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CC’ % Notes HH KE’ 2 VSEPR Theory ~ (Valence-shell electron pair repulsion theory): the repulsion between the valence electron pairs surrounding an atom cause these pairs to be oriented as far apart as possible. Hybridization = the mixing of a set of atomic orbitals on an atom to form a new set of hybrid orbitals with the same total electron capacity ahd with properties and energies intermediate between those of the original unhybridized orbitals. These hybrid orbitals are then able to overlap with other atoms orbitals to create a covalent fF % v 3, spd) Example of canoe 1 11 ¢ 1s94c2* aye (rll) > btn C $ CPA Ve Qs He H ybridi 2ation ye : Because of VSPER and hybridizatior| covalent compounds take on different shapes. be Table 6-5 page 186 of Formula Dot Structure | Ball and Stick | # of Atoms Shape and Bond(s) # of Unshared | Polarity of | Hybridization # of # of pi Model Bonded to Bond Angle EN electrons on Molecule | on Central | sigma bonds Central Atom Differerice | Central Atom (Polar or . bonds Nonpolar) [atom (sides) v feet = 0.4 Yi o—#: Linear . Hcl fc) ne Ny A igo’ |i Singles | yy | a Pola | 0 H-cl i Pole C N/A : H-o-L4 | Y sides | lone 3 ’ Bent or : - 2 Si le, a wd - 5 Angular ngley per? = ola 5 = <109.5° | Pator coy, ly Fe v p c-0=1.0 35+dey Trigonal | c-ci=0.5 O 7 | M Planar | de.ble, PC a Volar | 5 P | = 120 4. single, PC — 7 C-teoY gt Z ‘ Tetrahedral | |, . 4 Lt 109.5° 4 Single, O = Nonpel 5p Lt O ee Polar Cc = Trigonal 4 ides Pyramidal = 3 4 <109.5° | pe Ye Polar S P So O 
