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Chapter 22: Problem 117

In your own words, define the following terms: (a) polyhalide ion; (b) polyphosphate; (c) interhalogen; (d) disproportionation.

Short Answer

Expert verified
Polyhalide ion: An ion that contains atoms of the same halogen element in different oxidation states; Polyphosphate: A compound derived from multiple phosphate units via dehydration synthesis; Interhalogen: A molecule formed from two different halogens; Disproportionation: A redox reaction where an element from a reactant is simultaneously oxidized and reduced, resulting in two different products.

Step by step solution

01

Define Polyhalide Ion

A polyhalide ion is a type of ion that contains atoms of the same halogen element in different oxidation states. Examples include iodine pentoxide (\(I_2O_5\)).
02

Define Polyphosphate

Polyphosphates are compounds derived from multiple phosphate units. These units are joined together by dehydration synthesis, resulting in phosphoric anhydride bonds. A common example is the adenosine triphosphate (ATP), which has three interconnected phosphate groups.
03

Define Interhalogen

Interhalogens are a group of molecules formed from two different halogens. They can be of several types: diatomic, triatomic, tetraatomic, and hexatomic. An example of an interhalogen compound is iodine monofluoride (\(IF\)).
04

Define Disproportionation

Disproportionation refers to a specific type of redox reaction in which an element from a reactant is simultaneously oxidized and reduced, resulting in two different products. A common example involves the conversion of hydrogen peroxide (\(H_2O_2\)) into water and oxygen.

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Most popular questions from this chapter

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.

Use VSEPR theory to predict the probable geometric structures of the molecules (a) \(\mathrm{O}_{2} \mathrm{XeF}_{2} ;\) (b) \(\mathrm{O}_{3} \mathrm{XeF}_{2}\) (c) OXeF \(_{4}\).

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 name to each of the following compounds: (a) \(\mathrm{ZnS} ;\) (b) \(\mathrm{KHSO}_{3} ;\) (c) \(\mathrm{K}_{2} \mathrm{S}_{2} \mathrm{O}_{3} ;\) (d) \(\mathrm{SF}_{4}\).

The trichloride ion, \(\mathrm{Cl}_{3}^{-1}\), is not very stable in aqueous solution. The equilibrium constant for the following dissociation reaction is 5.5 at \(25^{\circ} \mathrm{C}\) : $$\mathrm{Cl}_{3}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Cl}_{2}(\mathrm{aq})$$ (a) Draw a Lewis structure for the \(\mathrm{Cl}_{3}^{-}\) ion and predict the geometry. (b) Calculate the equilibrium concentration of \(\mathrm{Cl}_{3}^{-}\) if 0.0010 moles each of \(\mathrm{KCl}\) and \(\mathrm{Cl}_{2}\) are dissolved in water at \(25^{\circ} \mathrm{C}\) to make \(1.0 \mathrm{L}\) of solution.
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