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Chapter 22: Problem 28

Identify the following hydrides as ionic, metallic, or molecular: (a) \(\mathrm{B}_{2} \mathrm{H}_{6}\), (b) \(\mathrm{RbH}\), (c) \(\mathrm{Th}_{4} \mathrm{H}_{1.5}\)

Short Answer

Expert verified
(a) \(\mathrm{B}_{2} \mathrm{H}_{6}\) is a molecular hydride; (b) \(\mathrm{RbH}\) is an ionic hydride; and (c) \(\mathrm{Th}_{4} \mathrm{H}_{1.5}\) is a metallic hydride.

Step by step solution

01

Identify the characteristics of each hydride type

Ionic hydrides: Formed between a highly electropositive metal (Group 1 or Group 2 elements) and hydrogen. These hydrides have ionic bonds due to the difference in electronegativity of metal and hydrogen. Metallic hydrides: Formed between transition, inner transition metals or actinides, and hydrogen. They have metallic bonds and are often non-stoichiometric compounds. Molecular hydrides: Formed between non-metals and hydrogen. They have covalent bonds and are characterized by discrete molecules.
02

Analyze each given hydride

(a) \(\mathrm{B}_{2} \mathrm{H}_{6}\): Boron is a non-metal, and the compound is composed of boron and hydrogen. The hydride has a well-defined stoichiometry, pointing towards a molecular hydride. (b) \(\mathrm{RbH}\): Rubidium (Rb) is a group 1 metal with low electronegativity, while hydrogen has a relatively high electronegativity. The ionic character of their bond suggests that this hydride is ionic. (c) \(\mathrm{Th}_{4} \mathrm{H}_{1.5}\): Thorium (Th) is an actinide element. Also, the given compound is non-stoichiometric, which is a characteristic of metallic hydrides.
03

State the type of hydride for each given example

(a) \(\mathrm{B}_{2} \mathrm{H}_{6}\): Molecular hydride (b) \(\mathrm{RbH}\): Ionic hydride (c) \(\mathrm{Th}_{4} \mathrm{H}_{1.5}\): Metallic hydride

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Most popular questions from this chapter

Consider the elements \(\mathrm{O}, \mathrm{Ba}, \mathrm{Co}, \mathrm{Be}, \mathrm{Br}\), and Se. From this list select the element that (a) is most electronegative, (b) exhibits a maximum oxidation state of \(+7\), (c) loses an electron most readily, (d) forms \(\pi\) bonds most readily, (e) is a transition metal.

Write a balanced equation for the reaction of each of the following compounds with water: (a) \(\mathrm{SO}_{2}(g)\), (b) \(\mathrm{Cl}_{2} \mathrm{O}_{7}(g)\), (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s)\) (d) \(\mathrm{BaC}_{2}(\mathrm{~s})\), (e) \(\mathrm{RbO}_{2}(\mathrm{~s})\), (f) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)\) (g) \(\mathrm{NaH}(s)\).

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Write the formulas for the following compounds, and indicate the oxidation state of the group \(4 \hat{A}\) element or of boron in each: (a) silicon dioxide, (b) germanium tetrachloride, (c) sodium borohydride, (d) stannous chloride, (e) diborane.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) chlorate ion, (b) hydroiodic acid, (c) iodine trichloride, (d) sodium hypochlorite, (e) perchloric acid, (f) xenon tetrafluoride.
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