Describe how the bond angles in TeF4 and BrF5 deviate from those found in a trigonal bipyramidal and an octahedron, respectively. In TeF4, the lone pair of electrons repels the Te-F bonding pairs, causing the F-Te-F angles to be smaller than v in the ideal trigonal bipyramid. In BRF5, the lone pair is located perpendicular v to the plane of four of the F atoms, giving a square pyramid geometry to the molecule. The angle between the four F in the plane and the F above the plane will be less than v 90° due to lone pair repulsion. The F-Br-F angles in the plane will remain i

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