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Electromagnetic Spectrum

Electromagnetic Spectrum. Objectives. Compare the wave and particle models of light Define a quantum of energy and explain how it is related to an energy change of matter Contrast continuous electromagnetic spectra and atomic emission spectra. Behavior of Light.

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Electromagnetic Spectrum

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  1. Electromagnetic Spectrum

  2. Objectives • Compare the wave and particle models of light • Define a quantum of energy and explain how it is related to an energy change of matter • Contrast continuous electromagnetic spectra and atomic emission spectra

  3. Behavior of Light In 1905, Einstein published a theory explaining the photoelectric effect. According to this theory, light consists of particles called photons, massless bundles of concentrated electromagnetic energy.

  4. Wave Nature of Light • Wavelength (represented by λ, the Greek letter lambda) is the shortest distance between equivalent points on a continuous wave.

  5. Wave Nature of Light • Frequency (represented by n, the Greek letter nu) is the number of “waves” that pass a given point per second. • One hertz (Hz), the SI unit of frequency, equals one wave per second.

  6. Wave Nature of Light • All electromagnetic waves, including visible light, travel at a speed of 3.00 x 108 m/s in a vacuum. • Because the speed of light is such an important and universal value, it is given its own symbol, c. • The speed of light is the product of its wavelength (λ) and its frequency (n).

  7. Wave Nature of Light

  8. Electromagnetic Spectrum and the Elements of the Periodic Table • Certain elements emit visible light when heated in a flame. • Analysis of the emitted light revealed that an element’s chemical behavior is related to the arrangement of the electrons in its atoms.

  9. STARS COMPOSITION

  10. Atomic Emission Spectra • An atomic emission spectrum is characteristic of the element being examined and can be used to identify that element. • The fact that only certain colors appear in an element’s atomic emission spectrum means that only certain specific frequencies of light are emitted.

  11. Jupiter’s Spectrum

  12. Excitation of an electron by energy, causing the electron to "jump" to another electron (energy) level known as the excited state.

  13. The photoelectric effect • That is, while a beam of light has many wavelike characteristics, it also can be thought of as a stream of tiny particles, or bundles of energy, called photons • Thus, a photon is a particle of electromagnetic radiation with no mass that carries a quantum of energy.

  14. The ‘Magical’ Electron • Electrons, because they move so fast (approximately at the speed of light), seem to straddle the fence separating energy from matter. Because of this, scientists think of electrons both as particles of matter (having mass is a property of matter) and as units (or quanta) of energy. When subjected to energy, electrons will acquire some of that energy.

  15. The quantum concept • Matter can gain or lose energy only in small, specific amounts called quanta. • That is, a quantum is the minimum amount of energy that can be gained or lost by an atom.

  16. The photoelectric effect • In the photoelectric effect, electrons, called photoelectrons, are emitted from a metal’s surface when light of a certain frequency shines on the surface.

  17. Atomic Emission Spectra • The atomic emission spectrum of an element is the set of frequencies of the electromagnetic waves emitted by atoms of the element.

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