Arrangement of Electrons in Atoms
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1 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 1 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? Modern Chemistry 25 Arrangement of Electrons in Atoms
2 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? Modern Chemistry 26 Arrangement of Electrons In Atoms
3 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 2 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. Modern Chemistry 27 Arrangement of Electrons in Atoms
4 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 Modern Chemistry 28 Arrangement of Electrons In Atoms
5 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 3 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 Modern Chemistry 29 Arrangement of Electrons in Atoms
6 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. Modern Chemistry 30 Arrangement of Electrons In Atoms
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