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Quantum numbers
- 2. The Major Players • Werner Heisenberg • Heisenberg Uncertainty Principle • Electron Density • Erwin Schrödinger • Wave functions (Ψ) • Atomic Orbital • Quantum Numbers
- 3. Werner Heisenberg • Tried to locate a subatomic particle that behaves like a wave.
- 4. Heisenberg Uncertainty Principle It is Impossible to know the exact momentum and position of a particle with any certainty.
- 5. Electron Density • Gives the probability of finding an electron in a particular region of an atom
- 6. Erwin Schrodinger • Created wave functions
- 7. Wave Functions Complicated mathematical expressions used to describe the probability of finding an electron around a nucleus.
- 8. Radial Distribution CurveOrbital Orbital (“electron cloud”) –Region in space where there is 90% probability of finding an e-
- 9. Quantum Numbers -zip codes for electrons- 4 Types of Quantum #s 1. Principal (n) • Distance from nucleus 2. Angular Momentum (l) • Orbital Shape 3. Magnetic (ml) • Orientation in space 4. Spin (ms) • Rotational Spin
- 10. PRINCIPAL QUANTUM NUMBER (n) Energy level / shell Size of the orbital n2 = # of orbitals in the energy level
- 11. Angular Momentum / Azimuthal (l) s p d f Energy sublevel / subshell Shape of the orbital
- 12. MAGNETIC (ml) Orientation of orbital Specifies the exact orbital within each sublevel px p pz
- 14. SPIN (ms) Electron spin ⇒ +½ or -½ –An orbital can hold 2 electrons that spin in opposite directions.
- 15. Quantum Numbers -zip codes for electrons- 4 Types of Quantum #s 1. Principal (n) • Distance from nucleus 2. Angular Momentum (l) • Orbital Shape 3. Magnetic (ml) • Orientation in space 4. Spin (ms) • Rotational Spin
- 16. • n = # of sublevels per level • n2 = # of orbitals per level • Sublevel sets: 1 s, 3 p, 5 d, 7 f
- 17. • Orbitals combine to form a spherical shape, which defines the “electron cloud.” 2s 2pz 2py 2px
- 18. Let’s see how it works.
- 19. Questions How many orbitals are in the following sublevels? 3p 2s 4p 3d 4f 3: px, py, pz 1: s 3: px, py, pz 5: dxy, dyz, dxz, dx2-y2, dz2 7: Don’t worry, just know it
- 20. Questions How many sublevels are contained in each of the following energy levels? n = 1 n = 2 n = 3 n = 4 1, the s sublevel 2, the s and p sublevels 3, the s, p, and d sublevels 4, the s, p, d, and f sublevels
- 21. Questions What is the maximum number of electrons that can go into each of the following sublevels? 4s 3p 4s 3d 4p 5s 4f 5p 2e- 6e- 2e- 10e- 6e- 2e- 14e- 6e-
Notas del editor
- Werner Heisenberg – tried to locate a subatomic particle that behaves like a wave (Particle Duality). He formulated. . . . Heisenberg Uncertainty Principle – it is impossible to know simultaneously both the momentum (p = mass *velocity) and position of a particle with any certainty. Although you don’t know exactly where a wave is, you can explain where you are most likely to find it. Electron Density – defines the probability of finding an electron in a particular region of an atom. Erwin Schrödinger – Used complicated math, taking equations from wave motion and particle motion to create wave functions () Wave functions () are used to describe the probability of finding an electron around a nucleus. Atomic orbital – the wave function of an electron in an atom. This idea gave birth to quantum numbers:
- Quantum numbers – describe the distribution of electrons in atoms. There are four 1. Principal (n) 2. Angular Momentum (l) 3. Magnetic (ml) Spin (ms) n – describes electron’s distance from the nucleus (as n increases, the e- moves further from the nucleus) l – describes orbital shape 0 = s 1 = p 2 = d 3 = f 4 = g ml – describes orientation of orbital in space what plane: X,Y,orZ ms – describes rotational spin
- Expressed as whole value starting at +1 Describes an electron’s distance from the nucleus Boundary surface diagram – encloses 90% of the total electron density in an orbital
- Possible value = (n-1) Describes orbital shape.
- Describes orientation of orbital in space. That is, what plane: X,Y,Z
- Quantum numbers – describe the distribution of electrons in atoms. There are four 1. Principal (n) 2. Angular Momentum (l) 3. Magnetic (ml) Spin (ms) n – describes electron’s distance from the nucleus (as n increases, the e- moves further from the nucleus) l – describes orbital shape 0 = s 1 = p 2 = d 3 = f 4 = g ml – describes orientation of orbital in space what plane: X,Y,orZ ms – describes rotational spin