The document discusses the Bohr model of the hydrogen atom. It explains that: 1) Electrons orbit the nucleus in fixed energy levels called orbits. 2) Electrons can move between energy levels by gaining or losing discrete amounts of energy. 3) Electrons cannot exist between energy levels, which are like rungs on a ladder with the lowest level closest to the nucleus.

1. Emission and Absorption of
Electromagnetic Energy

2. copper sodium lithium strontium

3. BOHR MODEL OF
HYDROGEN ATOM
 Electron circles the nucleus in fixed energy
ranges called orbits (energy levels)
 An electron can move from one energy level to
another by gaining discrete amounts of energy.
 Electron can not be found between energy levels
(energy levels are like rungs on a ladder…..)
 The lowest energy level is the closest to the
nucleus.

4. BOHR MODEL OF
HYDROGEN ATOM
 Electron circles the nucleus in fixed energy
ranges called orbits (energy levels)
 An electron can move from one energy level to
another by gaining discrete amounts of energy.
 Electron can not be found between energy levels
(energy levels are like rungs on a ladder…..)
 The lowest energy level is the closest to the
nucleus.

5. energy absorbed
=
energy released
=
energy of light produced
*some of this light is part of the visible
spectrum, and can be seen as unique colors for
different elements

6.  Bohr model helped us to understand the
movement of electrons around the
nucleus.
 However, the model does not account for
behavior of larger atoms with more than
one electron.

7. Bohr model from reference
table
When an electron
falls from
n = 6 to n = 2, what
wavelength of light
will be emitted?
What is the
region of the
spectrum that
corresponds to this
wavelength?

8. When an electron falls from
n = 6 to n = 2, what color of light will
be emitted?

9. Wavelength vs Frequency
 Inversely proportional (i.e. when one goes
up, the other goes down)
 http://amazing-
space.stsci.edu/resources/explorations/light/
makewaves-frames.html

10. Wave-Particle Duality of
Electrons
 Electrons act as waves as well as particles
 Energy can act as particles as well as waves