InterviewSolution
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InterviewSolution
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Use molecular orbital theory to explain why the `Be_(2)` molecules do not exist? |
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Answer» The electronic configuration of Beryllium is `1s^(2)2s^(2)`. The molecular orbital electronic configuration for `Be_(2)` molecule can be written as : `underset (1s)sigma^(2) underset(1s)sigma^(*2) underset(2s)sigma^(2) underset(2s)sigma^(*2)` Hence, the bond order for `Be_(2)` is `(1)/(2)(N_(b)-N_(a))` Where, `N_(b)`= Number of electrons in bonding orbitals `N_(a)`=Number of electrons in anti-bonding orbitals `therefore` Bond order of `Be_(2)=(1)/(2)(4-4)=0` A negative or zero bond order means that the molecules is unstable. Hence, `Be_(2)` molecule does not exist. |
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