Name: Class: Date: ID: A

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 principal quantum number indicates what property of an electron? a. position b. speed c. energy level d. 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? a. 1s 2 2s 2 2p 2 3s 2 3p 2 4s 1 b. 1s 2 2s 2 2p 10 3s 2 3p 3 c. 1s 2 2s 2 3s 2 3p 6 3d 1 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 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? a. 4f 7 b. 4f c. 4f 13 d. 4f 14 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 light given off by an electric discharge through sodium vapor is. a. a continuous spectrum b. an emission spectrum c. of a single wavelength d. 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 atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be a. the same. b. different from each other. c. the same as those of several other elements. d. 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 the elements Pt, V, Li, and Kr, which is a nonmetal? a. Pt b. V c. Li d. Kr 50. To what category of elements does an element belong if it is a poor conductor of electricity? a. transition elements b. metalloids c. nonmetals d. metals 51. What element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 2? 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 metals in Groups 1A, 2A, and 3A a. gain electrons when they form ions. b. all form ions with a negative charge. c. all have ions with a 1 + charge. d. 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 you move from left to right across the second period of the periodic table a. ionization energy increases. b. atomic radii increase. c. electronegativity decreases. d. 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: A PTS: 1 DIF: L1 REF: p. 131 2. ANS: F PTS: 1 DIF: L1 REF: p. 148 OBJ: 5.3.4 Distinguish between quantum mechanics and classical mechanics. 3. ANS: D PTS: 1 DIF: L1 REF: p. 145 OBJ: 5.3.3 Explain how the frequencies of light are related to changes in electron energies. 4. ANS: B PTS: 1 DIF: L1 REF: p. 134 5. ANS: C PTS: 1 DIF: L1 REF: p. 134 6. ANS: E PTS: 1 DIF: L1 REF: p. 134 7. ANS: D PTS: 1 DIF: L1 REF: p. 143 OBJ: 5.3.2 Describe how Einstein explained the photoelectric effect. 8. ANS: E PTS: 1 DIF: L1 REF: p. 129 OBJ: 5.1.1 Describe what Bohr proposed in his model of the atom. 9. ANS: B PTS: 1 DIF: L1 REF: p. 138 OBJ: 5.3.1 Explain what causes atomic emission spectra. 10. ANS: C PTS: 1 DIF: L1 REF: p. 138 OBJ: 5.3.1 Explain what causes atomic emission spectra. 11. ANS: F PTS: 1 DIF: L2 REF: p. 139 OBJ: 5.3.1 Explain what causes atomic emission spectra. 12. ANS: A PTS: 1 DIF: L2 REF: p. 140 OBJ: 5.3.1 Explain what causes atomic emission spectra. 13. ANS: H PTS: 1 DIF: L1 REF: p. 162 OBJ: 6.1.3 Describe how the modern periodic table is organized. 14. ANS: I PTS: 1 DIF: L1 REF: p. 162 OBJ: 6.1.3 Describe how the modern periodic table is organized. 1

ID: A 15. ANS: F PTS: 1 DIF: L1 REF: p. 162 OBJ: 6.1.3 Describe how the modern periodic table is organized. 16. ANS: D PTS: 1 DIF: L1 REF: p. 165 OBJ: 6.1.4 Identify three broad classes of elements. 17. ANS: E PTS: 1 DIF: L1 REF: p. 172 OBJ: 6.2.2 Classify elements based on electron configuration. 18. ANS: C PTS: 1 DIF: L1 REF: p. 174 OBJ: 6.3.1 Describe trends among elements for atomic size. 19. ANS: G PTS: 1 DIF: L1 REF: p. 161 OBJ: 6.1.2 Describe how Mendeleev organized his periodic table. 20. ANS: J PTS: 1 DIF: L1 REF: p. 176 OBJ: 6.3.2 Explain how ions form. 21. ANS: A PTS: 1 DIF: L1 REF: p. 181 OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. 22. ANS: B PTS: 1 DIF: L1 REF: p. 177 OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity. MULTIPLE CHOICE 23. ANS: A PTS: 1 DIF: L2 REF: p. 129 OBJ: 5.1.1 Describe what Bohr proposed in his model of the atom. 24. ANS: A PTS: 1 DIF: L2 REF: p. 129 OBJ: 5.1.2 Describe what the quantum mechanical model determines about the electrons in an atom. 25. ANS: C PTS: 1 DIF: L2 REF: p. 131 26. ANS: B PTS: 1 DIF: L2 REF: p. 131 27. ANS: B PTS: 1 DIF: L2 REF: p. 132 28. ANS: D PTS: 1 DIF: L2 REF: p. 132 29. ANS: D PTS: 1 DIF: L2 REF: p. 132 2

ID: A 30. ANS: B PTS: 1 DIF: L2 REF: p. 132 31. ANS: B PTS: 1 DIF: L1 REF: p. 132 32. ANS: C PTS: 1 DIF: L2 REF: p. 132 33. ANS: D PTS: 1 DIF: L2 REF: p. 134 34. ANS: D PTS: 1 DIF: L2 REF: p. 134 35. ANS: C PTS: 1 DIF: L2 REF: p. 135 p. 136 36. ANS: D PTS: 1 DIF: L2 REF: p. 135 p. 136 37. ANS: A PTS: 1 DIF: L2 REF: p. 134 p. 135 38. ANS: A PTS: 1 DIF: L2 REF: p. 137 39. ANS: D PTS: 1 DIF: L2 REF: p. 136 p. 137 40. ANS: A PTS: 1 DIF: L1 REF: p. 138 p. 139 OBJ: 5.3.1 Explain what causes atomic emission spectra. 41. ANS: B PTS: 1 DIF: L2 REF: p. 140 OBJ: 5.3.1 Explain what causes atomic emission spectra. 42. ANS: A PTS: 1 DIF: L2 REF: p. 140 OBJ: 5.3.1 Explain what causes atomic emission spectra. 43. ANS: A PTS: 1 DIF: L2 REF: p. 140 OBJ: 5.3.1 Explain what causes atomic emission spectra. 44. ANS: D PTS: 1 DIF: L1 REF: p. 143 OBJ: 5.3.2 Describe how Einstein explained the photoelectric effect. 45. ANS: D PTS: 1 DIF: L2 REF: p. 148 OBJ: 5.3.4 Distinguish between quantum mechanics and classical mechanics. 46. ANS: B PTS: 1 DIF: L2 REF: p. 162 OBJ: 6.1.3 Describe how the modern periodic table is organized. 3

ID: A 47. ANS: A PTS: 1 DIF: L1 REF: p. 172 OBJ: 6.2.2 Classify elements based on electron configuration. 48. ANS: C PTS: 1 DIF: L1 REF: p. 164 OBJ: 6.1.4 Identify three broad classes of elements. 49. ANS: D PTS: 1 DIF: L2 REF: p. 165 OBJ: 6.1.4 Identify three broad classes of elements. 50. ANS: C PTS: 1 DIF: L2 REF: p. 165 OBJ: 6.1.4 Identify three broad classes of elements. 51. ANS: C PTS: 1 DIF: L2 REF: p. 171 OBJ: 6.2.2 Classify elements based on electron configuration. 52. ANS: B PTS: 1 DIF: L2 REF: p. 172 OBJ: 6.2.2 Classify elements based on electron configuration. 53. ANS: B PTS: 1 DIF: L1 REF: p. 174 OBJ: 6.3.1 Describe trends among elements for atomic size. 54. ANS: A PTS: 1 DIF: L1 REF: p. 174 OBJ: 6.3.1 Describe trends among elements for atomic size. 55. ANS: A PTS: 1 DIF: L2 REF: p. 175 OBJ: 6.3.1 Describe trends among elements for atomic size. 56. ANS: B PTS: 1 DIF: L2 REF: p. 174 p. 175 OBJ: 6.3.1 Describe trends among elements for atomic size. 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. 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. 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. 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. 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. 63. ANS: A PTS: 1 DIF: L2 REF: p. 161 OBJ: 6.1.2 Describe how Mendeleev organized his periodic table. 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. 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. SHORT ANSWER 66. ANS: 1s 2 2s 2 PTS: 1 DIF: L2 REF: p. 136 67. ANS: 1s 2 2s 2 2p 6 3s 2 3p 5 PTS: 1 DIF: L2 REF: p. 136 5