Determine the electron geometry (eg) and molecular geometry (mg) of BrF₅. A) eg = octahedral, mg = square pyramidal B) eg = linear, mg = trigonal planar C) eg = trigonal planar, mg = bent D) eg = linear, mg = linear E) eg = tetrahedral, mg = trigonal pyramidal

Question

Quizplus · Accepted Answer

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

Br (central atom) - F - S - U1B15 - S - U1B0

Counting the total number of valence electrons, we have:
Br: 7
F: 7 x 1 = 7
S: 6
U1B15: 5 x 15 = 75
U1B0: 5 x 0 = 0

Total: 95 valence electrons

Using the octet rule, we can distribute the electrons:

Br:

F: :Br: :S: U1B15: :S: U1B0:

Now, we need to determine the electron geometry by looking at the arrangement of electron groups around the central atom. In this case, there are six electron groups (one from each atom bonded to the central Br atom, plus two lone pairs on the Br atom). This gives an octahedral electron geometry.

Next, we need to determine the molecular geometry by looking at the arrangement of atoms around the central atom. In this case, we have one lone pair and five bonded atoms. The four equatorial positions are occupied by four fluorine atoms, which gives a square planar arrangement. The lone pair occupies one of the axial positions, resulting in a square pyramidal molecular geometry. Therefore, the correct answer is A: eg = octahedral, mg = square pyramidal.

Determine the Electron Geometry (Eg) and Molecular Geometry (Mg) of BrF5

Determine the Electron Geometry (Eg) and Molecular Geometry (Mg) of BrF₅