29. The table below shows some properties of elements A, B, C, and D. Which element is most likely a nonmetal? A) A B) B C) C D) D

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1 1. On the modern Periodic Table, the elements are arranged in order of increasing A) atomic mass B) atomic number C) mass number D) oxidation number 2. Which two elements have the most similar chemical properties? A) Be and Mg B) Ca and Br C) Cl and Ar D) Na and P 3. Elements on the modern Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) number of neutrons D) number of valence electrons 4. 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. 5. Which quantity identifies an element? A) atomic number B) mass number C) total number of neutrons in an atom of the element D) total number of valence electrons in an atom of the element 6. 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. 7. Which substance can be decomposed by chemical means? A) tungsten B) antimony C) krypton D) methane 8. Which element has chemical properties that are most similar to those of calcium? A) Co B) K C) N D) Sr 9. Which list consists of elements that have the most similar chemical properties? A) Mg, Al, and Si B) Mg, Ca, and Ba C) K, Al, and Ni D) K, Ca, and Ga 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. An element that is malleable and a good conductor of heat and electricity could have an atomic number of A) 16 B) 18 C) 29 D) 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 13. Which element is malleable and can conduct electricity in the solid phase? A) iodine B) phosphorus C) sulfur D) tin 14. Which substance can not be decomposed by ordinary chemical means? A) methane B) mercury C) ethanol D) ammonia 15. The elements located in the lower left corner of the Periodic Table are classified as A) metals B) nonmetals C) metalloids D) noble gases 16. Which element is malleable and conducts electricity? A) iron B) iodine C) sulfur D) phosphorus 17. Which statement describes a chemical property of iron? A) Iron can be flattened into sheets. B) Iron conducts electricity and heat. C) Iron combines with oxygen to form rust. D) Iron can be drawn into a wire. 18. Which of these elements is the best conductor of electricity? A) S B) N C) Br D) Ni

2 19. 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. 20. Which element is classified as a nonmetal? A) Be B) Al C) Si D) Cl 21. At STP, an element that is a brittle solid and a poor conductor of heat and electricity could have an atomic number of A) 12 B) 13 C) 16 D) Which is a property of most nonmetallic solids? A) high thermal conductivity B) high electrical conductivity C) brittleness D) malleability 23. 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 24. Which property is characteristic of nonmetals? A) They have a high. B) They lose electrons easily. C) They have a low first ionization energy. D) They are good conductors of electricity. 25. A characteristic of a nonmetal is A) low ionization energy B) high C) high electrical conductivity D) the ability to form positive ions 26. Properties of nonmetal atoms include A) low ionization energy and low B) low ionization energy and high C) high ionization energy and low D) high ionization energy and high 27. Which element can be brittle or soft in the solid phase and is a poor conductor of heat and electricity? A) calcium B) sulfur C) strontium D) copper 28. In which area of the Periodic Table are the elements with the strongest nonmetallic properties located? A) lower left B) upper left C) lower right D) upper right

3 29. The table below shows some properties of elements A, B, C, and D. Which element is most likely a nonmetal? A) A B) B C) C D) D 30. An atom in the ground state has a stable valence electron configuration. This atom could be an atom of A) Al B) Cl C) Na D) Ne 31. Which element is a noble gas? A) krypton B) chlorine C) antimony D) manganese 32. Which substance can not be decomposed by a chemical change? A) Ne B) N 2O C) HF D) H 2O 33. Which element is classified as a noble gas at STP? A) hydrogen B) oxygen C) neon D) nitrogen 34. Which group in the Periodic Table contains elements that are all monatomic gases at STP? A) 15 B) 16 C) 17 D) Which substance at STP exists in the form of a monatomic gas? A) neon B) oxygen C) chlorine D) nitrogen 36. Which Group 14 element is a metalloid? A) tin B) silicon C) lead D) carbon 37. Which list of elements consists of metalloids, only? A) B, Al, Ga B) C, N, P C) O, S, Se D) Si, Ge, As 38. Which element has both metallic and nonmetallic properties? A) Rb B) Rn C) Si D) Sr 39. 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 40. The element in Group 14, Period 3 on the Periodic Table is classified as a A) metal B) noble gas C) metalloid D) nonmetal 41. Germanium is classified as a A) metal B) metalloid C) nonmetal D) noble gas 42. Which pair of symbols represents a metalloid and a noble gas? A) Si and Bi B) As and Ar C) Ge and Te D) Ne and Xe 43. Which list of elements contains two metalloids? A) Si, Ge, Po, Pb B) As, Bi, Br, Kr C) Si, P, S, Cl D) Po, Sb, I, Xe 44. At standard pressure, which element has a freezing point below standard temperature? A) In B) Ir C) Hf D) Hg 45. Which element has the greatest density at STP? A) barium B) beryllium C) magnesium D) radium 46. Which element is a brittle solid with low conductivity at STP? A) sulfur B) sodium C) argon D) aluminum

4 47. Which element is a metal that is in the liquid phase at STP? A) bromine B) cobalt C) hydrogen D) mercury 48. A 1.0-gram sample of which element will uniformly fill a closed 2.0-liter container at STP? A) antimony B) sulfur C) tellurium D) xenon 49. Which element is a solid at STP and a good conductor of electricity? A) iodine B) mercury C) nickel D) sulfur 50. Which list of radioisotopes contains an alpha emitter, a beta emitter, and a positron emitter? A) C-14, N-16, P-32 B) Cs-137, Fr-220, Tc-99 C) Kr-85, Ne-19, Rn-222 D) Pu-239, Th-232, U At STP, which list of elements contains a solid, a liquid, and a gas? A) Hf, Hg, He B) Cr, Cl 2, C C) Ba, Br 2, B D) Se, Sn, Sr 52. At standard pressure, which element has a melting point higher than standard temperature? A) F 2 B) Br 2 C) Fe D) Hg 53. 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 54. Which statement explains why ozone gas, O 3, and oxygen gas, O 2, have different properties? A) They are formed from different elements. B) They have different molecular structures. C) They have different oxidation numbers. D) They have different electronegativities. 55. What is the density of N 2 at STP? A) g/cm 3 B) g/cm 3 C) g/cm 3 D) g/cm Which gaseous element has the greatest density at STP? A) N 2 B) O 2 C) Cl 2 D) F Which Lewis electron-dot diagram represents calcium oxide? A) B) C) D) 58. 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? A) B) C) D) 59. Which Lewis electron-dot diagram is correct for CO 2? A) B) C) D) 60. Which Lewis electron-dot diagram is correct for a S 2 ion? A) B) C) D) 61. An atom of an element forms a 2 + ion. In which group on the Periodic Table could this element be located? A) 1 B) 2 C) 13 D) What is the total number of valence electrons in a sulfide ion in the ground state? A) 8 B) 2 C) 16 D) 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.

5 64. What is the net charge on an ion that has 9 protons, 11 neutrons, and 10 electrons? A) 1+ B) 2+ C) 1- D) How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus? A) Sodium has a larger atomic radius and is more metallic. B) Sodium has a larger atomic radius and is less metallic. C) Sodium has a smaller atomic radius and is more metallic. D) Sodium has a smaller atomic radius and is less metallic. 66. Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius? A) Be, Mg, Ca B) Ca, Mg, Be C) Ba, Ra, Sr D) Sr, Ra, Ba 67. Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? A) Their metallic properties decrease and their atomic radii decrease. B) Their metallic properties decrease and their atomic radii increase. C) Their metallic properties increase and their atomic radii decrease. D) Their metallic properties increase and their atomic radii increase. 68. Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? A) The atomic radius decreases, and the first ionization energy generally increases. B) The atomic radius decreases, and the first ionization energy generally decreases. C) The atomic radius increases, and the first ionization energy generally increases. D) The atomic radius increases, and the first ionization energy generally decreases.

6 69. The data table below shows elements Xx, Yy, and Zz from the same group on the Periodic Table. What is the most likely atomic radius of element Yy? A) 103 pm B) 127 pm C) 166 pm D) 185 pm 70. Which of the following ions has the smallest radius? A) F B) Cl C) K + D) Ca When an atom of phosphorus becomes a phosphide ion (P 3 ), the radius A) decreases B) increases C) remains the same 72. Which element forms an ion that is larger than its atom? A) aluminum B) chlorine C) magnesium D) sodium 73. Which ion has the largest radius? A) Na + B) Mg 2+ C) K + D) Ca For which element is the ionic radius larger than the atomic radius? A) Na B) Mg C) Al D) Cl 75. An atom with the electron configuration would most likely A) decrease in size as it forms a positive ion B) increase in size as it forms a positive ion C) decrease in size as it forms a negative ion D) increase in size as it forms a negative ion 76. Atoms of which element have the greatest tendency to gain electrons? A) bromine B) chlorine C) fluorine D) iodine 77. An atom of which element has the greatest attraction for the electrons in a bond with a hydrogen atom? A) chlorine B) phosphorus C) silicon D) sulfur 78. Based on Reference Table S, atoms of which of these elements have the strongest attraction for the electrons in a chemical bond? A) Al B) Si C) P D) S 79. In the ground state, each atom of an element has two valence electrons. This element has a lower first ionization energy than calcium. Where is this element located on the Periodic Table? A) Group 1, Period 4 B) Group 2, Period 5 C) Group 2, Period 3 D) Group 3, Period4 80. Which general trend is found in Period 2 on the Periodic Table as the elements are considered in order of increasing atomic number? A) decreasing atomic mass B) decreasing C) increasing atomic radius D) increasing first ionization energy 81. 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 82. 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) 83. Which element is most chemically similar to chlorine? A) Ar B) F C) Fr D) S

7 84. Which Period 4 element has the most metallic properties? A) As B) Br C) Ge D) Sc 85. Elements Q, X, and Z are in the same group on the Periodic Table and are listed in order of increasing atomic number. The melting point of element Q is 219 C and the melting point of element Z is 7 C. Which temperature is closest to the melting point of element X? A) 7 C B) 101 C C) 219 C D) 226 C 86. Which substance can not be decomposed by a chemical change? A) ammonia B) copper C) propanol D) water 87. Matter is classified as a A) substance, only B) substance or as a mixture of substances C) homogenous mixture, only D) homogenous mixture or as a heterogeneous mixture 88. Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion? A) solution B) compound C) homogeneous mixture D) heterogeneous mixture 89. Tetrachloromethane, CCl 4, is classified as a A) compound because the atoms of the elements are combined in a fixed proportion B) compound because the atoms of the elements are combined in a proportion that varies C) mixture because the atoms of the elements are combined in a fixed proportion D) mixture because the atoms of the elements are combined in a proportion that varies 90. Which substance can not be decomposed by a chemical change? A) AlCl 3 B) H 2O C) HI D) Cu 91. The compound XCl is classified as ionic if X represents the element A) H B) I C) Rb D) Br 92. What is the chemical formula for iron(iii) oxide? A) FeO B) Fe 2O 3 C) Fe 3O D) Fe 3O In which compound is the ratio of metal ions to nonmetal ions 1 to 2? A) calcium bromide B) calcium oxide C) calcium phosphide D) calcium sulfide 94. Which group on the Periodic Table of the Elements contains elements that react with oxygen to form compounds with the general formula X 20? A) Group 1 B) Group 2 C) Group 14 D) Group What is the total number of different elements present in NH 4NO 3? A) 7 B) 9 C) 3 D) Element X reacts with iron to form two different compounds with the formulas FeX and Fe 2X 3. To which group on the Periodic Table does element X belong? A) Group 8 B) Group 2 C) Group 13 D) Group A metal, M, forms an oxide compound with the general formula M 2O. In which group on the Periodic Table could metal M be found? A) Group 1 B) Group 2 C) Group 16 D) Group Which formula represents lead(ii) chromate? A) PbCrO 4 B) Pb(CrO 4) 2 C) Pb 2CrO 4 D) Pb 2(CrO 4) A compound is made up of iron and oxygen, only. The ratio of iron ions to oxide ions is 2:3 in this compound. The IUPAC name for this compound is A) triiron dioxide B) iron(ii) oxide C) iron(iii) oxide D) iron trioxide 100. What is the IUPAC name for the compound FeS? A) iron(ii) sulfate B) iron(iii) sulfate C) iron(ii) sulfide D) Iron(III) sulfide 101. The correct chemical formula for iron(ii) sulfide is A) FeS B) Fe 2S 3 C) FeSO 4 D) Fe 2(SO 4) 3

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