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Question
What are metallic/interstitial hydrides? How do they differ from molecular hydrides?
Solution
Metallic hydrides are formed by d- and f-:block elements. Their hydrides conduct heat and electricity. They are non-stoichiometric, being deficient in hydrogen. For example, \[\ce{LaH_{2.87}, ybH_{2.55}}\]etc.
| Metallic hydrides | Molecular hydrides | ||
| (1) | These are formed by eland f-block elements. | (1) | These are formed by p-block elements and some s-block elements (\[\ce{Be }\] and \[\ce{Mg}\]). |
| (2) | They conduct electricity. | (2) | They do not conduct electricity. |
| (3) | They are hard and have metallic luster. | (3) | They are volatile compounds having low melting and boiling points. |
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RELATED QUESTIONS
What do you understand by the term “non-stoichiometric hydrides”? Do you expect this type of the hydrides to be formed by alkali metals? Justify your answer.
How do you expect the metallic hydrides to be useful for hydrogen storage? Explain.
Metal hydrides are ionic, covalent or molecular in nature. Among \[\ce{LiH, NaH, KH, RbH, CsH}\], the correct order of increasing ionic character is ______.
Only one element of ______ forms hydride.
Which of the following statements are not true for hydrogen?
(i) It exists as diatomic molecule.
(ii) It has one electron in the outermost shell.
(iii) It can lose an electron to form a cation which can freely exist.
(iv) It forms a large number of ionic compounds by losing an electron.
Which of the following statements is correct?
(i) Hydrides of group 13 act as Lewis acids.
(ii) Hydrides of group 14 are electron deficient hydrides.
(iii) Hydrides of group 14 act as Lewis acids.
(iv) Hydrides of group 15 act as Lewis bases.
Which of the following statements is correct?
(i) Metallic hydrides are deficient of hydrogen.
(ii) Metallic hydrides conduct heat and electricity.
(iii) Ionic hydrides do not conduct electricity in solid-state.
(iv) Ionic hydrides are very good conductors of electricity in solid state.
