) b. \({NiO}_{2} \quad\quad\quad\quad g. {XeOF}_{4}\) c. \({Na}_{4} {Fe}({OH})_{6} \quad h. {SF}_{4}\) d. \({NH}_{4} {h}_{2} {HPO}_{4} \quad i. {CO}\) e. \({P}_{4} {O}_{6} \quad\quad\quad\quad\quad j. {C}_{6} {H}_{12} {O}_{6}\)

Short Answer

Expert verified
The oxidation states for the given compounds are: a. K(+1), Mn(+7), O(-2) b. Ni(+4), O(-2) c. Na(+1), Fe(+2), O(-2), H(+1) d. N(-3), H(+1), P(+5) e. P(+3), O(-2) f. Fe(+2, +3), O(-2) g. Xe(+6), O(-2), F(-1) h. S(+4), F(-1) i. C(+2), O(-2) j. C(0), H(+1), O(-2)

Step by step solution

01

Assign oxidation states for K, Mn, and O

Assign +1 for K, -2 for O. The sum of the oxidation states must be zero since it's a neutral compound. \(+1 + x + 4(-2) = 0\) \(x = +7\) So, the oxidation states are K(+1), Mn(+7), and O(-2). b. NiO2
02

Assign oxidation states for Ni and O

Assign -2 for O. The sum of oxidation states must be zero since it's a neutral compound. \(x + 2(-2) = 0\) \(x = +4\) So, the oxidation states are Ni(+4) and O(-2). c. Na4Fe(OH)6
03

Assign oxidation states for Na, Fe, O, and H

Assign +1 for Na, -2 for O, and +1 for H. The sum of oxidation states must be zero since it's a neutral compound. \(4(+1) + x + 6(-2) + 6(+1) = 0\) \(x = +2\) So, the oxidation states are Na(+1), Fe(+2), O(-2), and H(+1). d. NH4H2HPO4
04

Assign oxidation states for N, H, and P

Assign +1 for H (both in NH4 and H2). Assign -2 for O. The sum of oxidation states must be zero since it's a neutral compound. \(+1 + 4(+1) + 2(+1) + x + 4(-2) = 0\) \(x = +5\) So, the oxidation states are N(-3), H(+1), and P(+5). e. P4O6
05

Assign oxidation states for P and O

Assign -2 for O. The sum of oxidation states must be zero. \(4x + 6(-2) = 0\) \(x = +3\) So, the oxidation states are P(+3) and O(-2). f. Fe3O4
06

Assign oxidation states for Fe and O

Assign -2 for O. We know iron can have oxidation states of +2 or +3, and the sum of oxidation states must be zero. \(3x + 4(-2) = 0\) It becomes clear that there are two Fe(+3) and one Fe(+2). So, the oxidation states are Fe(+2, +3) and O(-2). g. XeOF4
07

Assign oxidation states for Xe, O, and F

Assign -2 for O and -1 for F. The sum of oxidation states must be zero. \(x - 2 + 4(-1) = 0\) \(x = +6\) So, the oxidation states are Xe(+6), O(-2), and F(-1). h. SF4
08

Assign oxidation states for S and F

Assign -1 for F. The sum of oxidation states must be zero. \(x + 4(-1) = 0\) \(x = +4\) So, the oxidation states are S(+4) and F(-1). i. CO
09

Assign oxidation states for C and O

Assign -2 for O. The sum of oxidation states must be zero. \(x + (-2) = 0\) \(x = +2\) So, the oxidation states are C(+2) and O(-2). j. C6H12O6
10

Assign oxidation states for C, H, and O

Assign -2 for O and +1 for H. In most organic compounds, carbon has an oxidation state of -4, 0, or +4. Each carbon atom \(x = \frac{12(+1) + 6(-2)}{6}\); thus, the oxidation state of carbon is 0. So, the oxidation states are C(0), H(+1), and O(-2).

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Most popular questions from this chapter

A \(10.00-\mathrm{mL}\) . sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right),\) is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH},\) and 16.58 mL is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{g} / \mathrm{cm}^{3},\) what is the mass percent of acetic acid in the vinegar?

One of the classic methods for determining the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas. This solution is then reacted with an acidic solution containing the periodate ion; the products are the permanganate and iodate ions. Write balanced chemical equations for both of these steps.

The thallium (present as \(\mathrm{Tl}_{2} \mathrm{SO}_{4} )\) in a \(9.486-\mathrm{g}\) pesticide sam- ple was precipitated as thallium(I) iodide. Calculate the mass percent of \(\mathrm{TI}_{2} \mathrm{SO}_{4}\) in the sample if 0.1824 \(\mathrm{g}\) of TIII was recovered.

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