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Electron Configuration Practice
1. State Hund’s rule and the Aufbau principle.
2. Use the table below to complete the following:
a. Write the total number of electrons for each neutral element.
b. Draw arrows in the boxes to show the proper placement of electrons.
c. Write the full electron configuration for each element.
3. Write the abbreviated electron configurations for the following atoms:
a. Co (#27)
b. Sn (#50)
c. Pb (#82)
d. Ra (#88)
e. Lr (#103)
4. Determine what elements are denoted by the following electron configurations:
a. 1s2 2s2 2p6 3s2 3p4
b. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
c. [Kr] 5s2 4d10 5p3
d. [Xe] 6s2 4f14 5d6
e. [Rn] 7s2 5f11
5. Determine which of the following electron configurations are not valid:
a. 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p5
d. [Kr] 5s2 4d10 5p5
b. 1s2 1p6 2s2
e. [Hg] 6p4
c. [Ra] 7s2 5f8
f. [Xe]
Unit 7 – Light, Electron, and Atomic Structure Review
The Nature of Light
1. Light consists of what type of wave? How fast does it travel?
2. Describe the relationship between frequency, wavelength, and energy.
3. What is a photon?
4. Use the quantum theory of light to define what light is.
5. Describe, in basic terms, the wave-particle duality.
Electrons and the Structure of the Atom
6. What is the difference between a line spectrum and continuous spectrum?
7. What are electrons responsible for?
8. Describe why Bohr opposed Rutherford’s planetary model.
9. Describe the atomic model proposed by Bohr.
10. Describe how atoms produce light.
11. How did Bohr’s model help lead to the discovery of many new elements?
12. Why does each element have its own unique line spectrum.
13. How did Schrӧdinger, Heisenberg, and Born influence the atomic model?
Electron Configurations and Quantum Numbers
14. Use ‘Quantum Practice Problems’ to review quantum numbers.
15. Review the ‘Electron Configuration Practice’ above.