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Kevin Mospan and Elizabeth Schultz Unit 6 Review Atomic and Molecular Structure Lewis structures- know how to draw the dot structures Molecular shapes oDifferent shape names/molecular geometry oBond angles (See Molecular orbital theory –other side) Formal charge oFormal charge closer to 0 is favorable Bond polarity oDifference in electronegativity 0.4<x<1.7 2 Molecular polarity oSymmetrical bonds cancel Electromagnetic radiation o. = c = 2.99792458 x 108 m/s oElectromagnetic spectrum Energy quantization oPlanck oE=h. (h≈6.6260755x10-34 J.s) Photoelectric effect oWhen light strikes the surface of a metal and e- are ejected oE=h.c/ Bohr model oRadius of the circular orbits increase as n increases oAn atom with its e- in the lowest possible energy levels is said to be in its “ground state” oWhen an e- occupies an orbit greater than the lowest possible energy level it is said to be in an “excited state” oΔE=-Rhc(1/nf2 - 1/ni2) Rhc=1312 kJ/mol Wave/particle duality oTaken from idea that light, usually considered to exhibit wave properties, actually consists of particles (photons) oSimilarly, massless particle, e-, can exhibit both particle and wave properties DeBroglie wavelength Value of l o=h/m. Corresponding subshell oh=Planck’s constant label om=mass (kg) 0 s o=velocity (m/s) Quantum #s 1 p on=principal quantum # 2 d integers from 1- ol=angular momentum quantum # 3 f characterizes subshell of orbital starts at 0 and goes to n-1 om l =magnetic quantum # 0, 1, 2,…, l # of values of ml for a given subshell is 2 l +1 oms= electron spin magnetic quantum# ½ Orbitals os, p, d, f (…) obattleship/revised periodic table method os has 1 orbital op has 3 orbitals od has 5 orbitals of has 7 orbitals Quantum numbers for electron configurations oDiamagnetic means not magnetic (diametrically opposed) oParamagnetic means exhibits magnetism caused by unpaired eoPauli exclusion principle: no two e- can have the same set of 4 quantum numbers (only two e- per box) Electron configurations of atoms and ions oHund’s rule: the most stable arrangement of e- is that with the maximum number of unpaired eoNoble gas notation oHalf filled orbitals are stable Atomic and chemical periodic trends (arrows indicate increase for all) oRadius ↓ ← oElectronegativity ↑ → oIonization energy ↑ → Valence bond theory oHybridization Bond angles oSigma and pi bonds oSigma bond necessary for a pi bond to occur Molecular orbital theory oBond order = ½( #e- in bonding MOs - #e- in antibonding MOs) oAnti-bonding –principle of molecular orbital theory that isn’t in valence bond theory, antibonding orbital are higher in energy than bonding orbitals