select the molecules that are polar.\n□ iof₅\n□ cf₄\n□ ch₂cl₂\n□ asf₃

select the molecules that are polar.\n□ iof₅\n□ cf₄\n□ ch₂cl₂\n□ asf₃

select the molecules that are polar.\n□ iof₅\n□ cf₄\n□ ch₂cl₂\n□ asf₃

Answer

Explanation:

Step1: Analyze $IOF_5$

$IOF_5$ has a square - pyramidal molecular geometry. The central iodine atom has a lone pair and five bonding pairs. The bond dipoles do not cancel out due to the asymmetric shape, so it is polar.

Step2: Analyze $CF_4$

$CF_4$ has a tetrahedral molecular geometry. The four C - F bonds are symmetrically arranged around the central carbon atom, and the bond dipoles cancel each other out, making it non - polar.

Step3: Analyze $CH_2Cl_2$

$CH_2Cl_2$ has a tetrahedral molecular geometry. But due to the difference in electronegativity between C - H and C - Cl bonds and the non - symmetric arrangement of the atoms, the bond dipoles do not cancel out, so it is polar.

Step4: Analyze $AsF_3$

$AsF_3$ has a trigonal - pyramidal molecular geometry. The central arsenic atom has a lone pair and three bonding pairs. The bond dipoles do not cancel out because of the asymmetric shape, so it is polar.

Answer:

IOF₅, CH₂Cl₂, AsF₃