University:
University of Virginia
Course:
CHEM 2410 | Organic Chemistry I
Academic year:

2024
Views:

88

Pages:

3
Author:

Kayli N.

8/29 textbook Wavefunction Y : corresponds · 1 7-1 . Ye , orbital is of region a for energy level to ↳ energy · 14 Yy -probability in an atom electron . occupied orbital = batomic only can of space cloud is [A0] at discrete - / - organic H, C N , - ,0 ↳ orbital Is 3 · charge & Is lowest In -electrons · s p , , are equal Parli ex Principle : . Carbon -1 - 1 ↳ 1522s2 zp2 lowest 2 25 25 , 3 energy in

- py energy Principle : degenerative Rule : , 2 IS Exclusion Hand's dese electron G O Aufbar density & further from nucleus : Y 1s level d ,f represents - closet to nucleus has I node 2ps particular location 4- electrical NOT in density ↓ 4 energy electron by delectron + 4 an electron Mantized occupied of electron Orbital finding electron exist the electron of [PJ is hold can , 2pz pX filled first max . 1 electron 2 electrons is 11 w/ opposite spin placed then paired up Nature of atomic orbital overlap Interference of Constructive electrons ampitude waves > - & 8 - Wavesarce A closer each < - constructive other Interference Distance Deconstructive Interference ~ orbital theory electrons 2 . Intermolecular undecular bigger MI . theory & waves like are Valence bond by explained : waves cancel ~ closer waves T Cancel = Nop out Destructive interference Valence Bond theory Interference of constructive ex is the Axis line : blu · · atomic orbital orbital : region Molecular orbital I : of : on the ↳ molecular I bond axis circular symmetryw/ respect are sigma bond axis bonds 1 in atom e same rules for occupying when Mo · destructive interference ↳ has a node-higher energy constructive Mo interference ↳NO Nodes occupied molecular [lowest orbitals they : I energy] = lower energy orbital (highest energy] waves overlap cease to exist replaced by molecular · from lowest = to single bonds entire molecule Oronding LOMO space to HOMO : highest atoms as a result theory CMOJ fantibonding & i 2 orbitals NODE . M ex energy overlap of 1s atomic density located all blu orbitals 2 atoms · Molecular sharing of their atomic electron : density of electron + SigmaObond Bond bond : 2 orbitals Excited State hybrized eX , : electrons in "used orbitals : to lower the satify excited up to are energies of bonding F orbitals/geometry * brizedmoreente ↳ # IS Increased strain from sp2-hybridized Atomic assymetrical bond angles small - less stable and more reactive orbitals · I , ex ↑ - 2p ↓ 113 degenerate sp2 > - hybridize ↳ pi(TT) bond : & when p overlap Node - triple bond orbitals formed by overlap from & carbon 1 shows interaction/ibond] Mo higher energy sp-hybrized : 1 o antibonding ( # Antibonding bonding MG 1 bond orbitals single bond a bonding 1 1bond to bonds cyclopropane , double bond -> p-orbitals form IS TI energy2s2 at aerative Let energy · higher hydrogen doesn't hybridize : only has s orbital atoms I·bridize ↑ - Sigma (6) bonds formed ↳ overlap of sp orbitals eX trick : = bonds - , 1 hybridization sp3 & 2 Sp3 # bonds Roverlap of MEC p orbitals ↑ - - H a = - I ↑ Sp2 Sp3 Sp => dreto- CE of bonding Interactions Stronger > - sp