H_2O has a net dipole moment while BeF_2 has | vedclass

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(D) The dipole moment of a molecule depends on its geometry and the polarity of its bonds.$H_2O$ has a bent geometry due to the presence of two lone p

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$BeF_2$ molecule is linear and $H_2O$ is bent

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(D) The dipole moment of a molecule depends on its geometry and the polarity of its bonds.$H_2O$ has a bent geometry due to the presence of two lone pairs on the oxygen atom,which results in a net dipole moment $(\mu 
eq 0)$.$BeF_2$ has a linear geometry with a bond angle of $180^{\circ}$,where the two $Be-F$ bond dipoles are equal in magnitude and opposite in direction,canceling each other out to result in a zero net dipole moment $(\mu = 0)$.

$H_2O$ has a net dipole moment while $BeF_2$ has zero dipole moment because

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