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Chapter 22: Problem 21

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

Short Answer

Expert verified
Hydrogen might be placed along with the Group 1 elements in the periodic table due to the similarity of having one electron in their outermost shell, which influences their chemical properties. However, hydrogen is a non-metal, unlike alkali metals, making its placement in the periodic table debatable.

Step by step solution

01

Understand Group 1 Elements

Group 1 elements are also known as alkali metals. They share some common properties: they have one electron in their outermost shell, react well with water, and are soft metals. Group 1 elements include Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr).
02

Explore Hydrogen's Properties

Hydrogen is a non-metal element, which is unique compared to the other elements in Group 1. It is also the lightest element in the periodic table, with an atomic number of 1. That means hydrogen has one electron orbiting its nucleus.
03

Compare Hydrogen to Group 1 Elements

Comparing hydrogen to Group 1 elements, we notice that hydrogen, like alkali metals, has one electron in its outer shell. This gives hydrogen a similar electron configuration to elements in Group 1, which is a crucial factor in determining the chemical properties of an element.
04

Conclusion

Based on the similarity of having one electron in their outermost shell, hydrogen might be placed along with Group 1 elements in the periodic table. However, it is essential to note that hydrogen is a non-metal, making it distinct from the alkali metals in Group 1. The placement of hydrogen in the periodic table is often debatable, as some periodic tables place it separately or within Group 1, considering its shared electron configuration property.

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Most popular questions from this chapter

Using \(\Delta G_{f}^{\circ}\) for \(\mathrm{NO}\) and \(\mathrm{NO}_{2},\) from Appendix \(\mathrm{C},\) calculate the equilibrium constant for the oxidation of \(\mathrm{NO}\) to \(\mathrm{NO}_{2}\) at \(298.0 \mathrm{~K}\) as described in equation \(22.38 .\)

When aluminum replaces up to half of the silicon atoms in \(\mathrm{SiO}_{2}\), a mineral class called feldspars result. The feldspars are the most abundant rock-forming minerals, comprising about \(50 \%\) of the minerals in Earth's crust. Orthoclase is a feldspar in which Al replaces one-fourth of the Si atoms of \(\mathrm{SiO}_{2},\) and charge balance is completed by \(\mathrm{K}^{+}\) ions. Determine the chemical formula for orthoclase.

Write a balanced chemical reaction for the condensation reaction between \(\mathrm{H}_{3} \mathrm{PO}_{4}\), molecules to form $\mathrm{H}_{6} \mathrm{P}_{4} \mathrm{O}_{13}$.

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 \(\mathrm{GeO}_{2}\).

Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.) (a) Hydrogen selenide can be prepared by reaction of an aqueous acid solution on aluminum selenide. (b) Sodium thiosulfate is used to remove excess \(\mathrm{Cl}_{2}\) from chlorine-bleached fabrics. The thiosulfate ion forms \(\mathrm{SO}_{4}^{2-}\) and elemental sulfur, while \(\mathrm{Cl}_{2}\) is reduced to \(\mathrm{Cl}^{-}\).
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