Use molecular orbital theory to explain why the $Be_{2}$ molecule does not exist.
Use molecular orbital theory to explain why the $Be_{2}$ molecule does not exist.
The electronic configuration of Beryllium is $1 s^{2}\, 2 s^{2}$
The molecular orbital electronic configuration for $Be _{2}$ molecule can be written as:
$\sigma _{1s}^2\,\,\sigma _{1s}^{ + 2}\,\,\sigma _{2s}^2\,\,\sigma _{2s}^{ + 2}$
Hence, the bond order for $Be _{2}$ is $\frac{1}{2}\left(N_{b}-N_{a}\right)$
Where
$N_{b}=$ Number of electrons in bonding orbitals
$N_{a}=$ Number of electrons in anti-bonding orbitals
$\therefore $ Bond order of $Be_{2}$ $=\frac{1}{2}(4-4)=0$
A negative or zero bond order means that the molecule is unstable. Hence, $Be _{2}$ molecule does not exist.
Similar Questions
The linear combination of atomic orbitals to form molecular orbitals takes place only when the combining atomic orbitals
$A$. have the same energy
$B$. have the minimum overlap
$C$. have same symmetry about the molecular axis
$D$. have different symmetry about the molecular axis
Choose the most appropriate from the options given below:
The linear combination of atomic orbitals to form molecular orbitals takes place only when the combining atomic orbitals
$A$. have the same energy
$B$. have the minimum overlap
$C$. have same symmetry about the molecular axis
$D$. have different symmetry about the molecular axis
Choose the most appropriate from the options given below:
- [JEE MAIN 2024]
The incorrect statement is :-
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The pair of species that has the same bond order in the following is
The pair of species that has the same bond order in the following is
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The bond order is not three for
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