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प्रश्न
Use molecular orbital theory to explain why the Be2 molecule does not exist.
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उत्तर
The electronic configuration of Beryllium is `1"s"^2 2"s"^2`.
The molecular orbital electronic configuration for Be2 molecule can be written as:
`sigma_(1"s")^2 sigma_(1"s")^(•2) sigma_(2"s")^2 sigma_(2"s")^(•2)`
Hence, the bond order for Be2 is `1/2 ("N"_"b" - "N"_"a")`
Where,
Nb = Number of electrons in bonding orbitals
Na = Number of electrons in anti-bonding orbitals
∴Bond order of Be2 = `1/2(4-4) =0`
A negative or zero bond order means that the molecule is unstable. Hence, Be2molecule does not exist.
संबंधित प्रश्न
Stable form of C may be represented by the formula:
The molecular formula of the compound formed from \[\ce{B}\] and \[\ce{C}\] will be ______.
The electronic configuration of the outer most shell of the most electronegative element is ______.
Amongst the following elements whose electronic configurations are given below, the one having the highest ionisation enthalpy is ______.
Dimagnetic species are those which contain no unpaired electrons. Which among the following are dimagnetic?
(i) \[\ce{N2}\]
(ii) \[\ce{N^{2-}2}\]
(iii) \[\ce{O2}\]
(iv) \[\ce{O^{2-}2}\]
Explain the shape of \[\ce{BrF5}\].
Explain why \[\ce{PCl5}\] is trigonal bipyramidal whereas \[\ce{IF5}\] is square pyramidal.
Which of the following statements is correct?
Molecular orbital electronic configuration for 'X' anion is- KK σ*2s2 σ*2s2 π2px2 π2py2 σ2pz2 π*2px1, the anion 'X' is.
