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Chapter 22: Problem 33

Name the following compounds and assign oxidation states to the halogens in them: (a) \(\mathrm{Fe}\left(\mathrm{ClO}_{3}\right)_{3},(\mathbf{b}) \mathrm{HClO}_{2}\) (c) \(\mathrm{XeF}_{6},(\mathbf{d}) \mathrm{BrF}_{5},(\mathbf{e}) \mathrm{XeOF}_{4},(\mathbf{f}) \mathrm{HIO}_{3}\)

Short Answer

Expert verified
The names of the compounds and the oxidation states of the halogens are as follows: a) Iron(III) chlorate, Cl oxidation state: +5 b) Chlorous acid, Cl oxidation state: +3 c) Xenon hexafluoride, F oxidation state: -1 d) Bromine pentafluoride, F oxidation state: -1 e) Xenon oxytetrafluoride, F oxidation state: -1 f) Iodic acid, I oxidation state: +5

Step by step solution

01

a) Naming Fe(ClO3)3 and finding the oxidation state of Cl

The compound \(\mathrm{Fe}\left(\mathrm{ClO}_{3}\right)_{3}\) is an ionic compound consisting of an iron(III) cation (Fe) and chlorate anions (ClO3). The name of this compound is iron(III) chlorate. To find the oxidation state of chlorine in this compound, we can use the rule that the sum of the oxidation states of all the atoms in the compound must be zero. Since oxygen has an oxidation state of -2 and iron has an oxidation state of +3, the equation for the sum of the oxidation states is: \( +3 + 3x + 9(-2) = 0 \) Solving for x, which is the oxidation state of Cl, we get \( x= +5 \) So, the oxidation state of chlorine in \(\mathrm{Fe}\left(\mathrm{ClO}_{3}\right)_{3}\) is +5.
02

b) Naming HClO2 and finding the oxidation state of Cl

The compound \(\mathrm{HClO}_{2}\) is a molecular compound consisting of hydrogen, chlorine, and oxygen. It is called chlorous acid. To find the oxidation state of Cl in this compound, we use the rule that the sum of the oxidation states of all the atoms in the compound must be zero. Hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. The equation for the sum of the oxidation states is: \( +1 + x + 2(-2) = 0 \) Solving for x, we get \( x= +3 \) So, the oxidation state of chlorine in \(\mathrm{HClO}_{2}\) is +3.
03

c) Naming XeF6 and finding the oxidation state of F

The compound \(\mathrm{XeF}_{6}\) is a molecular compound consisting of xenon and fluorine. It is called xenon hexafluoride. The oxidation state of F in any compound is always -1. Therefore, the oxidation state of F in \(\mathrm{XeF}_{6}\) is -1.
04

d) Naming BrF5 and finding the oxidation state of F

The compound \(\mathrm{BrF}_{5}\) is a molecular compound consisting of bromine and fluorine. It is called bromine pentafluoride. As mentioned earlier, the oxidation state of F in any compound is always -1. Therefore, the oxidation state of F in \(\mathrm{BrF}_{5}\) is -1.
05

e) Naming XeOF4 and finding the oxidation state of F

The compound \(\mathrm{XeOF}_{4}\) is a molecular compound consisting of xenon, oxygen, and fluorine. It is called xenon oxytetrafluoride. The oxidation state of F in any compound is always -1. Therefore, the oxidation state of F in \(\mathrm{XeOF}_{4}\) is -1.
06

f) Naming HIO3 and finding the oxidation state of I

The compound \(\mathrm{HIO}_{3}\) is a molecular compound consisting of hydrogen, iodine, and oxygen. It is called iodic acid. To find the oxidation state of I in this compound, we use the rule that the sum of the oxidation states of all the atoms in the compound must be zero. Hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. The equation for the sum of the oxidation states is: \( +1 + x + 3(-2) = 0 \) Solving for x, we get \( x= +5 \) So, the oxidation state of iodine in \(\mathrm{HIO}_{3}\) is +5.

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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.

Indicate whether each of the following statements is true or false (a) \(\mathrm{H}_{2}(g)\) and \(\mathrm{D}_{2}(g)\) are allotropic forms of hydrogen. (b) \(\mathrm{ClF}_{3}\) is an interhalogen compound. (c) MgO(s) is an acidic anhydride. (d) \(\mathrm{SO}_{2}(g)\) is an acidic anhydride. (e) \(2 \mathrm{H}_{3} \mathrm{PO}_{4}(l) \rightarrow \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}(l)+\mathrm{H}_{2} \mathrm{O}(g)\) is an example of a condensation reaction. (f) Tritium is an isotope of the element hydrogen. (g) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) is an example of a disproportionation reaction.

The standard heats of formation of \(\mathrm{H}_{2} \mathrm{O}(g), \mathrm{H}_{2} \mathrm{S}(g), \mathrm{H}_{2} \mathrm{Se}(g)\) and \(\mathrm{H}_{2} \mathrm{Te}(g)\) are \(-241.8,-20.17,+29.7,\) and \(+99.6 \mathrm{kJ} /\) mol, respectively. The enthalpies necessary to convert the elements in their standard states to one mole of gaseous atoms are \(248,277,227,\) and 197 \(\mathrm{kJ} / \mathrm{mol}\) atoms for \(\mathrm{O}, \mathrm{S},\) Se, and Te, respectively. The enthalpy for dissociation of \(\mathrm{H}_{2}\) is 436 \(\mathrm{kJ} / \mathrm{mol} .\) Calculate the average \(\mathrm{H}-\mathrm{O}, \mathrm{H} \mathrm{S}, \mathrm{H}-\mathrm{Se}\) and \(\mathrm{H}-\) Te bond enthalpies, and comment on their trend.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium nitrite, (b) ammonia, (c) nitrous oxide, (d) sodium cyanide, (e) nitric acid, (f) nitrogen dioxide, (g) nitrogen, (h) boron nitride.

(a) Determine the number of calcium ions in the chemical formula of the mineral hardystonite, \(\mathrm{Ca}_{x} \mathrm{Zn}\left(\mathrm{Si}_{2} \mathrm{O}_{7}\right) .(\mathbf{b})\) Determine the number of hydroxide ions in the chemical formula of the mineral pyrophylite, \(\mathrm{Al}_{2}\left(\mathrm{Si}_{2} \mathrm{O}_{5}\right)_{2}(\mathrm{OH})_{x}\)
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