# Chapter 7 Lecture Outline

## 7.2 The Nature of Light

1. The wave model of light ( Internet © Saunders, 1997) Figure 7.1 & 7.2
1. Wave model of light ([lambda]*v = c)
2. [lambda] = wavelength (meter, nm, etc.)
3. v = frequency (Hz or sec-1)
4. c = speed of light (3.0 * 108 m sec-1)

2. Planck, Blackbody Radiation & the Particle model of light ( Internet © Saunders, 1997)
1. E = hv
2. E = energy of a single photon
3. h = Planck's Constant (6.6 * 10-34 J s per photon)
4. v = frequency (Hz or sec-1)

3. Photoelectric Effect & Einstein. Figure 7.6
4. Light and energy Problems

## 7.3 Atomic Spectroscopy and the Bohr Model

1. Continuous Spectrum, Figure 7.7
2. Line Spectrum of Hydrogen, Figure 7.8, ( Internet © Saunders, 1997)
3. Line Spectrum of different elements, Figure 7.9
4. Emission spectra of elements from The Chemistry Set
5. Spectra of Gas Discharges by John Talbot a Physics student at the University of Ottawa.
6. Elemental Spectra (Emission and Absorption) at University of Oregon department of Physics
7. Rydberg Equation

8. Relate wavelength to energy
9. Energy Level Diagram, Figure 7.12
10. Practice Problems

## 7.4 The Wave Nature of Matter: the de Broglie Wavelength, the Uncertainty Principle, and Indeterminancy

1. Photons and Wavelength, Planck (E = h v)

2. Bohr Nucleus relates electron energy and spectrum ( Internet © Saunders, 1997)

3. Electrons and Wavelength, DeBroglie) ([lambda] = h/(mv)
4. Uncertainty Principle, Heisenberg ([delta] x * [delta] (m v) > h)

## The Modern View of Eelctronic Structure: Wave or Quantum Mechanics

1. Probability Functions ( Internet © Saunders, 1997)

2. ## 7.5 Quantum Mechanics and the Atom

 Quantum Number Name Value Meaning n Principal Quantum Number Integer (1, 2, 3, .). Shell l Angular Momentum 0 to n-1 Type of orbital (s, p, d, f) ml Magnetic Quantum Number -l to +l Orientation ms Spin + or - 1/2 Electron Spin

## 7.6 The Shapes of Atomic Orbitals

THe Shapes of Atomic Orbiatalss

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