powerpoint to accompany chapter 5 electronic structure of atoms part 1
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PowerPoint to accompany
Chapter 5
Electronic Structureof Atoms
Part 1
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Waves: Chemistry’s 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
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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.
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Which wave above has the highest energy?How can you tell?
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
b) Highest amplitude for greatest frequency.
Energy ~ frequency
Intensity ~ Amplitude2
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Black Body Radiation
& Optical Pyrometry
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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.
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Quantized Energy and Photons
Einstein used this assumption to explain the photoelectric effect.
He concluded that energy is proportional to frequency:
E = hwhere h is Planck’s constant, 6.6310−34 Js.
To know frequency is to know energy!
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Potential Energy = mghcontinuous h (ramp), quantized h (steps)
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
photoelectric effect
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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 = = h
= (hc)/
Quantized Energy and Photons
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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
Quantized Energy and Photons
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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
Quantized Energy and Photons: For Matter….
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Quantized Energy and Photons: Hydrogen green is visible
Niels Bohr adopted Planck’s 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 = hFigure 5.11
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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.
E = −RH ( )1nf
21ni
2-
Figure 5.11
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
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:
=h
mv
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
Brown, LeMay, Bursten, Murphy, Langford, Sagatys: Chemistry 2e © 2010 Pearson Australia
End of Chapter 5 part 1
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