Determine the electron geometry (eg), molecular geometry (mg), and polarity of HBrO₂. A) eg = trigonal bipyramidal, mg = trigonal planar, nonpolar B) eg = octahedral, mg = square planar, nonpolar C) eg = tetrahedral, mg = bent, polar D) eg = tetrahedral, mg = linear, nonpolar E) eg = linear, mg = linear, polar

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First, we need to draw the Lewis structure of the molecule:

H-Br-O-SB12US1B0

Based on the Lewis structure, we can determine the electron geometry (eg) by counting the number of regions of electron density around the central atom, which is S in this case. There are four regions around S, including two lone pairs and two bonding pairs. This leads to a tetrahedral electron geometry.

Next, we can determine the molecular geometry (mg) by looking only at the positions of the atoms (i.e. ignoring the lone pairs). In this case, the two bonding pairs are arranged in a bent shape because of the two lone pairs pushing the bonding pairs closer together. Hence, the molecular geometry is bent.

Finally, we can determine the polarity of the molecule by looking at the electronegativities of the atoms involved. In this case, Br and O are more electronegative than S, so the bonds between S-Br and S-O are polar, and the molecule has a net dipole moment, making it polar.

Determine the Electron Geometry (Eg), Molecular Geometry (Mg), and Polarity