Explain why $B e H_{2}$ molecule has a zero dipole moment although the Be–H bonds are polar.

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Solution

The Lewis structure for $B e H_{2}$ is as follows:

H:Be:H

There is no lone pair at the central atom (Be) and there are two bond pairs. Hence, $B e H_{2}$ is of the type $A B_{2}$ . It has a linear structure.

Dipole moments of each H–Be bond are equal and are in opposite directions. Therefore, they nullify each other. Hence, $B e H_{2}$ molecule has zero dipole moment.

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