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Chapter 22: Problem 27

Identify the following hydrides as ionic, metallic, or molecular: (a) \(\mathrm{BaH}_{2}\), (b) \(\mathrm{H}_{2} \mathrm{Te}\), (c) \(\mathrm{TiH}_{1.7}\).

Short Answer

Expert verified
(a) \(\mathrm{BaH}_{2}\) is an ionic hydride, as it consists of a metal (Ba) and a non-metal (H) that form ionic bonds. (b) \(\mathrm{H}_{2} \mathrm{Te}\) is a molecular hydride, as it consists of two non-metals (H and Te) that form covalent/molecular bonds. (c) \(\mathrm{TiH}_{1.7}\) is a metallic hydride, as it involves a transition metal (Ti) and a non-metal (H) that form non-stoichiometric metallic bonds.

Step by step solution

01

(a) Identify type of hydride for \(\mathrm{BaH}_{2}\)

For BaH2, we will proceed by analyzing the participating elements. Barium (Ba) is an alkaline earth metal belonging to Group 2 in the periodic table, and Hydrogen (H) is a non-metal in Group 1. Generally, when metals form bonds with non-metals, they transfer electrons and form ionic compounds. Hence, we can conclude that BaH2 is an ionic hydride.
02

(b) Identify type of hydride for \(\mathrm{H}_{2} \mathrm{Te}\)

H2Te consists of Hydrogen (H) and Tellurium (Te). Tellurium (Te) is a non-metal in Group 16 of the periodic table. As we have two non-metals here, they typically form covalent/molecular bonds. Therefore, H2Te is a molecular hydride.
03

(c) Identify type of hydride for \(\mathrm{TiH}_{1.7}\)

TiH1.7 involves Titanium (Ti) and Hydrogen (H). Titanium (Ti) is a transition metal from the d-block, and combines with the non-metal Hydrogen (H). Non-stoichiometric hydrides, such as TiH1.7, usually involve transition metals and are characterized by metallic bonding. Hence, TiH1.7 is a metallic hydride.

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Most popular questions from this chapter

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: (a) \(\mathrm{NH}_{4}^{+}\), (b) \(\mathrm{NO}_{2}^{-}\), (c) \(\mathrm{N}_{2} \mathrm{O}\), (d) \(\mathrm{NO}_{2}\).

Write balanced equations for each of the following reactions. (a) When mercury(II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. (b) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, \(\mathrm{PbS}(s)\), reacts with ozone to form \(\mathrm{PbSO}_{4}(s)\) and \(\mathrm{O}_{2}(g)\). (d) When heated in air, \(\mathrm{ZnS}(s)\) is converted to \(\mathrm{ZnO}\). (e) Potassium peroxide reacts with \(\mathrm{CO}_{2}(g)\) to give potassium carbonate and \(\mathrm{O}_{2}\) (f) Oxygen is converted to ozone in the upper atmosphere.

Manganese silicide has the empirical formula MnSi and melts at \(1280^{\circ} \mathrm{C}\). It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect MnSi to be: metallic, molecular, covalent- network, or ionic? (b) Write a likely balanced chemical equation for the reaction of \(\mathrm{MnSi}\) with concentrated aqueous HF.

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\). (e) Hydrazine reduces \(\mathrm{CrO}_{4}{ }^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}{ }^{-}\)in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) ).

Give a reason why hydrogen might be placed along with the group lA elements of the periodic table.
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