tomic Structure Name: ate: 1. Write one electron configuration for an atom of silicon in an excited state. 5. Which electron configuration represents an atom of chlorine in an excited state?. 2 8 7. 2 8 8. 2 8 6 1. 2 8 7 1 2. What is the total number of valence electrons in an atom with the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 3?. 15. 2. 3. 5 6. Which electron configuration represents the electrons in an atom of chlorine in an excited state?. 2-7-7. 2-7-8. 2-8-7. 2-8-8 3. What is the total number of protons in an atom with the electron configuration 2-8-18-32-18-1?. 69. 79. 118. 197 7. Which electron configuration is correct for a sodium ion?. 2 7. 2 8. 2 8 1. 2 8 2 4. n atom in the ground state has 7 valence electrons. Which electron configuration could represent the outermost principal energy level of this atom in the ground state?. 3s 1 3p 6. 3s 2 3p 5. 3s 1 3p 4 3d 2. 3s 2 3p 4 3d 1 8. Which electron configuration represents an excited state for a potassium atom?. 2-8-7-1. 2-8-7-2. 2-8-8-1. 2-8-8-2 page 1
9. ase your answer(s) to the following question(s) on the electron configuration table shown. 13. The bright-line spectra produced by four elements are represented in the diagram below. Element Electron onfiguration X 2-8-8-2 Y 2-8-7-3 Z 2-8-8 Which electron configuration represents the excited state of a calcium atom? Given the bright-line spectrum of a mixture formed from two of these elements: 10. Which electron configuration represents the electrons of an atom in an excited state? Which elements are present in this mixture?. 2-8-1. 2-8-6. 2-8-17-6. 2-8-18-5. and. and X. Z and. Z and X 11. Which ion has the same electron configuration as an Mg 2+ ion?. a 2+. l. Na +. S 2 14. Which is an electron configuration for an atom of chlorine in the excited state?. 2 8 7. 2 8 8. 2 8 6 1. 2 8 7 1 12. What is the total number of valence electrons in a sulfide ion in the ground state?. 8. 2. 16. 18 page 2 tomic Structure
15. ase your answer(s) to the following question(s) on the information below. The table below lists physical and chemical properties of six elements at standard pressure that correspond to known elements on the Periodic Table. The elements are identified by the code letters,, E, G, J, L, and Q. 18. s an electron in an atom moves from the ground state to an excited state, the potential energy of the electron. decreases. increases. remains the same Properties of Six Elements at Standard Pressure Element ensity 0.00018 g/cm 3 Melting point 272 oiling point -269 Oxide formula (none) Element J ensity 0.0013 g/cm 3 Melting point 210 oiling point 196 Oxide formula J 2O 5 Element E ensity 1.82 g/cm 3 Melting point 4 oiling point 280 Oxide formula E 2O 5 Element L ensity 0.86 g/cm 3 Melting point 64 oiling point 774 Oxide formula L 2O Element G ensity 0.53 g/cm 3 Melting point 181 oiling point 1347 Oxide formula G 2O Element Q ensity 0.97 g/cm 3 Melting point 98 oiling point 883 Oxide formula Q 2O n atom of element G is in the ground state. What is the total number of valence electrons in this atom? 16. Which electron configuration represents a potassium atom in the excited state?. 1s 2 2s 2 2p 6 3s 2 3p 3. 1s 2 2s 2 2p 6 3s 1 3p 4 19. ase your answer(s) to the following question(s) on the information below and on your knowledge of chemistry. Silver-plated utensils were popular before stainless steel became widely used to make eating utensils. Silver tarnishes when it comes in contact with hydrogen sulfide, H 2 S, which is found in the air and in some foods. However, stainless steel does not tarnish when it comes in contact with hydrogen sulfide. In the ground state, an atom of which noble gas has the same electron configuration as the sulfide ion in g 2 S?. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1. 1s 2 2s 2 2p 6 3s 2 3p 5 4s 2 17. Which electron configuration represents the electrons in an atom of Ga in an excited state?. 2-8-17-3. 2-8-17-4. 2-8-18-3. 2-8-18-4 20. Which electron configuration represents an atom in the excited state?. 1s 2 2s 1. 1s 2 2s 2 2p 4. 1s 2 2s 2 3s 1. 1s 2 2s 2 2p 6 3s 2 page 3 tomic Structure
21. ase your answer(s) to the following question(s) on the information below. ond energy is the amount of energy required to break a chemical bond. The table below gives a formula and the carbon-nitrogen bond energy for selected nitrogen compounds. Selected Nitrogen ompounds ompound Formula arbon-nitrogen ond Energy (kj/mol) hydrogen cyanide 890. isocyanic acid 615 methanamine 293 24. opper has two naturally occurring isotopes. Information about the two isotopes is shown in the table below. Isotope Naturally Occurring Isotopes of opper tomic Mass (atomic mass units, u) Percent Natural bundance (%) u-63 62.93 69.17 u-65 64.93 30.83 Show a numerical setup for calculating the atomic mass of copper. Identify the noble gas that has atoms in the ground state with the same electron configuration as the nitrogen in a molecule of isocyanic acid. 25. The nuclides 14 6 and 14 N are similar in that they 7 both have the same. mass number. atomic number. number of neutrons. nuclear charge 22. ompared to an atom of 12 6, an atom of 14 6 has. more protons. fewer protons. more neutrons. fewer neutrons 26. Given the nuclear reaction: 14 7 N + 4 2 He 1 1 H + X. Which isotope is represented by the X when the equation is correctly balanced?. 17 8 O. 18 8 O. 17 9 F. 18 9 F 23. Isotopes of an element must have different. atomic numbers. mass numbers. numbers of protons. numbers of electrons 27. Which element has no stable isotopes?. r. Kr. Rn. Xe page 4 tomic Structure
28. toms of 16 O, 17 O, and 18 O have the same number of 31. ll isotopes of a given element must have the same. neutrons, but a different number of protons. protons, but a different number of neutrons. atomic mass. atomic number. mass number. number of neutrons. protons, but a different number of electrons. electrons, but a different number of protons 29. ase your answer(s) to the following question(s) on the information below and on your knowledge of chemistry. Iodine has many isotopes, but only iodine-127 is stable and is found in nature. One radioactive iodine isotope, I-108, decays by alpha particle emission. Iodine-131 is also radioactive and has many important medical uses. Explain, in terms of protons and neutrons, why I-127 and I-131 are different isotopes of iodine. 32. Which two notations represent different isotopes of the same element?. 6 4 e and 9 4 e. 7 3 Li and 7 3 Li. 14 7 N and 14 6. 32 32 P and 15 16 S 33. Neutral atoms of 35 l and 37 l differ with respect to their number of 30. Which two notations represent atoms that are isotopes of the same element?. 121 50 Sn and 119 50 Sn. 121 50 Sn and 121 50 Sn. electrons. protons. neutrons. positrons. 19 8 O and 19 9 F. 39 39 l and 17 19 K page 5 tomic Structure
34. ase your answer(s) to the following question(s) on the information below. Isotope Naturally Occurring Isotopes of Sulfur tomic Mass (atomic mass units, u) Natural bundance (%) 32 S 31.97 94.93 37. Which pair most represents isotopes of the same element? 120 120. X and 51 52 X. 38 39 X and 18 18 X. 21X 2+ and 19 X 2+. 26X 2+ and 26 X 3+ 33 S 32.97 0.76 34 S 33.97 4.29 36 S 35.97 0.02 State, in terms of the number of subatomic particles, one similarity and one difference between the atoms of these isotopes of sulfur. 38. Which notations represent different isotopes of the element sodium?. 32 S and 34 S. S 2 and S 6+. Na + and Na 0. 22 Na and 23 Na 35. Which element has no known stable isotope?. Hg. Po. Se. Zn 39. toms of every isotope of calcium have the same. atomic mass. atomic number. number of neutrons. number of nucleons 36. ll atoms in a given sample of an element contain the same number of. nucleons and electrons. nucleons and neutrons. protons and electrons. protons and neutrons 40. Which atoms are isotopes of the same element?. 24 25 X and 12 12 X. 20 20 X and 10 11 X 31 32. X and 15 16 X. 31 31 X and 19 19 X page 6 tomic Structure
41. Which symbols represents atoms that are isotopes of each other?. 14 and 14 N. 16 O and 18 O. 131 I and 131 I. 222 Rn and 222 Ra 44. ase your answer(s) to the following question(s) on the data table below, which shows three isotopes of neon. Isotope tomic Mass (atomic mass units) Percent Natural bundance 20Ne 19.99 90.9% 21Ne 20.99 0.3% 22Ne 21.99 8.8% ased on natural abundances, the average atomic mass of neon is closest to which whole number? 42. If X is the symbol of an element, which pair correctly represents isotopes of X? 158 158. X and 64 64 X. 64 158 X and 158 158 159. X and 64 64 X. 158 158 X and 64 64 X 65 X 45. The atomic mass of element is 63.6 atomic mass units. The only naturally occurring isotopes of element are -63 and -65. The percent abundances in a naturally occurring sample of element are closest to 43. Element X has two isotopes. If 72.0% of the element has an isotopic mass of 84.9 atomic mass units, and 28.0% of the element has an isotopic mass of 87.0 atomic mass units, the average atomic mass of element X is numerically equal to. (72.0 + 84.9) (28.0 + 87.0). 31% -63 and 69% -65. 50% -63 and 50% -65. 69% -63 and 31% -65. 100% -63 and 0% -65. (72.0 84.9) (28.0 + 87.0). (72.0 84.9) 100 + (28.0 87.0) 100. (72.0 84.9) + (28.0 87.0) page 7 tomic Structure
46. ase your answer(s) to the following question(s) on the information below. The accepted values for the atomic mass and percent natural abundance of each naturally occurring isotope of silicon are given in the data table below. Naturally Occurring Isotopes of Silicon Isotope tomic Mass (atomic mass units) Percent Natural bundance (%) Si-28 27.98 92.22 Si-29 28.98 4.69 Si-30 29.97 3.09 48. 100.00-gram sample of naturally occurring boron contains 19.78 grams of boron-10 (atomic mass = 10.01 atomic mass units) and 80.22 grams of boron-11 (atomic mass = 11.01 atomic mass units). Which numerical setup can be used to determine the atomic mass of naturally occurring boron?. (0.1978)(10.01) + (0.8022)(11.01). (0.8022)(10.01) + (0.1978)(11.01). (0.1978)(10.01) (0.8022)(11.01) Show a correct numerical setup for calculating the atomic mass of Si.. (0.8022)(10.01) (0.1978)(11.01) 49. The table below gives information about two isotopes of element X. 47. If 75.0% of the isotopes of an element have a mass of 35.0 amu and 25.0% of the isotopes have a mass of 37.0 amu, what is the atomic mass of the element?. 35.0 amu. 35.5 amu. 36.0 amu. 37.0 amu Isotope Mass Relative bundance X-10 10.01 19.91% X-11 11.01 80.09% alculate the average atomic mass of element X. Show a correct numerical setup in the space provided below. Record your answer. Express your answer to the correct number of significant figures. page 8 tomic Structure
50. The atomic mass of an element is the weighted average of the masses of 53. Which statement best explains why most atomic masses on the Periodic Table are decimal numbers?. its two most abundant isotopes. its two least abundant isotopes. all of its naturally occurring isotopes. all of its radioactive isotopes. tomic masses are determined relative to an H 1 standard.. tomic masses are determined relative to an O 16 standard.. tomic masses are a weighted average of the naturally occurring isotopes.. tomic masses are an estimated average of the artificially produced isotopes. 51. ase your answer(s) to the following question(s) on the data table below, which shows three isotopes of neon. Isotope tomic Mass (atomic mass units) Percent Natural bundance 20Ne 19.99 90.9% 21Ne 20.99 0.3% 22Ne 21.99 8.8% ased on the atomic masses and the natural abundances shown in the data table, in the space below, show a correct numerical setup for calculating the average atomic mass of neon. 52. ase your answer(s) to the following question(s) on the information below. 54. ase your answer(s) to the following question(s) on the information below. Naturally occurring elemental carbon is a mixture of isotopes. The percent composition of the two most abundant isotopes is listed below. 98.93% of the carbon atoms have a mass of 12.00 atomic mass units. 1.07% of the carbon atoms have a mass of 13.00 atomic mass units. escribe, in terms of subatomic particles found in the nucleus, one difference between the nuclei of carbon-12 atoms and the nuclei of carbon-13 atoms. The response must include both isotopes. Isotope Naturally Occurring Isotopes of Sulfur tomic Mass (atomic mass units, u) Natural bundance (%) 32 S 31.97 94.93 33 S 32.97 0.76 34 S 33.97 4.29 36 S 35.97 0.02 Show a correct numerical setup for calculating the atomic mass of sulfur. 55. Which is the most abundant isotope found in a naturally occurring uranium deposit?. 233 92 U. 235 92 U. 238 92 U. 239 92 U page 9 tomic Structure
56. ase your answer(s) to the following question(s) on the information below. The element boron, a trace element in Earth s crust, is found in foods produced from plants. oron has only two naturally occurring stable isotopes, boron-10 and boron-11. ompare the abundance of the two naturally occurring isotopes of boron. 59. sample of element X contains 90 percent 35 X atoms, 8.0 percent 37 X atoms, and 2.0 percent 38 X atoms. The average isotopic mass is closest to. 32. 35. 37. 38 57. Naturally occurring boron is composed of two isotopes. The percent abundance and the mass of each isotope are listed below. 19.9% of the boron atoms have a mass of 10.013 atomic mass units. 80.1% of the boron atoms have a mass of 11.009 atomic mass units. alculate the atomic mass of boron. Your response must include both a correct numerical setup and the calculated result. 60. The atomic mass of an element is the weighted average of the. number of protons in the isotopes of that element. number of neutrons in the isotopes of that element. atomic numbers of the naturally occurring isotopes of that element. atomic masses of the naturally occurring isotopes of that element 58. The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (shown as percents) produces this average mass?. 50% 12 and 50% 13. 50% 35 l and 50% 37 l. 75% 35 l and 25% 37 l 61. Which pair of atoms are isotopes of element X? 226 226. X and 90 91 X. 226X and 227 91. 227X and 227 91 90 X. 226X and 227 90 91 X 91 X. 75% 12 and 25% 13 page 10 tomic Structure
62. Hydrogen has three isotopes with mass numbers of 1, 2, and 3 and has an average atomic mass of 1.00794 amu. This information indicates that. equal numbers of each isotope are present 65. What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons?. 2. 2+. 4. 4+. more isotopes have an atomic mass of 2 or 3 than of 1. more isotopes have an atomic mass of 1 than of 2 or 3. isotopes have only an atomic mass of 1 66. ompared to a calcium atom, the calcium ion a 2+ has. more protons. fewer protons 63. Which change occurs when a barium atom loses two electrons?. more electrons. fewer electrons. It becomes a negative ion and its radius decreases.. It becomes a negative ion and its radius increases.. It becomes a positive ion and its radius decreases.. It becomes a positive ion and its radius increases. 67. s an Na atom forms an Na 2+ ion, the number of protons in its nucleus. decreases. increases. remains the same 64. When an atom loses an electron, the atom becomes an ion that is. positively charged and gains a small amount of mass. positively charged and loses a small amount of mass. negatively charged and gains a small amount of mass 68. Which is the atomic number of an atom that forms an ion with 18 electrons and a charge of 2 +?. 18. 20. 30. 48. negatively charged and loses a small amount of mass page 11 tomic Structure
69. ased on Reference Table E, which saturated solution will contain the highest concentration of iodide ions? TLE OF SOLUILITIES IN WTER i nearly insoluable ss slightly soluable s soluable d decomposes n not isolated acetate bromide carbonate chloride chromate hydroxide iodide nitrate phosphate sulfate luminum ss s n s n i s s i s d mmonium s s s s s s s s s s s arium s s i s i s s s i i d alcium s s i s s ss s s i ss d opper II s s i s i i n s i s i Iron II s s i s n i s s i s i Iron III s s n s i i n s i ss d Lead s ss i ss i i ss s i i i Magnesium s s i s s i s s i s d Mercury I ss i i i ss n i s i ss i Mercury II s ss i s ss i i s i d i Potassium s s s s s s s s s s s Silver ss i i i ss n i s i ss i Sodium s s s s s s s s s s s Zinc s s i s s i s s i s i sulfide 71. K atom differs from a K + ion in that the K atom has one. more electron. less electron. more proton. less proton 72. When metals form ions, they tend to do so by. losing electrons and forming positive ions. losing electrons and forming negative ions. gaining electrons and forming positive ions. gaining electrons and forming negative ions. lead iodide. silver iodide. mercury (II) iodide. iron (II) iodide 73. When a calcium atom loses its valence electrons, the ion formed has an electron configuration which is the same as an atom of. l. r. K. Sc 70. s an atom becomes an ion, its mass number. decreases. increases. remains the same 74. Given the reaction between two different elements in the gaseous state: fter a neutral sulfur atom gains two electrons, what is the resulting charge of the ion? page 12 tomic Structure
75. ompared to a e 2+ ion, a e 0 atom has. more protons. fewer protons. more electrons. fewer electrons 79. Which symbol represents a particle that has the same total number of electrons as S 2?. O 2. Si. Se 2. r 76. What is the net charge on an ion that has 9 protons, 11 neutrons, and 10 electrons? 80. How many electrons are contained in an u 3+ ion?. 76. 79. 82. 197. 1+. 2+. 1. 2 77. What is the mass number of an ion that consists of 20 protons, 20 neutrons, and 18 electrons?. 18. 20. 38. 40 81. When a metal reacts with a nonmetal, the metal will. lose electrons and form a positive ion. lose protons and form a positive ion. gain electrons and form a negative ion. gain protons and form a negative ion 78. Given the equation: This equation represents the formation of a 82. What occurs when an atom of chlorine forms a chloride ion?. fluoride ion, which is smaller in radius than a fluorine atom. fluoride ion, which is larger in radius than a fluorine atom. fluorine atom, which is smaller in radius than a fluoride ion. fluorine atom, which is larger is radius than a fluoride ion. The chlorine atom gains an electron, and its radius becomes smaller.. The chlorine atom gains an electron, and its radius becomes larger.. The chlorine atom loses an electron, and its radius becomes smaller.. The chlorine atom loses an electron, and its radius becomes larger. page 13 tomic Structure
83. n atom of an element contains 20 protons, 20 neutrons, and 20 electrons. This element is. an alkali metal. an alkaline earth metal. a halogen 86. s the number of neutrons in the nucleus of a given atom of an element increases, the atomic number of that element. decreases. increases. remains the same. a noble gas 87. The diagram below represents the nucleus of an atom. 84. Elements on the modern Periodic Table are arranged in order of increasing. atomic mass. atomic number. number of neutrons. number of valence electrons What are the atomic number and mass number of this atom?. The atomic number is 9 and the mass number is 19.. The atomic number is 9 and the mass number is 20.. The atomic number is 11 and the mass number is 19.. The atomic number is 11 and the mass number is 20. 85. The elements in the Periodic Table are arranged in order of increasing. atomic number. atomic radius. mass number. neutron number 88. What is the atomic number of the element whose atoms bond to each other in chains, rings, and networks?. 10. 8. 6. 4 page 14 tomic Structure
89. The properties of elements are periodic functions of their. mass numbers. atomic masses. atomic radii. atomic numbers 93. Which statement concerning elements is true?. ifferent elements must have different numbers of isotopes.. ifferent elements must have different numbers of neutrons.. ll atoms of a given element must have the same mass number.. ll atoms of a given element must have the same atomic number. 90. The atomic number of an alkali metal is. 1. 11. 14. 20 94. sample of matter must be copper if. each atom in the sample has 29 protons 91. Which quantity represents the number of protons in an atom?. atomic number. atoms in the sample react with oxygen. the sample melts at 1768 K. the sample can conduct electricity. oxidation number. number of neutrons. number of valence electrons 95. ase your answer(s) to the following question(s) on the information below. 92. Which quantity can correctly be represented by the symbol He?. 1 mole of atoms. 10 grams of atoms. 3 10 23 atoms. 11.2 liters of atoms The element boron, a trace element in Earth s crust, is found in foods produced from plants. oron has only two naturally occurring stable isotopes, boron-10 and boron-11. State, in terms of subatomic particles, one difference between the nucleus of a carbon-11 atom and the nucleus of a boron-11 atom. page 15 tomic Structure
96. Which of the following atoms has the greatest nuclear charge? 100. Which is the atomic number of an atom with six valence electrons?. 14 7 N. 12 6. 2 1 H. 4 2 He. 6. 8. 10. 12 97. In a sample of pure copper, all atoms have atomic numbers which are. the same and the atoms have the same number of electrons 101. Which atom has a nucleus that contains 13 protons and 14 neutrons?. Mg. e. l. N. the same but the atoms have a different number of electrons. different but the atoms have the same number of electrons. different and the atoms have a different number of electrons 102. The observed regularities in the properties of elements are periodic functions of their. atomic numbers 98. ll of the atoms of argon have the same. mass number. mass numbers. oxidation states. nonvalence electrons. atomic number. number of neutrons. number of nucleons 103. n atom of 226 Rn contains 88. 88 protons and 138 neutrons 99. What is the atomic number of an element whose atoms each contain 47 protons, 60 neutrons, and 47 electrons?. 13. 47. 60. 107. 88 protons and 138 electrons. 88 electrons and 226 neutrons. 88 electrons and 226 protons page 16 tomic Structure
104. The atomic mass of an element is calculated using the 107. What is the mass number of an atom that contains 19 protons, 19 electrons, and 20 neutrons?. atomic number and the ratios of its naturally occurring isotopes. 19. 20. 39. 58. atomic number and the half-lives of each of its isotopes. masses and the ratios of its naturally occurring isotopes. masses and the half-lives of each of its isotopes 108. Which particles have approximately the same mass?. alpha particle and beta particle. alpha particle and proton 105. ase your answer(s) to the following question(s) on the information below.. neutron and positron. neutron and proton Key = electron Element tomic iagrams of Magnesium and luminum magnesium Lewis Electron-ot iagram Electron-Shell iagram aluminum 109. The nucleus is the part of the atom that. consist mostly of empty space. has a negative charge etermine the mass number of the magnesium atom represented by the electron-shell diagram.. occupies most of the atom s total volume. contains most of the atom s total mass 106. How many grams of sodium are represented by the symbol Na?. 1.0 g of Na. 10 g of Na. 11 g of Na. 23 g of Na 110. One atomic mass unit (1 amu) is equal to the mass of a carbon-12 atom multiplied by the quantity. 12. 1 12. 1836. 1 1836 page 17 tomic Structure
111. Which diagram represents the nucleus of an atom of 27 13 l? 114. The mass number of an atom is always equal to the total number of its... electrons, only. protons, only. electrons plus protons... protons plus neutrons 115. The mass of one carbon atom is approximately equal to the total mass of. 6 neutrons. 6 alpha particles. 12 nucleons. 12 beta particles 112. The atomic mass of an atom is measured in atomic mass units. This unit is based on. 1 H. 14 N. 16 O. 12 116. ase your answer(s) to the following question(s) on the information below. Isotope Notation Naturally Occurring Isotopes of opper Percent Natural bundance (%) tomic Mass (atomic mass units, u) u-63 69.17 62.930 u-65 30.83 64.928 In the space below, show a correct numerical setup for calculating the atomic mass of copper. 113. What is the mass number of an alpha particle?. 1. 2. 0. 4 117. The atomic mass unit is defined as exactly 1 12 the mass of an atom of. 12 6. 14 6. 24 12 Mg. 26 12 Mg page 18 tomic Structure
118. n atom of fluorine has a mass of 19 atomic mass units. The total number of protons and neutrons in its nucleus is. 9. 10. 19. 28 121. Which statement best describes the nucleus of an aluminum atom?. It has a charge of +13 and is surrounded by a total of 10 electrons.. It has a charge of +13 and is surrounded by a total of 13 electrons.. It has a charge of 13 and is surrounded by a total of 10 electrons.. It has a charge of 13 and is surrounded by a total of 13 electrons. 119. Which quantity is represented by the symbol Ne?. 1 gram of neon. 1 liter of neon. 1 mole of neon. 1 atomic mass unit of neon 122. particle has a mass of 1.0 atomic mass unit. What is the approximate mass of this particle in grams?. 1.0 g. 2.0 g. 1.7 10 24 g. 6.0 10 23 g 120. ompared to the mass of an SO 2 molecule, the mass of an O 2 molecule is. one-fourth as great. one-half as great. the same. twice as great 123. In which group do the particles contain only nucleons?. protons and electrons. neutrons and electrons. protons and neutrons. protons, neutrons, and electrons page 19 tomic Structure
124. What is the total number of protons in the nucleus of an atom of potassium 42? 127. ompared to an atom of calcium-40, an atom of potassium-39 contains fewer. 15. 19. 39. 42. protons. neutrons. occupied sublevels. occupied principal energy levels 125. n experiment in which alpha particles were used to bombard thin sheets of gold foil led to the conclusion that an atom is composed mostly of. empty space and has a small, negatively charged nucleus. empty space and has a small, positively charged nucleus. a large, dense, positively charged nucleus. a large, dense, negatively charged nucleus 128. Which kind of particle, when passed through an electric field, would be attracted to the negative electrode?. an alpha particle. a beta particle 126. In all samples of the element potassium, each atom has. a neutron. an electron. 19 protons. 20 neutrons. 39 protons and neutrons. 39 nucleons page 20 tomic Structure
129. ase your answer(s) to the following question(s) on the information below and on your knowledge of chemistry. student compares some models of the atom. These models are listed in the table below in order of development from top to bottom. alton model Thomson model Rutherford model ohr model Models of the tom Model Observation onclusion Matter is conserved during a chemical reaction. athode rays are deflected by magnetic/electric fields. Most alpha particles pass straight through gold foil but a few are deflected. Unique spectral lines are emitted by excited gaseous elements. toms are hard, indivisible spheres of different sizes. toms have small, negatively charged particles as part of their internal structure. n atom is mostly empty space with a small, dense, positively charged nucleus. Packets of energy are absorbed or emitted by atoms when an electron changes shells. State one conclusion about the internal structure of the atom that resulted from the gold foil experiment. 131. ase your answer(s) to the following question(s) on the information below. Elements with atomic numbers 112 and 114 have been produced and their IUP names are pending approval. However, an element that would be put between these two elements on the Periodic Table has not yet been produced. If produced, this element will be identified by the symbol Uut until an IUP name is approved. etermine the charge of an Uut nucleus. Your response must include both the numerical value and the sign of the charge. 132. n atom of 40 r has a nucleus that contains a 18 total of. 18 electrons. 18 protons. 18 neutrons. 18 nucleons 133. Which symbol represents a proton? 130. The atoms in a sample of an element must contain nuclei with the same number of. 1 1 H. 0 1 H. 1 0 H. 0 0 H. electrons. protons. neutrons. nucleons 134. ase your answer(s) to the following question(s) on the information below. Two isotopes of potassium are K-37 and K-42. Explain, in terms of subatomic particles, why K-37 and K-42 are isotopes of potassium. page 21 tomic Structure
135. neutral atom contains 12 neutrons and 11 electrons. The number of protons in this atom is. 1. 11. 12. 23 138. In Rutherford s gold foil experiments, some alpha particles were deflected from their original paths but most passed through the foil with no deflection. Which statement about gold atoms is supported by these experimental observations?. Gold atoms consist mostly of empty space.. Gold atoms are similar to alpha particles.. lpha particles and gold nuclei have opposite charges.. lpha particles are more dense than gold atoms. 136. Which statement is true about a proton and an electron?. They have the same masses and the same charges.. They have the same masses and different charges.. They have different masses and the same charges.. They have different masses and different charges. 139. The nucleus of an atom of K 42 contains. 19 protons and 23 neutrons. 19 protons and 42 neutrons. 20 protons and 19 neutrons. 23 protons and 19 neutrons 137. n experiment using alpha particles to bombard a thin sheet of gold foil indicated that most of the volume of the atoms in the foil is taken up by. electrons. protons. neutrons. empty space 140. The number of protons in the nucleus of 32 15 P is. 15. 17. 32. 47 page 22 tomic Structure
141. Which subatomic particles are located in the nucleus of a carbon atom?. protons, only. neutrons, only. protons and neutrons 143. ase your answer(s) to the following question(s) on the information below. n atom has an atomic number of 9, a mass number of 19, and an electron configuration of 2-6-1. What is the total number of neutrons in this atom?. protons and electrons 144. Which nucleus contains the greatest number of neutrons?. 31 16 S. 32 16 S. 31 15 P. 32 15 P 142. ase your answer(s) to the following question(s) on the information below. In 1897, J. J. Thomson demonstrated in an experiment that cathode rays were deflected by an electric field. This suggested that cathode rays were composed of negatively charged particles found in all atoms. Thomson concluded that the atom was a positively charged sphere of almost uniform density in which negatively charged particles were embedded. The total negative charge in the atom was balanced by the positive charge, making the atom electrically neutral. In the early 1900s, Ernest Rutherford bombarded a very thin sheet of gold foil with alpha particles. fter interpreting the results of the gold foil experiment, Rutherford proposed a more sophisticated model of the atom. State one aspect of the modern model of the atom that agrees with a conclusion made by Thomson. 145. What is the total number of neutrons in an atom of an element that has a mass number of 19 and an atomic number of 9?. 9. 10. 19. 28 146. ase your answer(s) to the following question(s) on the information below. Naturally occurring elemental carbon is a mixture of isotopes. The percent composition of the two most abundant isotopes is listed below. 98.93% of the carbon atoms have a mass of 12.00 atomic mass units. 1.07% of the carbon atoms have a mass of 13.00 atomic mass units. In the space provided below, show a correct numerical setup for calculating the average atomic mass of carbon. page 23 tomic Structure
147. What is the total number of neutrons in an atom of 7 3 Li? 151. In which pair of elements do the nuclei of the atoms contain the same number of neutrons?. 7. 10. 3. 4. 7 3 Li and 9 4 e. 14 7 N and 16 8 O 23. Na and 24 11 12 Mg. 32 35 S and 16 17 148. n atom of potassium-37 and an atom of potassium-42 differ in their total number of 152. Which particle is electrically neutral?. electrons. neutrons. protons. positrons. proton. positron. neutron. electron 149. n atom of carbon-14 contains. 8 protons, 6 neutrons, and 6 electrons. 6 protons, 6 neutrons, and 8 electrons. 6 protons, 8 neutrons, and 8 electrons. 6 protons, 8 neutrons, and 6 electrons 153. Which statement describes the relative masses of two different particles?. neutron has less mass than a positron.. beta particle has less mass than a neutron.. n alpha particle has less mass than a positron.. n alpha particle has less mass than a beta particle. 150. neutron has a charge of. +1. +2. 0. 1 154. What is the total number of neutrons in an atom of O-18?. 18. 16. 10. 8 page 24 tomic Structure
155. Which subatomic particle has no charge?. alpha particle. beta particle. neutron. electron 159. s a a atom undergoes oxidation to a 2+, the number of neutrons in its nucleus. decreases. increases. remains the same 156. What is the total number of neutrons in an atom of 57 26 Fe?. 26. 31. 57. 83 157. Which nucleus is from an isotope of an atom with 6n the nucleus 6p? 160. The table below indicates the stability of six nuclides. Stability of Six Nuclides Nuclide -12 stable Stability -14 unstable N-14 stable N-16 unstable O-16 stable O-19 unstable ll atoms of the unstable nuclides listed in this table have.. 6n 6p. 8n 6p. 4n 8p 6n 8p. an odd number of neutrons. an odd number of protons. more neutrons than protons. more protons than neutrons 158. What is the total number of neutrons in the nucleus of a neutral atom that has 19 electrons and a mass number of 39?. 19. 20. 39. 58 161. In which two atoms do both nuclides contain the same number of neutrons? 20 40. Ne and 10 18 r. 65 65 u and 29 30 Zn. 24 26 Mg and 12 12 Mg. 14 6 and 16 8 O page 25 tomic Structure
162. Which particle has the greatest chance to overcome the electrostatic forces surrounding the nucleus of an atom?. an alpha particle. a beta particle. a proton. a neutron 166. What can be concluded if an ion of an element is smaller than an atom of the same element?. The ion is negatively charged because it has fewer electrons than the atom.. The ion is negatively charged because it has more electrons than the atom.. The ion is positively charged because it has fewer electrons than the atom.. The ion is positively charged because it has more electrons than the atom. 163. Explain, in terms of subatomic particles, why the radius of a chloride ion is larger than the radius of a chlorine atom. 167. ompared to the charge and mass of a proton, an electron has 164. Which statement best describes an electron?. It has a smaller mass than a proton and a negative charge.. It has a smaller mass than a proton and a positive charge.. the same charge and a smaller mass. the same charge and the same mass. an opposite charge and a smaller mass. an opposite charge and the same mass. It has a greater mass than a proton and a negative charge.. It has a greater mass than a proton and a positive charge. 168. What is the most probable location of an electron?. an orbital. a nucleus 165. How many electrons are in an Fe 2+ ion?. 24. 26. 28. 56. a sublevel. a principal energy level page 26 tomic Structure
169. ase your answer(s) to the following question(s) on the information below. The nucleus of one boron atom has five protons and four neutrons. etermine the total number of electrons in the boron atom. 172. Which total mass is the smallest?. the mass of 2 electrons. the mass of 2 neutrons. the mass of 1 electron plus the mass of 1 proton. the mass of 1 neutron plus the mass of 1 electron 170. What is the approximate mass of an electron?. 1 atomic mass unit. 1 12 of a -12 atom 1. 1836 of a proton. 1835 1836 of a proton 173. Which of the following particles has the smallest mass?. neutron. electron. proton. hydrogen atom 171. John alton was an English scientist who proposed that atoms were hard, indivisible spheres. In the modern model, the atom has a different internal structure. a) Identify one experiment that led scientists to develop the modern model of the atom. 174. Which subatomic particle will be attracted by a positively charged object?. proton. neutron. electron. positron b) escribe this experiment. c) State one conclusion about the internal structure of the atom, based on this experiment. 175. Explain, in terms of valence electrons, why the bonding in magnesium oxide, MgO, is similar to the bonding in barium chloride, al 2. page 27 tomic Structure
176. What is the total number of valence electrons in a calcium atom in the ground state? 181. Which of the following particles has the least mass?. 8. 2. 18. 20. an electron. a proton. a deuteron. a neutron 177. Usually the term kernel includes all parts of the atom except the. neutrons. protons. valence electrons. orbital electrons 178. What is the number of electrons in an atom that has 3 protons and 4 neutrons?. 1. 7. 3. 4 182. Given the table below that shows students examples of proposed models of the atom: Proposed Models of the tom Model Location of Protons Location of Electrons in the nucleus specific shells in the nucleus regions of most probable location dispersed throughout the atom specific shells dispersed throughout the atom regions of most probable location Which model correctly describes the locations of protons and electrons in the wave-mechanical model of the atom?.... 179. The maximum number of electrons that may be found in the third principal energy level is. 8. 2. 18. 32 180. The total number of pairs of shared electrons in a nitrogen molecule is 183. Explain, in terms of atomic structure, why the atomic radius of iodine is greater than the atomic radius of fluorine.. 1. 2. 3. 4 page 28 tomic Structure
184. n atom of oxygen is in an excited state. When an electron in this atom moves from the third shell to the second shell, energy is. emitted by the nucleus 188. Which of the following atoms has the largest atomic radius?. Na. K. Mg. a. emitted by the electron. absorbed by the nucleus. absorbed by the electron 189. Which atom in the ground state has two unpaired electrons in its outermost principal energy level? 185. Which principal energy level can hold a maximum of 18 electrons?. Na. Mg. l. Si. 5. 2. 3. 4 186. n atom of an element has the electron configuration 1s 2 2s 2 2p 2. What is the total number of valence electrons in this atom?. 6. 2. 5. 4 190. The total number of sublevels in the fourth principal energy level of an atom is. 1. 2. 3. 4 187. When an electron in an atom moves from a lower energy state to a higher energy state, the electron will. absorb energy, only. release energy, only. both absorb and release energy 191. n atom in the ground state contains 8 valence electrons. This atom is classified as. metal. semimetal. noble gas. halogen. neither absorb nor release energy page 29 tomic Structure
192. n atom with the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2 has an incomplete. 2p sublevel. second principal energy level. third principal energy level 196. ompared to an electron in the first electron shell of an atom, an electron in the third shell of the same atom has. less mass. less energy. more mass. more energy. 4s sublevel 197. Which atom in the ground state has an outermost electron with the most energy? 193. What is the total number of electrons in a completely filled fourth principal energy level?. s. K. Li. Na. 8. 10. 16. 32 198. n atom contains a total of 25 electrons. When the atom is in the ground state, how many different principal energy levels will contain electrons? 194. Which electron configuration contains three half-filled orbitals?. 1. 2. 3. 4. 1s 2 2s 2 2p 6. 1s 2 2s 2 2p 5. 1s 2 2s 2 2p 3. 1s 2 2s 2 2p 4 199. When electrons in an atom in an excited state fall to lower energy levels, energy is 195. Which principal energy level can hold a maximum of eight electrons?. 1. 2. 3. 4. absorbed, only. released, only. neither released nor absorbed. both released and absorbed page 30 tomic Structure
200. Which element has a completely filled third principal energy level?. r. N. Fe. Zn page 31 tomic Structure
Problem-ttic format version 4.4.311 c 2011 2017 Educide Software Licensed for use by Mark Gironda Terms of Use at www.problem-attic.com tomic Structure 11/16/2017 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 2-7-4-1 2-7-5 2-8-3-1 1-8-5 Note: o not allow credit for 2-8-4. Y 2-8-7-3 1 or one. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. Ne neon element 10 (62.93u)(0.6917) + (64.93u)(0.3083) cceptable responses include, but are not limited to: I-127 atoms and I-131 atoms have the same number of protons, but different numbers of neutrons; oth have 53 p, but I-127 has 74 n while I-131 has 78 n; They have the same atomic number but different mass numbers; same atomic number but different numbers of neutrons; The only difference is the number of neutrons. 19. cceptable responses include, but are not limited to: r; argon; element 18
Teacher s Key Page 2 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. Similarity: ll atoms of these isotopes have the same number of protons. ifference: n S-32 atom has 16 neutrons, an S-33 atom has 17 neutrons, an S-34 atom has 18 neutrons, and an S-36 atom has 20 neutrons. Similarity: Every sulfur atom has 16 protons. ifference: The number of neutrons in an atom of one isotope is different than the number of neutrons in an atom of a different isotope. 44. 20 45. 46. (27.98)(0.9222) + (28.98)(0.0469) + (29.97)(0.0309) or equivalent. 47. 48. 49. (19.91)(10.01) + 80.09(11.01) 100 10.81 50. 51. (0.909)(19.99) + (0.003)(20.99) + (0.088)(21.99), (90.9)(19.99) + (0.3)(20.99) + (8.8)(21.99), (90.9)(19.99) + (0.3)(20.99) + (8.8)(21.99) 100 52. (31.97)(0.9493) + (32.97)(0.0076) + (33.97)(0.0429) + (35.97)(0.0002) 53. 54. 55. 56. arbon-12 has six neutrons and carbon-13 has seven neutrons. arbon-13 has one more neutron than carbon-12. -12 has 6n; -13 has 7n. oron-11 is about four times more abundant than boron-10. 57. (10.013)(0.199) + (11.009)(0.801) = 10.81 atomic mass units 58. 59. 60. 61. 62. 63. 64. 65. 66. 67.
68. 69. 70. 71. 72. 73. 74. 75. 76. 77. 78. 79. 80. 81. 82. 83. 84. 85. 86. 87. Objective: 88. 2 negative I.06 89. 90. 91. 92. 93. Objective: 94. 95. 96. 97. 98. 99. 100. 101. 102. 103. 104. I.06 Teacher s Key Page 3 The carbon-11 nucleus has one more proton than the nucleus of boron-11. 105. 23 106. 107. 108. 109. 110.
Teacher s Key Page 4 111. 130. 112. 131. +113 113. 132. 114. 133. 115. 116. 117. 118. 119. 120. 121. 122. 123. 124. 125. 126. 127. 128. 129. (0.6917)(62.930u) + (0.3083)(64.928u) (69.17)(62.930) + (30.83)(64.928) 100 proton p p + 1 1 p 1 1 H H + 134. 135. 136. 137. 138. 139. 140. 141. 142. same number of protons, different number of neutrons 143. 10 144. 145. n atom has equal amounts of negative and positive charge. n atom has an equal number of protons and electrons. ll atoms contain electrons. Electrons are negatively charged. 146. (12.00)(0.9893) + (13.00)(0.0107) 147. 148. 149.
Teacher s Key Page 5 150. 170. 151. 152. 153. 154. 155. 156. 157. 158. 159. 160. 161. 162. 163. 164. 165. 166. 167. 168. 169. l ion has 18 electrons and 17 protons, so there is less attraction by the nucleus for the electron shells, allowing the electron shells to expand. or The radius of l is larger because the nucleus can t hold 18 electrons as close as it can hold 17 electrons. five 171. 172. 173. 174. 175. 176. 177. 178. 179. 180. 181. 182. 183. 184. 185. 186. gold foil (Rutherford), cathode rays (Thomson), electron bombardment (Moseley); In the gold-foil experiment, gold foil was bombarded with alpha particles. Some alpha particles were deflected.; The gold-foil experiment shows that an atom is mostly empty space. n atom has a small dense core. n atom has a positively charged center. The bonding in each compound involves a transfer of valence electrons from the metal to the nonmetal. or oth metals lose all of their valence electrons. n iodine atom has more electron shells than a fluorine
Teacher s Key Page 6 187. 188. 189. 190. 191. 192. 193. 194. 195. 196. 197. 198. 199. 200.