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Fifth group elements form hydrides to type `AH_(3)`. The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides . The H-M-H bond angle of `V` group hydrides decrease from `107^(circ)` to `90^(circ)` for `NH_(3)` to `SbH_(3)` , this is due to:A. Increase in strength of bases with molecular weightB. use of pour p-orbital for M-H bonding in hydrides of higher molecular weightC. Bond energies of M-H bonds increaaseD. Bond pairs of electrons go closer to central atom |
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Answer» Correct Answer - B In successive hydrides starting from N to Sb, the lone pair causes distortion of M-H bonds. The bond angle decrease from `107^@` to `90^@`.This suggests tha orbitals used in M-H bonding are almost pure p-orbitals |
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