CHAPTER 4 Arrangement of Electrons in Atoms
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1 CHAPTER 4 Arrangement of Electrons in Atoms SECTION 1 The Development of a New Atomic Model 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. SECTION 2 The Quantum Model of the Atom OBJECTIVES 1. Discuss Louis de Broglie s role in the development of the quantum model of the atom. 2. Compare and contrast the Bohr model and the quantum model of the atom. 3. Explain how the Heisenberg uncertainty principle and the Schrödinger wave equation led to the idea of atomic orbitals. 4. List the four quantum numbers, and describe their significance. 5. 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. SECTION 3 Electron Configurations OBJECTIVES 1. List the total number of electrons needed to fully occupy each main energy level. 2. State the Aufbau principle, the Pauli exclusion principle, and Hund s rule. 3. Describe the electron configurations for the atoms of any element using orbital notation, electron-configuration notation, and when appropriate, noblegas notation. 1 Arrangement of Electrons in Atoms
2 Vocabulary Arrangement of Electrons in Atoms Sec 4-1 The Development of a New Atomic Model Electromagnetic radiation Electromagnetic spectrum Wavelength Frequency Photoelectric effect Quantum Photon Ground state Excited state Line-emission spectrum Continuous spectrum Sec 4-3 Electron Configurations Electron configuration Aufbau principle Pauli exclusion principle Hund s rule Noble gas Noble gas configuration Isoelectric Valence electrons Paired electrons Unpaired electrons Sec 4-2 The Quantum Model of the Atom Heisenburg Uncertainty Principle Quantum theory Orbital Quantum number Principal quantum number Angular momentum quantum number Magnetic quantum number Spin quantum number Sublevel Degenerate orbitals 2 Arrangement of Electrons in Atoms
3 CHAPTER 4 STUDY GUIDE Arrangement of Electrons in Atoms SECTION 1: The Development of a New Atomic Model SHORT ANSWER Answer the following questions in the space provided. 1. In what way does the photoelectric effect support the particle theory of light? 2. What is the difference between the ground state and the excited state of an atom? 3. Under what circumstances can an atom emit a photon? 4. How can the energy levels of the atom be determined by measuring the light emitted from an atom? 5. Why does electromagnetic radiation in the ultraviolet region represent a larger energy transition than does radiation in the infrared region? 2 Arrangement of Electrons in Atoms
4 SECTION 1 continued 6. Which of the waves shown below has the higher frequency? (The scale is the same for each drawing.) Explain your answer. 7. How many different photons of radiation were emitted from excited helium atoms to form the spectrum shown below? Explain your answer. PROBLEMS Write the answer on the line to the left. Show all your work in the space provided. 8. What is the frequency of light that has a wavelength of 310 nm? 9. What is the wavelength of electromagnetic radiation if its frequency is Hz? 2 Arrangement of Electrons in Atoms
5 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 2: The Quantum Model of the Atom SHORT ANSWER Answer the following questions in the space provided. 1. How many quantum numbers are used to describe the properties of electrons in atomic orbitals? (a) 1 (c) 3 (b) 2 (d) 4 2. A spherical electron cloud surrounding an atomic nucleus would best represent (a) an s orbital. (c) a combination of two different p orbitals. (b) a p orbital. (d) a combination of an s and a p orbital. 3. How many electrons can an energy level of n = 4 hold? (a) 32 (c) 8 (b) 24 (d) 6 4. How many electrons can an energy level of n = 2 hold? (a) 32 (c) 8 (b) 24 (d) 6 5. Compared with an electron for which n = 2, an electron for which n = 4 has more (a) spin. (c) energy. (b) particle nature. (d) wave nature. 6. According to Bohr, which is the point in the figure below where electrons cannot reside? (a) point A (c) point C (b) point B (d) point D 7. According to the quantum theory, point D in the above figure represents (a) the fixed position of an electron. (b) the farthest position from the nucleus that an electron can achieve. (c) a position where an electron probably exists. (d) a position where an electron cannot exist. 3 Arrangement of Electrons in Atoms
6 SECTION 2 continued 8. How did de Broglie conclude that electrons have a wave nature? 9. Identify each of the four quantum numbers and the properties to which they refer. 10. How did the Heisenberg uncertainty principle contribute to the idea that electrons occupy clouds, or orbitals? 11. Complete the following table: Principal quantum number, n Number of sublevels Types of orbitals 1 1 s 2 2 s, p 3 3 s,p,d 4 4 s,p,d,f 4 Arrangement of Electrons in Atoms
7 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 3: Electron Configuration SHORT ANSWER Answer the following questions in the space provided. 1. State the Pauli exclusion principle, and use it to explain why electrons in the same orbital must have opposite spin states. 2. Explain the conditions under which the following orbital notation for helium is possible: 1s 2s Write the ground-state electron configuration and orbital notation for each of the following atoms: 3. Phosphorus 4. Nitrogen 5. Potassium 5 Arrangement of Electrons in Atoms
8 SECTION 3 continued 6. Aluminum 7. Argon 8. Boron 9. Which guideline, Hund s rule or the Pauli exclusion principle, is violated in the following orbital diagrams? a. b. 6 Arrangement of Electrons in Atoms
9 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms MIXED REVIEW SHORT ANSWER Answer the following questions in the space provided. 1. Under what conditions is a photon emitted from an atom? 2. What do quantum numbers describe? 3. What is the relationship between the principal quantum number and the electron configuration? 4. In what way does the figure above illustrate Hund s rule? 5. In what way does the figure above illustrate the Pauli exclusion principle? 7 Arrangement of Electrons in Atoms
10 MIXED REVIEW continued 6. Elements of the fourth and higher main-energy levels do not seem to follow the normal sequence for filling orbitals. Why is this so? 7. How do electrons create the colors in a line-emission spectrum? 8. Write the ground-state electron configuration of the following atoms: a. Carbon b. Potassium c. Gallium d. Copper PROBLEMS Write the answer on the line to the left. Show all your work in the space provided. 9. What is the wavelength of light that has a frequency of Hz in a vacuum? 10. What is the energy of a photon that has a frequency of Hz? 8 Arrangement of Electrons in Atoms
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