YELLOW
St. Mark’s School Honor Pledge
“On my honor as a St. Marker, I pledge that I have properly
acknowledged all resources, and I have not given
inappropriate assistance to others on this assessment.”
Printed Name
Signature
Date
UNIT 3 THE QUANTUM ATOM ASSESSMENT
Read each question below carefully and be sure to answer fully.
1. In the drawings below are shown depictions of various atomic orbitals. For each orbital, provide the value of the
angular momentum quantum number and below the orbitals, rank them in order of increasing energy, if possible,
using the letters (a), (b), and (c).
(a)
a
(b)
a
(c)
a
n=1
n=1
n=1
l = _____
l = _____
l = _____
Ordering of orbital energy (from lowest energy à highest energy): _____________________________________
2. For the following, provide either the appropriate quantum number symbol or the name of the symbol itself. For all
terms, provide the physical meaning. Note: they MAY NOT be listed in an order that you are familiar with.
Name
Symbol
Physical Meaning
ml
Spin quantum number
n
Angular momentum quantum
number
3.
Which of the quantum numbers listed in question 2 above:
Specify the energy of an electron: ___________________________________________________________________
Specify the location of an electron: __________________________________________________________________
Are not related to the location or energy of an electron: __________________________________________________
Write your choices (if any) on the lines provided and explain!
4. There are various ways of writing and expressing the electron configuration for a given atom. Provide the name of
these different ways using the appropriate terminology and explain a key feature in which they differ from one
another. You may use a diagram or an example to help you explain.
5. Compare and contrast the Bohr model of the atom and the Schrödinger (or quantum) model of the atom. In particular,
give specifics of successes and drawbacks of each model. You may use bullet points in answering.
6. Describe the difference between shells, subshells, and orbitals. Do NOT simply use quantum numbers in your
response.
7. Which of the following equations describe particle-like behavior? Which describe wavelike behavior? Do any involve
behavior of both types? Explain the reasons for your choices.
a. c = λν
b. E = hν
c.
Where RH is the Rydberg constant and n1 and n2 are integers.
8. Is 1s2 2s2 2p6 the symbol for a microscopic property or a macroscopic property? Explain.
9. Give numerical values of n and l corresponding to each of the following orbital designations:
a. 3p
n=
l=
b. 2s
n=
l=
c. 4f
n=
l=
10. Write the ground state electron configurations for
a. Silicon _____________________________________
b. Iron _______________________________________
c. Bromine ____________________________________
11. Determine which of the following sets of quantum numbers for the hydrogen atom are valid. If a set is NOT valid,
indicate which of the quantum numbers has a value that is not valid:
a. n = 4, l = 1, ml = 2, ms = -1/2
b. n = 4, l = 3, ml = -3, ms = +1/2
c. n = 3, l = 2, ml = -1, ms = +1/2
12. In one area of Australia, the cattle did not thrive despite the presence of suitable plant matter. An investigation
showed the cause to be the absence of cobalt in the soil. Cobalt forms two cations: Co2+ and Co3+. Write the electron
configuration for the neutral atom.
13. Write out the orbital diagram for the cobalt atom described in problem 12 above.
14. You may consult the periodic table in answering this question, but no reasoning = no credit. Which row of the
periodic table does the following electron configuration represent?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2
row _______________
How do you know this?
What would you expect the element directly above this one on the periodic table to have as its electron configuration?
Why?
15. The average distance from the nucleus of a 3s electron in a chlorine atom is smaller than that for a 3p electron. In light
of this fact, which orbital is higher in energy? Explain.
16. Four possible electron configurations for a nitrogen atom are shown below, but only one figure represents the correct
configuration for nitrogen in its ground state.
a. Which one is the correct configuration?
b. Which configuration violates the Pauli exclusion
principle? How do you know?
c. Which configuration violates Hund’s rule? How
do you know?
17. The diagram to the right represents one of the orbitals for the n = 3 shell of a
hydrogen atom.
a. What is the quantum number l for this orbital?
b. How do we label this orbital?
c. If we were to modify the magnetic quantum number, ml, choose the best
answer from the following for how the diagram to the right might be
modified. Circle the best response. Assume that the modification to ml is
still a valid quantum number for this atom.
i.
ii.
iii.
iv.
It would be drawn larger
The number of lobes would change
The lobes of the orbital would point in a different direction
There would be no change in the diagram