Question

Which of the following is not an example of ionic hydride ?
LiH
CsH
CaH₂
GeH₂​

Answer 1

Answer:

GeH₂​ is not an example of ionic hydride.

Explanation:

Ionic Hydrides:

• These are produced by metals with electronegativity values that are lower than those of hydrogen.
• Ionic hydrides are formed when all group 1 and group 2 elements are heated to a high temperature.

Properties of Ionic Hydrides:

• These contain hydride ions and are created when metal electrons are transferred from one hydrogen atom to another.
• These are crystalline solids that are white and have an ionic crystal structure.
• They conduct electricity in the fused state and have high melting and boiling temperatures, releasing dihydrogen at the anode.
• They are always stoichiometric and have a high heat of formation.
• With the exception of LiH, they burn in air when heated vigorously because they break down into combustible hydrogen.
• They strongly react with water to produce the matching metal hydroxide and release dihydrogen. They so serve as a solid foundation.
• They have strong reducing properties, particularly at high temperatures.

Uses of Ionic hydride:

• As a reducing agent, ionic hydrides and their complexes are employed.
• Ionic hydrides are utilized as solid fuels because when heated, they break down to produce dihydrogen, which spontaneously ignites.

Final answer:

LiH ,CsH  and CaH₂ are alkali metal hydride is an example of ionic hydride and GeH₂​ is alkali earth metal hydride is not an example of ionic hydride

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Answer 2

Answer:

GeH₂​ is not an example of ionic hydride.

Explanation:

Ionized Hydrogen:

Metals whose electronegativity values are lower than those of hydrogen form these.

When all group 1 and group 2 elements are heated to a high temperature, ionic hydrides are produced.

Ionic Hydride Characteristics:

These are made when metal electrons are moved from one hydrogen atom to another and contain hydride ions.

1.These are white crystalline solids with ionic crystal structures.

2.They have high melting and boiling points and conduct electricity when fused, releasing dihydrogen at the anode.

3.They always have a high heat of formation and are stoichiometric.

4.They decompose into combustible hydrogen when heated vigorously, with the exception of LiH, and burn in air.

5.They vehemently respond to water .

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