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Name Date CHAPTER 5 Class STUDY GUIDE FOR CONTENT MASTERY Electrons in Atoms Section 5.1 Light and Quantized Energy In your textbook, read about the wave nature of light. Use each of the terms below just once to complete the passage. amplitude energy frequency hertz light wave wavelength speed that behaves like a(n) Electromagnetic radiation is a kind of (1) as it travels through space. (3) (2) is one type of electromagnetic radiation. Other examples include X rays, radio waves, and microwaves. All waves can be characterized by their wavelength, amplitude, frequency, and . The shortest distance between equivalent points on a continuous wave is (4) . The height of a wave from the origin to a crest or from the called a(n) (5) . (7) origin to a trough is the (6) is the number of Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. waves that pass a given point in one second. The SI unit for frequency is the , which is equivalent to one wave per second. (8) Use the figure to answer the following questions. A D B Origin C 9. Which letter(s) represent one wavelength? 10. Which letter(s) represent the amplitude? 11. If twice the length of A passes a stationary point every second, what is the frequency of the wave? Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 5 25 Name Date 5 CHAPTER Section 5.2 Class STUDY GUIDE FOR CONTENT MASTERY Quantum Theory and the Atom In your textbook, read about the Bohr model of the atom. Use each of the terms below to complete the statements. atomic emission spectrum electron frequencies higher energy levels lower ground state 1. The lowest allowable energy state of an atom is called its . 2. Bohr’s model of the atom predicted the of the lines in hydrogen’s atomic emission spectrum. 3. According to Bohr’s atomic model, the smaller an electron’s orbit, the the atom’s energy level. 4. According to Bohr’s atomic model, the larger an electron’s orbit, the the atom’s energy level. 5. Bohr proposed that when energy is added to a hydrogen atom, its moves to a higher-energy orbit. Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 6. According to Bohr’s atomic model, the hydrogen atom emits a photon corresponding to the difference between the associated with the two orbits it transitions between. 7. Bohr’s atomic model failed to explain the of elements other than hydrogen. In your textbook, read about the quantum mechanical model of the atom. Answer the following questions. 8. If you looked closely, could you see the wavelength of a fast-moving car? Explain your answer. h 9. Using de Broglie’s equation, m which would have the larger wavelength, a slow-moving proton or a fast-moving golf ball? Explain your answer. Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 5 27 Name Date CHAPTER Section 5.3 5 Class STUDY GUIDE FOR CONTENT MASTERY Electron Configurations In your textbook, read about ground-state electron configurations. Use each of the terms below just once to complete the passage. Aufbau principle electron configuration ground-state electron configuration Hund’s rule lowest Pauli exclusion principle spins stable The arrangement of electrons in an atom is called the atom’s . Electrons in an atom tend to assume the arrangement (1) that gives the atom the (2) possible energy. This arrangement of electrons is the most (3) arrangement and is called the . atom’s (4) Three rules define how electrons can be arranged in an atom’s orbitals. The states that each electron occupies the lowest energy (5) states that a maximum of two orbital available. The (6) electrons may occupy a single atomic orbital, but only if the electrons have opposite . (8) Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. (7) states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins occupy the same orbitals. Complete the following table. Element Atomic Number Orbitals 1s 2s 2px Electron Configuration 2py 2pz 1s2 9. Helium 10. 11. Neon Study Guide for Content Mastery 7 )( )( )( )( )( Chemistry: Matter and Change • Chapter 5 29 Name Date CHAPTER 5 Class STUDY GUIDE FOR CONTENT MASTERY Section 5.3 continued Answer the following questions. 12. What is germanium’s atomic number? How many electrons does germanium have? 13. What is noble-gas notation, and why is it used to write electron configurations? 14. Write the ground-state electron configuration of a germanium atom, using noble-gas notation. In your textbook, read about valence electrons. Circle the letter of the choice that best completes the statement or answers the question. 15. The electrons in an atom’s outermost orbitals are called b. quantum electrons. c. valence electrons. d. noble-gas electrons. 16. In an electron-dot structure, the element’s symbol represents the a. nucleus of the noble gas closest to the atom in the periodic table. b. atom’s nucleus and inner-level electrons. c. atom’s valence electrons. d. electrons of the noble gas closest to the atom in the periodic table. 17. How many valence electrons does a chlorine atom have if its electron configuration is [Ne]3s23p5? a. 3 b. 21 c. 5 d. 7 18. Given boron’s electron configuration of [He]2s22p1, which of the following represents its electron-dot structure? a. • Be • • b. •B• •• c. B•• •• d. Be 19. Given beryllium’s electron configuration of 1s22s2, which of the following represents its electron-dot structure? a. • Be • • b. •B• •• c. B •• •• d. Be 20. Which electrons are represented by the dots in an electron-dot structure? 30 a. valence electrons c. only s electrons b. inner-level electrons d. both a and c Chemistry: Matter and Change • Chapter 5 Study Guide for Content Mastery Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. a. electron dots. Name Date CHAPTER 5 Class CHAPTER ASSESSMENT Electrons in Atoms Reviewing Vocabulary Match the definition in Column A with the term in Column B. Column A Column B 1. The set of frequencies of the electromagnetic waves emitted by the atoms of an element b. photoelectric effect 2. The minimum amount of energy that can be lost or gained by an atom 3. A form of energy that exhibits wavelike behavior as it travels through space c. photon d. quantum e. atomic orbital 4. A three-dimensional region around the nucleus of an atom that describes an electron’s probable location 5. The shortest distance between equivalent points on a continuous wave f. atomic emission spectrum g. principal quantum number 6. The lowest allowable energy state of an atom h. ground state 7. A particle of electromagnetic radiation with no mass that Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. a. wavelength carries a quantum of energy i. electromagnetic radiation 8. The emission of electrons from a metal’s surface when light of a certain frequency shines on it 9. A figure indicating the relative sizes and energies of atomic orbitals Describe how each pair is related. 10. frequency, amplitude 11. valence electron, electron-dot structure 12. principal energy levels, energy sublevels Chapter Assessment Chemistry: Matter and Change • Chapter 5 25 Name CHAPTER Date 5 Class CHAPTER ASSESSMENT Understanding Main Ideas (Part B) Circle the letter of the choice that best completes the statement or answers the question. Use the following figure to answer questions 1 and 2. D C E A B 1. According to Bohr’s atomic model, which letter(s) in the figure represents a place where an electron cannot be? a. A b. B, C and E c. A and D d. D 2. According to the quantum mechanical model of the atom, point E in the figure represents a a. point where an electron cannot be. c. position where an electron must be. b. position where an electron probably is. d. point beyond which no electron can go. 3. What can you conclude from the figure on the right? )( ) ) a. Hund’s rule has been violated. 2p )( Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. b. The Pauli exclusion principle has been violated. 2s c. The Aufbau principle has been violated. 1s d. This is a valid orbital diagram. 4. What can you conclude from the figure on the right? )) a. Hund’s rule has been violated. 2p )( b. The Pauli exclusion principle has been violated. c. The Aufbau principle has been violated. 2s )( 1s d. This is a valid orbital diagram. 5. Which of the following can you conclude based on the de Broglie equation? a. Waves behave like particles. c. All matter has an associated wavelength. b. Most particles are electrons. d. All matter behaves like particles. 6. Which of the following best describes the Heisenberg uncertainty principle? a. Light behaves like a particle and like a wave. b. The shorter the wavelength, the higher the frequency. c. It is impossible to know both the velocity and the position of a particle at the same time. d. You cannot measure an object without disturbing it. Chapter Assessment Chemistry: Matter and Change • Chapter 5 27 Name Date 5 CHAPTER Class CHAPTER ASSESSMENT Thinking Critically Answer the following questions. 1. A radio station has a frequency of 103.7 MHz. (1 MHz 106 s1) What is the wavelength of the radiation emitted by the station? Indicate where this wavelength falls on the electromagnetic spectrum shown below. Electromagnetic Spectrum 106 105 107 109 108 1010 1011 1012 1013 1014 1015 1016 1017 1018 1019 (Hz) 103 102 101 10–1 10–2 10–3 10–4 10–5 10–6 10–7 10–8 rays X rays Ultraviolet Visible Infrared Microwave UHF-TV 1 10–9 10–10 10–11 (m) Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 104 FM radio VHF-TV AM radio Radio 2. Look at the electromagnetic spectrum again. Are the microwaves used to cook food higher or lower in frequency than radio waves? Are microwaves longer or shorter in wavelength than radio waves? 3. Write the orbital diagram of aluminum. 4. Write the complete electron configuration and the noble-gas notation for aluminum. 5. Write the noble-gas notation for iodine. 6. Identify each atom. a. 1s22s22p1 b. [Ar]4s1 7. Write electron-dot structures for the following atoms. 28 a. neon c. carbon b. hydrogen d. sulfur Chemistry: Matter and Change • Chapter 5 Chapter Assessment Name CHAPTER Date 5 Class CHAPTER ASSESSMENT Applying Scientific Methods A chemist isolated four samples, A, B, C, and D. She obtained the following atomic emission spectra of the samples. A B C D 400 500 600 Nanometers 700 1. Examine each sample’s atomic emission spectra. Assume that each sample represents a Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. single element. What can you conclude by looking at the spectra? Do the samples represent the same element or different elements? 2. Which part of the electromagnetic spectrum do the atomic emission spectra show? 3. Would the atomic emission spectrum for each sample change if you repeated the proce- dure? Explain your answer 4. What does each line in an atomic emission spectrum represent? Chapter Assessment Chemistry: Matter and Change • Chapter 5 29 CHAPTER 5 SUPPLEMENTAL PROBLEMS Electrons in Atoms 1. Orange light has a frequency of 4.8 1014 s1. 6. List the sequence in which the following orbitals fill up: 1s, 2s, 3s, 4s, 5s, 6s, 7s, 2p, 3p, 4p, 5p, 6p, 7p, 3d, 4d, 5d, 6d, 4f, 5f. What is the energy of one quantum of orange light? 7. Which element has the ground-state electron 2. Which is greater, the energy of one photon configuration [Kr]5s24d105p4? of orange light or the energy of one quantum of radiation having a wavelength of 3.36 109m? 8. Which element has the ground-state electron configuration [Ar]4s23d10? 3. Use the relationships E h and c v to write E in terms of h, c, and . 9. Write electron-dot structures for the following atoms. 4. A radio station emits radiation at a wavelength a. [Ne]3s23p3 of 2.90 m. What is the station’s frequency in megahertz? b. [Ar]4s23d3 c. potassium 5. Record the frequency of your favorite radio Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. station. What is the wavelength of the radiation emitted from the station? 10. Complete the following table. Orbitals Element Symbol 1s 2s 2px 2py 2pz 1s22s22p3 a. Nitrogen b. Electron Configuration F )( )( )( )( ) c. Carbon d. Supplemental Problems 1s22s1 Chemistry: Matter and Change • Chapter 5 7 CHAPTER 5 Electrons in Atoms Name: Date: In question 1, the speed of light, c, equals 3.00 108 m/s. 3 Yellow light has a wavelength of 5.60 10–7 meters. According to the formula, c = , what is the frequency of this yellow light? 1 the release of gamma rays from the nucleus B the return of excited electrons to lower energy levels C the movement of electrons to higher energy levels the absorption of photons by the electrons 5.36 1014 s–1 B 5.36 1016 s–1 C 1.87 10–15 s–1 D D 1.87 1015 s–1 This question covers TEKS 6A. This question tests the material that was covered in the textbook on pages 125–126. Use the diagram below to answer question 2. In question 4, Planck’s constant, h, equals 6.626 10–34 J.s 4 0 Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc. A A This question covers TEKS 2C. This question tests the material that was covered in the textbook on pages 119–121. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 wavelength 2 When a potassium compound is placed in a flame, energy is released and a violet color is produced. This energy release is due to — What is the wavelength of the wave shown above? A 3.2 cm B 3.5 cm C 3.7 cm D 4.0 cm According to Einstein, Ephoton = h. What is the energy of a photon if it has a frequency of 6.82 1014s–1? A 9.72 10–20J B 1.03 10–20J C 4.52 10–19J D 4.52 10–20J This question covers TEKS 2C. This question tests the material that was covered in the textbook on pages 123–124. This question covers TEKS 2B. This question tests the material that was covered in the textbook on page 118. Reviewing Chemistry: Mastering the TEKS Chemistry: Matter and Change 9 CHAPTER 5 Electrons in Atoms, continued Name: 5 Date: Which of these is the ground-state electron configuration for an atom of fluorine (atomic number = 9)? A 1s22s2 B 1s22s22p3 C 1s22s22p4 D 1s22s22p5 7 Which of these orbital diagrams represents a chlorine atom in the ground state? Chlorine has an atomic number of 17. A B This question covers TEKS 6A. This question tests the material that was covered in the textbook on pages 135–139. C 6 The electron configuration for an atom of iron is [Ar] 3d64s2. Which of the following is the correct electron-dot structure for iron? A Fe Fe C Fe Fe This question covers TEKS 6A. This question tests the material that was covered in the textbook on pages 140–141. 2p 1s 2s 2p 1s 2s 2p 3s 3p 1s 2s 2p 3s 3p This question covers TEKS 2D and 5A. This question tests the material that was covered in the textbook on page 137. 8 The arrangement of electrons in an atom of an element determines the chemical properties of that element. Our present-day understanding of how electrons are arranged in an atom is the result of all of these scientific contributions EXCEPT — A Rutherford’s gold foil experiment that proved the existence of the nucleus B Bohr’s orbits that explained hydrogen’s quantized energy states C De Broglie’s equation that led to thinking of electrons as both particles and waves D Schrödinger’s wave equation that predicted atomic orbitals This question covers TEKS 3C and 3E. This question tests the material that was covered in the textbook on pages 127–132. 10 Chemistry: Matter and Change Reviewing Chemistry: Mastering the TEKS Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc. B D D 1s 2s