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Chapter 8: Problem 15

In the periodic table, the element hydrogen is sometimes grouped with the alkali metals (as in this book) and sometimes with the halogens. Explain why hydrogen can resemble the Group \(1 \mathrm{~A}\) and the Group 7A elements.

Short Answer

Expert verified
Hydrogen resembles both Group 1A (Alkali metals) and Group 7A (Halogens) elements because it has one electron in its outer shell. Like the alkali metals, it can lose this electron to form a +1 ion. Alternatively, like the halogens, it can gain an electron to fill its outer shell to form a -1 ion.

Step by step solution

01

Understanding the structure of hydrogen

Hydrogen is the first element on the periodic table and consists of 1 proton and 1 electron. This means it has one electron in its outer shell.
02

Comparing hydrogen to alkali metals (Group 1A)

The alkali metals are elements in group 1A on the periodic table and they also have one electron in their outer shell. These elements can easily lose one electron to achieve a stable configuration. Hydrogen also has this capacity, and is, therefore, sometimes grouped with the alkali metals.
03

Comparing hydrogen to halogens (Group 7A)

Elements in Group 7A are known as halogens. Each halogen atom has seven electrons in its outermost shell and can easily accept an electron to achieve a stable configuration. Since hydrogen atom has one electron, it can also gain one more electron to complete its shell. Hence, it has properties similar to the halogens, and it is sometimes categorized in Group 7A.

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Most popular questions from this chapter

Write ground-state electron configurations for these transition metal ions: (a) \(\mathrm{Sc}^{3+}\) (b) \(\mathrm{Ti}^{4+}\) (c) \(\mathrm{V}^{5+}\) (d) \(\mathrm{Cr}^{3+}\) , (e) \(\mathrm{Mn}^{2+},\) (f) \(\mathrm{Fe}^{2+}\) (h) \(\mathrm{Co}^{2+}\) (g) \(\mathrm{Fe}^{3+}\) (i) \(\mathrm{Ni}^{2+}\) (i) \(\mathrm{Cu}^{+}\) (k) \(\mathrm{Cu}^{2+}\) (1) \(\mathrm{Ag}^{+}\) \((\mathrm{m}) \mathrm{Au}^{+}\) (n) \(\mathrm{Au}^{3+},\) (o) \(\mathrm{Pt}^{2+}\)

Sketch an outline of the periodic table and show group and period trends in the first ionization energy of the elements. What types of elements have the highest ionization energies and what types the lowest ionization energies?

For each pair of elements listed here, give three properties that show their chemical similarity: (a) sodium and potassium and (b) chlorine and bromine.

When carbon dioxide is bubbled through a clear calcium hydroxide solution, the solution becomes milky. Write an equation for the reaction and explain how this reaction illustrates that \(\mathrm{CO}_{2}\) is an acidic oxide.

Arrange the following atoms in order of decreasing atomic radius: \(\mathrm{Na}, \mathrm{Al}, \mathrm{P}, \mathrm{Cl}, \mathrm{Mg}\).
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