Chem I Day IX

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Chem I Day IX

  1. 1. Welcome to Chemistry I – Day IXPortland Evening ScholarsMr. Treothe Bullock - Instructor Unit 3 - Work which should becompleted – ready for questionsand review Chapter 3 Review We will sign off on andgo over Math Take Home Test - 1stproblem set done – we willcontinue 1stproblem signoffs Minimum of 1 Radioactivity orHalf Life labs – Recovery contract work -turn in as done Unit 3 - Chapter 4 – Arrangementof the electrons in the atom Emission Spectrum Lab –how have models changed? Equations of Light &Electromagnetic Energy Quantum numbers & ElectronConfigurations Forgotten Genius Project –Science & Society Homework for next week Complete Chapter 4 review Complete Orbital Diagrams Recovery Completions
  2. 2. Mathematical Philosophy inChemistry’s Quantum Model The Heisenberg UncertaintyPrinciple Werner Heisenberg “It is impossible to determinesimultaneously both the positionand velocity of an electron orparticle.” Schrödinger Wave Equation Solutions to this equation are knownas wave functions. Based on theHeisenberg uncertainty principlequantum theory determined that wavefunctions give only the probability offinding an electron at a given placearound the nucleus Electron are located in 3 dimensionalprobability clouds or orbitals centeredaround the nucleus. Erwin Schrödinger
  3. 3. Old atomic modelQuantum atomicmodel
  4. 4. Quantum numbers – specify the properties ofatomic orbitals and the properties of electronsin the orbitals Quantum theory describesmathematically the waveproperties of electrons and othervery small particles. Principal Quantum Number –symbolized by n, indicates themain energy level occupied by theelectron Total number of orbitals at a levelis n2 Angular Momentum QuantumNumber – At all but the firstsublevel multiple orbital shapesexist. Angular momentumquantum number symbolized by lindicates the shape of the orbital s, spherical p, dumbbell d, four are double dumbbell one isa donut around a dumbbell shape f etc. correspond to l levels 0,1,2,3
  5. 5. Quantum numbers Magnetic QuantumNumber – symbolized bym, indicates theorientation of an orbitalaround the nucleus s m=0 p m=-1,0 or +1 d m= -2,-1,0,+1,+2 Etc. Spin Quantum Number –has only two possiblevalues +1/2 , -1/2 whichindicate the twofundamental spin states ofan electron in an orbital

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