Chapter 8

Arrange these species in isoelectronic pairs: \(\mathrm{O}^{+}, \mathrm{Ar},\) \(\mathrm{S}^{2-}, \mathrm{Ne}, \mathrm{Zn}, \mathrm{Cs}^{+}, \mathrm{N}^{3-}, \mathrm{As}^{3+}, \mathrm{N}, \mathrm{Xe}\) In which of these are the species written in decrease.

In which of these are the species written in decreasing radius? (a) \(\mathrm{Be}, \mathrm{Mg}, \mathrm{Ba}\) (b) \(\mathrm{N}^{3-}, \mathrm{O}^{2-}, \mathrm{F}^{-}\) (c) \(\mathrm{Tl}^{3+}, \mathrm{Tl}^{2+}, \mathrm{Tl}^{+}\)

When carbon dioxide is bubbled through a clear calcium hydroxide solution, the solution becomes milky. Write an equation for the reaction and explain how this reaction illustrates that \(\mathrm{CO}_{2}\) is an acidic oxide.

You are given four substances: a fuming red liquid, a dark metallic-looking solid, a pale-yellow gas, and a yellow-green gas that attacks glass. You are told that these substances are the first four members of Group \(7 \mathrm{~A},\) the halogens. Name each one.

For each pair of elements listed here, give three properties that show their chemical similarity: (a) sodium and potassium and (b) chlorine and bromine.

Name the element that forms compounds, under appropriate conditions, with every other element in the periodic table except He and Ne.

Explain why the first electron affinity of sulfur is \(200 \mathrm{~kJ} / \mathrm{mol}\) but the second electron affinity is \(-649 \mathrm{~kJ} / \mathrm{mol}\),

The \(\mathrm{H}^{-}\) ion and the He atom have two \(1 \mathrm{~s}\) electrons each. Which of the two species is larger? Explain.

Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions.

Write the formulas and names of the oxides of the second-period elements (Li to \(\mathrm{N}\) ). Identify the oxides as acidic, basic, or amphoteric.