Download Quantum Numbers Practice Problems Name: AP Physics Period: 1

Quantum Numbers Practice Problems
AP Physics
Name:
Period:
1. Heisenberg changed our understanding of electrons in ways that ruined the Bohr model of the Hydrogen
atom. How did the uncertainty principle change our understanding of how electrons behave inside
2. According to the deBroglie theory, electrons orbiting around the nucleus of an atom are waves (as well as
particles). How does our understanding of electron waves change when we give up the idea of a simple orbit
for an electron (like the ones that Bohr envisioned)?
3. a) What does the principal
quantum number (n) tell us about
the wave for the electron in a
particular orbital?
b) What does the angular
momentum quantum number (l)
tell us about the wave for the
electron in a particular orbital?
c) What does the magnetic
quantum number (ml) tell us about
the wave for the electron in a
particular orbital?
4. In terms of quantum theory, why is the periodic table of elements organized the way it is? What do the
elements in a particular group (column) have in common? What do the elements in a particular period (row)
have in common?
5. a) How many possible combinations of quantum numbers (orbitals) are there for the n = 2 shell? Explicitly
write out all of the possible combinations.
b) How many possible combinations of quantum numbers (orbitals) are there for the n = 3 shell? Explicitly
write out all of the possible combinations.
c) How many different photons could an atom emit if an electron drops from the n = 3 shell to the n = 2 shell?
Explain.
6. a) Within the n = 4 energy level, how many sets of quantum numbers are there that have l = 0?
b) Within the n = 4 energy level, how many sets of quantum numbers are there that have l = 2?
c) If the electron dropped from an orbital with l = 2 to one with l = 0 within the n = 2 energy level, how many
different photons could it possibly emit? Explain.
7. a) An electron in a multielectron atom has a magnetic quantum number of ml = 2. What are the minimum
values of l and n for that electron?
b) An electron in a multielectron atom has a magnetic quantum number of ml = –4. What are the minimum
values of l and n for that electron?
8. a) If electrons did not have spin (and therefore a spin quantum number), what would be the first two inert or
noble gases? Explain.
b) If electrons could have three different values for spin, what would be the first two inert or noble gases?
Explain.