Which one of the following species does not exist under normal conditions?

  • A
    $Be_2^+$
  • B
    $Be_2$
  • C
    $B_2$
  • D
    $Li_2$

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Similar Questions

The bond dissociation energy $(E)$ and bond length $(R)$ of $O_2$,$N_2$,and $F_2$ follow the order as:

As per molecular orbital theory,the pair of molecules which do not exist is:

Match List-$I$ with List-$II$.
List-$I$ List-$II$
$A$. $\Psi_{MO} = \Psi_{A} - \Psi_{B}$ $I$. Dipole moment
$B$. $\mu = Q \times r$ $II$. Bonding molecular orbital
$C$. $\frac{N_{b} - N_{a}}{2}$ $III$. Anti-bonding molecular orbital
$D$. $\Psi_{MO} = \Psi_{A} + \Psi_{B}$ $IV$. Bond order

When $\psi_A$ and $\psi_B$ are the wave functions of atomic orbitals,then $\sigma^*$ is represented by :

Match the following molecules/ions in List-$I$ with their respective bond orders in List-$II$:
| List-$I$ (Molecules/ions) | List-$II$ (Bond order) |
| :--- | :--- |
| $A. N_2^+$ | $I. 1.0$ |
| $B. CO$ | $II. 1.5$ |
| $C. O_2$ | $III. 2.0$ |
| $D. O_2^-$ | $IV. 2.5$ |
| | $V. 3.0$ |

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