The correct order regarding the covalent nature of hydrides is:

B e H_{2} > M g H_{2} > C a H_{2} > S r H_{2} > B a H_{2}

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M g H_{2} > C a H_{2} > B e H_{2} > B a H_{2} > S r H_{2}

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B a H_{2} > M g H_{2} > C a H_{2} > B e H_{2} > S r H_{2}

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B e H_{2} > C a H_{2} > M g H_{2} > B a H_{2} > S r H_{2}

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Solution

The correct option is A $B e H_{2} > M g H_{2} > C a H_{2} > S r H_{2} > B a H_{2}$
On moving down the group of alkline earth metals, the covalent nature of hydrides decreases. The decreasing order is $B e H_{2} > M g H_{2} > C a H_{2} > S r H_{2} > B a H_{2}$ .
The hydrides of beryllium and magnesium are covalent, whereas the hydrides of strontium, calcium and barium are ionic. On moving down the group of alkaline earth metals, the size of metal cations increases and the polarization power decreases. Hence, the covalent nature decreases.

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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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