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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 shares similarities with Group 1A elements, including having one electron in its outermost shell, high reactivity, and the ability to form compounds with a +1 oxidation state. These properties provide a reason to place hydrogen alongside Group 1A elements in the periodic table, despite some differences such as being a nonmetal and having a lower atomic mass.

Step by step solution

01

Understand the properties of hydrogen

Before explaining why hydrogen might be placed alongside Group 1A elements, it is essential to comprehend hydrogen's properties. Hydrogen is the lightest and simplest element in the periodic table, with atomic number 1 and atomic mass 1.00794. Hydrogen forms a diatomic gas (H2) at room temperature and is highly reactive. It exists in various isotopes, the most common being protium (鹿H), deuterium (虏H), and tritium (鲁H).
02

Understand the properties of Group 1A elements

Group 1A elements, also known as alkali metals, include elements such as lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These elements have the following properties: - They are very reactive and readily form compounds with other elements. - They have one electron in their outermost shell, making them highly electropositive (easily lose an electron to become positively charged). - They typically form +1 ions when combined with nonmetals. - They are soft, shiny metals with low melting points.
03

Comparing hydrogen with Group 1A elements

Hydrogen has similarities with Group 1A elements, which make it reasonable to place it alongside those elements: - Both hydrogen and Group 1A elements have one electron in their outermost shell. This property enables hydrogen to lose one electron, similar to alkali metals, resulting in a +1 oxidation state in their compounds. - Hydrogen, like Group 1A elements, is highly reactive. This reactivity comes from its ability to lose its one valence electron easily. - Hydrogen can form compounds with nonmetals through ionic or covalent bonding, much like alkali metals.
04

Conclusion

Hydrogen exhibits properties that are similar to those of Group 1A elements, specifically its single electron in the outermost shell, high reactivity, and ability to form compounds that display the oxidation state of +1. This is the reason why hydrogen might be placed alongside Group 1A elements in the periodic table. However, it is important to note that hydrogen also has some distinctly different properties from alkali metals, such as being a nonmetal, existing as a diatomic gas, and having a much lower atomic mass.

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Most popular questions from this chapter

Two silicate anions are known in which the linking of the tetrahedra forms a closed ring. One of these cyclic silicate anions contains three silicate tetrahedra, linked into a ring. The other contains six silicate tetrahedra. (a) Sketch these cyclic silicate anions. (b) Determine the formula and charge of each of the anions.

Explain the following observations: (a) \(\mathrm{HNO}_{3}\) is a stronger oxidizing agent than \(\mathrm{H}_{3} \mathrm{PO}_{4}\). (b) Silicon can form an ion with six fluorine atoms, \(\mathrm{SiF}_{6}{ }^{2-}\), whereas carbon is able to bond to a maximum of four, \(\mathrm{CF}_{4}\). (c) There are three compounds formed by carbon and hydrogen that contain two carbon atoms each \(\left(\mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{C}_{2} \mathrm{H}_{4}\right.\), and \(\left.\mathrm{C}_{2} \mathrm{H}_{6}\right)\), whereas silicon forms only one analogous compound \(\left(\mathrm{Si}_{2} \mathrm{H}_{6}\right)\).

Write balanced equations for each of the following reactions (some of these are analogous to reactions shown in the chapter). (a) Aluminum metal reacts with acids to form hydrogen gas. (b) Steam reacts with magnesium metal to give magnesium oxide and hydrogen. (c) Manganese(IV) oxide is reduced to manganese(II) oxide by hydrogen gas. (d) Calcium hydride reacts with water to generate hydrogen gas.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group \(6 \mathrm{~A}\) element in each: (a) sulfur tetrachloride, (b) selenium trioxide, (c) sodium thiosulfate, (d) hydrogen sulfide, (e) sulfuric acid.

(a) How does the structure of diborane \(\left(\mathrm{B}_{2} \mathrm{H}_{6}\right)\) differ from that of ethane \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right) ?\) (b) By using concepts discussed in Chapter 8, explain why diborane adopts the geometry that it does. (c) What is the significance of the statement that the hydrogen atoms in diborane are described as hydridic?
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