1. Chapter 6 Electronic Structure of Atoms

2. The Wave Nature of Light The light that we can see with our eyes, visible light, is an example of electromagnetic radiation. All electromagnetic radiation travels at the same velocity, the speed of light, 3.00 x 10 8 m/s.

3. The Wave Nature of Light

4. We can perform calculations using the speed of light, wavelength, and frequency using the following equation. c = λv In this equation, c is the speed of light, λ is the wavelength, and v is the frequency.

5. Quantized Energy and Photons The energy of a photon is given by the equation: E = hν The constant h is called Planck’s constant and has a value of 6.626 x 10 -34 joule-second (J-s). The variable v represents the frequency of the radiation.

6. Line Spectra and the Bohr Model We can calculate the energy that is emitted or absorbed in a hydrogen atom using the following equation: The value of (-hcR H ) is 2.18 x 10 -18 J. The n f and n i are the final and initial energy levels of the electron.

7. The Wave Behavior of Matter de Broglie Wavelength: h is Planck’s constant, m is the mass of the particle, v is the velocity of the particle

8. The Wave Behavior of Matter Heisenberg uncertainty principle: It is impossible to simultaneously specify position and momentum of a particle with an extremely small mass, such as electrons

9. Quantum Mechanics and Atomic Orbitals principle quantum number: n angular momentum quantum number: l Value of l0123 Type of orbitalspdf

10. Quantum Mechanics and Atomic Orbitals

11. Representations of Orbitals

14. Energies of Orbitals

16. Pauli Exclusion Principle Only two electrons can exist in any one orbital and those two electrons must have opposite spins.

17. © 2009, Prentice-Hall, Inc. Orbital Diagrams Each box in the diagram represents one orbital. Half-arrows represent the electrons. The direction of the arrow represents the relative spin of the electron.

18. © 2009, Prentice-Hall, Inc. Hund’s Rule

19. © 2009, Prentice-Hall, Inc. Periodic Table

20. Some Anomalies