Atomic Structure CONTENT REVIEW. indicates a fluorine atom that contains
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1 Atomic Structure Multiple Choice Identify the letter the choice that best completes the statement or answers the question. CONTENT REVIEW 1. Which the following statements is part Dalton's atomic theory matter? a. All atoms are identical. b. All atoms a given element are identical. c. All atoms differ from one another. d. All atoms a given element have the same mass. 2. The electron was discovered by a. Thomson. c. Millikan. b. Faraday. d. Rutherford. 3. Rutherford called the core the atom the a. neutron. c. nucleus. b. proton. d. electron. 4. Which the following particles is normally found outside the nucleus the atom? a. electron c. neutron b. proton d. alpha particle 5. The atomic number an atom is defined as its a. mass in amu. c. number neutrons. b. number electrons. d. number protons. 6. The mass number an atom is defined as its a. mass in amu. c. total number protons and electrons. b. number protons. d. total number neutrons and protons. 7. An element's identity is based on its a. atomic mass. c. number neutrons. b. mass number. d. atomic number. 8. An ion always contains an a. unequal number protons and electrons. b. equal number protons and electrons. c. unequal number protons and neutrons. d. equal number protons and neutrons. 9. Two atoms are isotopes if they contain a. different numbers electrons. b. different numbers protons and different numbers neutrons. c. the same number protons but different numbers neutrons. d. the same number neutrons but different numbers protons. 10. The symbol indicates a fluorine atom that contains a. 19 protons and 9 neutrons c. 9 protons and 19 neutrons. b. 9 protons and 10 neutrons. d. 9 protons and 10 electrons.
2 Figure Which the four particles in the atom illustrated in Figure 3-3 represents a neutron? 12. Which the particles in Figure 3-3 represents an electron? 13. Which the particles in Figure 3-3 represents a nucleus? 14. What type structure is represented by the entirety Figure 3-3? a. negatively charged ion c. positively charged atom b. negatively charged atom d. positively charged ion 15. In Figure 3-3, what is the atom's atomic number? a. 1 c. 4 b. 3 d What charge does the structure in Figure 3-3 have? a. 1- c. 2+ b. 1+ d In Figure 3-3, what is the mass number the ion? a. 1 c. 4 b. 3 d. 7 Isotope Atomic number Mass number protons neutrons electrons Charge L M Figure How many protons are in the nucleus isotope L in Figure 3-4? a. 30 c. 28 b. 36 d What is the mass number isotope L in Figure 3-4?
3 a. 30 c. 64 b. 36 d What is the charge the ion isotope L in Figure 3-4? a. 2- c. 6+ b. 2+ d What is the atomic number isotope M in Figure 3-4? a. 80 c. 35 b. 45 d What is the number neutrons in the ion isotope M in Figure 3-4? a. 45 c. 80 b. 79 d In Figure 3-4, what is the number electrons in the ion isotope M? a. 1 c. 36 b. 34 d How would isotope L in Figure 3-4 have to change in order to have the same charge as isotope M? a. Isotope L would have to gain three electrons. b. Isotope L would have to lose three protons. c. Isotope L would have to gain three neutrons. d. Isotope L would have to lose three electrons. Essay PROBLEM SOLVING Use the skills you have developed in this chapter to solve each problem. 25. Using a periodic table, how many protons and how many electrons are there in an ion Al 3+? 26. Using a periodic table, write the formula for an ion that contains 34 protons and 36 electrons. 27. Using a periodic table, write the formula for an ion that contains 19 protons and 18 electrons. 28. Using a periodic table, how many electrons and protons are there in a phosphorus atom that has three excess electrons? Write the symbol for the ion. 29. Using a periodic table, determine the number protons, neutrons, and electrons in the ion Cr 3+.
4 Atomic Structure Answer Section MULTIPLE CHOICE 1. B 2. A 3. C 4. A 5. D 6. D 7. D 8. A 9. C 10. B 11. B 12. C 13. D 14. D 15. B 16. B 17. D 18. A 19. D 20. B 21. C 22. A 23. C 24. A ESSAY 25. Aluminum's atomic number is 13, so it has 13 protons. The ion, Al 3+, has three more protons than electrons, so it has 13 minus 3, or 10, electrons. 26. An atom with 34 protons has atomic number 34 and must therefore be an atom selenium (Se). The uncharged atom also has 34 electrons. The two extra electrons give the ion a 2 charge, so the symbol is Se An atom with 19 protons has atomic number 19 and must therefore be an atom potassium (K). The uncharged atom also has 19 electrons. The deficit one electron gives the ion a net charge 1+, so the symbol is K Phosphorus (P) has an atomic number 15. Since the ion has an excess three electrons, it has = 18 electrons. This excess indicates a charge 3. The symbol is P = mass number = total number protons and neutrons 24 = atomic number = number protons = 28 = number neutrons
5 3+ = charge = number protons - number electrons 24 - x = 3+; x = number electrons = 21
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