Honors Chemistry Study Guide: Chemical Nomenclature, Introduction to the Atom (ch 4, sections 1-3) and the Periodic Table (ch 6, sections 1-2) Provide the correct name or formula for each the following. 1. hydroiodic acid 22. Sulfur hexafluoride 2. HNO 2 23. KF 3. zinc nitrate 24. Barium dihydrogen phosphate 4. Ca(ClO 3 ) 2 25. Pb(OH) 2 5. Hg(OH) 2 26. Mercury (I) carbonate 6. ammonium phosphate 27. Mg(ClO) 2 7. FeI 3 28. Iron (II) oxide 8. zinc phosphide 29. Hydrochloric acid 9. Al 2 O 3 30. Tin (IV) sulfide 10. strontium sulfide 11. ammonium chloride 12. CO 2 13. Carbon tetrachloride 14. H 3 PO 4 15. H 2 Se 16. sulfurous acid 17. Al 2 (SO 4 ) 3 18. cobalt (II) acetate 19. barium phosphate 20. CaH 2 21. BrF Study Guide Honors Chemistry Introduction to the Periodic Table and the Atom 1. An atom is defined as the smallest part an element that a. contains at least one proton, neutron, and electron. b. retains the chemical identity that element. c. can carry an electric charge. d. is affected in a cathode ray tube.
3.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. 4. A cathode ray consists a. protons. c. neutrons. b. electrons. d. gamma rays. 5. The electron was discovered by a. Thomson. c. Millikan. b. Faraday. d. Rutherford. 6. The scientist who measured the charge the electron was a. Thomson. c. Millikan. b. Faraday. d. Rutherford. 7. The experiment that revealed the charge the electron involved the use (5.2) a. gold foil. c. oil droplets. b. photographic film. d. cathode ray tubes. 8. Rutherford called the core the atom the a. neutron. c. nucleus. b. proton. d. electron. 9. Which the following is not one the three fundamental particles that makeup atoms? a. electron c. neutron b. proton d. alpha particle 10. Which the following particles is normally found outside the nucleus the atom? a. electron c. neutron b. proton d. alpha particle 11. What is the approximate atomic mass a neutron, in amu? a. essentially 0 c. 1- b. 9.1 10-28 d. 1 12. What is the approximate atomic mass an electron, in amu? a. essentially 0 c. 1- b. 9.1 10-28 d. 1 13. The atomic number an atom is defined as its a. mass in amu. c. number neutrons. b. number electrons. d. number protons. 14. 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. 15.An element's identity is based on its a. atomic mass. c. number neutrons. b. mass number. d. atomic number. 16.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. 17. 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.
18.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. 19.The atomic mass unit (amu) is defined in terms a. carbon-12. c. oxygen-16. b. carbon-14. d. hydrogen-1. 20. The force that holds protons together is called a. strong nuclear force. c. gravitation. b. electrical attraction. d. static electricity. Isotope Atomic number Mass number protons neutrons electrons Charge L 30 36 28 M 80 35 1 Figure 3-4 21. How many protons are in the nucleus isotope L in Figure 3-4? a. 30 c. 28 b. 36 d. 54 22. What is the mass number isotope L in Figure 3-4? a. 30 c. 64 b. 36 d. 66 23. What is the charge the ion isotope L in Figure 3-4? a. 2- c. 6+ b. 2+ d. 30+ 24. What is the atomic number isotope M in Figure 3-4? a. 80 c. 35 b. 45 d. 115 25. What is the number neutrons in the ion isotope M in Figure 3-4? a. 45 c. 80 b. 79 d. 115 26. In Figure 3-4, what is the number electrons in the ion isotope M? a. 1 c. 36 b. 34 d. 81 27.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. 28. Which the following describes the pattern repetition elemental properties every eight elements? a. the periodic law c. Mendeleev's law b. the law octaves d. Meyer's periodicity 29. The relationship in which the physical and chemical properties elements show a periodic pattern when the elements are arranged by increasing atomic number is called a. the periodic law. c. Mendeleev's law. b. the law octaves. d. Meyer's periodicity. 30. Who classified elements into triads? a. Mendeleev c. Newlands b. Moseley d. Dobereiner
31. The scientist credited with the first periodic table elements was a. Mendeleev. c. Newlands. b. Moseley. d. Dobereiner. 32. The scientist who observed a pattern properties that repeated every eight elements was a. Mendeleev. c. Newlands. b. Moseley. d. Dobereiner. 33. Who discovered the concept atomic number? a. Dobereiner c. Meyer b. Moseley d. Mendeleev 34. Mendeleev arranged the elements in his periodic table in order increasing a. atomic number. c. ionization energy. b. mass number. d. atomic mass. 35. In the periodic table, the periods are the a. vertical columns. c. chemical families. b. horizontal rows. d. blocks elements. 36. How many periods are in the periodic table? a. 7 c. 18 b. 8 d. 109 37.How many labeled groups are in the periodic table? a. 7 c. 18 b. 8 d. 109 38. How many elements are in the first period the periodic table? a. 2 c. 8 b. 7 d. 18 39. The elements in Group 1A the periodic table are called the 40. The elements in Group 2A the periodic table are called the 41. What are the elements in Group 7A the periodic table called? a. Halogens c. alkaline earth metals b. alkali metals d. noble gases 42. The elements in Group 8A the periodic table are called the 43. Malleability is characteristic a. all elements. c. nonmetals. b. semimetals. d. metals. 44. Those electrons that are largely responsible for an atom's chemical behavior are called a. core electrons. c. high energy electrons. b. valence electrons. d. stable electrons. 45. The valence electrons in an atom are always a. inside the nucleus. c. the outermost electrons. b. the innermost electrons. d. in s orbitals. 46. The second period the periodic table contains a. the s-block elements only. c. the s-, p-, and d-block elements only. b. the s-and p-block elements only. d. the p-block elements only. c. one atom to the next atom. d. the center an atom s nucleus to the center an adjacent atom s nucleus. 47. When an atom loses electrons, it a. collapses. c. becomes smaller. b. becomes negatively charged. d. becomes larger.
48. Suppose you have just discovered three new elements. Element 1 is a solid at room temperature, a fair conductor heat and electricity, and not ductile. Element 2 is a solid at room temperature and lustrous. Element 3 is a gas at room temperature and a poor conductor heat and electricity. Classify each element as either a metal, nonmetal, or semimetal. Explain your reasoning. Then state one additional property that each element is likely to have. 49. Based on their positions in the periodic table, describe some the properties the following elements: nitrogen (N), manganese (Mn), and antimony (Sb). ANSWERS 1 a 3 b 4 b 5 a 6 c 7 c 8 c 9 d 10 a 11 d 12 a 13 d 14 d 15 d 16 a 17 c 18 b 19 a 20 a 21 a 22 d 23 b 24 c 25 a 26 c 27 a 28 b 29 a 30 d 31 a 32 c 33 b 34. d 35 b 36. a 37. c 38. a 39. b 40. c 41. a 42.d 43. d 44. b 45. c 46. b 47. c 48. 1 = metalloid (some properties metals but not all 2= metal (metal prop) 3= nonmetal (nonmetal prop) 49. N = gas, insulator, low m.p., brittle Mn= malleable, ductile, conductor, high mp Sb= intermediate prop Provide the correct name or formula for each the following. 22. hydroiodic acid HI 22. Sulfur hexafluoride SF 6 23. HNO 2 nitrous acid 23. KF potassium fluoride 24. zinc nitrate Zn(NO 3 ) 2 24. Barium dihydrogen phosphate Ba(H 2 PO 4 ) 2 25. Ca(ClO 3 ) 2 calcium chlorate 25. Pb(OH) 2 lead (II) hydroxide 26. Hg(OH) 2 mercury (II) hydroxide 26. Mercury (I) carbonate Hg 2 CO 3 27. ammonium phosphate (NH 4 ) 3 PO 4 27. Mg(ClO) 2 magnesium hypochlorite 28. FeI 3 iron (III) iodide 28. Iron (II) oxide FeO 29. zinc phosphide Zn 3 P 2 29. Hydrochloric acid HCl 30. Al 2 O 3 aluminum oxide 30. Tin (IV) sulfide SnS 2 31. strontium sulfide SrS 32. ammonium chloride NH 4 Cl 33. CO 2 carbon dioxide 34. Carbon tetrachloride CCl 4 35. H 3 PO 4 phosphoric acid 36. H 2 Se hydroselenic acid 37. sulfurous acid H 2 SO 3 38. Al 2 (SO 4 ) 3 Aluminum sulfate 39. cobalt (II) acetate Co(C 2 H 3 O 2 ) 2 40. barium phosphate Ba 3 (PO 4 ) 2 41. CaH 2 calcium hydride 42. BrF bromine monluoride