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<table bgcolor=beige border=2> <tr> <th colspan=8 align=center>VSPER & Geometry Table</th> <tr> <tr> <th> #pairs of electron around central atom</th> <th># lone pair on central atom</th> <th>#single bonds </th> <th>Hybrid.</th> <th>Formula </th> <th>Name of shape</th> <th>Bond angle</th> <tr> <tr> <th> 2 </th> <th>0 </th> <th>2 </th> <th>sp</th> <th>YX<sub>2</sub> </th> <th>Linear</th> <th>180</th> <tr> <tr> <th> 3 </th> <th>0 </th> <th>3 </th> <th>sp<sup>2</sup></th> <th>YX<sub>3</sub> </th> <th>Trigonal planar</th> <th>120</th> <tr> <tr> <th> 4 </th> <th>0 </th> <th>4 </th> <th>sp<sup>3</sup></th> <th>Y X<sub>4</sub> </th> <th>Tetrahedral</th> <th>109.5</th> <tr> <tr> <th> 4 </th> <th>1 </th> <th>3 </th> <th>sp<sup>3</sup></th> <th>Y X<sub>3</sub> </th> <th>Pyramidal </th> <th>107.0</th> <tr> <tr> <th> 4 </th> <th>2 </th> <th>2 </th> <th>sp<sup>3</sup></th> <th>Y X<sub>2</sub> </th> <th>Bent</th> <th>104.5</th> <tr> <tr> <th> 5 </th> <th>0 </th> <th>5 </th> <th>dsp<sup>3</sup></th> <th>Y X<sub>5</sub> </th> <th>Trigonal bipyramidal</th> <th>90, 120</th> <tr> <tr> <th> 6 </th> <th>0 </th> <th>6 </th> <th>d<sup>2</sup>sp<sup>3</sup></th> <th>Y X<sub>6</sub> </th> <th>Octahedral</th> <th>90,90</th> <tr> </table> <tr> '''Notes: ''' #Two atoms bonding will always give linear geometry #Hybridization is only on the central atom. #All compounds with multiple bonds (i.e. double bonds) have a planar geometry #C,N,O,F (sometime P,S,Cl) are the most common elements that form multiple bonds #Compounds that have the potential to have d-orbitals (this excludes C,N,O,F) can exceed the Octet Rule/ Rule of 8. #For compounds w/elements in 3rd energy (row) and higher, look for Lewis Dot Structure with single bonding first before more complex structure w/double bonds. #The simple way of determining the Hybridization on the Central atom: ##Add up the number of outside atoms that central atom is bonding with. ##Add up the number of lone pairs on central atom ##Add together to get number. ##This number is number of Hybridized orbital *Example CH<sub>4</sub> **Central atom is bonded to 4 outside atoms and no lone pair so hybridization is sp<sup>3</sup> where there are 4 of them.
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