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Name: ______________________ Class: _________________ Date: _________ ID: A EOC review II Matching Match each item with the correct statement below. a. atomic orbital d. ground state b. aufbau principle e. Pauli exclusion principle c. electron configuration f. Heisenberg uncertainty principle ____ 1. region of high probability of finding an electron ____ 2. states the impossibility of knowing both velocity and position of a moving particle at the same time ____ 3. lowest energy level ____ 4. tendency of electrons to enter orbitals of lowest energy first ____ 5. arrangement of electrons around atomic nucleus ____ 6. each orbital has at most two electrons Match each item with the correct statement below. a. atomic emission spectrum d. photon b. frequency e. quantum c. wavelength f. spectrum ____ 7. discrete bundle of electromagnetic energy ____ 8. energy needed to move an electron from one energy level to another ____ 9. number of wave cycles passing a point per unit of time ____ 10. distance between wave crests ____ 11. separation of light into different wavelengths ____ 12. frequencies of light emitted by an element Match each item with the correct statement below. a. electronegativity f. periodic law b. ionization energy g. atomic mass c. atomic radius h. period d. metal i. group e. transition metal j. electrons ____ 13. horizontal row in the periodic table ____ 14. vertical column in the periodic table ____ 15. A repetition of properties occurs when elements are arranged in order of increasing atomic number. ____ 16. type of element that is a good conductor of heat and electric current ____ 17. type of element characterized by the presence of electrons in the d orbital 1 Name: ______________________ ID: A ____ 18. one-half the distance between the nuclei of two atoms when the atoms are joined ____ 19. basis for Mendeleev’s arrangement of the periodic table ____ 20. subatomic particles that are transferred to form positive and negative ions ____ 21. ability of an atom to attract electrons when the atom is in a compound ____ 22. energy required to remove an electron from an atom Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 23. In Bohr's model of the atom, where are the electrons and protons located? a. The electrons move around the protons, which are at the center of the atom. b. The electrons and protons move throughout the atom. c. The electrons occupy fixed positions around the protons, which are at the center of the atom. d. The electrons and protons are located throughout the atom, but they are not free to move. ____ 24. How does the energy of an electron change when the electron moves closer to the nucleus? a. It decreases. b. It increases. c. It stays the same. d. It doubles. ____ 25. The a. b. c. d. principal quantum number indicates what property of an electron? position speed energy level electron cloud shape ____ 26. What is the shape of the 3p atomic orbital? a. sphere b. dumbbell c. bar d. two perpendicular dumbbells ____ 27. How many energy sublevels are in the second principal energy level? a. 1 b. 2 c. 3 d. 4 ____ 28. What is the maximum number of f orbitals in any single energy level in an atom? a. 1 b. 3 c. 5 d. 7 2 Name: ______________________ ID: A ____ 29. What is the maximum number of d orbitals in a principal energy level? a. 1 b. 2 c. 3 d. 5 ____ 30. What is the maximum number of orbitals in the p sublevel? a. 2 b. 3 c. 4 d. 5 ____ 31. What is the maximum number of electrons in the second principal energy level? a. 2 b. 8 c. 18 d. 32 ____ 32. What types of atomic orbitals are in the third principal energy level? a. s and p only b. p and d only c. s, p, and d only d. s, p, d, and f ____ 33. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p? a. 2d b. 3d c. 3f d. 4s ____ 34. According to the aufbau principle, a. an orbital may be occupied by only two electrons. b. electrons in the same orbital must have opposite spins. c. electrons enter orbitals of highest energy first. d. electrons enter orbitals of lowest energy first. ____ 35. What is the number of electrons in the outermost energy level of an oxygen atom? a. 2 b. 4 c. 6 d. 8 ____ 36. What is the electron configuration of potassium? 2 2 2 2 2 1 a. 1s 2s 2p 3s 3p 4s 2 2 10 2 3 b. 1s 2s 2p 3s 3p 2 2 2 6 1 c. 1s 2s 3s 3p 3d 2 2 6 2 6 1 d. 1s 2s 2p 3s 3p 4s 3 Name: ______________________ ID: A ____ 37. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals? a. one electron in each orbital b. two electrons in one orbital, one in another, none in the third c. three in one orbital, none in the other two d. Three electrons cannot fill three empty 2p atomic orbitals. ____ 38. What is the basis for exceptions to the aufbau diagram? a. Filled and half-filled energy sublevels are more stable than partially-filled energy sublevels. b. Electron configurations are only probable. c. Electron spins are more important than energy levels in determining electron configuration. d. Some elements have unusual atomic orbitals. ____ 39. Which electron configuration of the 4f energy sublevel is the most stable? 7 a. 4f b. 4f 13 c. 4f 14 d. 4f ____ 40. How are the frequency and wavelength of light related? a. They are inversely proportional to each other. b. Frequency equals wavelength divided by the speed of light. c. Wavelength is determined by dividing frequency by the speed of light. d. They are directly proportional to each other. ____ 41. The a. b. c. d. light given off by an electric discharge through sodium vapor is ____. a continuous spectrum an emission spectrum of a single wavelength white light ____ 42. Emission of light from an atom occurs when an electron a. drops from a higher to a lower energy level. b. jumps from a lower to a higher energy level. c. moves within its atomic orbital. d. falls into the nucleus. ____ 43. The a. b. c. d. atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be the same. different from each other. the same as those of several other elements. the same as each other only in the ultraviolet range. ____ 44. What are quanta of light called? a. charms b. excitons c. muons d. photons 4 Name: ______________________ ID: A ____ 45. According to the Heisenberg uncertainty principle, if the position of a tiny moving particle is known, the a. mass of the particle cannot be exactly determined. b. charge of the particle cannot be exactly determined. c. spin of the particle cannot be exactly determined. d. velocity of the particle cannot be exactly determined. ____ 46. Which of the following elements is in the same period as phosphorus? a. carbon b. magnesium c. nitrogen d. oxygen ____ 47. Each period in the periodic table corresponds to a(n) ____. a. principal energy level b. energy sublevel c. orbital d. suborbital ____ 48. Which of the following categories includes the majority of the elements? a. metalloids b. liquids c. metals d. nonmetals ____ 49. Of a. b. c. d. the elements Pt, V, Li, and Kr, which is a nonmetal? Pt V Li Kr ____ 50. To a. b. c. d. what category of elements does an element belong if it is a poor conductor of electricity? ____ transition elements metalloids nonmetals metals 2 2 6 2 2 ____ 51. What element has the electron configuration 1s 2s 2p 3s 3p ? a. nitrogen b. selenium c. silicon d. silver ____ 52. Which of the following is true about the electron configurations of the representative elements? a. The highest occupied s and p sublevels are completely filled. b. The highest occupied s and p sublevels are partially filled. c. The electrons with the highest energy are in a d sublevel. d. The electrons with the highest energy are in an f sublevel. 5 Name: ______________________ ID: A ____ 53. How does atomic radius change from top to bottom in a group in the periodic table? a. It tends to decrease. b. It tends to increase. c. It first increases, then decreases. d. It first decreases, then increases. ____ 54. How does atomic radius change from left to right across a period in the periodic table? a. It tends to decrease. b. It tends to increase. c. It first increases, then decreases. d. It first decreases, then increases. ____ 55. What causes the shielding effect to remain constant across a period? a. Electrons are added to the same principal energy level. b. Electrons are added to different principal energy levels. c. The charge on the nucleus is constant. d. The atomic radius increases. ____ 56. What element in the second period has the largest atomic radius? a. carbon b. lithium c. potassium d. neon ____ 57. Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases? a. more shielding of the electrons in the highest occupied energy level b. an increase in size of the nucleus c. an increase in number of protons d. fewer electrons in the highest occupied energy level ____ 58. The a. b. c. d. metals in Groups 1A, 2A, and 3A gain electrons when they form ions. all form ions with a negative charge. + all have ions with a 1 charge. lose electrons when they form ions. ____ 59. What is the element with the lowest electronegativity value? a. cesium b. helium c. calcium d. fluorine ____ 60. What is the element with the highest electronegativity value? a. cesium b. helium c. calcium d. fluorine 6 Name: ______________________ ID: A ____ 61. Which of the following elements has the smallest ionic radius? a. Li b. K c. O d. S ____ 62. Which of the following decreases with increasing atomic number in Group 2A? a. shielding effect b. ionic size c. ionization energy d. number of electrons ____ 63. Which of the following statements correctly compares the relative size of an ion to its neutral atom? a. The radius of an anion is greater than the radius of its neutral atom. b. The radius of an anion is identical to the radius of its neutral atom. c. The radius of a cation is greater than the radius of its neutral atom. d. The radius of a cation is identical to the radius of its neutral atom. ____ 64. Which of the following factors contributes to the increase in ionization energy from left to right across a period? a. an increase in the shielding effect b. an increase in the size of the nucleus c. an increase in the number of protons d. fewer electrons in the highest occupied energy level ____ 65. As a. b. c. d. you move from left to right across the second period of the periodic table ionization energy increases. atomic radii increase. electronegativity decreases. atomic mass decreases. Short Answer 66. Give the electron configuration for a neutral atom of beryllium. 67. Give the electron configuration for a neutral atom of chlorine. 7 ID: A EOC review II Answer Section MATCHING 1. ANS: OBJ: BLM: 2. ANS: OBJ: BLM: 3. ANS: OBJ: BLM: 4. ANS: OBJ: BLM: 5. ANS: OBJ: BLM: 6. ANS: OBJ: BLM: A PTS: 1 DIF: L1 REF: p. 131 5.1.3 Explain how sublevels of principal energy levels differ. knowledge F PTS: 1 DIF: L1 REF: p. 148 5.3.4 Distinguish between quantum mechanics and classical mechanics. knowledge D PTS: 1 DIF: L1 REF: p. 145 5.3.3 Explain how the frequencies of light are related to changes in electron energies. knowledge B PTS: 1 DIF: L1 REF: p. 134 5.2.1 List the three rules for writing the electron configurations of elements. knowledge C PTS: 1 DIF: L1 REF: p. 134 5.2.1 List the three rules for writing the electron configurations of elements. knowledge E PTS: 1 DIF: L1 REF: p. 134 5.2.1 List the three rules for writing the electron configurations of elements. knowledge 7. ANS: OBJ: BLM: 8. ANS: OBJ: BLM: 9. ANS: OBJ: 10. ANS: OBJ: 11. ANS: OBJ: 12. ANS: OBJ: D PTS: 1 DIF: L1 REF: p. 143 5.3.2 Describe how Einstein explained the photoelectric effect. knowledge E PTS: 1 DIF: L1 REF: p. 129 5.1.1 Describe what Bohr proposed in his model of the atom. knowledge B PTS: 1 DIF: L1 REF: p. 138 5.3.1 Explain what causes atomic emission spectra. BLM: knowledge C PTS: 1 DIF: L1 REF: p. 138 5.3.1 Explain what causes atomic emission spectra. BLM: knowledge F PTS: 1 DIF: L2 REF: p. 139 5.3.1 Explain what causes atomic emission spectra. BLM: comprehension A PTS: 1 DIF: L2 REF: p. 140 5.3.1 Explain what causes atomic emission spectra. BLM: comprehension 13. ANS: OBJ: BLM: 14. ANS: OBJ: BLM: H PTS: 1 DIF: L1 REF: p. 162 6.1.3 Describe how the modern periodic table is organized. knowledge I PTS: 1 DIF: L1 REF: p. 162 6.1.3 Describe how the modern periodic table is organized. knowledge 1 ID: A 15. ANS: OBJ: BLM: 16. ANS: OBJ: 17. ANS: OBJ: BLM: 18. ANS: OBJ: 19. ANS: OBJ: BLM: 20. ANS: OBJ: 21. ANS: OBJ: BLM: 22. ANS: OBJ: BLM: F PTS: 1 DIF: L1 REF: 6.1.3 Describe how the modern periodic table is organized. knowledge D PTS: 1 DIF: L1 REF: 6.1.4 Identify three broad classes of elements. BLM: E PTS: 1 DIF: L1 REF: 6.2.2 Classify elements based on electron configuration. knowledge C PTS: 1 DIF: L1 REF: 6.3.1 Describe trends among elements for atomic size. BLM: G PTS: 1 DIF: L1 REF: 6.1.2 Describe how Mendeleev organized his periodic table. knowledge J PTS: 1 DIF: L1 REF: 6.3.2 Explain how ions form. BLM: knowledge A PTS: 1 DIF: L1 REF: 6.3.3 Describe periodic trends for first ionization energy, ionic knowledge B PTS: 1 DIF: L1 REF: 6.3.3 Describe periodic trends for first ionization energy, ionic knowledge p. 162 p. 165 knowledge p. 172 p. 174 knowledge p. 161 p. 176 p. 181 size, and electronegativity. p. 177 size, and electronegativity. MULTIPLE CHOICE 23. ANS: OBJ: BLM: 24. ANS: OBJ: BLM: 25. ANS: OBJ: BLM: 26. ANS: OBJ: BLM: 27. ANS: OBJ: BLM: 28. ANS: OBJ: BLM: 29. ANS: OBJ: BLM: A PTS: 1 DIF: L2 REF: p. 129 5.1.1 Describe what Bohr proposed in his model of the atom. comprehension A PTS: 1 DIF: L2 REF: p. 129 5.1.2 Describe what the quantum mechanical model determines about the electrons in an atom. application C PTS: 1 DIF: L2 REF: p. 131 5.1.3 Explain how sublevels of principal energy levels differ. comprehension B PTS: 1 DIF: L2 REF: p. 131 5.1.3 Explain how sublevels of principal energy levels differ. comprehension B PTS: 1 DIF: L2 REF: p. 132 5.1.3 Explain how sublevels of principal energy levels differ. comprehension D PTS: 1 DIF: L2 REF: p. 132 5.1.3 Explain how sublevels of principal energy levels differ. comprehension D PTS: 1 DIF: L2 REF: p. 132 5.1.3 Explain how sublevels of principal energy levels differ. comprehension 2 ID: A 30. ANS: OBJ: BLM: 31. ANS: OBJ: BLM: 32. ANS: OBJ: BLM: 33. ANS: OBJ: BLM: 34. ANS: OBJ: BLM: 35. ANS: OBJ: BLM: 36. ANS: OBJ: BLM: 37. ANS: OBJ: BLM: 38. ANS: OBJ: BLM: 39. ANS: OBJ: BLM: 40. ANS: OBJ: 41. ANS: OBJ: 42. ANS: OBJ: 43. ANS: OBJ: 44. ANS: OBJ: BLM: 45. ANS: OBJ: BLM: 46. ANS: OBJ: BLM: B PTS: 1 DIF: L2 REF: p. 132 5.1.3 Explain how sublevels of principal energy levels differ. comprehension B PTS: 1 DIF: L1 REF: p. 132 5.1.3 Explain how sublevels of principal energy levels differ. knowledge C PTS: 1 DIF: L2 REF: p. 132 5.1.3 Explain how sublevels of principal energy levels differ. comprehension D PTS: 1 DIF: L2 REF: p. 134 5.2.1 List the three rules for writing the electron configurations of elements. application D PTS: 1 DIF: L2 REF: p. 134 5.2.1 List the three rules for writing the electron configurations of elements. comprehension C PTS: 1 DIF: L2 REF: p. 135 | p. 136 5.2.1 List the three rules for writing the electron configurations of elements. application D PTS: 1 DIF: L2 REF: p. 135 | p. 136 5.2.1 List the three rules for writing the electron configurations of elements. application A PTS: 1 DIF: L2 REF: p. 134 | p. 135 5.2.1 List the three rules for writing the electron configurations of elements. comprehension A PTS: 1 DIF: L2 REF: p. 137 5.2.1 List the three rules for writing the electron configurations of elements. comprehension D PTS: 1 DIF: L2 REF: p. 136 | p. 137 5.2.1 List the three rules for writing the electron configurations of elements. application A PTS: 1 DIF: L1 REF: p. 138 | p. 139 5.3.1 Explain what causes atomic emission spectra. BLM: knowledge B PTS: 1 DIF: L2 REF: p. 140 5.3.1 Explain what causes atomic emission spectra. BLM: comprehension A PTS: 1 DIF: L2 REF: p. 140 5.3.1 Explain what causes atomic emission spectra. BLM: comprehension A PTS: 1 DIF: L2 REF: p. 140 5.3.1 Explain what causes atomic emission spectra. BLM: comprehension D PTS: 1 DIF: L1 REF: p. 143 5.3.2 Describe how Einstein explained the photoelectric effect. knowledge D PTS: 1 DIF: L2 REF: p. 148 5.3.4 Distinguish between quantum mechanics and classical mechanics. comprehension B PTS: 1 DIF: L2 REF: p. 162 6.1.3 Describe how the modern periodic table is organized. comprehension 3 ID: A 47. ANS: A PTS: 1 DIF: L1 REF: p. 172 OBJ: 6.2.2 Classify elements based on electron configuration. BLM: knowledge 48. ANS: C PTS: 1 DIF: L1 REF: p. 164 OBJ: 6.1.4 Identify three broad classes of elements. BLM: knowledge 49. ANS: D PTS: 1 DIF: L2 REF: p. 165 OBJ: 6.1.4 Identify three broad classes of elements. BLM: application 50. ANS: C PTS: 1 DIF: L2 REF: p. 165 OBJ: 6.1.4 Identify three broad classes of elements. BLM: comprehension 51. ANS: C PTS: 1 DIF: L2 REF: p. 171 OBJ: 6.2.2 Classify elements based on electron configuration. BLM: application 52. ANS: B PTS: 1 DIF: L2 REF: p. 172 OBJ: 6.2.2 Classify elements based on electron configuration. BLM: comprehension 53. ANS: B PTS: 1 DIF: L1 REF: p. 174 OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: knowledge 54. ANS: A PTS: 1 DIF: L1 REF: p. 174 OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: knowledge 55. ANS: A PTS: 1 DIF: L2 REF: p. 175 OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: comprehension 56. ANS: B PTS: 1 DIF: L2 REF: p. 174 | p. 175 OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: comprehension 57. ANS: A PTS: 1 DIF: L2 REF: p. 174 | p. 175 OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: analysis 58. ANS: D PTS: 1 DIF: L2 REF: p. 176 OBJ: 6.3.2 Explain how ions form. BLM: comprehension 59. ANS: A PTS: 1 DIF: L2 REF: p. 181 OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. BLM: comprehension 60. ANS: D PTS: 1 DIF: L2 REF: p. 181 OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. BLM: comprehension 61. ANS: A PTS: 1 DIF: L2 REF: p. 179 OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. BLM: application 62. ANS: C PTS: 1 DIF: L2 REF: p. 175 | p. 182 OBJ: 6.3.1 Describe trends among elements for atomic size. | 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. BLM: comprehension 63. ANS: A PTS: 1 DIF: L2 REF: p. 161 OBJ: 6.1.2 Describe how Mendeleev organized his periodic table. BLM: comprehension 64. ANS: C PTS: 1 DIF: L2 REF: p. 178 OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. BLM: comprehension 4 ID: A 65. ANS: A PTS: 1 DIF: L2 REF: p. 175 | p. 182 OBJ: 6.3.1 Describe trends among elements for atomic size. | 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. BLM: comprehension SHORT ANSWER 66. ANS: 2 2 1s 2s PTS: 1 DIF: L2 REF: p. 136 OBJ: 5.2.1 List the three rules for writing the electron configurations of elements. BLM: application 67. ANS: 2 2 6 2 5 1s 2s 2p 3s 3p PTS: 1 DIF: L2 REF: p. 136 OBJ: 5.2.1 List the three rules for writing the electron configurations of elements. BLM: application 5