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

2024
Views:

195

Pages:

2
Author:

Kayli N.

912 lecture nonpolar bonds covalent Delectronegativity covalent bonds polar <0 5 0 57x . >1 . . 75 4) larger need more energy to + 9- - electronegativity Lonic ⑦ difference > 1 7 . strong Interaction , break easily broze but forces weater intermolecular even if Bonds electrons closer to nucleus = same higher ↳ Degenerate : sphere snape bigger = & further from constructive Interference z reds blues DeconstructiveInterference I red if if 1 blue + electrons z if too close, - creates more they togther node start to repel # of p ⑲ bonds ble lower (must are orbitals have presence 2 H different ways into 1 delocialized rotate to each pi higher ↓ a interact higher orbitals bond) [ other > no overlap CHOMO]fills & delocalize 1 breaking pibond) single bonds J frontiera coMoccupied Deconstructive - energy molecular orbital them density of (just sigma bonds highest occupied of electron have to H weater than H- there'sNo interaction bin of free rotating breaks the bond blc it's double Not rotationally symmetrical pi but double bonds are stronger than Perpendicular independent are change bond is ↳ equally shared rotate sphere, 1 and 1 - triple bond-1 and 2 localized electrons 2 that s-orbitals = XX · interaction to other result doesn't orbitals L pi stablizing , bonds have rotational symmetry have without ⑨ D # energy be same phase D 1 in ↑ pi It bond-overlap must interchanged be can antibonding if orbital · blue/red or is # banding single-bond can't bonding of CSorbits overlap molecular orbital - plays role each yd p- orbitals the reduction in -> · valeare ,of theory I larger ampitude - or I geometry D sex if same shape level energy same different but nucleus D & if p-orbitals Atomic orbitals s orbitals - negative more lowest , ·antibondingorbia lower energy orbital first of opposite spins energy difference of 000 1 > - occupied-occupied light energy, orbital it can absorb it to release , absorb , or glow of banding constructive matches light/heat (colors) eX - H -X &worePronegative H ⑰ Is orbital & Antibonding orbital F + - Not larger (defficient on less electronegative orbitals 2 p real of = sp3 orbital explain yeometry to - ↑ the al space on LUMO interacts lower · Bonding Orbital more (SN) Steric Number ↳ # E OLP tetrahedral ILP Sp ↓ density coefficient H electronegativity - it c =C and (VSEPR) + PLPL 21P bent SN = bent 1 = N hybridized o LP linear 2 Hzc 2 sp ↓ ILP planar - Sigma bonds steric I lone pairs ~ CH3 Sigma o I H o is D. 3 X - beut bond #3 sp2 & 2 pi it bonds H hybrid & Sp2 and Double bond : = frigonal trigadial H Trigonal # of lone pairs SN Trigonal planar sp2 linearsp density electron sp3 * due to 4 Y electron 1 Sigma bonds = higher higher of SN # #[H tetrahedral by giving electrons on the It W/ energy larger X on on another Molecule In H It Pyramdial lone It pair

Chemical Bonding, Hybridization, and Molecular Geometry

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