hem term # 1 review sheet Name: ate: 1. n isotope of which element has an atomic number of 6 and a mass number of 14?. carbon. magnesium. nitrogen. silicon 6. Which atoms represent different isotopes of the same element? 39 39. r and 18 19 K. 58 59 o and 27 28 Ni. 12 6 and 13 6. 35l and 35 17 17 l 2. Isotopes of the same element must have the same. atomic number. mass number 7. Which is the symbol for the deutrium isotope of hydrogen?. 1 1 H. 2 1 H. 3 1 H. 4 2 H. number of nucleons. number of neutrons 8. toms of every isotope of calcium have the same 3. Which of the following nuclei is an isotope of 10p 11n?. atomic mass. atomic number. number of neutrons. number of nucleons. 10p 9n *YT*. 11p *YT* 10n. 9p *YT* 11n. 11p *YT* 12n 9. Which pair most represents isotopes of the same element?. 120X and 120 51 52 X. 38 39 X and 18 18 X. 21X 2+ and 19 X 2+. 26X 2+ and 26 X 3+ 4. If X is the symbol of an element, which pair correctly represents isotopes of X?. 158X and 158 64 64 X. 64X and 158 158 64 X. 158 159 X and 64 64 X. 158X and 158 64 65 X 10. neutral atom with 6 electrons and 8 neutrons is an isotope of. carbon. silicon. nitrogen. oxygen 5. ifferent isotopes of the same element must have a different. mass number. atomic number. number of protons. number of electrons 11. ll isotopes of which element in Group 16 (VI) are naturally radioactive?. S. Se. Po. Te page 1
hem term # 1 review sheet 12. The nuclides 14 6 and 14 N are similar in that they both have the 7 same 17. Neutral atoms of 35 l and 37 l differ with respect to their number of. mass number. atomic number. electrons. protons. neutrons. positrons. number of neutrons. nuclear charge 18. Which pair must represent atoms of the same element? 13. Which element has no known stable isotope?. carbon. potassium. 14X and 14 6 7 X. 12X and 13 6 6 X. 2 1 X and 4 2 X. 13X and 14 6 7 X. polonium. phosphorus 14. In the reaction 27 13 l + 4 2 He X + 1 n, the isotope represented by 0 X is 19. Given the nuclear reaction: 14 7 N + 4 2 He 1 H + X. Which isotope 1 is represented by the X when the equation is correctly balanced?. 17 8 O. 18 8 O. 17 9 F. 18 9 F. 29 12 Mg. 28 13 l. 27 14 Si. 30 15 P 20. ll atoms in a given sample of an element contain the same number of 15. n element occurs as a mixture of isotopes. The atomic mass of the element is based upon. the masses of the individual isotopes, only. nucleons and electrons. nucleons and neutrons. protons and electrons. protons and neutrons. the relative abundances of the isotopes, only. both the masses and the relative abundances of the individual isotopes. neither the masses nor the relative abundances of the individual isotopes 21. 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 16. ll isotopes of a given element must have the same. atomic mass. atomic number. mass number. number of neutrons 22. Which element has no stable isotopes?. r. Kr. Rn. Xe page 2
hem term # 1 review sheet 23. Which atoms are isotopes of the same element?. 24X and 25 12 12 X. 20X and 20 10 11 X. 31 X and 32 15 16 X. 31 X and 31 19 19 X 24. toms of different isotopes of the same element differ in their total number of 27. The total number of protons, electrons, and neutrons in each of four different atoms are shown in the table below. tom Subatomic Particles in Four ifferent toms Total Number of Protons Total Number of Electrons Total Number of Neutrons 6 6 7 6 6 8 X 7 7 8 Z 8 8 9 Which two atoms are isotopes of the same element?. and. and Z. X and. X and Z. electrons. neutrons. protons. valence electrons 28. Which two nuclides are isotopes of the same element? 25. Which two notations represent different isotopes of the same element?. 6 4 e and 9 4 e. 7 3 Li and 7 3 Li. 20Na and 20 11 10 Ne. 39K and 40 19 20 a 39. K and 42 19 19 K. 14 6 and 14 7 N. 14 7 N and 14 6. 32P and 32 15 16 S 26. 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 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. 29. The table below shows the number of subatomic particles in atom X and in atom Z. tom Subatomic Particles in Two toms Number of Protons Number of Neutrons Number of Electrons X 6 6 6 Z 6 7 6 tom X and atom Z are isotopes of the element. aluminum. carbon. magnesium. nitrogen page 3
hem term # 1 review sheet 30. 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 35. The volume of an acid required to neutralize exactly 15.00 milliliters (ml) of a base could be measured most precisely if it were added to the base solution from a. 100 ml graduate. 125 ml Erlenmeyer flask. 50 ml buret. 50 ml beaker Show a numerical setup for calculating the atomic mass of copper. 36. Which of the following atoms has the smallest covalent atomic radius? 31. In the modern Periodic Table, the elements are arranged in order of increasing. Li. e.. F. atomic number. mass number. oxidation number. valence number 37. ompared to the covalent atomic radius of a sodium atom, the covalent atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having 32. Which symbol represents an alkaline earth element?. Na. Mg. Ne. g. a larger nuclear charge. a smaller nuclear charge. more principal energy levels. fewer principal levels 33. In the reaction Zn + u 2+ Zn 2+ + u, the u 2+ ions. gain electrons. lose electrons. gain protons. lose protons 38. Which element in Period 2 has the greatest tendency to form a negative ion?. lithium. carbon. neon. fluorine 34. Which is the most active nonmetal in the Periodic Table of the Elements? 39. The most active metal in Group 2 (II) is. Na. F. I. l. Mg. Sr. a. a page 4
hem term # 1 review sheet 40. In Period 4 of the Periodic Table, the atom with the largest covalent radius is located in Group 46. In which period are all the elements gases at 298 K and standard pressure?. 1 (I). 13 (III). 3 (III). 18 (O). 1. 2. 3. 4 41. Which element in Period 3 has the greatest tendency to gain electrons?. Na. Si. l. r 47. Which of the Group 15 (V) elements can lose an electron most readily?. N. P. Sb. i 42. Element X forms the compounds Xl 3 and X 2 O 3. In the Periodic Table, element X would most likely be found in Group. 1 (I). 2 (II). 13 (III). 14 (IV) 48. s the Group 1 (I) 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. nuclear charge is decreasing 43. s the elements in Group 2 (II) of the Periodic Table are considered from top to bottom, the chemical reactivity of each succeeding element generally. decreases. increases. number of neutrons is increasing. number of principal energy levels is decreasing. distance between the valence electron and the nucleus is increasing. remains the same 44. The highest ionization energies in any period are found in Group. 1 (I). 2 (II) 49. Which element in Group 15 (V) has the most metallic character?. N. P. s. i. 17 (VII). 18 (O) 45. Which of the following Group 17 (VII) elements has the highest melting point?. fluorine. chlorine. bromine. iodine 50. Which element in Group 18 (O) of the Periodic Table has the highest first ionization energy?. Kr. r. Ne. He page 5
hem term # 1 review sheet 51. s the atoms of the metals of Group 1 (I) in the ground state are considered in order from top to bottom, the number of occupied principal energy levels 54. toms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms. decreases. increases. remains the same. number of principal energy levels. number of valence electrons. atomic numbers. atomic masses 52. Which diagram correctly shows the relationship between electronegativity and atomic number for the elements of Period 3? 55. Which element in Group 17 is the most active nonmetal?... r. I. l. F.. 56. s elements in Group 15 of the Periodic Table are considered in order from top to bottom, the metallic character of each successive element generally. decreases. increases. remains the same 57. Which sequence of Group 18 elements demonstrates a gradual decrease in the strength of the van der Waals forces?. r(l), Kr(l), Ne(l), Xe(l). Kr(l), Xe(l), r(l), Ne(l) 53. s the elements Li to F in Period 2 of the Periodic Table are considered in succession how do the relative electronegativity and the covalent radius of each successive element compare?. Ne(l), r(l), Kr(l), Xe(l). Xe(l), Kr(l), r(l), Ne(l). The relative electronegativity decreases, and the covalent radius decreases.. The relative electronegativity decreases, and the covalent radius increases.. The relative electronegativity increases, and the covalent radius decreases.. The relative electronegativity increases, and the covalent radius increases. 58. In the ground state, atoms of the elements in Group 15 of the Periodic Table all have the same number of. filled principal energy levels. occupied principal energy levels. neutrons in the nucleus. electrons in the valence shell page 6
hem term # 1 review sheet 59. s the elements in Period 3 are considered from left to right, they tend to 63. toms of which of the following elements have the smallest covalent radius?. lose electrons more readily and increase in metallic character. Si. P. S. l. lose electrons more readily and increase in nonmetallic character. gain electrons more readily and increase in metallic character. gain electrons more readily and increase in nonmetallic character 64. t which location in the Periodic Table would the most active metallic element be found?. in Group 1 at the top. in Group 1 at the bottom. in Group 17 at the top. in Group 17 at the bottom 60. Which element in Group 15 has the greatest metallic character?. nitrogen. phosphorus. antimony. bismuth 65. s the elements of Group 16 are considered in order from top to bottom, the covalent radius of each successive element increases. This increase is primarily due to an increase in. atomic number 61. s the elements in Group 2 are considered in order of increasing atomic number, the atomic radius of each successive element increases. This increase is primarily due to an increase in the number of. mass number. the number of protons occupying the nucleus. the number of occupied principal energy levels. occupied principal energy levels. electrons in the outermost shell. neutrons in the nucleus. unpaired electrons 66. s the elements in Period 2 of the Periodic Table are considered in succession from left to right, there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the. number of protons increases, and the number of shells of electrons remains the same 62. In which area of the Periodic Table are the elements with the strongest nonmetallic properties located?. lower left. upper left. lower right. upper right. number of protons increases, and the number of shells of electrons increases. number of protons decreases, and the number of shells of electrons remains the same. number of protons decreases, and the number of shells of electrons increases page 7
hem term # 1 review sheet 67. What determines the order of placement of the elements on the modern Periodic Table?. atomic number. atomic mass. the number of neutrons, only. the number of neutrons and protons 69. s the elements in Group 17 on the Periodic Table are considered from top to bottom, what happens to the atomic radius and the metallic character of each successive element?. The atomic radius and the metallic character both increase.. The atomic radius increases and the metallic character decreases.. The atomic radius decreases and the metallic character increases.. The atomic radius and the metallic character both decrease. 68. ase your answer(s) to the following question(s) on the reading passage below and on your knowledge of chemistry. Glow in the ark, and Scientific Peril The [Marie and Pierre] uries set out to study radioactivity in l898. Their first accomplishment was to show that radioactivity was a property of atoms themselves. Scientifically, that was the most important of their findings, because it helped other researchers refine their understanding of atomic structure. More famous was their discovery of polonium and radium. Radium was the most radioactive substance the uries had encountered. Its radioactivity is due to the large size of the atom, which makes the nucleus unstable and prone to decay, usually to radon and then lead, by emitting particles and energy as it seeks a more stable configuration. Marie urie struggled to purify radium for medical uses, including early radiation treatment for tumors. ut radium s bluish glow caught people s fancy, and companies in the United States began mining it and selling it as a novelty: for glow-in-the-dark light pulls, for instance, and bogus cure-all patent medicines that actually killed people. What makes radium so dangerous is that it forms chemical bonds in the same way as calcium, and the body can mistake it for calcium and absorb it into the bones. Then, it can bombard cells with radiation at close range, which may cause bone tumors or bone-marrow damage that can give rise to anemia or leukemia. enise Grady, The New York Times, October 6, 1998 Using information from the Periodic Table, explain why radium forms chemical bonds in the same way as calcium does. 70. The elements in Period 5 on the Periodic Table are arranged from left to right in order of. decreasing atomic mass. decreasing atomic number. increasing atomic mass. increasing atomic number 71. The data table below shows elements Xx, Yy, and Zz from the same group on the Periodic Table. Element tomic Mass (atomic mass unit) tomic Radius (pm) Xx 69.7 141 Yy 114.8? Zz 204.4 171 What is the most likely atomic radius of element Yy?. 103 pm. 127 pm. 166 pm. 185 pm 72. The elements located in the lower left corner of the Periodic Table are classified as. metals. nonmetals. metalloids. noble gases page 8
hem term # 1 review sheet 73. t STP, an element that is a brittle solid and a poor conductor of heat and electricity could have an atomic number of 78. s the elements of Group 17 are considered in order of increasing atomic number, there is an increase in. 12. 13. 16. 17. atomic radius. electronegativity. first ionization energy 74. Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number?. number of electrons in the first shell. The atomic radius decreases, and the first ionization energy generally increases.. The atomic radius decreases, and the first ionization energy generally decreases.. The atomic radius increases, and the first ionization energy generally increases.. The atomic radius increases, and the first ionization energy generally decreases. 79. Which statement describes the general trends in electronegativity and metallic properties as the elements in Period 2 are considered in order of increasing atomic number?. oth electronegativity and metallic properties decrease.. oth electronegativity and metallic properties increase.. Electronegativity decreases and metallic properties increase.. Electronegativity increases and metallic properties decrease. 75. 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 and the melting point of element Z is 7. Which temperature is closest to the melting point of element X?. 7. 101. 219. 226 80. The electron dot symbol X: represents. an alkali metal. an alkaline earth metal. a halogen. a transition element 76. 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. 81. Which group is represented by the electron dot symbol.... X:?. 17 (VII). 16 (VI). 15 (V). 14 (IV) Identify one element that would be chemically similar to Uut. 82. n element whose atoms have the electron configuration 2 8 18 1 is 77. Which element is a metalloid?. l. r. s. u. a transition element. a noble gas. an alkali metal. an alkaline earth metal page 9
hem term # 1 review sheet 83. Given the electron dot formula: H :..X: Which atom represented as X would have the least attraction for the electrons that form the bond?. F. l. I. r 89. Which electron dot diagram represents a molecule that has a polar covalent bond?.... 84. student determined in the laboratory that one mole of KMnO 4 had a mass of 171.54 grams. The mass of one mole of KMnO 4 in an accepted chemistry reference is 158.04 grams. What is the percent error of the mass of one mole of KMnO 4 as determined by the student? 90. Which electron-dot formula represents a substance that contains a nonpolar covalent bond?. 0.787%. 7.87%. 8.54%. 13.5%.... 85. In an experiment the gram atomic mass of magnesium was determined to be 24.7. ompared to the accepted value 24.3, the percent error for this determination was. 0.400. 1.65. 24.7. 98.4 86. student determined the melting point of a substance to be 55.2. If the accepted value is 50.1, the percent error in her determination is 91. Which electron-dot symbol represents an atom of argon in the ground state?..... 5.10. 9.24. 10.2. 12.0 87. Which is the correct electron dot representation of an atom of sulfur in the ground state?. S:.. Ṡ:.... Ṣ:. :.... S: 92. Which electron-dot structure represents a nonpolar molecule?.. 88. Which is the electron dot symbol of an atom of boron in the ground state?..... Ḅ:.... Ḃ:. Ḃ: page 10
hem term # 1 review sheet 93. In the box provided below, draw the electron-dot (Lewis) structure of an atom of calcium. 96. Which Lewis electron-dot structure is drawn correctly for the atom it represents?.... 97. Given the Lewis electron-dot diagram: 94. In the box provided below, draw the electron-dot (Lewis) structure of an atom of chlorine. Which electrons are represented by all of the dots?. the carbon valence electrons, only. the hydrogen valence electrons, only. the carbon and hydrogen valence electrons. all of the carbon and hydrogen electrons 95. ase your answer(s) to the following question(s) on the information below. Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are bonded together. 98. ase your answer(s) to the following question(s) on your knowledge of chemical bonding and on the Lewis electron-dot diagrams of H2S, O2, and F2 below. Molecule : l 2 Molecule : l 4 Molecule : NH 3 Which atom, when bonded as shown, has the same electron configuration as an atom of argon? In the box below, draw the electron-dot (Lewis) structure for the NH 3 molecule. 99. ase your answer(s) to the following question(s) on the balanced equation below. 2Na(s) + l 2 (g) 2Nal(s) raw a Lewis electron-dot diagram for a molecule of chlorine, l 2. page 11
hem term # 1 review sheet 100. Which Lewis electron-dot diagram is correct for a S 2 ion?.. 106. Which atom has the least attraction for the electrons in a bond between that atom and an atom of hydrogen?. carbon. nitrogen. oxygen. fluorine.. 107. The relatively high boiling point of water is primarily due to the presence of 101. Which is the predominate type of attraction between molecules of HF in the liquid state?. hydrogen bonding. electrocovalent bonding. hydrogen bonds. van der Waals forces. molecule-ion attractions. ion-ion attractions. ionic bonding. covalent bonding 102. Hydrogen bonds are strongest between molecules of. H 2 O(l). H 2 S(l). H 2 Se(l). H 2 Te(l) 108. How does the ground state electron configuration of the hydrogen atom differ from that of a ground state helium atom?. Hydrogen has one electron in a higher energy level.. Hydrogen has two electrons in a lower energy level.. Hydrogen contains a half-filled orbital. 103. The strongest hydrogen bonds are formed between molecules in which hydrogen is covalently bonded to an element with. Hydrogen contains a completely filled orbital.. high electronegativity and large atomic radius. high electronegativity and small atomic radius. low electronegativity and large atomic radius. low electronegativity and small atomic radius 109. The light produced by signs using neon gas results from electrons that are. moving from a higher to a lower principal energy level. moving from a lower to a higher principal energy level 104. Hydrogen bonds are strongest between molecules of. being lost by the Ne(g) atoms. being gained by the Ne(g) atoms. HF. Hl. Hr. HI 105. In which of the following liquids are hydrogen bonds between molecules the strongest?. HI(l). Hr(l). Hl(l). HF(l) 110. Which metal must be combined with chromium to produce stainless steel?. radium. iron. copper. zinc page 12
hem term # 1 review sheet 111. Mobile electrons are a distinguishing characteristic of 117. The P l bond in a molecule of Pl 3 is. an ionic bond. an electrovalent bond. a metallic bond. a covalent bond. nonpolar covalent. polar covalent. coordinate covalent. electrocovalent 112. Which type of bond is present in copper wire?. covalent. ionic. electrovalent. metallic 113. Which substance contains particles held together by metallic bonds? 118. Which electron dot formula represents a molecule that contains a nonpolar covalent bond?. x r x. r:..... H x. r:..... Na +[. x Fx x]. H. x Fx x. Ni(s). Ne(s). N 2 (s). L 2 (s) 114. The ability to conduct electricity in the solid state is a characteristic of metallic bonding. This characteristic is best explained by the presence of. high ionization energies. high electronegativities. mobile electrons. mobile protons 119. What type of bonding is found in the molecule Hr?. ionic. metallic. nonpolar covalent. polar covalent 115. Metallic bonding occurs between metal atoms that have. full valence orbitals and low ionization energies. full valence orbitals and high ionization energies. vacant valence orbitals and low ionization energies. vacant valence orbitals and high ionization energies 120. Which substance contains a polar covalent bond?. Na 3 N. Mg 3 N 2. NH 3. N 2 116. Which molecule is a dipole?. He. H 2. NH 3. H 4 page 13
cces format version 4.4.158 c 1997 2011 Educide Software Licensed for use by Problem-ttic hem term # 1 review sheet 01/23/2013 1. 21. 2. 22. 3. 23. 4. 24. 5. 25. 6. 7. 8. 9. 10. 11. 26. 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. 12. 27. 13. 28. 14. 29. 15. 30. (62.93u)(0.6917) + (64.93u)(0.3083) 16. 31. 17. 32. 18. 33. 19. 34. 20.
Teacher s Key Page 2 35. 57. 36. 58. 37. 59. 38. 60. 39. 61. 40. 62. 41. 63. 42. 64. 43. 65. 44. 66. 45. 67. 46. 47. 48. 49. 50. 51. 52. 53. 54. 55. 56. 68. 69. 70. 71. 72. 73. 74. 75. 76. oth are located in Group 2 on the periodic table. ny element in Group 13. cceptable responses include, but are not limited to: Tl, boron
Teacher s Key Page 3 77. 78. 79. 80. 81. 82. 83. 84. 85. 86. 87. 88. 89. 90. 91. 92. 93. 94. 95. 96. 97. 98. S sulfur 99. 100. 101. 102. 103. 104.
Teacher s Key Page 4 105. 106. 107. 108. 109. 110. 111. 112. 113. 114. 115. 116. 117. 118. 119. 120.