1. Explain why different colors of light result
from electron behavior in the atom.
When an electron returns to their ground
state from an excited state, the atom emits
a photon whose frequency corresponds to
the energy difference between the two
energy levels. Each frequency corresponds
to a certain color.

2. Explain the Heisenberg uncertainty principle.
The Heisenberg uncertainty principle states
That it is not possible to know precisely the
velocity and the position of a particle at the
same time.

3. Compare and contrast Bohr’s model and the
quantum mechanical model.
Both models limit an electron’s energy to
certain values. Unlike the Bohr model, the
quantum model make no attempt to describe
The electron’s path around the nucleus.

4. Describe where electrons are located in an
atom.
Electrons are located around the nucleus at
a position that can be described only by a
probability map. A boundary surface is
chosen to contain the region that the
electron can be expected to occupy 90% of
the time.

5. Explain the relationship between energy
levels and sublevels.
The number of energy sublevels in a
principal energy level increases as n
increases. (# sublevels = n for n< 4)

6. Describe the shapes of s and p orbitals.
s orbitals s are spherical and p orbitals are
dumbell shaped.