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Electrons in Atoms

This article explains the characteristics of light waves, including wavelength, frequency, and amplitude. It also discusses the wave equation and Planck's equation. Additionally, it explores the electromagnetic spectrum and emission spectra of elements. The Bohr model of an atom and its relation to light emission are also covered.

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Electrons in Atoms

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  1. Electrons in Atoms Chap. 5

  2. Light (electromagnetic radiation)

  3. Light (electromagnetic radiation) A. Two components

  4. Light (electromagnetic radiation) A. Two components • Electrical wave

  5. Light (electromagnetic radiation) A. Two components • Electrical wave • Magnetic wave

  6. Light (electromagnetic radiation) A. Two components B. Two natures

  7. Light (electromagnetic radiation) A. Two components B. Two natures • Particle

  8. Light (electromagnetic radiation) A. Two components B. Two natures • Particle • Wave

  9. Light • Characteristics of a Light Wave

  10. Light • Characteristics of a Light Wave • wavelength

  11. Light • Characteristics of a Light Wave • wavelength The distance between successive wave crests

  12. Light • Characteristics of a Light Wave • wavelength • frequency The time it takes a wave to pass a given point

  13. Light • Characteristics of a Light Wave • wavelength • frequency • amplitude The height of a wave

  14. Light • Characteristics of a Light Wave • wavelength • frequency • amplitude • speed

  15. Light • Characteristics of a Light Wave • The Wave Equation

  16. Light • Characteristics of a Light Wave • The Wave Equation • inverse relation of wavelength and frequency

  17. Light • Characteristics of a Light Wave • The Wave Equation • inverse relation of wavelength and frequency • check the units

  18. The Wave Equation c = λxυ

  19. Self Check – Ex. 1 A light wave has a frequency of 2.6 x 1014 Hz. What is the wavelength?

  20. Self Check – Ex. 2 What is the frequency of light with a wavelength of 0.0000072 m?

  21. Light • Characteristics of a Light Wave • The Wave Equation • Planck’s Equation

  22. Planck’s Equation E = hxυ h = 6.63 x 10-34 J·s

  23. Self Check – Ex. 3 A light photon has 4.2 x 10-19 J of energy. What is the frequency of this light?

  24. Self Check – Ex. 4 How much energy does a photon of orange light have (λ = 630 nm)? 109 nm = 1 m

  25. Light • Characteristics of a Light Wave • The Wave Equation • Planck’s Equation • The Electromagnetic Spectrum

  26. Electromagnetic Spectrum Long waves Short waves

  27. Electromagnetic Spectrum Long waves Short waves Radio waves

  28. Electromagnetic Spectrum Long waves Short waves Radio waves Micro-waves

  29. Electromagnetic Spectrum Long waves Short waves Radio waves Infra-red Micro-waves

  30. Electromagnetic Spectrum Long waves Short waves Radio waves Infra-red Micro-waves Visible

  31. Electromagnetic Spectrum Long waves Short waves Radio waves Infra-red Ultra-violet Micro-waves Visible

  32. Electromagnetic Spectrum Long waves Short waves Radio waves Infra-red Ultra-violet Micro-waves Visible X-rays

  33. Electromagnetic Spectrum Long waves Short waves Radio waves Infra-red Ultra-violet Gamma rays Micro-waves Visible X-rays

  34. Emission Spectra

  35. Emission Spectra • Definition

  36. Emission Spectrum: The various types of light given off when an atom is excited

  37. Emission Spectra • Definition • Examples

  38. Hydrogen’s Spectrum 400 nm 500 nm 600 nm 700 nm Note – only a few colors are present

  39. Mercury’s Spectrum 400 nm 500 nm 600 nm 700 nm

  40. Neon’s Spectrum 400 nm 500 nm 600 nm 700 nm

  41. Emission Spectra • Definition • Examples • Explanation – Bohr’s Model

  42. e- Bohr’s Model of an Atom

  43. e- Bohr’s Model of an Atom Electrons orbit the nucleus (like planets orbiting the sun)

  44. e- Bohr’s Model of an Atom Electrons must be in a specific orbit (never between orbits) n=1 n=2 n=3

  45. e- Bohr’s Model of an Atom Electron wants to be in the lowest unoccupied level

  46. e- Bohr’s Model of an Atom The energy of the electrons depends on the distance from the nucleus high energy low energy

  47. Bohr’s Model of an Atom Light is emitted when electrons fall to lower energy levels e-

  48. e- Bohr’s Model of an Atom Only certain sized falls are permitted.

  49. Hydrogen’s Spectrum What is the energy for each line produced? 410 nm 486 nm 656 nm 434 nm

  50. Hydrogen’s Spectrum What is the energy for each line produced? 410 nm 486 nm 656 nm 434 nm

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