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CHEMISTRY CHAPTER 4 – QUANTUM THEORY VOCABULARY (26) angular momentum quantum number Aufbau principle continuous spectrum electromagnetic radiation electromagnetic spectrum electron configuration excited state frequency ground state Heisenberg uncertainty principle Hund’s rule inner shell electrons line-emission spectrum magnetic quantum number noble gas noble gas configuration orbital Pauli exclusion principle photoelectric effect photon principal quantum number quantum quantum numbers quantum theory spin quantum number wavelength LEARNING OBJECTIVES 1. Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiation. 2. Discuss the dual wave-particle nature of light. 3. Discuss the significance of the photoelectric effect and the line-emission spectrum of hydrogen to the development of the atomic model. 4. Describe the Bohr model of the hydrogen atom. 5. Discuss Louis de Broglie’s role in the development of the quantum model of the atom. 6. Compare and contrast the Bohr model and the quantum model of the atom. 7. Explain how the Heisenberg uncertainty principle and the Schrödinger wave equation led to the idea of atomic orbitals. 8. List the four quantum numbers and describe their significance. 9. Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of orbitals per sublevel, and the number of orbitals per main energy level. 10. List the total number of electrons needed to fully occupy each main energy level. 11. State the Aufbau principle, the Pauli exclusion principle, and Hund’s rule. 12. Describe the electron configurations for the atoms of any element using orbital notation, electron configuration notation, and noble gas notation.