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Chapter 8: Problem 66

Based on your knowledge of the chemistry of the alkali metals, predict some of the chemical properties of francium, the last member of the group.

Short Answer

Expert verified
Francium, as an alkali metal, is predicted to be highly reactive due to its single valence electron. It will likely form a \(Fr^{+}\) ion. Francium may also react with water, oxygen, and halogens.

Step by step solution

01

General Properties of Alkali Metals

Understand that alkali metals, which are in Group 1 of the periodic table, are characterized by their softness and silvery appearance. They are highly reactive due to their single valence electron which they tend to lose in reactions to form +1 ions.
02

Trend in Reactivity of Alkali Metals

Realize that the reactivity of alkali metals increases from top to bottom in the periodic table. This means that as we proceed down the group, the reactivity increases. Francium, being at the bottom, would be highly reactive.
03

Predicting Francium's Reactivity

Based on the aforementioned characteristics, it can be predicted that francium, like other group 1 elements, will be highly reactive due to its single valence electron and would readily lose this electron to form a \(Fr^{+}\) ion.
04

Francium's Reaction with Other Substances

Francium can be expected to react vigorously with non-metals such as oxygen and halogens, and would react with water in a similar way as other alkali metals, and produce hydrogen gas and an alkali.

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Most popular questions from this chapter

Use the alkali metals and alkaline earth metals as examples to show how we can predict the chemical properties of elements simply from their electron configurations.

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

List these ions in order of increasing ionic radius: \(\mathrm{N}^{3-}, \mathrm{Na}^{+}, \mathrm{F}^{-}, \mathrm{Mg}^{2+}, .\mathrm{O}^{2-}\)

Explain why the electron affinity of nitrogen is approximately zero, although the elements on either side, carbon and oxygen, have substantial positive electron affinities.

Group these electron configurations in pairs that would represent similar chemical properties of their atoms: (a) \(1 s^{2} 2 s^{2} 2 p^{5}\) (b) \(1 s^{2} 2 s^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6}\)
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