Name ____________________________
Electron Configuration Test Review
1.
Define an orbital.
2. Main energy levels are subdivided into _______________________; designated with the
following letter: ________, _______, _________, and _______.
3. Which possible sublevels are present in the 1st energy level? __________ 2nd? ________
3rd? _________4th? _____________.
4. How many orbitals are in the s sublevel? ________ p sublevel? _______ d sublevel? _______
f sublevel? ___________.
5. What is the shape of an s orbital? __________ p orbital? ______________
6. How many electrons can a single orbital hold? ________________
7. How many electrons will fill an s sublevel? _________ p sublevel ?__________
d sublevel? _______ f sublevel? ___________
8. How many electrons in the 1st energy level? _______ 2nd? ____________ 3rd? _______
4th? ___________
9. Write the complete order of electron filling, starting with 1s and ending with 6s.
10. Explain Aufbau’s Principle and how it is used in electron configurations.
11. Explain Pauli’s Exclusion Principle and how it is used in orbital spin diagrams.
12. Explain Hund’s Rule and how it is used in orbital spin diagrams.
13. How many electrons are in the 2nd energy level in carbon? ________
14. 3rd Energy level in nickel? _______
15. Fill out the following information for PHOSPHORUS
a. Orbital spin diagram
b. Electron configuration
c. Shorthand Configuration
16. Fill out the following information for IRON
a. Orbital spin diagram
b. Electron configuration
c. Shorthand Configuration
17. Write the electron configuration for the Calcium Ion.
18. Write the electron configuration for the Sulfur Ion.
19. Draw the hill of oxidation numbers
20. Describe the electron cloud of the atoms in terms of a probability model (QMM).
21. How many valence electrons are in the following electron configurations?
a.
b.
c.
d.
e.
1s22s22p63s23p64s23d1
1s22s22p1
[Kr]5s24d5
[Xe]6s1
[Ne]3s23p4
22. Identify the elements from number 21 based on their electron configurations.
a. _________________
b. _________________
c. _________________
d. _________________
e. _________________
23. What would the charge (ion) be for the elements in number 21 based on the electron
configurations?
a. _____
b. _____
c. _____
d. _____
e. _____
24. Predict the electron configuration for an element with no more than 36 electrons.
25. Which is the electronic configuration of calcium?
a.
1s22s22p63s23p8
b.
1s22s22p63s23p64s2
c.
1s22s22p63s23p63d2
d.
1s22s22p83s23p6
26. Use the Bohr model to explain the release of energy in the return of electrons to a ground state.
27. An electron in an atom of hydrogen goes from energy level 6 to energy level 2. What is the
wavelength of the electromagnetic radiation emitted?
a.
410 nm
b.
434 nm
c.
486 nm
d.
656 nm
28. Which occurs if an electron transitions from n = 5 to n = 2 in a hydrogen atom?
A
Energy is absorbed, and visible light is emitted.
B
Energy is released, and visible light is emitted.
C
Energy is released, and visible light is not emitted.
D
Energy is absorbed, and visible light is not emitted
29. Given the following:
4p3
What does the 4 represent? ______________________
What does the p represent? _______________________
What does the 3 represent? _______________________