* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download The Structure of the Atom
Survey
Document related concepts
Transcript
Name Date CHAPTER 4 Class STUDY GUIDE FOR CONTENT MASTERY The Structure of the Atom Section 4.1 Early Theories of Matter In your textbook, read about the philosophers, John Dalton, and defining the atom. For each statement below, write true or false. 1. Ancient philosophers regularly performed controlled experiments. 2. Philosophers formulated explanations about the nature of matter based on their own experiences. 3. Both Democritus and Dalton suggested that matter is made up of atoms. 4. Dalton’s atomic theory stated that atoms separate, combine, or rearrange in chemical reactions. 5. Dalton’s atomic theory stated that matter is mostly empty space. 6. Dalton was correct in thinking that atoms could not be divided into smaller particles. 7. Dalton’s atomic theory stated that atoms of different elements combine in Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. simple whole-number ratios to form compounds. 8. Dalton thought that all atoms of a specific element have the same mass. 9. Democritus proposed that atoms are held together by chemical bonds, but no one believed him. 10. Dalton’s atomic theory was based on careful measurements and extensive research. 11. There are no instruments powerful enough to magnify atoms so that they can be seen. 12. The smallest particle of an element that retains the properties of that element is called an atom. Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 4 19 Name Date CHAPTER 4 Class CHAPTER ASSESSMENT The Structure of the Atom Reviewing Vocabulary Match each definition in Column A with the term in Column B. Column A Column B 1. Radiation deflected toward the positively charged plate a. atom 2. Atoms with the same number of protons but different numbers b. nucleus of neutrons c. atomic mass 3. High-energy radiation that has no charge and no mass 4. The smallest particle of an element that retains the properties of that element d. isotopes e. gamma ray f. 6. The center-most part of an atom where the protons and neutrons g. beta radiation are contained h. atomic mass unit 7. Radiation deflected toward the negatively charged plate Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. alpha radiation 5. The weighted average mass of an element’s isotopes 8. The rays and particles emitted by radioactive material i. radiation 9. Equal to 1/12 the mass of a carbon-12 atom j. Dalton’s atomic theory 10. Ray of radiation traveling from the cathode to the anode 11. Process (not requiring energy) by which unstable nuclei lose energy 12. States that all matter is composed of atoms k. cathode ray l. radioactivity m. radioactive 13. Process whereby some substances spontaneously emit radiation decay Compare and contrast each pair of related terms. 14. mass number, atomic number 15. nuclear reaction, nuclear equation Chapter Assessment Chemistry: Matter and Change • Chapter 4 19 Name CHAPTER Section 4.3 Date 4 Class STUDY GUIDE FOR CONTENT MASTERY How Atoms Differ In your textbook, read about atomic number. For each statement below, write true or false. 1. The number of neutrons in an atom is referred to as its atomic number. 2. The periodic table is arranged by increasing atomic number. 3. Atomic number is equal to the number of electrons in an atom. 4. The number of protons in an atom identifies it as an atom of a particular element. 5. Most atoms have either a positive or a negative charge. Answer the following questions. 6. Lead has an atomic number of 82. How many protons and electrons does lead have? 7. Oxygen has 8 electrons. How many protons does oxygen have? 8. Zinc has 30 protons. What is its atomic number? Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 9. Astatine has 85 protons. What is its atomic number? 10. Rutherfordium has an atomic number of 104. How many protons and electrons does it have? 11. Polonium has an atomic number of 84. How many protons and electrons does it have? 12. Nobelium has an atomic number of 102. How many protons and electrons does it have? In your textbook, read about isotopes and mass number. Determine the number of protons, electrons, and neutrons for each isotope described below. 13. An isotope has atomic number 19 and mass number 39. 14. An isotope has 14 electrons and a mass number of 28. 15. An isotope has 21 neutrons and a mass number of 40. Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 4 21 Name Date CHAPTER 4 Class STUDY GUIDE FOR CONTENT MASTERY Section 4.3 continued 16. An isotope has an atomic number 51 and a mass number 123. Answer the following question. 17. Which of the isotopes in problems 13–16 are isotopes of the same element? Identify the element. Write each isotope below in symbolic notation. Use the periodic table to determine the atomic number of each isotope. 18. neon-22 20. cesium-133 19. helium 21. uranium-234 Label the mass number and the atomic number on the following isotope notation. 22. 24Mg 12 23. Circle the letter of the choice that best completes the statement. 24. The mass of an electron is 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 a. 1/12 the mass of a carbon-12 atom. b. 1/16 the mass of an oxygen-16 atom. c. exactly the mass of one proton. d. approximately the mass of one proton plus one neutron. 26. The atomic mass of an atom is usually not a whole number because it accounts for a. only the relative abundance of the atom’s isotopes. b. only the mass of each of the atom’s isotopes. c. the mass of the atom’s electrons. d. both the relative abundance and the mass of each of the atom’s isotopes. 22 Chemistry: Matter and Change • Chapter 4 Study Guide for Content Mastery Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. In your textbook, read about mass of individual atoms. Name Date CHAPTER 4 Class STUDY GUIDE FOR CONTENT MASTERY Section 4.3 continued Use the figures to answer the following questions. Osmium 76 Niobium 41 Os Nb 190.2 92.906 27. What is the atomic number of osmium? 28. What is the chemical symbol for niobium? 29. What is the atomic mass of osmium? 30. What units is the atomic mass reported in? 31. How many protons and electrons does an osmium atom have? A niobium atom? Calculate the atomic mass of each element described below. Then use the periodic table to identify each element. Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 32. 33. Isotope Mass (amu) Percent Abundance 63X 62.930 69.17 65X 64.928 30.83 Isotope Mass (amu) Percent Abundance 35X 34.969 75.77 37X 36.966 24.23 Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 4 23 Name Date 1 Enrichment Class How do isotopes differ? Chapter 9 Directions: Most elements exist in nature as isotopes. Isotopes of an element are almost identical in their chemical properties and reactions. However, the nuclear properties of isotopes are different. Not only do isotopes differ in mass, but some may be radioactive. Using a periodic table, complete the information in the chart below. Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 1. 1 1H 2. 2 1H 3. 3 1H 4. 4 2 He Atomic number Number of protons Mass number Number of neutrons 1 1 Meeting Individual Needs Symbol 1 3 2 2 5. 12 6C 12 6. 14 6C 14 7. 18 8O 18 8. 49 21 Sc 9. 63 27 Co 10. 212 82 Pb 212 11. 222 88 Ra 222 12. 226 88 Ra 226 13. 235 92 U 235 14. 238 92 U 238 21 28 63 Radioactivity and Nuclear Reactions 31 Name Date Directed Reading for Content Mastery Section 1 ■ Section 2 ■ Class Structure of the Atom Masses of Atoms Chapter 18 Directions: Use the terms below to complete the following paragraphs about atoms , atomic mass, and isotopes. Terms may be used more than once. six number electrons isotopes electron cloud neutron(s) proton(s) mass quarks six protons The electron has very little mass compared to the 1. ________________ or many 3. ________________ and 4. ________________ it has. The sum of the protons and neutrons is the mass 5. ________________ of an atom. The number of neutrons in an atom can be found by subtracting the atomic number from the 6. ________________ number. The mass of the atom is so small that there is a measure called the atomic 7. ________________ unit designated by amu. 8. ________________ and 9. ________________ make up the nucleus and are made up of 10. ________________. There are 11. ________________ uniquely different quarks. 12. ________________ are found in an area around the nucleus called the 13. ________________. The nuclei of all atoms of a given element always have the same number of 14. ________________. They will also have the same number of 15. ________________ around the nucleus. Some atoms may have more or fewer 16. ________________ than will other atoms of the same element. Atoms of the same element with different numbers of neutrons are called 17. ________________. Every atom of carbon must contain 18. ________________ but some contain six neutrons and others have eight neutrons. 20 Properties of Atoms and the Periodic Table Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Meeting Individual Needs 2. ________________. The mass of the atom depends on the nucleus and how Name 2 Date Reinforcement Masses of Atoms Class Chapter 18 Directions: Answer the following questions on the lines provided. 1. What are isotopes? 3. What is the average atomic mass of an element? 4. Compare and contrast the atomic structure of the chlorine-35 and chlorine-37 isotopes. 5. Suppose that a newly discovered element called centium has three isotopes that occur in nature. These are centium-200, centium-203, and centium-209. Assume that these isotopes occur in equal amounts in nature. What will be the average atomic mass of this element? 28 Properties of Atoms and the Periodic Table Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Meeting Individual Needs 2. How do Boron-10 and Boron-11 differ? Name Date CHAPTER 4 Class CHAPTER ASSESSMENT Understanding Main Ideas (Part B) For each description in Column A, write the letter of the matching symbol in Column B. Column A Column B 1. Isotope in which the number of neutrons is six more than the isotope’s atomic number a. 178O b. 63 29Cu 2. Copper-63 c. 126C 3. Copper with seven neutrons more than its atomic number 4. Isotope that has one neutron more than its number of protons 5. Carbon with equal numbers of neutrons, protons, and electrons 6. Carbon with two more neutrons than its number of protons 7. Chromium with two more neutrons than its number of protons d. 50 24Cr e. 146C f. 65Cu 29 g. 52 24Cr h. 54 24Cr 8. Isotope in which the difference between the neutrons and number of protons is 4 Answer the following questions. 9. Calculate the atomic mass of gallium (Ga). Gallium has two isotopes: 69Ga and 71Ga. Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. 69Ga has a relative abundance of 60.12% and an atomic mass of 68.9257 amu. 71Ga has a relative abundance of 39.88% and an atomic mass of 70.9249 amu. Show all your work. 10. Calculate the atomic mass of the element X. Then use the periodic table to identify the element. Show all your work. Isotope Mass (amu) Percent Abundance 27X 27.977 92.23 28X 28.976 4.67 29X 29.974 3.10 Chapter Assessment Chemistry: Matter and Change • Chapter 4 21 Name Date 4 Reinforcement Class Chapter Nuclear Reactions 9 Directions: Use the diagrams below to complete the following activities. 1p 1n + 1p 1n 2p 2n Energy 56p 85n n n 92p 143n n n Ene rgy 36p 56n 1. The diagrams show two types of nuclear reactions: nuclear fission and nuclear fusion. Label the type of reaction shown in each diagram in the space provided. 2. Circle the letter of the equation that correctly explains the nuclear reaction shown in the top diagram. a. H-2 + H-2 → H-4 c. H-1 + H-1 → H-2 b. H-2 + H-2 → He-4 d. H-1 + H-1 → He-2 3. Circle the letter of the equation that correctly explains the nuclear reaction shown in the bottom diagram. a. 1 neutron + U-235 → Ba-141 + Kr-92 + 3 neutrons + energy b. 1 neutron + U-238 → Ba-141 + Kr-92 + 4 neutrons c. Ba-141 + Kr-92 → U-235 + 3 neutrons d. Ba-141 + Kr-92 → U-238 4. What two elements are involved in the nuclear fusion reaction? 5. Label each atom in the fusion reaction with its correct symbol and isotope notation. 6. What three elements are involved in the fission reaction shown? 7. Label each atom in the nuclear fission reaction with its chemical symbol and its correct isotope notation. 30 Radioactivity and Nuclear Reactions Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Meeting Individual Needs gy Ener + Name Date 4 CHAPTER Section 4.4 Class STUDY GUIDE FOR CONTENT MASTERY Changes to the Nucleus—Nuclear Reactions In your textbook, read about radioactivity. For each item in Column A, write the letter of the matching item in Column B. Column A Column B 1. The rays and particles that are emitted by a radioactive material a. nuclear reaction 2. A reaction that involves a change in an atom’s nucleus b. beta radiation 3. The process in which an unstable nucleus loses energy c. radiation spontaneously d. radioactive decay 4. Fast-moving electrons In your textbook, read about types of radiation. Use the diagram to answer the questions. Hole Gamma rays (no charge) Alpha particles (2 charge) Radioactive source Negative plate Zinc sulfide coated screen 5. Which plate do the beta particles bend toward? Explain. 6. Explain why the gamma rays do not bend. 7. Explain why the path of the beta particles bends more than the path of the alpha particles. Complete the following table of the characteristics of alpha, beta, and gamma radiation. Radiation Type Composition Symbol Mass (amu) Charge 8. Alpha 9. 10. 24 1/1840 High-energy electromagnetic radiation Chemistry: Matter and Change • Chapter 4 Study Guide for Content Mastery Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Lead block Beta particles (1 charge) Positive plate CHAPTER 4 The Structure of the Atom Name: Date: Use the diagram below to answer question 1. + + + + 92 p + + proton (p) + neutron (n) 146 n + + + + uranium-238 nucleus daughter (parent nucleus) nucleus ++ Use the chart below to answer questions 3 and 4. 2p 2n Element Atomic Isotope # helium-4 nucleus (alpha particle) hydrogen hydrogen-1 hydrogen-2 1.01 amu 2.01 amu 99.985 0.015 6 carbon-12 carbon-13 carbon-14 12.00 amu 13.00 amu 14.00 amu 98.90 1.09 0.01 8 oxygen-16 oxygen-17 oxygen-18 15.99 amu 17.00 amu 18.00 amu 98.90 0.038 0.200 copper-63 copper-65 62.94 amu 64.93 amu 69.17 30.83 1 carbon Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc. 1 The diagram above illustrates a nuclear reaction in which uranium-238 emits an alpha particle. How many protons and neutrons will the daughter nucleus have? A 90 p and 144 n B 92 p and 142 n C 92 p and 150 n D 94 p and 148 n oxygen copper 29 3 This question covers TEKS 6B. This question tests the material that was covered in the textbook on page 106. 2 In his latest dig, Dr. Butrell found an abundance of lead (Pb) in some ancient artifacts. What is the atomic number of Pb? A 80 B 81 C 82 D 83 This question covers TEKS 3D. This question tests the material that was covered in the textbook on page 105. % Atomic mass of isotope abundance The chart shows isotopes of some common elements. Which property is used to name the isotopes? A Atomic number B Atomic mass C Mass number D Percent natural occurrence This question covers TEKS 6B. This question tests the material that was covered in the textbook on page 100. 4 The atomic mass of an element is the weighted average mass of the isotopes of that element. Based on this definition, which of these does NOT show the correct atomic mass for an element? A Hydrogen: 1.008 amu B Carbon: 12.011 amu C Oxygen: 15.999 amu D Copper: 63.017 amu This question covers TEKS 6B. This question tests the material that was covered in the textbook on page 104. Reviewing Chemistry: Mastering the TEKS Chemistry: Matter and Change 7 CHAPTER 4 The Structure of the Atom, continued Name: Date: Use the diagram below to answer question 5. Use the diagram below to answer question 7. rays alpha particle + —nucleus of gold atom paths of alpha particles + + rays rays + - + + 5 The diagram above shows the results of Rutherford’s experiment in which he used a radioactive source to “shoot” alpha particles at a thin sheet of gold foil. Based on these results, what were Rutherford’s conclusions? Atoms are solid matter with positive and negative charges scattered throughout. B Atoms are solid, positively charged matter with negatively charged electrons scattered throughout. C 7 Atoms are mostly empty space with small, dense, positively charged centers. D Atoms are mostly empty space with small, dense, negatively charged centers. This question covers TEKS 3A. This question tests the material that was covered in the textbook on page 95. 6 The cathode ray tube is a key component of which of the following revolutionary inventions? A Automobile B Fax machine C Television D Photocopier This question covers TEKS 3C. This question tests the material that was covered in the textbook on pages 92–93. 8 Chemistry: Matter and Change The diagram above shows how alpha, beta, and gamma rays are affected by two electrically charged plates. Based on the paths the rays follow, what are the respective charges of alpha, beta, and gamma rays? A negative, positive, none B positive, negative, none C negative, none, positive D positive, none, negative This question covers TEKS 6A. This question tests the material that was covered in the textbook on page 106. 8 In the fourth century BC, Greek scholars rejected Democritus’s ideas about the atom. This rejection was most likely based on — A experimentation B government legislation C religious beliefs D the popularity of Aristotle’s ideas on nature This question covers TEKS 3C. This question tests the material that was covered in the textbook on page 89. Reviewing Chemistry: Mastering the TEKS Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc. A radioactive substance lead shield