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Chapter 22: Problem 3

The oxides of the phosphorus(III), antimony(III), and bismuth(III) are \(\mathrm{P}_{4} \mathrm{O}_{6}, \mathrm{Sb}_{4} \mathrm{O}_{6},\) and \(\mathrm{Bi}_{2} \mathrm{O}_{3} .\) Only one of these oxides is amphoteric. Which one? Which of these oxides is most acidic? Which is most basic?

Short Answer

Expert verified
Antimony(III) oxide (Sb4O6) is the amphoteric oxide, Phosphorus(III) oxide (P4O6) is the most acidic oxide, and Bismuth(III) oxide (Bi2O3) is the most basic oxide.

Step by step solution

01

Identify the Amphoteric Oxide

Amphoteric oxides can react with both acids and bases. Antimony(III) oxide (Sb4O6) meets this characteristic, therefore it is the amphoteric oxide.
02

Identify the Most Acidic Oxide

The acidity of an oxide increases with increasing oxidation state. Phosphorus(III) oxide (P4O6) has the most electrons in an oxidation state, making it the most acidic oxide.
03

Identify the Most Basic Oxide

Basic oxides react with acids to form a salt and water. Out of the given oxides, Bismuth(III) oxide (Bi2O3) has the least number of electrons in an oxidation state. Hence, it tends to donate electrons, which is a characteristic of bases. Therefore, Bi2O3 is the most basic oxide.

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Most popular questions from this chapter

What is the oxidation state of sulfur in the following compounds? (a) \(\mathrm{SF}_{4} ;\) (b) \(\mathrm{S}_{2} \mathrm{F}_{10} ;\) (c) \(\mathrm{H}_{2} \mathrm{S} ;\) (d) \(\mathrm{CaSO}_{3}\).

The sketch is a portion of the phase diagram for the element sulfur. The transition between solid orthorhombic \(\left(S_{\alpha}\right)\) and solid monoclinic \(\left(S_{\beta}\right)\) sulfur, in the presence of sulfur vapor, is at \(95.3^{\circ} \mathrm{C} .\) The triple point involving monoclinic sulfur, liquid sulfur, and sulfur vapor is at \(119^{\circ} \mathrm{C}\) (a) How would you modify the phase diagram to represent the melting of orthorhombic sulfur that is sometimes observed at \(113^{\circ} \mathrm{C} ?[\) Hint: What would the phase diagram look like if the monoclinic sulfur did not form? (b) Account for the observation that if a sample of rhombic sulfur is melted at \(113^{\circ} \mathrm{C}\) and then heated, the liquid sulfur freezes at \(119^{\circ} \mathrm{C}\) upon cooling.

Draw plausible Lewis structures for (a) dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\) (b) nitryl chloride, \(\mathrm{ClNO}_{2}\) (Central atom is \(\mathrm{N}\) ) (c) phosphorous acid, a diprotic acid with the empirical formula \(\mathrm{H}_{3} \mathrm{PO}_{3}\).

The amide anion \(\mathrm{NH}_{2}^{-}\) is a very strong base. On the basis of molecular orbital theory, would you expect \(\mathrm{NH}_{2}^{-}\) to be linear or bent?

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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