Electronic Structure of Atoms

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Chapter 5

• Electronic Structureof Atoms
• Part 1

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Waves Chemistrys best tool

• To understand the electronic structure of atoms,
  one must understand the nature of electromagnetic
  radiation.
• The distance between corresponding points on
  adjacent waves is the wavelength (?).

Figure 5.3
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Waves

• The number of waves passing a given point per
  unit of time is the frequency (?).
• For waves travelling at the same velocity, the
  longer the wavelength, the smaller the frequency.

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Which wave above has the highest energy?How can
you tell?
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b) Highest amplitude for greatest
frequency.Energy frequencyIntensity
Amplitude2
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Electromagnetic Radiation

• All electromagnetic radiation travels at the same
  velocity in vacuum.
• The speed of light (c) is 3.00 ? 108 m/s
• and ?? c.

Figure 5.4
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Black Body Radiation Optical Pyrometry
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Quantized Energy and Photons

• The wave nature of light does not explain how an
  object can glow when its temperature increases.
• Max Planck explained the statistical distribution
  of light, by assuming that energy comes in
  packets called quanta.

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Quantized Energy and Photons

• Einstein used this assumption to explain the
  photoelectric effect.
• He concluded that energy is proportional to
  frequency
• E h?
• where h is Plancks constant, 6.63?10-34 Js.
• To know frequency is to know energy!

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Potential Energy mghcontinuous h (ramp),
quantized h (steps)
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photoelectric effect
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Quantized Energy and Photons
Quantized Energy and Photons

• Therefore, if one knows the wavelength of light,
  one can calculate the energy in one photon, or
  packet, of that light
• c ??
• E h?
• E (hc)/l

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Quantized Energy and Photons
Quantized Energy and Photons

• Another mystery involved the emission spectra
  observed from energy emitted by atoms and
  molecules.
• Different gases have different bright line
  emission spectra (or dark line absorbtion spectra)

Figure 5.9
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Quantized Energy and Photons For Matter.

• One does not observe a continuous spectrum as one
  gets from a white light source.
• Only a line spectrum of discrete wavelengths is
  observed.

Figure 5.8
Figure 5.10 Sodium versus Hydrogen
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Quantized Energy and Photons Hydrogen green is
visible

• Niels Bohr adopted Plancks assumption and
  explained these phenomena in this way
• 1. Electrons in an atom can only occupy certain
  orbits (corresponding to certain energies).
• 2. Electrons in permitted orbits have specific,
  allowed energies these energies will not be
  radiated from the atom.
• 3. Energy is only absorbed or emitted in such a
  way as to move an electron from one allowed
  energy state to another the energy is defined
  by
• E h?

Figure 5.11
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Quantized Energy and Photons

• The energy absorbed or emitted from the process
  of electron promotion or demotion can be
  calculated by the equation
• where RH is the Rydberg constant, 2.18 ? 10-18 J,
  and ni and nf are the initial and final energy
  levels of the electron.

Figure 5.11
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The Wave Nature of Matter

• Louis de Broglie posited that if light can have
  material properties, matter should exhibit wave
  properties.
• He demonstrated that the relationship between
  mass and wavelength is

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End of Chapter 5 part 1