What is the molecular geometry of BrF5, and how can it be sketched using the bond conventions shown in 'Representing Molecular Geometries on Paper' in Section 10.4?

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1. <Determine the total number of valence electrons in BrF_5. Bromine (Br) has 7 valence electrons, and each fluorine (F) has 7 valence electrons. Calculate the total for BrF_5.>
2. <Draw the Lewis structure for BrF_5. Place Br in the center and arrange the 5 F atoms around it, using single bonds. Distribute the remaining electrons to satisfy the octet rule for each F atom.>
3. <Identify the electron pair geometry. BrF_5 has 6 regions of electron density (5 bonding pairs and 1 lone pair), which corresponds to an octahedral electron pair geometry.>
4. <Determine the molecular geometry. With one lone pair, the molecular geometry of BrF_5 is square pyramidal.>
5. <Sketch the molecular geometry using bond conventions. Represent the square pyramidal shape with Br at the center, 4 F atoms forming a square plane, and the 5th F atom above the plane. Use solid lines for bonds in the plane, a wedge for the bond coming out of the plane, and a dashed line for the bond going into the plane.>