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Chapter 8: Problem 89

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

Short Answer

Expert verified
(a) Sodium and potassium: They are both soft and have low melting and boiling points, they are highly reactive- specifically with water, and they form ions with a single positive charge. (b) Chlorine and bromine: They are less reactive than alkali metals but still reactive, they exist as diatomic molecules in their elemental form, and they form ions with a single negative charge.

Step by step solution

01

Determine chemical properties of Sodium (Na) and Potassium (K)

Sodium and potassium are both in Group 1 of the periodic table. They are both alkali metals which means they have similar properties. They are soft enough to cut with a knife, they have low melting and boiling points compared to metals, and they are highly reactive, especially with water, to which they react vigorously, forming hydroxides and hydrogen gas. Furthermore, both elements are monovalent, meaning they tend to form ions with a single positive charge after losing a single electron.
02

Determine chemical properties of Chlorine (Cl) and Bromine (Br)

Chlorine and bromine are both in Group 7 of the periodic table, making them halogens. They share several common properties. These include: both are diatomic molecules in their elemental form, they have relatively high melting and boiling points and they are less reactive than the alkali metals. Further, they each have seven valence electrons, which leads them to gain one electron when forming ions, resulting in ions with a single negative charge.
03

Formulate the similarities based on their chemical properties

For sodium and potassium: 1) They are both soft and have low melting and boiling points. 2) Both are highly reactive, especially with water, forming hydroxides and Hydrogen gas. 3) They form ions with a single positive charge. For chlorine and bromine: 1) Both are less reactive than alkali metals but still reactive enough to gain an electron. 2) They exist as diatomic molecules in their elemental form. 3) They form ions with a single negative charge.

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Most popular questions from this chapter

(a) The formula of the simplest hydrocarbon is \(\mathrm{CH}_{4}\) (methane). Predict the formulas of the simplest compounds formed between hydrogen and the following elements: silicon, germanium, tin, and lead. (b) Sodium hydride (NaH) is an ionic compound. Would you expect rubidium hydride (RbH) to be more or less ionic than NaH? (c) Predict the reaction between radium (Ra) and water. (d) When exposed to air, aluminum forms a tenacious oxide \(\left(\mathrm{Al}_{2} \mathrm{O}_{3}\right)\) coating that protects the metal from corrosion. Which metal in Group 2 A would you expect to exhibit similar properties? Why?

Compare the work function for cesium ( \(206 \mathrm{~kJ} / \mathrm{mol}\) ) with its first ionization energy ( \(376 \mathrm{~kJ} / \mathrm{mol}\) ). Explain the difference.

A hydrogenlike ion contains only one electron. The energies of the electron in a hydrogenlike ion are given by $$ E_{n}=-\left(2.18 \times 10^{-18} \mathrm{~J}\right) Z^{2}\left(\frac{1}{n^{2}}\right) $$ where \(n\) is the principal quantum number and \(Z\) is the atomic number of the element. Calculate the ionization energy (in \(\mathrm{kJ} / \mathrm{mol}\) ) of the \(\mathrm{He}^{+}\) ion.

Arrange the following in order of increasing first ionization energy: \(\mathrm{F}, \mathrm{K}, \mathrm{P}, \mathrm{Ca},\) and \(\mathrm{Ne} .\)

Write a balanced equation that predicts the reaction of rubidium (Rb) with (a) \(\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{Cl}_{2}(g)\) (c) \(\mathrm{H}_{2}(g)\)
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