The order of stability of the hydrides is as follows:

BeH₂ > CaH₂ > MgH₂ > SrH₂> BaH₂

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BeH₂ > MgH₂ > CaH₂ > SrH₂> BaH₂

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BeH₂ < MgH₂ < CaH₂ < SrH₂< BaH₂

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BeH₂ < CaH₂ < MgH₂ < SrH₂< BaH₂

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Solution

The correct option is B
BeH₂ > MgH₂ > CaH₂ > SrH₂> BaH₂

The stability of hydrides decreases with increasing atomic no because the metallic nature of the elements increases. The first two hydrides - $B e H_{2}$ and $M g H_{2}$ are covalent and exist as polymeric structures while the other hydrides are ionic in nature.

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C a H_{2}

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Arrange the following

(i) CaH₂, BeH₂ and TiH₂ in order of increasing electrical conductance.

(ii) LiH, NaH and CsH in order of increasing ionic character.

(iii) H–H, D–D and F–F in order of increasing bond dissociation enthalpy.

(iv) NaH, MgH₂ and H₂O in order of increasing reducing property.

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