Question

determine whether each molecule is polar or nonpolar.
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sicl₄ ch₂f₂ sef₆
nonpolar
polar

Explanation:

Step1: Analyze SiCl₄

SiCl₄ has a tetrahedral geometry. The Si - Cl bonds are polar, but due to the symmetric tetrahedral shape, the bond dipoles cancel out. So SiCl₄ is nonpolar.

Step2: Analyze SeF₆

SeF₆ has an octahedral geometry. The Se - F bonds are polar, but the symmetric octahedral arrangement makes the bond dipoles cancel. Thus, SeF₆ is nonpolar.

Step3: Analyze CH₂F₂

CH₂F₂ has a tetrahedral geometry, but the H and F atoms have different electronegativities. The bond dipoles (C - H and C - F) do not cancel out due to the asymmetric distribution of H and F. So CH₂F₂ is polar.

Answer:

Nonpolar: SiCl₄, SeF₆
Polar: CH₂F₂