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Chapter 7: Problem 71

(a) As described in Section 7.7, the alkali metals react with hydrogen to form hydrides and react with halogens to form halides. Compare the roles of hydrogen and halogens in these reactions. Write balanced equations for the reaction of fluorine with calcium and for the reaction of hydrogen with calcium. (b) What is the oxidation number and electron configuration of calcium in each product?

Short Answer

Expert verified
In reactions with alkali metals, hydrogen and halogens both act as electron acceptors. For the reaction between calcium (Ca) and fluorine (F₂): \(Ca + F_2 \rightarrow CaF_2\). For the reaction between calcium (Ca) and hydrogen (H₂) gas: \(Ca + H_2 \rightarrow CaH_2\). In both products, the oxidation number of calcium is +2, and its electron configuration is [Ar], as it loses two valence electrons from the 4s orbital.

Step by step solution

01

Comparing the Roles of Hydrogen and Halogens in Reactions with Alkali Metals

When alkali metals react with hydrogen, they form metal hydrides. And when they react with halogens, they form metal halides. In both these reactions, alkali metals lose electrons and get oxidized. Hydrogen and halogens act as electron acceptors; hydrogen gains an electron to form a hydride ion (H⁻), while halogens, like fluorine, gain an electron to form a halide ion (e.g., F⁻).
02

Writing Balanced Equations for the Reaction of Calcium with Fluorine and Hydrogen

For the reaction between calcium (Ca) and fluorine (F₂): Ca + F₂ → CaF₂ For the reaction between calcium (Ca) and hydrogen (H₂) gas: Ca + H₂ → CaH₂
03

Finding Oxidation Number and Electron Configuration of Calcium in Both Products

(a) In CaF₂: The oxidation number of calcium is +2 because it loses two electrons to form a Ca²⁺ ion, and two fluorine atoms each gain one electron to form F⁻ ions. Thus, the electron configuration of calcium in CaF₂ is [Ar], where it has lost the two valence electrons from the 4s orbital. (b) In CaH₂: The oxidation number of calcium is also +2 because it loses two electrons to form a Ca²⁺ ion, and two hydrogen atoms each gain one electron to form H⁻ ions (hydride ions). The electron configuration of calcium in CaH₂ is also [Ar], where it has lost its two valence electrons from the 4s orbital.

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Most popular questions from this chapter

Arrange each of the following sets of atoms and ions, in order of increasing size: (a) \(\mathrm{Pb}, \mathrm{Pb}^{2+}, \mathrm{Pb}^{4+}\) (b) \(\mathrm{V}^{3+}, \mathrm{Co}^{2+}, \mathrm{Co}^{3+}\) (c) \(\mathrm{Se}^{2-}, \mathrm{S}^{2-}, \mathrm{Sn}^{2+}\) (d) \(\mathrm{K}^{+}, \mathrm{Rb}^{+}, \mathrm{Br}^{-}\)

Consider \(\mathrm{S}, \mathrm{Cl},\) and \(\mathrm{K}\) and their most common ions. (a) List the atoms in order of increasing size. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.

Arrange the following atoms in order of increasing effective nuclear charge experienced by the electrons in the \(n=2\) shell: Be, Br, Na, P, Se.

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7} .\) (a) What is the name of this product (see Table 2.6)? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q) ?(\mathbf{d})\) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the -2 oxidation state, what is the oxidation state of the \(\mathrm{Cl}\) ? What is the electron configuration of \(\mathrm{Cl}\) in this oxidation state?

Give examples of transition metal ions with +3 charge that have an electron configuration of \(n d^{5}(n=3,4,5 \ldots)\).
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