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Chapter 22: Problem 7

Identify the true statements concerning the atoms and ions of the group 16 elements. [Sections 22.5 and 22.6\(]\) (a) The ionic radii are larger than the atomic radii because the ions have more electrons than their corresponding atoms. (b) Atomic radii increase going down the group because of increasing nuclear charge. (c) The ionic radii increase going down the group because of the increase in the principal quantum number of outermost electrons. (d) Of these ions, \(\mathrm{Se}^{2-}\) is the strongest base in water because it is largest.

Short Answer

Expert verified
The true statements concerning the atoms and ions of group 16 elements are: (a) The ionic radii are larger than the atomic radii because the ions have more electrons than their corresponding atoms. (c) The ionic radii increase going down the group because of the increase in the principal quantum number of outermost electrons.

Step by step solution

01

Statement (a)

The ionic radii are larger than the atomic radii because the ions have more electrons than their corresponding atoms. This statement is true. When an atom gains electrons to form a negatively charged ion, it results in an increase in the ionic radius as the ions have more electrons than their corresponding atoms. Additionally, the increase in the electron-electron repulsion in the ion leads to a larger ionic radius.
02

Statement (b)

Atomic radii increase going down the group because of increasing nuclear charge. This statement is false. Although the nuclear charge does increase down the group, it is not the main reason for the increase in atomic radius. Atomic radii increase going down the group due to the increase in the principal quantum number (n) of the outermost electrons. As we go down the group, the number of electron shells increases, making the atomic radius larger.
03

Statement (c)

The ionic radii increase going down the group because of the increase in the principal quantum number of outermost electrons. This statement is true. As we go down the group, the principal quantum number (n) of the outermost electrons increases, leading to a larger ionic radius. The increase in n results in a greater distance between the outermost electrons and the nucleus, hence a larger ionic radius.
04

Statement (d)

Of these ions, \(\mathrm{Se}^{2-}\) is the strongest base in water because it is the largest. This statement is false. Basicity typically decreases as we go down the group, due to the decrease in the electron affinity of the element. This causes the larger ions to have a weaker attraction for protons in water, and thus they form weaker bases. In the case of group 16 elements, \(\mathrm{O}^{2-}\) would be the strongest base in water, not \(\mathrm{Se}^{2-}\).

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Most popular questions from this chapter

(a) What is the oxidation state of \(\mathrm{P}\) in \(\mathrm{PF}_{6}^{-}\) and of \(\mathrm{N}\) in \(\mathrm{NF}_{3} ?\) (b) Why doesn't \(\mathrm{N}\) form \(\mathrm{NF}_{6}^{-}\) ion analogous to \(\mathrm{P} ?\)

In aqueous solution, hydrogen sulfide reduces (a) \(\mathrm{Fe}^{3+}\) to \(\mathrm{Fe}^{2+},(\mathbf{b}) \mathrm{Br}_{2}\) to \(\mathrm{Br}^{-},(\mathbf{c}) \mathrm{MnO}_{4}^{-}\) to \(\mathrm{Mn}^{2+},(\mathbf{d}) \mathrm{HNO}_{3}\) to \(\mathrm{NO}_{2}\) In all cases, under appropriate conditions, the product is elemental sulfur. Write a balanced net ionic equation for each reaction.

Account for the following observations: (a) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) is a diprotic acid. (b) Nitric acid is a strong acid, whereas phos- (c) Phosphate rock is ineffective as a phoric acid is weak. phosphate fertilizer. (d) Phosphorus does not exist at room temperature as diatomic molecules, but nitrogen does. (e) Solutions of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) are quite basic.

A sulfuric acid plant produces a considerable amount of heat. This heat is used to generate electricity, which helps reduce operating costs. The synthesis of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) consists of three main chemical processes: (a) oxidation of \(S\) to \(\mathrm{SO}_{2}\), (b) oxidation of \(\mathrm{SO}_{2}\) to \(\mathrm{SO}_{3},\) (c) the dissolving of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and the subsequent reaction with water to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\). If the third process produces \(130 \mathrm{~kJ} / \mathrm{mol}\), how much heat is produced in preparing a mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from a mole of \(S\) ? How much heat is produced in preparing \(2000 \mathrm{~kg}\) of $\mathrm{H}_{2} \mathrm{SO}_{4} ?$

The maximum allowable concentration of \(\mathrm{H}_{2} \mathrm{~S}(g)\) in air is \(20 \mathrm{mg}\) per kilogram of air ( 20 ppm by mass). How many grams of FeS would be required to react with hydrochloric acid to produce this concentration at \(101.3 \mathrm{kPa}\) and \(25^{\circ} \mathrm{C}\) in an average room measuring $3.5 \mathrm{~m} \times 6.0 \mathrm{~m} \times 2.5 \mathrm{~m} ?\( (Under these conditions, the average molar mass of air is \)29.0 \mathrm{~g} / \mathrm{mol} .)$
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