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Chapter 22: Problem 15

Make a general prediction about which of the halogen elements, \(\mathrm{F}_{2}, \mathrm{Cl}_{2}, \mathrm{Br}_{2},\) or \(\mathrm{I}_{2},\) displaces other halogens from a solution of halide ions. Which of the halogens is able to displace \(\mathrm{O}_{2}(\mathrm{g})\) from water? Which is able to displace \(\mathrm{H}_{2}(\mathrm{g})\) from water?

Short Answer

Expert verified
Fluorine can displace all other halogens from their halide solutions. Chlorine, bromine, and iodine can displace the halogens below them in the Group 7. None of the halogens can displace oxygen from water. Only fluorine can displace hydrogen from water.

Step by step solution

01

Predicting the Halogen Displacement

Reactivity of halogens decreases down the group. This means, \( \mathrm{F}_{2} \) being at the top of the group is the most reactive and can displace all other halogens from their halide solution. Similarly, \( \mathrm{Cl}_{2} \) can displace \( \mathrm{Br}_{2} \) & \( \mathrm{I}_{2} \), \( \mathrm{Br}_{2} \) can only displace \( \mathrm{I}_{2} \), and \( \mathrm{I}_{2} \) being the least reactive, cannot displace any of the halogens.
02

Predicting the Displacement of \(\mathrm{O}_{2}(\mathrm{g})\) from Water

None of the halogens can displace oxygen from water. This is because oxygen is a strong oxidizing agent and less reactive than any halogen.
03

Predicting the Displacement of \(\mathrm{H}_{2}\)(g) from Water

Fluorine, being the strongest oxidising agent among the halogens, is the only one able to react with water to displace \( \mathrm{H}_{2}(\mathrm{g})\) . The reaction is: \(2 \mathrm{F}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 4 \mathrm{HF}(\mathrm{g})+ \mathrm{O}_{2}(\mathrm{g})\)

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Most popular questions from this chapter

Peroxonitrous acid is an unstable intermediate formed in the oxidation of \(\mathrm{HNO}_{2}\) by \(\mathrm{H}_{2} \mathrm{O}_{2}\). It has the same formula as nitric acid, HNO \(_{3}\). Show how you would expect peroxonitrous and nitric acids to differ in structure.

All of the following compounds yield \(\mathrm{O}_{2}(\mathrm{g})\) when heated to about \(1000 \mathrm{K}\) except (a) \(\mathrm{KClO}_{3} ;\) (b) \(\mathrm{KClO}_{4}\) (c) \(\mathrm{N}_{2} \mathrm{O} ;\) (d) \(\mathrm{CaCO}_{3} ;\) (e) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\).

Give an appropriate formula for each of the following compounds: (a) calcium sulfate dihydrate; (b) hydrosulfuric acid; (c) sodium hydrogen sulfate; (d) disulfuric acid.

One reaction for the production of adipic acid, \(\mathrm{HOOC}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH},\) used in the manufacture of nylon, involves the oxidation of cyclohexanone, \(\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{O},\) in a nitric acid solution. Assume that dinitrogen monoxide is also formed, and write a balanced equation for this reaction.

Use Lewis structures and other information to explain the observation that (a) \(\mathrm{H}_{2} \mathrm{S}\) is a gas at room temperature, whereas \(\mathrm{H}_{2} \mathrm{O}\) is a liquid. (b) \(\mathrm{O}_{3}\) is diamagnetic.
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