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?

Verified step by step guidance

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.