Unit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016

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1 Name: PRACTICE QUESTIONS Date: 2/23/ Which pair of symbols represents a metalloid and a noble gas? 1) Si and Bi 2) As and Ar 3) Ge and Te 4) Ne and Xe 2. What determines the order of placement of the elements on the modern Periodic Table? 1) atomic number 2) atomic mass 3) the number of neutrons, only 4) the number of neutrons and protons 3. What are the horizontal rows on the periodic table are called? 1) groups 2) periods 3) families 4) sections 4. Elements with chemical properties similar to neon are found only in 1) Period 1 2) Period 2 3) Group 1 4) Group The element krypton is classified as a 1) metal 2) salt 3) noble gas 4) metalloid 6. The vertical columns of the Periodic Table are called 1) groups 2) periods 3) spectra 4) energy levels 7. Which element is a metalloid? 1) Ar 2) Na 3) As 4) F 8. Bromine has chemical properties most similar to 1) hydrogen 2) oxygen 3) chlorine 4) neon 9. An example of a nonmetallic element is 1) sodium 2) nickel 3) mercury 4) phosphorus 10. Which of the following elements has the greatest atomic mass? 1) H 2) Na 3) Rb 4) Fr Page 1 Ms. Roman Page 1

2 11. Elements that conduct heat and electricity are: Unit 4 - Periodic Table Exam 1) metals 2) nonmetals 3) metalloids 4) noble gases 12. Which of the following elements is an active metal? 1) sodium 2) aluminum 3) chlorine 4) argon 13. An element that will not react with another element is a 1) metal 2) nonmetal 3) metalloid 4) noble gas 14. Which element is chemically active and forms compounds? 1) potassium 2) helium 3) argon 4) krypton 15. Which of the following elements in Period 3 has the greatest metallic character? 1) Ar 2) Si 3) Mg 4) S 16. An element that is malleable, ductile, and a good conductor of electricity is most likely 1) a metal 2) a metalloid 3) a non-metal 4) none of these 17. Which property of steel is illustrated by its ability to be shaped into automobile fenders? 1) luster 2) conductivity 3) malleability 4) ductility 18. Surfaces "reflecting back" light are associated with the property called 1) luster 2) ductility 3) tenacity 4) malleability 19. Which properties are characteristic of non-metals? 1) low heat conductivity and low electrical conductivity 2) low heat conductivity and high electrical conductivity 3) high heat conductivity and low electrical conductivity 4) high heat conductivity and high electrical conductivity 20. Which list of elements consists of a metal, a metalloid, and a nonmetal? 1) Li, Na, Rb 2) Cr, Mo, W 3) Sn, Si, C 4) O, S, Te Page 2 Ms. Roman Page 2

3 21. Which statement explains why sulfur is classified as a Group 16 element? 1) A sulfur atom has 6 valence electrons. 2) A sulfur atom has 16 neutrons. 3) Sulfur is a yellow solid at STP. 4) Sulfur reacts with most metals. 22. Which list consists of elements that have the most similar chemical properties? 1) Mg, Al, and Si 2) Mg, Ca, and Ba 3) K, Al, and Ni 4) K, Ca, and Ga 23. Which element has the highest melting point? 1) tantalum 2) rhenium 3) osmium 4) hafnium 24. Which property is characteristic of nonmetals? 1) They have a high electronegativity. 2) They lose electrons easily. 3) They have a low first ionization energy. 4) They are good conductors of electricity. 25. What are two properties of most nonmetals? 1) high ionization energy and poor electrical conductivity 2) high ionization energy and good electrical conductivity 3) low ionization energy and poor electrical conductivity 4) low ionization energy and good electrical conductivity 26. A characteristic of a nonmetal is 1) low ionization energy 2) high electronegativity 3) high electrical conductivity 4) the ability to form positive ions 27. Properties of nonmetal atoms include 1) low ionization energy and low electronegativity 2) low ionization energy and high electronegativity 3) high ionization energy and low electronegativity 4) high ionization energy and high electronegativity Page 3 Ms. Roman Page 3

4 28. In which area of the Periodic Table are the elements with the strongest nonmetallic properties located? 1) lower left 2) upper left 3) lower right 4) upper right 29. Which properties are characteristic of non-metals? 1) low thermal conductivity and low electrical conductivity 2) low thermal conductivity and high electrical conductivity 3) high thermal conductivity and low electrical conductivity 4) high thermal conductivity and high electrical conductivity 30. Which statement explains why neon is a Group 18 element? 1) Neon is a gas at STP. 2) Neon has a low melting point. 3) Neon atoms have a stable valence electron configuration. 4) Neon atoms have two electrons in the first shell. 31. An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has 1) more protons than neutrons 2) more neutrons than protons 3) a total of two valence electrons 4) a total of eight valence electrons 32. An atom in the ground state has a stable valence electron configuration. This atom could be an atom of 1) Al 2) Cl 3) Na 4) Ne 33. Which group on the Periodic Table has elements with atoms that tend not to bond with atoms of other elements? 1) Group 1 2) Group 2 3) Group 17 4) Group Which Group 14 element is a metalloid? 1) tin 2) silicon 3) lead 4) carbon 35. Arsenic and silicon are similar in that they both 1) have the same ionization energy 2) have the same covalent radius 3) are transition metals 4) are metalloids Page 4 Ms. Roman Page 4

5 36. Which element exhibits both metallic and nonmetallic properties? 1) bismuth 2) helium 3) silver 4) tellurium 37. Which element would have properties characteristic of both a metal and a nonmetal? 1) Ag 2) K 3) Si 4) Xe 38. Which element is not a metalloid? 1) arsenic 2) boron 3) silicon 4) sulfur 39. Which group of elements contains a metalloid? 1) Group 8 2) Group 2 3) Group 16 4) Group Which element is a liquid at STP? 1) bromine 2) cesium 3) francium 4) iodine 41. Which Lewis electron-dot diagram represents a nitrogen atom in the ground state? 1) 2) 3) 4) 42. An atom in the ground state contains a total of 5 electrons, 5 protons, and 5 neutrons. Which Lewis electron-dot diagram represents this atom? 1) 2) 3) 4) 43. Which Lewis electron-dot diagram represents a boron atom in the ground state? 1) 2) 3) 4) 44. Which is the electron-dot symbol for an atom with an electron configuration of 2-5? 1) 2) 3) 4) 45. Which ion has no electrons? 1) H + 2) Li + 3) Na + 4) Rb + Page 5 Ms. Roman Page 5

6 46. The valence electrons of a germanium atom in the ground state are located in the 1) first shell 2) second shell 3) third shell 4) fourth shell 47. Aqueous solutions of compounds containing element X are blue. Element X could be 1) carbon 2) copper 3) sodium 4) sulfur 48. Which compound forms a green aqueous solution? 1) RbCl 2) CaCl 2 3) NiCl2 4) ZnCl2 49. Which ionic compound dissolves in water to form a colored solution? 1) Ca(NO3)2 2) Cu(NO3)2 3) KNO 3 4) Al(NO 3)3 50. Which set of properties is most characteristic of transition elements? 1) colorless ions in solution, multiple positive oxidation states 2) colorless ions in solution, multiple negative oxidation states 3) colored ions in solution, multiple positive oxidation states 4) colored ions in solution, multiple negative oxidation states 51. Which salt contains an ion that forms a colored solution? 1) Mg(NO 3)2 2) Ca(NO3)2 3) Ni(NO3)3 4) Al(NO 3)3 52. Which physical characteristic of a solution may indicate the presence of a transition element? 1) its density 2) its color 3) its effect on litmus 4) the effect on phenolphthalein 53. Which aqueous solution is colored? 1) CuSO4(aq) 2) BaCl(aq) 3) KCl(aq) 4) MgSO 4(aq) 54. Which compound is colorless in a water solution? 1) Al 2(SO 4)3 2) Cr 2(SO 4)3 3) Fe2(SO 4)3 4) Co 2(SO 4)3 Page 6 Ms. Roman Page 6

7 55. Which element would most likely form a compound whose water solution is colored? 1) H 2) P 3) Mg 4) Cu 56. When an atom of lithium loses an electron, the atom becomes a 1) negative ion with a radius smaller than the radius of the atom 2) negative ion with a radius larger than the radius of the atom 3) positive ion with a radius smaller than the radius of the atom 4) positive ion with a radius larger than the radius of the atom 57. An atom of an element forms a 2 + ion. In which group on the Periodic Table could this element be located? 1) 1 2) 2 3) 13 4) What is the total number of electrons in a S 2 ion? 1) 10 2) 14 3) 16 4) Compared to a phosphorus atom, a P 3 ion has 1) more electrons and a larger radius 2) more electrons and a smaller radius 3) fewer electrons and a larger radius 4) fewer electrons and a smaller radius 60. What is the total number of electrons in a Mg 2+ ion? 1) 10 2) 12 3) 14 4) Which changes occur as a cadmium atom, Cd, becomes a cadmium ion, Cd 2+? 1) The Cd atom gains two electrons and its radius decreases. 2) The Cd atom gains two electrons and its radius increases. 3) The Cd atom loses two electrons and its radius decreases. 4) The Cd atom loses two electrons and its radius increases. 62. Which atom has the largest atomic radius? 1) potassium 2) rubidium 3) francium 4) cesium Page 7 Ms. Roman Page 7

8 63. An atom of which element has the largest atomic radius? 1) Fe 2) Mg 3) Si 4) Zn 64. As the elements of Group 17 are considered in order of increasing atomic number, there is an increase in 1) atomic radius 2) electronegativity 3) first ionization energy 4) number of electrons in the first shell 65. How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus? 1) Sodium has a larger atomic radius and is more metallic. 2) Sodium has a larger atomic radius and is less metallic. 3) Sodium has a smaller atomic radius and is more metallic. 4) Sodium has a smaller atomic radius and is less metallic. 66. As the atoms in Period 3 of the Periodic Table are considered from left to right, the atoms generally show 1) an increase in radius and an increase in ionization energy 2) an increase in radius and a decrease ionization energy 3) a decrease in radius and an increase in ionization energy 4) a decrease in radius and a decrease in ionization energy 67. The diagram represents two adjacent atoms of sulfur. Distance X is closest to 1) 63.5 pm 2) 127 pm 3) 190 pm 4) 254 pm 68. An ion of which element has a larger radius than an atom of the same element? 1) aluminum 2) chlorine 3) magnesium 4) sodium Page 8 Ms. Roman Page 8

9 69. An atom with the electron configuration would most likely 1) decrease in size as it forms a positive ion 2) increase in size as it forms a positive ion 3) decrease in size as it forms a negative ion 4) increase in size as it forms a negative ion Unit 4 - Periodic Table Exam 70. How does the size of a barium ion compare to the size of a barium atom? 1) The ion is smaller because it has fewer electrons. 2) The ion is smaller because it has more electrons. 3) The ion is larger because it has fewer electrons. 4) The ion is larger because it has more electrons. 71. Which element forms an ion larger than its atom? 1) Na 2) Ne 3) Ba 4) Br 72. The atom of which element has an ionic radius smaller than its atomic radius? 1) N 2) S 3) Br 4) Rb 73. 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? 1) Electronegativity increases, and first ionization energy decreases. 2) Electronegativity decreases, and first ionization energy increases. 3) Electronegativity and first ionization energy both increase. 4) Electronegativity and first ionization energy both decrease. 74. Which term represents the attraction one atom has for the electrons in a bond with another atom? 1) electronegativity 2) electrical conductivity 3) first ionization energy 4) mechanical energy 75. Which general trend is found in Period 3 as the elements are considered in order of increasing atomic number? 1) increasing atomic radius 2) increasing electronegativity 3) decreasing atomic mass 4) decreasing first ionization energy Page 9 Ms. Roman Page 9

10 76. Which of these elements has the least attraction for electrons in a chemical bond? 1) oxygen 2) fluorine 3) nitrogen 4) chlorine 77. Based on Reference Table S, atoms of which of these elements have the strongest attraction for the electrons in a chemical bond? 1) Al 2) Si 3) P 4) S 78. Which atom in the ground state requires the least amount of energy to remove its valence electron? 1) lithium atom 2) potassium atom 3) rubidium atom 4) sodium atom 79. In Period 2 of the Periodic Table, which Group contains the element with the highest first ionization energy? 1) alkali metals 2) alkaline earth metals 3) halogens 4) noble gases 80. Which noble gas has the highest first ionization energy? 1) radon 2) krypton 3) neon 4) helium 81. Which of these metals loses electrons most readily? 1) calcium 2) magnesium 3) potassium 4) sodium 82. Which element has atoms that can form halide ions? 1) iodine 2) silver 3) strontium 4) xenon 83. Most metals have the properties of 1) brittleness and high ionization energy 2) brittleness and low ionization energy 3) ductility and high ionization energy 4) ductility and low ionization energy Page 10 Ms. Roman Page 10

11 84. Which statement is true about the properties of the elements in any one period of the Periodic Table? 1) They are determined by the number of neutrons. 2) They are determined by the number of electrons in the first shell. 3) They change in a generally systematic manner. 4) They change in a random, unpredictable manner. 85. At which location in the Periodic Table would the most active metallic element be found? 1) in Group 1 at the top 2) in Group 1 at the bottom 3) in Group 17 at the top 4) in Group 17 at the bottom 86. The most active metals are in Group 1) 1 2) 15 3) 13 4) 17 Page 11 Ms. Roman Page 11