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Chapter 22: Problem 32

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) chlorate ion, (b) hydroiodic acid, (c) iodine trichloride, (d) sodium hypochlorite, (e) perchloric acid, (f) xenon tetrafluoride.

Short Answer

Expert verified
(a) The chlorate ion has the formula \(ClO_3^-\) and chlorine's oxidation state is +5. (b) Hydroiodic acid has the formula HI and iodine's oxidation state is -1. (c) Iodine trichloride has the formula ICl3 and iodine's oxidation state is +3. (d) Sodium hypochlorite has the formula NaClO and chlorine's oxidation state is +1. (e) Perchloric acid has the formula HClO4 and chlorine's oxidation state is +7. (f) Xenon tetrafluoride has the formula XeF4 and xenon's oxidation state is +4.

Step by step solution

01

(a) Chlorate ion

The chlorate ion consists of one chlorine atom and three oxygen atoms, with an overall negative charge. Its chemical formula is \(ClO_3^-\). To find the oxidation state of chlorine, we use the fact that the sum of oxidation states in a compound must equal its overall charge, which is -1 in this case. Since oxygen has an oxidation state of -2, we get the following equation: 1 * (oxidation state of Cl) + 3 * (-2) = -1 Solving for the oxidation state of chlorine: Oxidation state of Cl = +5 The chlorate ion has the formula \(ClO_3^-\) and chlorine's oxidation state is +5.
02

(b) Hydroiodic acid

Hydroiodic acid is a binary acid containing hydrogen and iodine. Its chemical formula is HI. In this case, the hydrogen atom has an oxidation state of +1. So, the oxidation state of iodine is -1. Hydroiodic acid has the formula HI and iodine's oxidation state is -1.
03

(c) Iodine trichloride

Iodine trichloride consists of one iodine atom and three chlorine atoms. Its chemical formula is ICl3. The oxidation state of chlorine is -1. Therefore, the oxidation state of iodine is +3 to balance the overall charge of the compound: 1 * (oxidation state of I) + 3 * (-1) = 0 Iodine trichloride has the formula ICl3 and iodine's oxidation state is +3.
04

(d) Sodium hypochlorite

Sodium hypochlorite is a compound consisting of sodium, oxygen, and chlorine. Its chemical formula is NaClO. The oxidation state of sodium is +1 and oxygen is -2. To balance the overall charge of the compound, the oxidation state of chlorine is: 1 * +1 + 1 * (oxidation state of Cl) + 1 * (-2) = 0 Oxidation state of Cl = +1 Sodium hypochlorite has the formula NaClO and chlorine's oxidation state is +1.
05

(e) Perchloric acid

Perchloric acid is an oxyacid with chlorine and four oxygen atoms. Its chemical formula is HClO4. The oxidation state of hydrogen is +1, and oxygen is -2. To balance the overall charge of the compound, the oxidation state of chlorine is: 1 * +1 + 1 * (oxidation state of Cl) + 4 * (-2) = 0 Oxidation state of Cl = +7 Perchloric acid has the formula HClO4 and chlorine's oxidation state is +7.
06

(f) Xenon tetrafluoride

Xenon tetrafluoride consists of one xenon atom and four fluorine atoms. Its chemical formula is XeF4. The oxidation state of fluorine is -1. To balance the overall charge of the compound, the oxidation state of xenon is: 1 * (oxidation state of Xe) + 4 * (-1) = 0 Oxidation state of Xe = +4 Xenon tetrafluoride has the formula XeF4 and xenon's oxidation state is +4.

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Most popular questions from this chapter

Give the chemical formula for (a) hydrocyanic acid, (b) nickel tetracarbonyl, (c) barium bicarbonate, (d) calcium acetylide, (e) potassium carbonate.

The solubility of \(\mathrm{Cl}_{2}\) in 100 \(\mathrm{g}\) of water at STP is 310 \(\mathrm{cm}^{3}\) . Assume that this quantity of \(\mathrm{Cl}_{2}\) is dissolved and equilibrated as follows: $$\mathrm{Cl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Cl}^{-}(a q)+\mathrm{HClO}(a q)+\mathrm{H}^{+}(a q)$$ (a) If the equilibrium constant for this reaction is \(4.7 \times 10^{-4}\) , calculate the equilibrium concentration of HClO formed. (b) What is the pH of the final solution?

Write a balanced equation for the reaction of each of the following compounds with water: (a) \(\mathrm{SO}_{2}(g),(\mathbf{b}) \mathrm{Cl}_{2} \mathrm{O}_{7}(g)\) (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s),\) (d) \(\mathrm{BaC}_{2}(s),\) (e) \(\mathrm{RbO}_{2}(s)\) (f) \(\mathrm{Mg}_{3} \mathrm{N}_{2}(s)\) , (g) \(\mathrm{NaH}(s) .\)

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to GeCl_ by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; GeCl_ is then hydrolyzed in water to GeO \(_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\) . The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from GeO \(_{2} .\)

Select the member of group 4 \(\mathrm{A}\) that best fits each description: (a) forms chains to the greatest extent, (b) forms the most basic oxide, ( \(\mathbf{c} )\) is a metalloid that can form \(2+\) ions.
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