Import Question JSON

$\text{Hint: If the dipole moment is zero then the molecule is non-polar.}\n\n\text{The structure of } CCl_4 \text{ is as follows:}\n\n\text{In } CCl_4\text{, even though each of the four C-Cl bonds is distinctly polar, the resultant moment of any three of them is equal in magnitude but opposite in direction to the moment due to the fourth one. So, the molecule's net dipole moment is zero, and it is non-polar.}\n\n\text{The net dipole moment in } CCl_4 \text{ is zero.}\n\n\text{The structure of } SO_3 \text{ is as follows:}\n\n\text{In } SO_3\text{, even though each of the three S-O bonds is distinctly polar, the resultant moment of any two of them is equal in magnitude but opposite in direction to the moment due to the third one. So, the molecule's net dipole moment is zero, and it is non-polar.}\n\n\text{The net dipole moment is zero, hence, the molecule is non-polar.}\n\n\text{The structure of } B_3N_3H_6 \text{ is as follows:}\n\n\text{Borazine is a highly polar molecule because of the difference in electronegativity between nitrogen (3.04) and boron (2.04). In borazine, uneven distribution of charges between each nitrogen-boron bond occurs.}\n\n\text{This makes nitrogen partially negative and boron partially positive, and due to charge separation between nitrogen and boron, the } B_3N_3H_6 \text{ is non-polar.}\n\n\text{Therefore, } B_3N_3H_6 \text{ is not a perfect nonpolar molecule.}