Chapter 11 Lecture Notes
Wednesday, April 12, 2000
Review of quanta of light and the two mathematical equations:
one which relates wavelength and frequency to the speed of
light, and the other that relates the energy of light to its
Look at the emission spectrum for hydrogen atoms to see the
difference between it and a continuous spectrum.
Look at the emission spectrum for several other elements and
ask several questions about what the nature of the hydrogen
atom could be to get the type of emission spectrum we
Introduction to the Bohr model of the hydrogen atom, and
discuss energy levels, the 'orbiting' electron and how an
electron can move from one energy level to another.
Part V: An
electron orbiting the nucleus in the Bohr model must absorb a
specific amount of energy to 'jump' to a higher energy level.
The term energy level is discussed further in this segment.
In this segment we watch an electron being excited from one
energy level (low) to another energy level (higher). exciting
an electron to a higher energy level requires the absorption
of a photon of light.
Introduction of the quantum number n. The
interesting arrangement of the energy levels in the Bohr
model of the hydrogen atom is also discussed.
The Bohr model of the atom works great for hydrogen, but not
so great for helium. Why? The concept of the electron in
terms of a wave is discussed.
Introduction of the concept of an orbital. The difference
between an electron orbiting the nucleus (Bohr model) and the
electron occuping an orbital (Quantum Mechanical model).
Introduction to the energy level diagram for the Bohr model,
and the quantum Mechanical model of the hydrogen atom..
Levels, sublevels and orbitals what do these terms mean in
our Quantum mechanical model of the hydrogen atom.