ELECTRON ARRANGEMENT PRACTICE PROBLEMS – PART A
1. Write out each of the rules below in your own words:
a. Aufbau Principle
b. Hund’s Rule:
c. Pauli Exclusion Principle
2. Use the boxes below to show the orbital notation for boron and for aluminum. Then write out the electron
configuration for each.
Boron: _________________________
1
Aluminum: ______________________
ELECTRON ARRANGEMENT PRACTICE PROBLEMS – PART B
1. Complete the chart below:
Element
28
14𝑆𝑖
88
38𝑆𝑟
57
25𝑀𝑛
184
74𝑊
122
51𝑆𝑏
Electron Configuration
(complete or abbreviated)
Orbital Filling Diagram
(complete or abbreviated)
Electron
Dot
Diagram
[Ne] 3s23p2
[Kr] 5s2
[Ar] 4s23d5
[Xe] 6s24f145d4
[Kr] 5s24d105p3
2. Which element in the chart above would you suspect to be an exception to the orbital filling
pattern?_W____
3. How many half filled orbitals does a manganese atom have? __5___________________________
4. How many unpaired electrons does a nitrogen atom have?
___3__________________________
5. How many electrons can fit in the fifth principle energy level? ____2n2_______________________
6. What is the lowest principle energy level that has an “f” sublevel? ____4____________________
7. How many orbitals are in an “f” sublevel? _______7____________________________________
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SCIENTIST MATCHING
1. G
Developed the quantum mechanical model of the atom
A. Thomson
2. A
Experiments with cathode ray tubes led to the determination of the
charge/mass ratio of the electron
B. Bohr
3. F
His Uncertainty Principle states that it is impossible to know both the
velocity and position of a particle at the same time
C. DeBroglie
4. B
Developed the quantum mechanical model for hydrogen
D. Einstein
5. E
Proposed that energy is quantized
E. Planck
6. D
Photoelectric effect
F. Heisenberg
7. C
All moving particles have wave characteristics
G. Schrödinger
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