In which of the following pairs of molecules/ions, both the species are not likely to exist?
In which of the following pairs of molecules/ions, both the species are not likely to exist?
- [JEE MAIN 2013]
- A
$H_{2}^+, He_2^{2-}$
- B
$H_{2}^-, He_2^{2-}$
- C
$H_{2}^{+2}, He_2$
- D
$H_{2}^-, He_2^{2+}$
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Give electron configuration, Magnetic property, bond order and energy diagram for carbon $\left( {{{\rm{C}}_2}} \right)$.
Give electron configuration, Magnetic property, bond order and energy diagram for carbon $\left( {{{\rm{C}}_2}} \right)$.
The species having no $P\pi - P\pi $ bond but has bond order equal to $O_2$
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Assuming that Hund's rule is violated, the bond order and magnetic nature of the diatomic molecule $B_2$ is
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- [IIT 2010]
According to Molecular Orbital Theory,
($A$) $\mathrm{C}_2^{2-}$ is expected to be diamagnetic
($B$) $\mathrm{O}_2{ }^{2+}$ is expected to have a longer bond length than $\mathrm{O}_2$
($C$) $\mathrm{N}_2^{+}$and $\mathrm{N}_2^{-}$have the same bond order
($D$) $\mathrm{He}_2^{+}$has the same energy as two isolated He atoms
According to Molecular Orbital Theory,
($A$) $\mathrm{C}_2^{2-}$ is expected to be diamagnetic
($B$) $\mathrm{O}_2{ }^{2+}$ is expected to have a longer bond length than $\mathrm{O}_2$
($C$) $\mathrm{N}_2^{+}$and $\mathrm{N}_2^{-}$have the same bond order
($D$) $\mathrm{He}_2^{+}$has the same energy as two isolated He atoms
- [IIT 2016]