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]
- A
$A,D$
- B
$A,C$
- C
$A,B$
- D
$A,D,B$
Similar Questions
When two atoms of chlorine combine to form one molecule of chlorine gas, the energy of the molecule
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What is meant by the term bond order ? Calculate the bond order of: $N _{2}, O _{2}, $ $O _{2}^{+}$ and $O _{2}^{-}$
What is meant by the term bond order ? Calculate the bond order of: $N _{2}, O _{2}, $ $O _{2}^{+}$ and $O _{2}^{-}$
The bond order is maximum in
The bond order is maximum in
- [AIPMT 1994]
Use the molecular orbital energy level diagram to show that $\mathrm{N}_{2}$ would be expected to have a triple bond, $\mathrm{F}_{2}$ a single bond and $\mathrm{Ne}_{2}$ no bond.
Use the molecular orbital energy level diagram to show that $\mathrm{N}_{2}$ would be expected to have a triple bond, $\mathrm{F}_{2}$ a single bond and $\mathrm{Ne}_{2}$ no bond.
In which change bond order and number of unpaired $e^-$ both are increased
In which change bond order and number of unpaired $e^-$ both are increased