Chemical Bonding Flashcards
Hypovalent elements
Be, B, Al
Hypervalent elements
(More than octet)
P S Cl
As Se Br
VSEPR Theory made by
Nylholm and Gillespie
Order of bond pairs / lone pairs
LP—LP > BP—LP > BP—BP
most least
If outer atoms are more EN, bond angle will
Decrease
Linear sp (180º) examples
BeCl2, CO2, HgCl2, CS2, NO2+
Bent angular (120º) sp2 examples
SO2, NO2, O3, SnCl2, GeCl2
Bent/ V-shape (104-109º) sp3 examples
H2O, H2S, H2Se, H2Te
F2O, Cl2O, Br2O, I2O
Trigonal planar
AB3 120º sp2
Trigonal planar examples
AlCl3, BrF3, SO3, CH3+, CO3 2-, NO3-
Trigonal pyramidal
AB3 (107-109º) sp3
Trigonal pyramidal examples
NH3, PH3, AsH3, SbH3, BiH3, H3O+
Tetrahedral
AB4 (109º) sp3
Tetrahedral examples
CH4, SiH4, PbH4, CCl4, SiCl4, GeCl4, SO4 -2, PO4 -3
AB5 AB6 AB7 AB8
AB5 = Trigonal bipyramidal (e.g. PCl5)
AB6 = Square planar bipyramidal (e.g. SF6, SeCl6)
AB7 = Pentagonal bipyramidal (e.g. IF7)
AB8 = Hexagonal bipyramidal
s—s bond has
p—p bond has
s—s bond has free rotation
p—p bond has limited rotation