What do you expect the nature of hydrides is, if formed by elements of atomic numbers 15, 19, 23 and 44 with dihydrogen? Compare their behaviour with water.

Asked by Abhisek | 11 months ago |  113

##### Solution :-

The elements of atomic numbers 15 is phosphorus, 19 potassium, 23 is vanadium and 44 is ruthenium.

Hydride of Phosphorus

Hydride of phosphorus (PH3) is covalent in nature. Due to the presence of excess electrons as a lone pair on Phosphorus, it is electron rich.

Hydride of potassium

Due to high electropositive nature of potassium, the dihydrogen forms ionic hydrides along with potassium. Naturally it is non – volatile and crystalline.

Vanadium belongs to d- block in the periodic table. The metals of d- block forms non-stoichiometric or metallic hydrides. Hydrides of vanadium are naturally metallic and have deficiency of hydrogen.

Hydrides of Ruthenium

Ruthenium belongs to d- block in the periodic table. The metals of d- block forms non- stoichiometric or metallic hydrides. Hydrides of ruthenium are naturally metallic and have deficiency of hydrogen.

Behaviour of hydrides towards water

Potassium hydride reacts violently with water as:

$$KH_{(s)}+H_{2}O_{(aq)}\rightarrow KOH_{(aq)}+H_{2(g)}$$

Ammonia (NH3) behaves as a Lewis base and reacts with water as:

$$H_{2}O_{(l)}+NH_{3(aq)}\rightarrow OH^{-}_{(aq)}+NH^{+}_{4(aq)}$$

Hydrides of vanadium and Ruthenium do not react with water. Hence, the increasing order of reactivity of the hydrides is (V, Ru) H < PH3 < KH.

Answered by Pragya Singh | 11 months ago

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