Quantum Model of the Atom Electrons in Atoms. A. Electrons as Waves zLouis de Broglie (1924) yApplied wave-particle theory to e - ye - exhibit wave properties.

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<ul><li><p>Quantum Model of the Atom</p><p>Electrons in Atoms</p><p>C. Johannesson</p></li><li><p>A. Electrons as WavesLouis de Broglie (1924)Applied wave-particle theory to e-e- exhibit wave propertiesQUANTIZED WAVELENGTHS</p></li><li><p>A. Electrons as WavesQUANTIZED WAVELENGTHS</p></li><li><p>A. Electrons as WavesEVIDENCE: DIFFRACTION PATTERNS</p></li><li><p>B. Quantum MechanicsHeisenberg Uncertainty PrincipleImpossible to know both the velocity and position of an electron at the same time</p></li><li><p>B. Quantum MechanicsSchrdinger Wave Equation (1926)finite # of solutions quantized energy levelsdefines probability of finding an e-</p></li><li><p>B. Quantum MechanicsOrbital (electron cloud)Region in space where there is 90% probability of finding an e-</p></li><li><p>C. Quantum NumbersFour Quantum Numbers:Specify the address of each electron in an atom</p></li><li><p>C. Quantum Numbers1. Principal Quantum Number ( n )Energy levelSize of the orbitaln2 = # of orbitals in the energy level</p></li><li><p>C. Quantum Numbers2. Angular Momentum Quantum # ( l )Energy sublevelShape of the orbital</p></li><li><p>C. Quantum Numbersn=# of sublevels per leveln2=# of orbitals per levelSublevel sets: 1 s, 3 p, 5 d, 7 f</p></li><li><p>C. Quantum Numbers3. Magnetic Quantum Number ( ml )Orientation of orbitalSpecifies the exact orbital within each sublevel</p></li><li><p>C. Quantum Numberspxpypz</p></li><li><p>C. Quantum NumbersOrbitals combine to form a spherical shape.</p></li><li><p>C. Quantum Numbers4. Spin Quantum Number ( ms )Electron spin + or -An orbital can hold 2 electrons that spin in opposite directions.</p></li><li><p>C. Quantum Numbers1. Principal #2. Ang. Mom. #3. Magnetic #4. Spin #energy levelsublevel (s,p,d,f)orbitalelectronPauli Exclusion PrincipleNo two electrons in an atom can have the same 4 quantum numbers.Each e- has a unique address:</p></li><li><p>Feeling overwhelmed?Read Section 4-2!</p><p>*</p></li></ul>

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