Molecular Orbital Theory electrons as waves constructive ~ ~ + + t + N = = MO ° the electron whenever is between it favors in t ← F- e ← - - e → t net → F force = attractive F destructive ✓ + favors bonding , ← F \ bonding , F F → , = " ' - + t - anti = . E + e- ← F example : F F → ← → OH F does - Ha + HB Ho not - electrons are favor bonding low energy t exothermic Ha as \ Isa bonding e- anti - , BE ABO 2- bonding = = = I usually single SB bonding Gs - Bond order bonding l Jeasytogodon.nl 11 - releases energy as they form a bond ' - e - HB anti l MO \ node high Ha bonding outside H, = - . . F e- + → , , bond MO MO example - Hz : Ha - Ha - HB Bond order 1 ✓ 2 electrons for H = = 'T - ÷ ISB ISA Gio :* n , - Els example : He , Hez He He Bond order ff Qs* ' . . 2 = = o ✓ no bond so this molecule does not exist ! It 11 IS IS 11 oisoistx o IS example : Liz Liz L; L; L; - → - %* I as ) 71 → / 1 q; u 25 Li 25 IS Li BO = ' Is electrons do not 25 ( l = participate orbitals would overlap orbital ) Is 025 IS only Is Is I Zpx 2Pa spy in # - €p- - , ,§" phase Ozp = t thigh probability ' . out of side - phase At + side %* node constructive a = . destructive + head - If Thp* = head overlap T2px - z bonding I = overlap + . 02ps , Tlzpx Tlzpy , : - anti - bonding