Common Molecular Shapes
{"Image DocumentName": "Common Molecular Shapes", "Image ImageDescription": "6 total. 6 bond. 0 lone. B. A. SF6. In some cases, the location of lone pairs is important. AB4: SF4. Step 1 \u2014 S atom has six valence electrons and each F has seven. Step 2 \u2014 there are five electron pairs around S; electron-pair geometry is trigonal bipyramidal. Step 3 \u2014 there are five electron pairs but only four bonded F atoms; there must be one lone pair. Step 4 \u2014 in a trigonal bipyramid, the five positions are not equivalent; there are three equatorial positions separated 120\u00ba from one another and two axial positions at 90\u00ba to the equatorial plane. \u2013 The lone electron pair can be placed in either the axial or equatorial position; must choose structure that minimizes electrostatic repulsions: most stable structure is equatorial position and molecular geometry is seesaw. OCTAHEDRAL. 90\u00b0 Courtesy Christy Johannesson", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}