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(B) molecule is non-polar if its net dipole moment is zero. $1$. $H_2$: Homonuclear diatomic molecule,dipole moment = $0$. $2$. $CO_2$: Linear geometr

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$4$

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(B) molecule is non-polar if its net dipole moment is zero. $1$. $H_2$: Homonuclear diatomic molecule,dipole moment = $0$. $2$. $CO_2$: Linear geometry,dipole moments of $C=O$ bonds cancel each other,net dipole moment = $0$. $3$. $CH_4$: Tetrahedral geometry,bond dipoles cancel each other,net dipole moment = $0$. $4$. $BF_3$: Trigonal planar geometry,bond dipoles cancel each other,net dipole moment = $0$. Other molecules like $HF, H_2O, SO_2, NH_3, HCl,$ and $CHCl_3$ have a net dipole moment greater than zero. Therefore,the non-polar molecules are $H_2, CO_2, CH_4,$ and $BF_3$. The total count is $4$.

The number of non-polar molecules from the following is . . . . . . $HF, H_2O, SO_2, H_2, CO_2, CH_4, NH_3, HCl, CHCl_3, BF_3$

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