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Chapter 6

Chapter 6. Electronic Structure and the Periodic Table. c= λf. λ = c/f f = c/ λ. c = speed of light, 2.998 x 10 8 m/s λ = wavelength, m f = frequency, Hertz, Hz. Problem. Microwaves have a wavelength of 1.000 cm. Calculate their frequency in Hz. 1.000 cm = 1.000 x 10 -2 m

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Chapter 6

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  1. Chapter 6 Electronic Structure and the Periodic Table

  2. c= λf • λ = c/f • f = c/λ c = speed of light, 2.998 x 108m/s λ = wavelength, m f = frequency, Hertz, Hz

  3. Problem Microwaves have a wavelength of 1.000 cm. Calculate their frequency in Hz. 1.000 cm = 1.000 x 10-2m f = (2.998 x 108m/s)/1.000 x 10-2m = 2.998 x 1010Hz

  4. Problem Calculate the wavelength of a band on your AM radio with a frequency of 4.56 x 105Hz. λ = (2.998 x 108m/s)/(4.56 x 105Hz) = 657 m

  5. Wave

  6. Energy E = hc/λ E = hf E = energy, Joules, J c = speed of sound, 2.998 x 108m/s h = Planck’s constant, 6.626 x 10-34J*s

  7. Problem Calculate the the energy of microwaves in Joules, using the frequency 2.998 x 1010Hz. E = hf E = (6.626 x 10-34J*s)(2.998 x 1010Hz) = 1.986 x 10-23J

  8. Problem Calculate the energy in Joules of an AM radio wave having a wavelength of 657 m. E = hc/λ E = (6.626 x 10-34J*s)(2.998 x 108m/s)/657 m = 3.0 x 10-28J

  9. Quantum Numbers

  10. Principle Quantum Number • Symbolized by n • Indicates the main energy level occupied by the electron • Values are integers starting with 1

  11. Angular Momentum Quantum Number • Symbolized by l • Indicates shape • Values are 0, 1, 2, 3

  12. Magnetic Quantum Number • Symbolized by ml • Indicates the orientation of the orbital around the nucleus • Values are l,…, +1, 0, -1, ..., -l

  13. Spin Quantum Number • Symbolized by ms • Indicates the fundamental spin states of an electron in an orbital • Values are + ½ and -1/2

  14. Review • Electron Configurations • Orbital Diagrams • Noble Gas Configurations • Periodic trends • Atomic Radius • Ionization Energy • Electronegativty

  15. Periodic Trends • Atomic Radius • Decreases across periodic table from left to right • Increases down a group • Ionization Energy • Increases across periodic table from left to right • Decreases down a group • Electronegativity • Increases across periodic table from left to right • Decreases down a group

  16. Ionic Radius • Ionic Radii increase down a group. • Cations are smaller than their corresponding atoms. • Anions are larger than their corresponding atoms.

  17. Chapter 6 Assignment Summary problem page 158 Chapter Review p. 159 2, 5, 10, 30, 32, 34, 34, 38, 40

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