In which of following option is wrong about stability of diatomic molecules
In which of following option is wrong about stability of diatomic molecules
- A
$N_2 > N_2^+ > N_2^-$
- B
$O_2^{+2} > O^+_2 > O_2$
- C
$N_2^+ > N_2 > N_2^-$
- D
$O_2^{+2} > O_2 > O_2^{-2}$
Similar Questions
Give features of Molecular orbital $( \mathrm{MO} )$ theory:
Give features of Molecular orbital $( \mathrm{MO} )$ theory:
Which information obtained by electronic configuration of Molecule in $\mathrm{MO}$ ?
Which information obtained by electronic configuration of Molecule in $\mathrm{MO}$ ?
The paramagnetic nature of oxygen molecule is best explained on the basis of
The paramagnetic nature of oxygen molecule is best explained on the basis of
Which of the following facts given is not correct ?
$(I)$ Bond length order : $H^-_2 = H^+_2 > H_2$
$(II)\, O^+_2 ,NO,N^-_2$ have same bond order of $2 \frac{1}{2}$
$(III)$ Bond order can assume any value including zero upto four
$(IV)\, NO^-_3$ and $BO^-_3$ have same bond order for $X - O$ bond (where $X$ is central atom)
Which of the following facts given is not correct ?
$(I)$ Bond length order : $H^-_2 = H^+_2 > H_2$
$(II)\, O^+_2 ,NO,N^-_2$ have same bond order of $2 \frac{1}{2}$
$(III)$ Bond order can assume any value including zero upto four
$(IV)\, NO^-_3$ and $BO^-_3$ have same bond order for $X - O$ bond (where $X$ is central atom)
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.