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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.