Explain why $BeH_{2}$ molecule has a zero dipole moment although the $Be-H$ bonds are polar.
(N/A) $BeH_{2}$ molecule has a linear geometry with a bond angle of $180^{\circ}$.
In a $Be-H$ bond,the electronegativity of $Be$ is $1.57$ and $H$ is $2.20$. Due to this difference,the bonding electron pair is shifted towards the $H$ atom,making the $Be-H$ bond polar.
However,in the linear $BeH_{2}$ molecule,the two $Be-H$ bond dipoles are equal in magnitude and point in exactly opposite directions.
As a result,the two bond dipoles cancel each other out,leading to a net dipole moment of zero.
Therefore,$BeH_{2}$ is a non-polar molecule: $H^{\delta-} \leftarrow Be^{2+} \rightarrow H^{\delta-}$.
In a $Be-H$ bond,the electronegativity of $Be$ is $1.57$ and $H$ is $2.20$. Due to this difference,the bonding electron pair is shifted towards the $H$ atom,making the $Be-H$ bond polar.
However,in the linear $BeH_{2}$ molecule,the two $Be-H$ bond dipoles are equal in magnitude and point in exactly opposite directions.
As a result,the two bond dipoles cancel each other out,leading to a net dipole moment of zero.
Therefore,$BeH_{2}$ is a non-polar molecule: $H^{\delta-} \leftarrow Be^{2+} \rightarrow H^{\delta-}$.
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