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Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Study Guide for Content Mastery Answer Key Name Date CHAPTER 4 Class Name Date 4 CHAPTER STUDY GUIDE FOR CONTENT MASTERY The Structure of the Atom Section 4.2 Class STUDY GUIDE FOR CONTENT MASTERY Subatomic Particles and the Nuclear Atom In your textbook, read about discovering the electron and the nuclear atom. Section 4.1 For each item in Column A, write the letter of the matching item in Column B. Early Theories of Matter Column A In your textbook, read about the philosophers, John Dalton, and defining the atom. For each statement below, write true or false. false true 1. Ancient philosophers regularly performed controlled experiments. 2. Philosophers formulated explanations about the nature of matter based on Column B c 1. Proposed the nuclear atomic model a. Thomson a 2. Determined the mass-to-charge ratio of an electron b. Millikan b 3. Calculated the mass of an electron c. Rutherford their own experiences. true 3. Both Democritus and Dalton suggested that matter is made up of atoms. true 4. Dalton’s atomic theory stated that atoms separate, combine, or rearrange Draw and label a diagram of each atomic model. 4. plum pudding model Drawing should look like a ball of chocolate chip cookie dough. The chocolate chips should be labeled with negative charge or as electrons. The dough should be labeled as evenly distributed positive charges. in chemical reactions. false 5. Dalton’s atomic theory stated that matter is mostly empty space. false 6. Dalton was correct in thinking that atoms could not be divided into smaller particles. true 7. Dalton’s atomic theory stated that atoms of different elements combine in true 8. Dalton thought that all atoms of a specific element have the same mass. false 9. Democritus proposed that atoms are held together by chemical bonds, but simple whole-number ratios to form compounds. 5. nuclear atomic model Drawing should look like a peach with a pit. The pit should be labeled nucleus and should include labeled protons and neutrons. The outer circle of the peach should be labeled electrons. no one believed him. true 10. Dalton’s atomic theory was based on careful measurements and extensive research. Chemistry: Matter and Change false 11. There are no instruments powerful enough to magnify atoms so that they can be seen. true 12. The smallest particle of an element that retains the properties of that element is called an atom. In your textbook, read about the discovery of protons and neutrons. Complete the following table of proton, electron, and neutron characteristics. Particle T167 Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 4 19 Symbol Location Relative Charge Relative Mass 6. Proton p In the nucleus 1 1 7. Neutron n0 In the nucleus 0 1 8. Electron e In the space surrounding the nucleus 1 1/1840 20 Chemistry: Matter and Change • Chapter 4 Study Guide for Content Mastery T168 Name Date CHAPTER 4 Class Name STUDY GUIDE FOR CONTENT MASTERY Date CHAPTER 4 Class STUDY GUIDE FOR CONTENT MASTERY Chemistry: Matter and Change Section 4.3 continued Section 4.3 How Atoms Differ 16. An isotope has an atomic number 51 and a mass number 123. 51 protons, 51 electrons, 72 neutrons In your textbook, read about atomic number. For each statement below, write true or false. false 1. The number of neutrons in an atom is referred to as its atomic number. Answer the following question. true 2. The periodic table is arranged by increasing atomic number. 17. Which of the isotopes in problems 13–16 are isotopes of the same element? Identify the true 3. Atomic number is equal to the number of electrons in an atom. true 4. The number of protons in an atom identifies it as an atom of a false 5. Most atoms have either a positive or a negative charge. element. The two isotopes with atomic number 19 are both isotopes of potassium. particular element. Write each isotope below in symbolic notation. Use the periodic table to determine the atomic number of each isotope. 18. neon-22 Answer the following questions. 19. helium 22Ne 10 20. cesium-133 4He 2 21. uranium-234 133Cs 55 234U 92 6. Lead has an atomic number of 82. How many protons and electrons does lead have? 82 protons; 82 electrons Label the mass number and the atomic number on the following isotope notation. 8 protons 7. Oxygen has 8 electrons. How many protons does oxygen have? 8. Zinc has 30 protons. What is its atomic number? 9. Astatine has 85 protons. What is its atomic number? 30 85 22. mass number 23. atomic number 24Mg 12 In your textbook, read about mass of individual atoms. 10. Rutherfordium has an atomic number of 104. How many protons and electrons does it have? Circle the letter of the choice that best completes the statement. 104 protons; 104 electrons 24. The mass of an electron is Study Guide for Content Mastery Answer Key 11. Polonium has an atomic number of 84. How many protons and electrons does it have? 84 protons; 84 electrons a. smaller than the mass of a proton. c. a tiny fraction of the mass of an atom. b. smaller than the mass of a neutron. d. all of the above. 25. One atomic mass unit is 12. Nobelium has an atomic number of 102. How many protons and electrons does it have? a. 1/12 the mass of a carbon-12 atom. 102 protons; 102 electrons b. 1/16 the mass of an oxygen-16 atom. c. exactly the mass of one proton. In your textbook, read about isotopes and mass number. d. approximately the mass of one proton plus one neutron. Determine the number of protons, electrons, and neutrons for each isotope described below. 26. The atomic mass of an atom is usually not a whole number because it accounts for 13. An isotope has atomic number 19 and mass number 39. a. only the relative abundance of the atom’s isotopes. 19 protons, 19 electrons, 20 neutrons b. only the mass of each of the atom’s isotopes. 14. An isotope has 14 electrons and a mass number of 28. c. the mass of the atom’s electrons. 14 protons, 14 electrons, 14 neutrons d. both the relative abundance and the mass of each of the atom’s isotopes. 15. An isotope has 21 neutrons and a mass number of 40. 19 protons, 19 electrons, 21 neutrons Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 4 Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 21 22 Chemistry: Matter and Change • Chapter 4 Study Guide for Content Mastery Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Study Guide for Content Mastery Answer Key Name Date CHAPTER 4 Class Name STUDY GUIDE FOR CONTENT MASTERY Date 4 CHAPTER Class STUDY GUIDE FOR CONTENT MASTERY Section 4.3 continued Use the figures to answer the following questions. Section 4.4 Changes to the Nucleus—Nuclear Reactions In your textbook, read about radioactivity. Osmium 76 Niobium 41 Os Nb 190.2 92.906 For each item in Column A, write the letter of the matching item in Column B. Column A 76 27. What is the atomic number of osmium? Nb 28. What is the chemical symbol for niobium? 30. What units is the atomic mass reported in? 1. The rays and particles that are emitted by a radioactive material a. nuclear reaction a 2. A reaction that involves a change in an atom’s nucleus b. beta radiation d 3. The process in which an unstable nucleus loses energy c. radiation spontaneously 190.2 29. What is the atomic mass of osmium? Column B c b d. radioactive decay 4. Fast-moving electrons atomic mass units In your textbook, read about types of radiation. 31. How many protons and electrons does an osmium atom have? A niobium atom? Use the diagram to answer the questions. osmium: 76 protons, 76 electrons; niobium: 41 protons, 41 electrons Lead block Beta particles (1 charge) Positive plate Hole Calculate the atomic mass of each element described below. Then use the periodic table to identify each element. 32. Isotope Mass (amu) Gamma rays (no charge) Percent Abundance 63X 62.930 69.17 65X 64.928 30.83 Chemistry: Matter and Change (62.930 amu)(69.17%) 43.53 amu 65X: (64.928 amu)(30.83%) 20.02 amu ␣ Negative plate Zinc sulfide coated screen the positive plate, because beta particles are negatively charged 6. Explain why the gamma rays do not bend. Gamma rays have no charge. The element is copper. Isotope ␥ 5. Which plate do the beta particles bend toward? Explain. Atomic mass of X 43.53 amu 20.02 amu 63.55 amu 33. Alpha particles (2 charge) Radioactive source Mass contribution (mass)(percent abundance) 63X:  7. Explain why the path of the beta particles bends more than the path of the alpha particles. Mass (amu) Percent Abundance 35X 34.969 75.77 37X 36.966 24.23 The beta particles have less mass than the alpha particles and are more greatly affected by the electric field. Complete the following table of the characteristics of alpha, beta, and gamma radiation. Mass contribution (mass)(percent abundance) 35X: (34.969 amu)(75.77%) 26.50 amu 37X: (36.966 amu)(24.23%) 8.957 amu Radiation Type Atomic mass of X 26.50 amu 8.957 amu 35.46 amu T169 Chemistry: Matter and Change • Chapter 4 Symbol 8. Alpha Helium nuclei, or alpha particles 4 2 9. Beta Electrons, or beta particles 4He 2 0 1 1/1840 1 High-energy electromagnetic radiation 0 0 0 0 10. Gamma The element is chlorine. Study Guide for Content Mastery Composition 23 24 Chemistry: Matter and Change • Chapter 4 Mass (amu) Charge Study Guide for Content Mastery