SeF6 is not a polar compound. The SeF6 molecule possesses an octahedral coordination symmetry, and the net dipole moment due to the six polar Se-F bonds is zero, despite the fact that the Se-F bond is polar.
A net dipole moment exists in a polar molecule. To establish whether a molecule is polar, first apply the valence shell electron pair repulsion laws to calculate the molecule’s three-dimensional geometry. The net dipole moment attributable to the molecule’s polar bonds should then be determined. On their two ends, these bonds frequently have atoms with varying electronegativities. Selenium, for example, has an electronegativity of approximately 2.55, whereas fluorine has an electronegativity of approximately 3.98.
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