B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal

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1 1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and a nonmetal? A) Li, Na, Rb B) Cr, Mo, W C) Sn, Si, C D) O, S, Te 3. Which list includes elements with the most similar chemical? A) Br, Ga, Hg B) Cr, Pb, Xe C) O, S, Se D) N, O, F 4. If an element, X, can form an oxide that has the formula X 2O3, then element X would most likely be located on the Periodic Table in the same group as A) Ba B) Cd C) In D) Na 5. Which substance can be decomposed by chemical means? A) tungsten B) antimony C) krypton D) methane 6. Element X is a solid that is brittle, lacks luster,and has six valence electrons. In which group on the Periodic Table would element X be found? A) 1 B) 2 C) 15 D) Which element is an alkali metal? A) hydrogen B) calcium C) sodium D) zinc 8. Which element has most like those of magnesium? A) calcium B) cesium C) potassium D) sodium 9. In which section of the Periodic Table are the most active metals located? A) upper right corner B) lower right corner C) upper left corner D) lower left corner 10. A sample of an element is malleable and can conduct electricity. This element could be A) H B) He C) S D) Sn 11. Metallic substances will conduct electricity in A) the solid phase, only B) the liquid phase, only C) both the solid and the liquid phase D) neither the solid nor the liquid phase 12. Which element is malleable and ductile? A) S B) Si C) Ge D) Au 13. An element that has a low first ionization energy and good conductivity of heat and electricity is classified as a A) metal B) metalloid C) nonmetal D) noble gas 14. Which element is malleable and can conduct electricity in the solid phase? A) iodine B) phosphorus C) sulfur D) tin 15. Which of the following Group 15 elements has the greatest metallic character? A) nitrogen B) phosphorus C) antimony D) bismuth 16. In the formula XF2, the element represented by X can be classified as a A) Group 1 metal B) Group 2 metal C) Group 1 nonmetal D) Group 2 nonmetal 17. Which property is generally characteristic of metallic elements? A) low electrical conductivity B) high heat conductivity C) existence as brittle solids D) existence as molecular solids 18. What is a property of most metals? A) They tend to gain electrons easily when bonding. B) They tend to lose electrons easily when bonding. C) They are poor conductors of heat. D) They are poor conductors of electricity. 19. Which substance can not be broken down by a chemical change? A) methane B) propanal C) tungsten D) water

2 20. Which of these elements is the best conductor of electricity? A) S B) N C) Br D) Ni 21. Which Group 14 element is classified as a metal? A) carbon B) germanium C) silicon D) tin 22. Which two characteristics are associated with metals? A) low first ionization energy and low B) low first ionization energy and high C) high first ionization energy and low D) high first ionization energy and high 23. Which elements have the most similar chemical? A) Si, As, and Te B) N2, O2, and F2 C) Mg, Sr, and Ba D) Ca, Cs, and Cu 24. Which element is a liquid at STP and has low electrical conductivity? A) silver B) mercury C) barium D) bromine 25. Which phrase describes the molecular structure and of two solid forms of carbon, diamond and graphite? A) the same molecular structures and the same B) the same molecular structures and different C) different molecular structures and the same D) different molecular structures and different 26. Which particle diagram represents the arrangement of F 2 molecules in a sample of fluorine at 95 K and standard pressure? A) B) C) D) 27. Which elements have the most similar chemical? A) boron and carbon B) oxygen and sulfur C) aluminum and bromine D) argon and silicon 28. Which element at STP is a poor conductor of electricity and has a relatively high? A) Cu B) S C) Mg D) Fe 29. Which group in the Periodic Table contains elements that are all monatomic gases at STP? A) 15 B) 16 C) 17 D) Which element at STP exists as monatomic molecules? A) N B) O C) Cl D) Ne 31. Which element is a noble gas? A) W B) Ar C) N D) Er 32. Which element exhibits both metallic and nonmetallic? A) B B) Ba C) K D) Kr 33. Which isotopic notation identifies a metalloid that is matched with the corresponding number of protons in each of its atoms? A) 24 Mg and 12 protons B) 28 Si and 14 protons C) 75 As and 75 protons D) 80 Br and 80 protons

3 34. The element arsenic (As) has the of A) metals, only B) nonmetals, only C) both metals and nonmetals D) neither metals nor nonmetals 35. According to Reference Table N, which pair of isotopes spontaneously decays? A) C-12 and N-14 B) C-12 and N-16 C) C-14 and N-14 D) C-14 and N Given the particle diagram: At kpa and 298 K, which element could this diagram represent? A) Rn B) Xe C) Ag D) Kr 37. Which element is a brittle, nonconducting solid at 25 C? A) Br B) S C) Al D) Bi 38. Which element is a liquid at room temperature? A) K B) I2 C) Hg D) Mg 39. At STP, a 7.49-gram sample of an element has a volume of 1.65 cubic centimeters. The sample is most likely A) Ta B) Tc C) Te D) Ti 40. Which group contains elements in three phases of matter at STP? A) Group 2 B) Group 6 C) Group 15 D) Group Which Group 16 element has only unstable isotopes? A) Po B) Te C) Se D) S 42. Which statement explains why ozone gas, O3, and oxygen gas, O2, have different? A) They are formed from different elements. B) They have different molecular structures. C) They have different oxidation numbers. D) They have different electronegativities. 43. The two forms of oxygen, O2(g) and O3(g), have A) different molecular structures and identical B) different molecular structures and different C) identical molecular structures and identical D) identical molecular structures and different 44. A 10.0-gram sample of which element has the smallest volume at STP? A) aluminum B) magnesium C) titanium D) zinc 45. Which Lewis electron-dot diagram is correct for CO2? A) B) C) D) 46. Which is the correct electron-dot symbol for an aluminum atom in the ground state? A) B) C) D) 47. Which Lewis electron-dot diagram is correct for a S 2 ion? A) B) C) D) 48. What is the total number of electrons in the outermost shell of a phosphorus atom in the ground state? A) 1 B) 2 C) 3 D) The elements in Period 3 all contain the same number of A) protons B) neutrons C) valence electrons D) occupied principal energy levels 50. What is the total number of electrons in the valence shell of an atom of aluminum in the ground state? A) 8 B) 2 C) 3 D) 10

4 51. How do the chemical of the Na atom and the Na + ion compare? A) They are the same because each has the same atomic number. B) They are the same because each has the same electron configuration. C) They are different because each has a different atomic number. D) They are different because each has a different electron configuration. 52. An atom of aluminum in the ground state and an atom of gallium in the ground state have the same A) mass B) C) total number of protons D) total number of valence electrons 53. Which element will lose only valence electrons every time its atoms enter into a chemical reaction? A) Fe B) Cu C) Cr D) Mg 54. Which element would most likely be found uncombined in nature? A) K B) I C) Ag D) Mg 55. A metallic element whose aqueous ions produce colorless solutions would be found in Period 4 and Group A) IA B) VIIA C) VIII D) O 56. Which element can form a chloride with a general formula of MCl2 or MCl3? A) Fe B) Mg C) Al D) Zn 57. After a neutral sulfur atom gains two electrons, what is the resulting charge of the ion? 58. Compared to a Be 2+ ion, a Be 0 atom has A) more protons B) fewer protons C) more electrons D) fewer electrons 59. An atom of an element has a total of 12 electrons. An ion of the same element has a total of 10 electrons. Which statement describes the charge and radius of the ion? A) The ion is positively charged and its radius is smaller than the radius of the atom. B) The ion is positively charged and its radius is larger than the radius of the atom. C) The ion is negatively charged and its radius is smaller than the radius of the atom. D) The ion is negatively charged and its radius is larger than the radius of the atom. 60. As the atoms in Period 3 of the Periodic Table are considered from left to right, the atoms generally show A) an increase in radius and an increase in ionization energy B) an increase in radius and a decrease ionization energy C) a decrease in radius and an increase in ionization energy D) a decrease in radius and a decrease in ionization energy 61. Within Period 2 of the Periodic Table, as the atomic number increases, the atomic radius generally A) decreases B) increases C) remains the same 62. How does the size of a barium ion compare to the size of a barium atom? A) The ion is smaller because it has fewer electrons. B) The ion is smaller because it has more electrons. C) The ion is larger because it has fewer electrons. D) The ion is larger because it has more electrons. 63. Which ion would have the smallest radius? A) Ba 2+ B) Ca 2+ C) Mg 2+ D) Sr Which of the following ions has the smallest radius? A) Na + B) K + C) Mg 2+ D) Ca Compared to atoms of metals, atoms of nonmetals generally A) have higher electronegativities B) have lower first ionization energies C) conduct electricity more readily D) lose electrons more readily

5 66. Which statement describes the general trends in and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? A) Electronegativity increases, and first ionization energy decreases. B) Electronegativity decreases, and first ionization energy increases. C) Electronegativity and first ionization energy both increase. D) Electronegativity and first ionization energy both decrease. 67. What is the first ionization energy of an element that has the electron configuration 2-8? A) 2372 kj B) 2081 kj C) 1313 kj D) 10 kj 68. As the Group 1 elements of the Periodic Table are considered from top to bottom, the first ionization energy of each successive element decreases. One reason for this is that the A) nuclear charge is decreasing B) number of neutrons is increasing C) number of principal energy levels is decreasing D) distance between the valence electron and the nucleus is increasing 69. Which atom requires the least energy to form a positive ion? A) Ge B) Ca C) Ga D) K 70. Which element in Group 15 has the greatest metallic character? A) nitrogen B) phosphorus C) antimony D) bismuth 71. As the elements in Group 17 are considered in order of increasing atomic number, the chemical reactivity of each successive element A) decreases B) increases C) remains the same 72. Which element has the highest electrical conductivity? A) Mg B) H C) He D) Cl 73. Two solid samples each contain sulfur, oxygen, and sodium, only. These samples have the same color, melting point, density, and reaction with an aqueous barium chloride solution. It can be concluded that the two samples are the same A) compound B) element C) mixture D) solution 74. Which substance can be decomposed by a chemical change? A) Co B) CO C) Cr D) Cu 75. Which diagram represents a physical change, only? A) B) C) D) 76. Which substance can be decomposed by a chemical change? A) sodium B) argon C) sulfur D) ammonia 77. Which species represents a chemical compound? A) N2 B) NH4 + C) Na D) NaHCO3

6 78. What is the total number of different elements present in? A) 7 B) 9 C) 3 D) What is the chemical formula for sodium sulfate? A) Na2SO3 B) Na2SO4 C) NaSO3 D) NaSO4 80. If X represents an element of Group 1, the formula of its oxide would be A) XO B) X2O C) XO2 D) X2O3 81. Element X forms the compounds XCl3 and X2O3. In the Periodic Table, element X would most likely be found in Group A) 1 (IA) B) 2 (IIA) C) 13 (IIIA) D) 14 (IVA) 82. In which Group do the elements usually form oxides which have the general formula M2O3? A) 1 B) 2 C) 13 D) What is the name of the polyatomic ion in the compound Na2O2? A) hydroxide B) oxalate C) oxide D) peroxide 84. The correct formula for lead (IV) oxide is A) PbO B) Pb2O C) PbO2 D) Pb2O2 85. An example of a compound containing only two elements is A) mercury B) ethanol C) sodium D) ammonia

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