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Chapter 8: Problem 92

What factors account for the unique nature of hydrogen?

Short Answer

Expert verified
Hydrogen is unique due to its simple atomic structure (a single proton and electron), it's placement on the periodic table (group 1 but is a non-metal), and its reactivity and combination with nearly all elements to form both inorganic and organic compounds.

Step by step solution

01

Atomic Structure

Understand the atomic structure of hydrogen. Hydrogen is the first element on the periodic table with an atomic number of '1'. Its atomic structure is simple with one proton in its nucleus and one electron in its shell.
02

Unique Positioning on the Periodic Table

Relate hydrogen's uniqueness to its placement on the periodic table. Although hydrogen is part of Group 1 (alkali metals) in the periodic table, it's not a metal but a non-metal. This is attributed to its ability to gain as well as lose an electron, bringing it closer to both alkali metals and halogens in behavior.
03

Reactivity and Compounds

Note the reactivity and the compounds that hydrogen forms. Hydrogen is highly reactive due to its single electron and can combine with nearly all elements. It forms both inorganic compounds (like water) and organic compounds (like hydrocarbons), showcasing its versatility.

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Most popular questions from this chapter

Arrange these species in isoelectronic pairs: \(\mathrm{O}^{+}, \mathrm{Ar},\) \(\mathrm{S}^{2-}, \mathrm{Ne}, \mathrm{Zn}, \mathrm{Cs}^{+}, \mathrm{N}^{3-}, \mathrm{As}^{3+}, \mathrm{N}, \mathrm{Xe}\) In which of these are the species written in decrease.

The first four ionization energies of an element are approximately \(738 \mathrm{~kJ} / \mathrm{mol}, \quad 1450 \mathrm{~kJ} / \mathrm{mol}, 7.7 \times\) \(10^{3} \mathrm{~kJ} / \mathrm{mol}\), and \(1.1 \times 10^{4} \mathrm{~kJ} / \mathrm{mol}\). To which periodic group does this element belong? Why?

Write formulas and give names for the binary hydrogen compounds of the second- period elements (Li to F). Describe the changes in physical and chemical properties of these compounds as we move across the period from left to right.

In each of the following pairs, indicate which one of the two species is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-},\) (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+},\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\).

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.
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