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Modern Atomic Model and EMR

Modern Atomic Model and EMR. Describe the electromagnetic spectrum in terms of frequency , wavelength , and energy. Understand how line spectra are created. Additional KEY Terms Spectroscopy Emission Quantum Line spectrum.

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Modern Atomic Model and EMR

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  1. Modern Atomic Model and EMR

  2. Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. • Understand how line spectra are created. Additional KEY Terms Spectroscopy Emission Quantum Line spectrum

  3. Maxwell (1860) - all energy radiated from objects (including visible light) is electromagnetic radiation. Composed of radiated waves of both electrical and magnetic energy.

  4. Wavelength(λ - “lambda”): distance from point to the same point on the next wave. Frequency(ν – “nu” or ƒ): number of wavelengths, or cycles, that pass a point per unit time. Frequency measured in cycles per second (s-1), or the SI unit hertz (Hz) Amplitude: height of the wave from origin to crest. Wavelength and frequency do not affect amplitude Wavelength and frequency are inversely related

  5. Types of Electromagnetic radiation f and λ determine what you see or hear, amplitude determines how loud or bright

  6. All EMRradiates at 3.00 x 108 m/s in a vacuum. This universal value (c) is a product of the wavelength and frequency of the radiated energy. “speed of light” c = λƒ c = λν

  7. Sunlight (white light) shone through a prism separates into a continuousspectrum of colours. Each colour represents light of a different frequency – increasing frequency - ROYGBIV

  8. Planck(1900) Elements give off a unique colour of light when burned - used to detect the presence of a metal This is known as a If the light emitted is focused through a prism, a spectrum with distinctlinesis produced.

  9. Disclaimer – This is not as simple as my drawing.

  10. Energy emitted by a heated element can be separated – producing emission spectrum. (line spectrum)

  11. C O The colored lines of the atoms (or Spectral Lines) are a kind of "signature" for the atoms.

  12. Spectroscopy and spectrophotometry are techniques used to determine a substance’s emission spectrum

  13. Planck's law: postulated that energy can only be gained or lost in discrete amounts – quanta. Quantum is the minimum amount of energy gained or lost by an atom. Energy contained in a quantum was directly related to the frequency of radiation emitted. E = hf

  14. E = hf E – energy of a quantum (Joules) h – Plank’s constant (6.626 x 10-34 J s) f – frequency of absorbed or emitted EMR

  15. CAN YOU / HAVE YOU? • Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. • Understand how line spectra are created. Additional KEY Terms Spectroscopy Emission Quantum Line spectrum

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