Periodic Table Practice 11/29 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 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 properties? A) Br, Ga, Hg B) Cr, Pb, Xe C) O, S, Se D) N, O, F 4. The elements in Group 2 are classified as A) metals B) metalloids C) nonmetals D) noble gases 5. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have A) fewer valence electrons B) more valence electrons C) fewer electron shells D) more electron shells 6. Which statement identifies the element arsenic? A) Arsenic has an atomic number of 33. B) Arsenic has a melting point of 84 K. C) An atom of arsenic in the ground state has eight valence electrons. D) An atom of arsenic in the ground state has a radius of 146 pm. 7. Which statement explains why sulfur is classified as a Group 16 element? A) A sulfur atom has 6 valence electrons. B) A sulfur atom has 16 neutrons. C) Sulfur is a yellow solid at STP. D) Sulfur reacts with most metals. 8. Which substance can be decomposed by chemical means? A) tungsten B) antimony C) krypton D) methane 9. 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) 16 10. Which element is an alkali metal? A) hydrogen B) calcium C) sodium D) zinc 11. Most of the groups in the Periodic Table of the Elements contain A) nonmetals, only B) metals, only C) nonmetals and metals D) metals and metalloids 12. Which of the following Period 4 elements has the most metallic characteristics? A) Ca B) Ge C) As D) Br 13. Which Group 15 element exists as a diatomic molecule at STP? A) phosphorus B) nitrogen C) bismuth D) arsenic 14. In which set do the elements exhibit the most similar chemical properties? A) N, O, and F B) Hg, Br, and Rn C) Li, Na and K D) Al, Si and P 15. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? A) nonmetal metalloid metal B) metalloid metal nonmetal C) metal metalloid nonmetal D) metal nonmetal metalloid 16. All of the atoms of the elements in Period 2 have the same number of A) protons B) neutrons C) valence electrons D) occupied energy levels (shells) Page 1
17. The observed regularities in the properties of elements are periodic functions of their A) atomic numbers B) mass numbers C) oxidation states D) non-valence electrons 18. Five cubes of iron are tested in a laboratory. The tests and the results are shown in the table below. Which tests demonstrate chemical properties? A) 1, 3, and 4 B) 1, 3, and 5 C) 2 and 4 D) 2 and 5 19. Which property can be defined as the ability of a substance to be hammered into thin sheets? A) conductivity B) malleability C) melting point D) solubility 20. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a A) metal B) metalloid C) noble gas D) nonmetal 21. Which element is a liquid at 305 K and 1.0 atmosphere? A) magnesium B) fluorine C) gallium D) iodine 22. Which two characteristics are associated with metals? A) low first ionization energy and low electronegativity B) low first ionization energy and high electronegativity C) high first ionization energy and low electronegativity D) high first ionization energy and high electronegativity 23. Which element is malleable and can conduct electricity in the solid phase? A) iodine B) phosphorus C) sulfur D) tin 24. Which substance can not be decomposed by ordinary chemical means? A) methane B) mercury C) ethanol D) ammonia 25. The elements located in the lower left corner of the Periodic Table are classified as A) metals B) nonmetals C) metalloids D) noble gases 26. 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. Page 2
27. The element in Period 4 and Group 1 of the Periodic Table would be classified as a A) metal B) metalloid C) nonmetal D) noble gas 28. Which of the following Group 15 elements has the greatest metallic character? A) nitrogen B) phosphorus C) antimony D) bismuth 29. At STP, graphite and diamond are two solid forms of carbon. Which statement explains why these two forms of carbon differ in hardness? A) Graphite and diamond have different ionic radii. B) Graphite and diamond have different molecular structures. C) Graphite is a metal, but diamond is a nonmetal. D) Graphite is a good conductor of electricity, but diamond is a poor conductor of electricity. 30. Which list of symbols represents nonmetals, only? A) B, Al, Ga B) Li, Be, B C) C, Si, Ge D) P, S, Cl 31. Which two gases can not be broken down by chemical means? A) CO and He B) CO and NH3 C) Xe and He D) Xe and NH3 32. Which phrase describes the molecular structure and properties of two solid forms of carbon, diamond and graphite? A) the same molecular structures and the same properties B) the same molecular structures and different properties C) different molecular structures and the same properties D) different molecular structures and different properties 33. Which particle diagram represents the arrangement of F2 molecules in a sample of fluorine at 95 K and standard pressure? A) B) C) D) 34. What are two properties of most nonmetals? A) high ionization energy and poor electrical conductivity B) high ionization energy and good electrical conductivity C) low ionization energy and poor electrical conductivity D) low ionization energy and good electrical conductivity 35. Which is a property of most nonmetallic solids? A) high thermal conductivity B) high electrical conductivity C) brittleness D) malleability 36. Which element is least likely to undergo a chemical reaction? A) lithium B) carbon C) flourine D) neon 37. Which statement explains why neon is a Group 18 element? A) Neon is a gas at STP. B) Neon has a low melting point. C) Neon atoms have a stable valence electron configuration. D) Neon atoms have two electrons in the first shell. Page 3
38. Which group in the Periodic Table contains elements that are all monatomic gases at STP? A) 15 B) 16 C) 17 D) 18 39. Which element has both metallic and nonmetallic properties? A) Rb B) Rn C) Si D) Sr 40. Which list of elements consists of metalloids, only? A) B, Al, Ga B) C, N, P C) O, S, Se D) Si, Ge, As 41. 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 42. Which element is a liquid at STP? A) bromine B) cesium C) francium D) iodine 43. Nuclei of U-238 atoms are A) stable and spontaneously absorb alpha particles B) stable and spontaneously emit alpha particles C) unstable and spontaneously absorb alpha particles D) unstable and spontaneously emit alpha particles 44. 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 45. Solid samples of the element phosphorus can be white, black, or red in color. The variations in color are due to different A) atomic masses B) molecular structures C) ionization energies D) nuclear charges 46. Which statement correctly describes two forms of oxygen, O2 and O3? A) They have identical molecular structures and identical properties. B) They have identical molecular structures and different properties. C) They have different molecular structures and identical properties. D) They have different molecular structures and different properties. 47. Which Lewis electron-dot diagram represents a nitrogen atom in the ground state? A) B) C) D) 48. Which Lewis electron-dot diagram is correct for a S 2 ion? A) B) C) D) 49. What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table? A) the number of neutrons in the atom B) the number of protons in the atom C) the number of valence electrons in the atom D) the total number of electrons in the atom 50. The number of valence electrons in each atom of an element affects the element's A) chemical properties B) number of isotopes C) decay mode D) half-life 51. Aqueous solutions of compounds containing element X are blue. Element X could be A) carbon B) copper C) sodium D) sulfur Page 4
52. An element with a partially filled d sublevel in the ground state is classified as A) a halogen B) a transition metal C) an alkali metal D) an alkaline earth metal 53. Which set of properties is most characteristic of transition elements? A) colorless ions in solution, multiple positive oxidation states B) colorless ions in solution, multiple negative oxidation states C) colored ions in solution, multiple positive oxidation states D) colored ions in solution, multiple negative oxidation states 54. What occurs when a magnesium atom becomes a magnesium ion? A) Electrons are gained and the oxidation number increases. B) Electrons are gained and the oxidation number decreases. C) Electrons are lost and the oxidation number increases. D) Electrons are lost and the oxidation number decreases. 55. What is the number of electrons in an Al 3+ ion? A) 10 B) 13 C) 3 D) 16 56. When an atom of lithium loses an electron, the atom becomes a A) negative ion with a radius smaller than the radius of the atom B) negative ion with a radius larger than the radius of the atom C) positive ion with a radius smaller than the radius of the atom D) positive ion with a radius larger than the radius of the atom 57. What can be concluded if an ion of an element is smaller than an atom of the same element? A) The ion is negatively charged because it has fewer electrons than the atom. B) The ion is negatively charged because it has more electrons than the atom. C) The ion is positively charged because it has fewer electrons than the atom. D) The ion is positively charged because it has more electrons than the atom. 58. What is the total number of electrons in a S 2 ion? A) 10 B) 14 C) 16 D) 18 59. Which ion has the smallest radius? A) B) C) D) 60. As the elements is Period 3 are considered in order of increasing atomic number, there is a general decrease in A) atomic mass B) atomic radius C) electronegativity D) first ionization energy 61. Which grouping of circles, when considered in order from the top to the bottom, best represents the relative size of the atoms of Li, Na, K, and Rb, respectively? A) B) C) D) 62. Which list of elements is arranged in order of increasing electronegativity? A) Be, Mg, Ca B) F, Cl, Br C) K, Ca, Sc D) Li, Na, K Page 5
63. Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right? A) Both electronegativity and atomic radius increase. B) Both electronegativity and atomic radius decrease. C) Electronegativity increases and atomic radius decreases. D) Electronegativity decreases and atomic radius increases. 64. Which statement describes the general trends in electronegativity 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. 65. Which atom has the weakest attraction for electrons in a chemical bond? A) a boron atom B) a calcium atom C) a fluorine atom D) a nitrogen atom 66. As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally A) decreases B) increases C) remains the same 67. The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as A) first ionization energy B) activation energy C) conductivity D) electronegativity 68. As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to A) decreasing radius and decreasing shielding effect B) decreasing radius and increasing shielding effect C) increasing radius and decreasing shielding effect D) increasing radius and increasing shielding effect 69. Which element has atoms that can form halide ions? A) iodine B) silver C) strontium D) xenon 70. When the elements in Group 1 are considered in order from top to bottom, each successive element at standard pressure has A) a higher melting point and a higher boiling point B) a higher melting point and a lower boiling point C) a lower melting point and a higher boiling point D) a lower melting point and a lower boiling point 71. Which phrase describes a compound that consists of two elements? A) a mixture in which the elements are in a variable proportion B) a mixture in which the elements are in a fixed proportion C) a substance in which the elements are chemically combined in a variable proportion D) a substance in which the elements are chemically combined in a fixed proportion 72. Which statement explains why water is classified as a compound? A) Water can be broken down by chemical means. B) Water is a liquid at room temperature. C) Water has a heat of fusion of 334 J/g. D) Water is a poor conductor of electricity. Page 6
73. Base your answer to the following question on the information below. Given: Samples of Na, Ar, As, Rb Which two of the given elements have the most similar chemical properties? 74. Base your answer to the following question on the information below and on your knowledge of chemistry. Potassium phosphate, K3PO4, is a source of dietary potassium found in a popular cereal. According to the Nutrition-Facts label shown on the boxes of this brand of cereal, the accepted value for a one-cup serving of this cereal is 170 milligrams of potassium. The minimum daily requirement of potassium is 3500 milligrams for an adult human. Identify the noble gas whose atoms have the same electron configuration as a potassium ion. Base your answers to questions 75 and 76 on the information below and on your knowledge of chemistry. Some properties of the element sodium are listed below. is a soft, silver-colored metal melts at a temperature of 371 K oxidizes easily in the presence of air forms compounds with nonmetallic elements in nature forms sodium chloride in the presence of chlorine gas 75. Convert the melting point of sodium to degrees Celsius. 76. Identify one chemical property of sodium from this list. Page 7
77. Base your answer to the following question on the information below and on your knowledge of chemistry. The Lewis electron-dot diagrams for three substances are shown below. Identify the noble gas that has atoms with the same electron configuration as the positive ion represented in diagram 1, when both the atoms and the ion are in the ground state. Base your answers to questions 78 through 80 on the information below and on your knowledge of chemistry. There are six elements in Group 14 on the Periodic Table. One of these elements has the symbol Uuq, which is a temporary, systematic symbol. This element is now known as flerovium. 78. State the expected number of valence electrons in an atom of the element flerovium in the ground state. 79. Explain, in terms of electron shells, why each successive element in Group 14 has a larger atomic radius, as the elements are considered in order of increasing atomic number. 80. Identify an element in Group 14 that is classified as a metalloid. Page 8