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Chapter 22: Problem 21

Give a reason why hydrogen might be placed along with the group 1 A elements of the periodic table.

Short Answer

Expert verified
Hydrogen is placed along with Group 1A elements in the periodic table due to its similar electron configuration and chemical reactivity. Both hydrogen and Group 1A elements have one electron in their outermost energy level and tend to lose this electron to form a +1 charged ion during chemical reactions.

Step by step solution

01

Understanding the Periodic Table and Group 1A Elements

In the periodic table, elements are arranged according to their atomic number and similar properties. Group 1A elements, also known as alkali metals, include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These elements have a common characteristic: they all have one electron in their outermost energy level (valence electron).
02

Identifying Hydrogen's Electron Configuration

Hydrogen (H) is the first element in the periodic table, with an atomic number of 1. Its electron configuration is 1s^1, meaning that it has one electron in its outermost energy level (the 1s orbital), just like the other Group 1A elements.
03

Discussing the Similarity in Chemical Reactivity

Hydrogen and other Group 1A elements share similar chemical reactivity due to having one valence electron. Elements in this group tend to lose their single valence electron readily to achieve a stable electron configuration. This results in the formation of a positive ion (cation) with a +1 charge. Therefore, hydrogen resembles the group 1A elements in its reactivity and tendency to form +1 charged ions. To summarize: Hydrogen might be placed along with the Group 1A elements of the periodic table because it shares similar electron configuration and chemical reactivity with these elements. Specifically, hydrogen has one electron in its outermost energy level like alkali metals and tends to lose this electron to form a +1 charged ion during chemical reactions.

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Most popular questions from this chapter

Write a balanced equation for the preparation of \(\mathrm{H}_{2}\) using (a) \(\mathrm{Mg}\) and an acid, (b) carbon and steam, (c) methane and steam.

Complete and balance the following equations: (a) \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(I) \longrightarrow\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (f) \(\mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow\)

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to \(\mathrm{GeCl}_{4}\) by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; \(\mathrm{GeCl}_{4}\) is then hydrolyzed in water to \(\mathrm{GeO}_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\). The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from \(\mathrm{GeO}_{2}\).

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Although the \(\mathrm{ClO}_{4}^{-}\) and \(\mathrm{IO}_{4}^{-}\) ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\) was not synthesized until \(1965 .\) The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. Write the balanced equation for this reaction.
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