Observe the following list of molecules. The | vedclass

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(C) To determine the polarity,we check the net dipole moment of each molecule:$1$. $NH_3$: Polar (Pyramidal geometry,non-zero dipole moment).$2$. $BF_

Vedclass · Accepted Answer

$5, 3$

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(C) To determine the polarity,we check the net dipole moment of each molecule:$1$. $NH_3$: Polar (Pyramidal geometry,non-zero dipole moment).$2$. $BF_3$: Non-polar (Trigonal planar,symmetric,dipole moments cancel out).$3$. $NF_3$: Polar (Pyramidal geometry,non-zero dipole moment).$4$. $H_2S$: Polar (Bent geometry,non-zero dipole moment).$5$. $CO_2$: Non-polar (Linear,symmetric,dipole moments cancel out).$6$. $CH_4$: Non-polar (Tetrahedral,symmetric,dipole moments cancel out).$7$. $CHCl_3$: Polar (Tetrahedral,asymmetric,non-zero dipole moment).$8$. $H_2O$: Polar (Bent geometry,non-zero dipole moment).Polar molecules: $NH_3, NF_3, H_2S, CHCl_3, H_2O$ (Total = $5$).Non-polar molecules: $BF_3, CO_2, CH_4$ (Total = $3$).Therefore,the number of polar and non-polar molecules are $5$ and $3$ respectively.

Observe the following list of molecules. The number of polar and non-polar molecules are respectively: $NH_3, BF_3, NF_3, H_2S, CO_2, CH_4, CHCl_3, H_2O$

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