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Page 1 of 4 Chapter Review A substance’s atomic structure determines its physical and chemical properties. CONTENT REVIEW CLASSZONE.COM KEY CONCEPTS SUMMARY 1 2 Atoms are the smallest form of elements. VOCABULARY • All matter is made of the atoms of approximately 100 elements. • Atoms are made of protons, neutrons, and electrons. • Different elements are made of different atoms. • Atoms form ions by gaining or losing electrons. proton p. 331 neutron p. 331 nucleus p. 331 electron p. 331 atomic number p. 332 atomic mass number p. 332 isotope p. 332 ion p. 334 nucleus proton neutron electron cloud Elements make up the periodic table. VOCABULARY • Elements can be organized by similarities. • The periodic table organizes the atoms of the elements by properties and atomic number. atomic mass p. 337 periodic table p. 338 group p. 342 period p. 342 Groups of elements have similar properties. Elements in a period have varying properties. 3 The periodic table is a map of the elements. VOCABULARY • The periodic table has distinct regions. • Most elements are metals. • Nonmetals and metalloids have a wide range of properties. • Some atoms can change their identity through radioactive decay. reactive p. 346 metal p. 347 nonmetal p. 349 metalloid p. 350 radioactivity p. 350 half-life p. 352 354 Unit 3: Chemical Interactions Page 2 of 4 Reviewing Vocabulary Describe how the vocabulary terms in the following pairs are related to each other. Explain the relationship in a one- or two-sentence answer. Underline each vocabulary term in your answer. 1. isotope, nucleus 2. atomic mass, atomic number 3. electron, proton 4. atomic number, atomic mass number 5. group, period 6. metals, nonmetals 7. radioactivity, half-life Reviewing Key Concepts Multiple Choice Choose the letter of the best answer. 8. The central part of an atom is called the a. electron c. proton b. nucleus d. neutron 9. The electric charge on a proton is a. positive c. neutral b. negative d. changing 10. The number of protons in the nucleus is the a. atomic mass c. atomic number b. isotope d. half-life 11. Nitrogen has atomic number 7. An isotope of nitrogen containing seven neutrons would be a. nitrogen-13 c. nitrogen-15 b. nitrogen-14 d. nitrogen-16 12. How does the size of a negative ion compare to the size of the atom that formed it? a. It’s smaller. b. It’s larger. c. It’s the same size. d. It varies. 13. The modern periodic table is organized by a. size of atom b. atomic mass c. number of neutrons d. atomic number 14. Elements in a group have a. a wide range of chemical properties b. the same atomic radius c. similar chemical properties d. the same number of protons 15. Elements in a period have a. a wide range of chemical properties b. the same atomic radius c. similar chemical properties d. the same number of protons 16. From left to right in a period, the size of atoms a. increases c. remains the same b. decreases d. shows no pattern 17. The elements in Group 1 of the periodic table are commonly called the a. alkali metals c. alkaline earth metals b. transition metals d. rare earth metals 18. The isotope nitrogen-13 has a half-life of 10 minutes. If you start with 40 grams of this isotope, how many grams will you have left after 20 minutes? a. 10 c. 20 b. 15 d. 30 Short Answer Write a short answer to each question. You may need to consult a periodic table. 19. Rubidium forms the positive ion Rb+. Is this ion larger or smaller than the neutral atom? Explain. 20. How can you find the number of neutrons in the isotope nitrogen-16? 21. Explain how density varies across and up and down the periodic table. 22. Place these elements in order from least reactive to most reactive: nickel (Ni), xenon (Xe), lithium (Li). How did you determine the order? Chapter 10: Atomic Structure and the Periodic Table 355 Page 3 of 4 Below is an element square from the periodic table. Use it to answer the next two questions. Thinking Critically The table below lists some properties of six elements. Use the information and your knowledge of the properties of elements to answer the next three questions. Element Appearance Density (g/cm3) Conducts Electricity A dark purple crystals 4.93 no B shiny silvery solid 0.97 yes C shiny silvery solid 22.65 yes D yellow powder 2.07 no E shiny gray solid 5.32 semiconductor F shiny bluish solid 8.91 yes 23. ANALYZE Based on the listed properties, identify each of the elements as a metal, nonmetal, or metalloid. 80 Hg Mercury 200.59 29. CALCULATE One of the more common isotopes of mercury is mercury-200. How many protons and neutrons are in the nucleus of mercury-200? 30. INFER Cadmium occupies the square directly above mercury on the periodic table. Is a cadium atom larger or smaller than a mercury atom? 31. CALCULATE An isotope has a half-life of 40 minutes. How much of a 100-gram sample would remain unchanged after two hours? 32. APPLY When a uranium atom with 92 protons and 146 neutrons undergoes radioactive decay, it produces a particle that consists of two protons and two neutrons from its nucleus. Into which element is the uranium atom transformed? 24. APPLY Which would weigh more: a cube of element A or a same-sized cube of element D? 25. HYPOTHESIZE Which element(s) do you think you might find in electronic devices? Why? 33. ANALYZE Look again at the photograph on pages 326–327. Answer the question again, using what you have learned in the chapter. 26. HYPOTHESIZE The thyroid gland, located in your throat, secretes hormones. In 1924 iodine was added to table salt. As more and more Americans used iodized salt, the number of cases of thyroid diseases decreased. Write a hypothesis that explains the observed decrease in thyroid-related diseases. 34. DRAW CONCLUSIONS Suppose you’ve been given the ability to take apart and assemble atoms. How could you turn lead into gold? 27. INFER How does the size of a beryllium (Be) atom compare with the size of an oxygen (O) atom? 28. PREDICT Although noble gases do not naturally react with other elements, xenon and krypton have been made to react with halogens such as chlorine in laboratories. Why are the halogens most likely to react with the noble gases? 356 Unit 3: Chemical Interactions 35. ANALYZE Explain how the structure of an atom determines its place in the periodic table. If you are doing a unit project, make a folder for your project. Include in your folder a list of the resources you will need, the date on which the project is due, and a schedule to track your progress. Begin gathering data. Page 4 of 4 Standardized Test Practice For practice on your state test, go to . . . TEST PRACTICE CLASSZONE.COM Interpreting Tables The table below shows part of the periodic table of elements. Group 1 Period 1 2 3 4 18 1 H 2 2 13 14 15 16 17 He 3 4 5 6 7 8 9 10 Li Be B C N O F Ne 11 12 13 14 15 16 17 18 Al Si P S Cl Ar Na Mg 19 20 31 32 33 34 35 36 K Ca Ga Ge As Se Br Kr Answer the questions based on the information given in the table. 1. What does the number above the symbol for each element represent? a. Its number of isotopes b. Its atomic number c. Its number of neutrons d. Its atomic mass 2. The atom of what element is in Period 4, Group 13? a. Na c. Al b. Ga d. K Extended Response Answer the following two questions in detail. Include some of the terms shown in the word box at right. Underline each term you use in your answer. 7. Democritus was an ancient Greek philosopher who claimed that all matter was made of tiny particles he called atoms. Democritus said that all atoms were made of the same material. The objects of the world differed because each was made of atoms of different sizes and shapes. How does the modern view of atoms differ from this ancient view? How is it similar? 3. What do the elements on the far right of the table (He, Ne, Ar, and Kr) have in common? a. They do not generally react with other elements. b. They are in liquids under normal conditions. c. They are metals that rust easily. d. They are very reactive gases. 4. How many electrons does a neutral chlorine (Cl) atom contain? a. 16 c. 18 b. 17 d. 19 5. If a sodium (Na) atom loses one electron to form a positive ion, how many electrons would lithium (Li) lose to form a positive ion? a. 0 c. 2 b. 1 d. 3 6. If a fluorine (F) atom gains one electron to form a negative ion, how many electrons would bromine (Br) gain to form a negative ion? a. 0 c. 2 b. 1 d. 3 electron isotope nucleus neutron proton radioactivity 8. Half-life is a measure of the time it takes half of the radioactive atoms in a substance to decay into other atoms. If you know how much radioactive material an object had to begin with, how could you use half-life to determine its age now? Chapter 10: Atomic Structure and the Periodic Table 357