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Question
Molecular hydrides are classified as electron deficient, electron precise and electron rich compounds. Explain each type with two examples.
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Solution
Molecular hydrides are classified according to the relative numbers of electrons and bonds in their Lewis structure into : (i) electron-deficient, (ii) electron-precise, and (iii) electron-rich hydrides.
Electron deficient hydrides:
An electron-deficient hydride, as the name suggests, has too few electrons for writing its conventional Lewis structure.
Examples are the hydrides of group 13 such as B2H6,AlH3 etc.
Due to their deficiency of electrons, they can act as Lewis acids[ i.e. electron Acceptors]
Electron precise hydrides:
These have the required number of electrons to write their conventional Lewis structures, or we can say, they have exact number of electrons to form normal covalent bonds.
Examples are the hydrides of group 14 such as CH4,SiH4 etc.
Electron rich hydrides:
These have a greater number of electrons than normal covalent bonds. The excess electrons are present in the form of lone pairs.
Examles are the hydrides of group 15, 16 and 17 such as NH3,H2O etc.
Electron deficient hydrides:
An electron-deficient hydride, as the name suggests, has too few electrons for writing its conventional Lewis structure.
Examples are the hydrides of group 13 such as B2H6,AlH3 etc.
Due to their deficiency of electrons, they can act as Lewis acids[ i.e. electron Acceptors]
Electron precise hydrides:
These have the required number of electrons to write their conventional Lewis structures, or we can say, they have exact number of electrons to form normal covalent bonds.
Examples are the hydrides of group 14 such as CH4,SiH4 etc.
Electron rich hydrides:
These have a greater number of electrons than normal covalent bonds. The excess electrons are present in the form of lone pairs.
Examles are the hydrides of group 15, 16 and 17 such as NH3,H2O etc.
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