1. C. Johannesson Quantum Model of the Atom Unit 10: Electrons in Atoms

2. C. Johannesson A. Electrons as Waves zLouis de Broglie (1924) yApplied wave-particle theory to e - ye - exhibit wave properties QUANTIZED WAVELENGTHS

3. C. Johannesson A. Electrons as Waves QUANTIZED WAVELENGTHS

4. C. Johannesson A. Electrons as Waves EVIDENCE: DIFFRACTION PATTERNS ELECTRONS VISIBLE LIGHT

5. C. Johannesson B. Quantum Mechanics zHeisenberg Uncertainty Principle yImpossible to know both the velocity and position of an electron at the same time

6. C. Johannesson B. Quantum Mechanics zSchrödinger Wave Equation (1926) yfinite # of solutions  quantized energy levels ydefines probability of finding an e -

7. C. Johannesson B. Quantum Mechanics Radial Distribution Curve Orbital zOrbital (“electron cloud”) yRegion in space where there is 90% probability of finding an e -

8. C. Johannesson C. Quantum Numbers UPPER LEVEL zFour Quantum Numbers: ySpecify the “address” of each electron in an atom  The periodic table is actually a map (or seating chart) for electrons.

9. C. Quantum Numbers zElectron “address” LPHS 10189 N 4800 W Highland, UT 84003 yPeople use:  State  City  Street  House # yElectrons use:  Energy level  Sublevel  Orbital  Spin

10. C. Johannesson C. Quantum Numbers 1. Principal Quantum Number ( n ) yEnergy level ySize of the orbital yn 2 = # of orbitals in the energy level

11. C. Johannesson C. Quantum Numbers 1. Principal Quantum Number ( n ) yRanges from 1   yPeriodic table: Row yEach block is numbered SEPARATELY.

12. C. Quantum Numbers

13. s p d f 2. Azimuthal or Angular Momentum Quantum # ( l ) yEnergy sublevel yShape of the orbital

14. C. Quantum Numbers s p d f 2. Azimuthal or Angular Momentum Quantum # ( l ) yRange: 0  n-1 yPeriodic table: block l = 0 l = 1 l = 2 l = 3

15. C. Quantum Numbers ? ? ? ?

16. C. Johannesson C. Quantum Numbers 3. Magnetic Quantum Number ( m l ) yOrientation of orbital  Specifies the exact orbital within each sublevel

17. C. Johannesson C. Quantum Numbers 3. Magnetic Quantum Number ( m l )  Range: -l  +l  For the d-block, l = 2  m l = -2  +2 0 12-2

18. C. Quantum Numbers Important factoids: m l is pronounced “em-sub-el” The orbital numbers (-1, 0, +1, etc.) are NOT permanently assigned to specific orientations, i.e., it doesn’t matter which picture you put “-2” on.

19. C. Quantum Numbers pxpx pypy pzpz p = 1  m l = -1 0 +1

20. C. Johannesson C. Quantum Numbers zOrbitals combine to form a spherical shape. 2s 2p z 2p y 2p x

21. C. Quantum Numbers zn=# of sublevels per level zn 2 =# of orbitals per level z# orbitals per sublevel: 1 s, 3 p, 5 d, 7 f

22. C. Johannesson C. Quantum Numbers 4. Spin Quantum Number ( m s ) yElectron spin  +½ or -½ yAn orbital can hold 2 electrons that spin in opposite directions.

23. C. Johannesson C. Quantum Numbers 1. Principal #  2. Azim (Ang. Mom.) #  3. Magnetic #  4. Spin #  energy level sublevel (s,p,d,f) orbital electron zPauli Exclusion Principle yNo two electrons in an atom can have the same 4 quantum numbers. yEach e - has a unique “address”: