Applications of Metallic Hydrides

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1. Applications of Metallic Hydrides Submitted by- Vansh Patil 11th/C Roll no.-S11C36 SNBP International School Affiliation no.-1130522

2. Index Introduction What are Hydrides Types of Hydrides Ionic or Saline Hydrides Covalent Hydrides Metallic Hydrides Applications of Metallic Hydrides

3. Introduction Hydride, in simple terms, is said to be the anion of hydrogen. It is a chemical compound where the hydrogen atoms exhibit nucleophilic, basic or reducing properties. Usually, in a hydride, the hydrogen has the oxidation number equal to −1. Some of the most popular examples include water (H2O), methane (CH4) and ammonia (NH3).

4. What are Hydrides? Compounds of hydrogen with less electronegative elements are known as hydrides. So, when hydrogen reacts with any other element the product formed is a hydride. If we closely observe the periodic table hydrides formation is not seen from VA group elements and this condition is known as hydride gap. Hydrogen molecule usually reacts with many elements except noble gases to form hydrides. However, the properties may vary depending on the type of intermolecular force that exists between the elements, its molecular masses, temperature, and other factors.

5. Types of Hydrides Hydrides are mainly divided into three major types or groups. The categories are decided based on what elements the hydrogen forms bonds with or simply based on chemical bonding. The three types of hydrides are ionic, covalent, and metallic hydrides.

6. Ionic or Saline Hydrides They are formed when hydrogen molecule reacts with highly electropositive s-block elements (Alkali Metals and Alkaline Earth Metals). In solid-state, the ionic hydrides are crystalline, non-conducting and non-volatile. However, in a liquid state, they conduct electricity. Ionic hydrides on electrolysis liberate hydrogen gas at the anode. Saline or ionic hydrides does not dissolve in conventional solvents, and they are mostly used as bases or reducing reagents in organic synthesis. Example of Ionic Hydrides: Nah, KH, CaH2, etc. These contain hydrogen as the negatively charged (H–) ion.

7. Covalent Hydrides Covalent hydrides are formed when hydrogen reacts with other similar electronegative elements like Si, C, etc. The most common examples are CH4 and NH3. In general, compounds that are formed when hydrogen is reacted with non-metals are called covalent hydrides. The compound shares a covalent bond and are either volatile or non-volatile compounds. Covalent hydrides are also either liquids or gases. Example of Covalent Hydrides: SiH4 (silane)

8. Metallic Hydrides A hydrogen compound that forms a bond with another metal element is classified as a metal hydride. The bond is mostly covalent type but sometimes the hydrides are formed with ionic bonds. These are usually formed by transition metals and are mostly non-stoichiometric, hard, high melting and boiling points. Example of Metallic Hydrides: TiH aluminum, cadmium, magnesium, etc.

9. Application of Hydrides Several applications of metallic hydrides such as hydrogen storage, rechargeable batteries, hydrogen compressors, heat storage and heat pumps, isotope separation, powder metallurgy, sensors and activators, and hydrogen purification.

10. Hydrogen Storage Hydrogen storage is a term used for any of several methods for storing hydrogen for later use. These methods encompass mechanical approaches such as high pressures and low temperatures, or chemical compounds that release H2 upon demand. ... Achieving such low temperatures requires significant energy.

11. Rechargeable Batteries Rechargeable batteries store energy through a reversible chemical reaction, which allows charge to be stored again after the battery has been drained.

12. Hydrogen Compressors A hydrogen compressor is a device that increases the pressure of hydrogen by reducing its volume resulting in compressed hydrogen or liquid hydrogen.

13. Heat Storage Thermal energy storage (TES) comprises a collection of technologies that store energy in thermal form (heat or cold) either directly or indirectly through energy conversion processes.

14. Isotope Separation Isotope separation is the process of concentrating specific isotopes of a chemical element by removing other isotopes. The use of the nuclides produced is varied. The largest variety is used in research (e.g., in chemistry where atoms of "marker" nuclide are used to figure out reaction mechanisms). By tonnage, separating natural uranium into enriched uranium and depleted uranium is the largest application. In the following text, mainly the uranium enrichment is considered. This process is crucial in the manufacture of uranium fuel for nuclear power plants and is also required for the creation of uranium-based nuclear weapons. Plutonium-based weapons use plutonium produced in a nuclear reactor, which must be operated in such a way as to produce plutonium already of suitable isotopic mix or grade. While different chemical elements can be purified through chemical processes, isotopes of the same element have nearly identical chemical properties, which makes this type of separation impractical, except for separation of deuterium.

15. Powder Metallurgy Powder metallurgy (PM) is a term covering a wide range of ways in which materials or components are made from metal powders. PM processes can avoid, or greatly reduce, the need to use metal removal processes, thereby drastically reducing yield losses in manufacture and often resulting in lower costs.