The molecular size of $ICl$ and $Br_2$ is approximately the same,but the $b.p.$ of $ICl$ is about $40 \ ^oC$ higher than that of $Br_2$. This is because:

Carbon tetrachloride has no net dipole moment because of

Which of the following orders of dipole moment for the stated molecules is correct?

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

Each of the following options contains a set of four molecules. Identify the option$(s)$ where all four molecules possess a permanent dipole moment at room temperature.
$(1)$ $BeCl_2, CO_2, BCl_3, CHCl_3$
$(2)$ $SO_2, C_6H_5Cl, H_2Se, BrF_5$
$(3)$ $BF_3, O_3, SF_6, XeF_6$
$(4)$ $NO_2, NH_3, POCl_3, CH_3Cl$

Which of the following is the correct order of dipole moment for the given molecules?