1. The mass of a proton is approximately equal to the mass of A) an electron B) a neutron C) an alpha particle D) a beta particle 2. What is the number of electrons in an atom that has 20 protons and 17 neutrons? A) 37 B) 20 C) 3 D) 17 3. Which phrase describes an Al atom? A) a negatively charged nucleus, surrounded by negatively charged electrons B) a negatively charged nucleus, surrounded by positively charged electrons C) a positively charged nucleus, surrounded by negatively charged electrons D) a positively charged nucleus, surrounded by positively charged electrons 4. Which particle has the least mass? A) a proton B) an electron C) a helium atom D) a hydrogen atom 5. Four statements about the development of the atomic model are shown below. A: Electrons have wavelike properties. B: Atoms have small, negatively charged particles. C: The center of an atom is a small, dense nucleus. D: Atoms are hard, indivisible spheres. Which order of statements represents the historical development of the atomic model? A) C D A B B) C D B A C) D B A C D) D B C A
6. The table below gives the masses of two different subatomic particles found in an atom. Which of the subatomic particles are each paired with their corresponding name? A) X, proton and Z, electron B) X, proton and Z, neutron C) X, neutron and Z, proton D) X, electron and Z, proton 7. What is the number of electrons in a potassium atom? A) 18 B) 19 C) 20 D) 39 8. Which phrase describes the charge and mass of a neutron? A) a charge of +1 and no mass B) a charge of +1 and an approximate mass of 1 u C) no charge and no mass D) no charge and an approximate mass of 1 u 9. Compared to the charge of a proton, the charge of an electron has A) a greater magnitude and the same sign B) a greater magnitude and the opposite sign C) the same magnitude and the same sign D) the same magnitude and the opposite sign 10. What is the approximate mass of a proton? A) 1 u B) 0.0005 u C) 1 g D) 0.0005 g 11. What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons? A) 2 B) 2+ C) 4 D) 4+ 12. Which statement describes the distribution of charge in an atom? A) A neutral nucleus is surrounded by one or more negatively charged electrons. B) A neutral nucleus is surrounded by one or more positively charged electrons. C) A positively charged nucleus is surrounded by one or more negatively charged electrons. D) A positively charged nucleus is surrounded by one or more positively charged electrons. 13. As a result of the gold foil experiment, it was concluded that an atom A) contains protons, neutrons, and electrons B) contains a small, dense nucleus C) has positrons and orbitals D) is a hard, indivisible sphere 14. The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space because most alpha particles directed at the foil A) passed through the foil B) remained trapped in the foil C) were deflected by the nuclei in gold atoms D) were deflected by the electrons in gold atoms 15. Which conclusion was a direct result of the gold foil experiment? A) An atom is mostly empty space with a dense, positively charged nucleus. B) An atom is composed of at least three types of subatomic particles. C) An electron has a positive charge and is located inside the nucleus. D) An electron has properties of both waves and particles. 16. On the Periodic Table, the number of protons in an atom of an element is indicated by its A) atomic mass B) atomic number C) selected oxidation states D) number of valence electrons
17. All phosphorus atoms have the same A) atomic number B) mass number C) number of neutrons plus the number of electrons D) number of neutrons plus the number of protons 18. Which electron configuration represents the electrons in an atom of Ga in an excited state? A) 2-8-17-3 B) 2-8-17-4 C) 2-8-18-3 D) 2-8-18-4 19. Every chlorine atom has A) 7 electrons B) 17 neutrons C) a mass number of 35 D) an atomic number of 17 20. What is the charge of the nucleus of an oxygen atom? A) 0 B) 2 C) +8 D) +16 21. The notation for the nuclide gives information about A) mass number, only B) atomic number, only C) both mass number and atomic number D) neither mass number nor atomic number 22. What can be determined if only the atomic number of an atom is known? A) the total number of neutrons in the atom, only B) the total number of protons in the atom, only C) the total number of protons and the total number of neutrons in the atom D) the total number of protons and the total number of electrons in the atom 23. What is the total number of protons in an atom with the electron configuration 2-8-18-32-18-1? A) 69 B) 79 C) 118 D) 197 24. What is the total charge of the nucleus of a nitrogen atom? A) +5 B) +2 C) +7 D) +1 25. Compared to an atom of C-12, an atom of C-14 has a greater A) number of electrons B) number of protons C) atomic number D) mass number 26. The atomic mass of an element is the weighted average of the atomic masses of A) the least abundant isotopes of the element B) the naturally occurring isotopes of the element C) the artificially produced isotopes of the element D) the natural and artificial isotopes of the element 27. The atomic mass of magnesium is the weighted average of the atomic masses of A) all of the artificially produced isotopes of Mg B) all of the naturally occurring isotopes of Mg C) the two most abundant artificially produced isotopes of Mg D) the two most abundant naturally occurring isotopes of Mg 28. The mass of a proton is approximately equal to the mass of A) an alpha particle B) an electron C) a neutron D) a positron 29. In which list are the elements arranged in order of increasing atomic mass? A) Cl, K, Ar B) Fe, Co, Ni C) Te, I, Xe D) Ne, F, Na 30. What is the mass number of 19 9F? A) 9 B) 10 C) 19 D) 28 31. An atomic mass unit is defined as exactly A) B) C) D)
32. The numbers of protons and neutrons in each of four different atoms are shown in the table below. 36. Each diagram below represents the nucleus of a different atom. Which diagrams represent nuclei of the same element? A) D and E, only B) D, E, and Q C) Q and R, only D) Q, R, and E Which two atoms represent isotopes of the same element? A) A and D B) A and G C) E and D D) E and G 33. The nucleus of an atom of cobalt-58 contains A) 27 protons and 31 neutrons B) 27 protons and 32 neutrons C) 59 protons and 60 neutrons D) 60 protons and 60 neutrons 34. All the isotopes of a given atom have A) the same mass number and the same atomic number B) the same mass number but different atomic numbers C) different mass numbers but the same atomic number D) different mass numbers and different atomic numbers 35. Which notations represent different isotopes of the element sodium? A) B) C) D)
37. Which two notations represent different isotopes of the same element? A) and B) and C) and D) and 38. The table below gives the atomic mass and the abundance of the two naturally occurring isotopes of bromine. Which numerical setup can be used to calculate the atomic mass of the element bromine? A) (78.92 u)(50.69) + (80.92 u)(49.31) B) (78.92 u)(49.31) + (80.92 u)(50.69) C) (78.92 u)(0.5069) + (80.92 u)(0.4931) D) (78.92 u)(0.4931) + (80.92 u)(0.5069) 39. Some information about the two naturally occurring isotopes of gallium is given in the table below. Which numerical setup can be used to calculate the atomic mass of gallium? A) (0.6011)(68.926 u) + (0.3989)(70.925 u) B) (60.11)(68.926 u) + (39.89)(70.925 u)a C) (0.6011)(70.925 u) + (0.3989)(68.926 u) D) (60.11)(70.925 u) + (39.89)(68.926 u)
40. The table below gives the atomic mass and the abundance of the two naturally occurring isotopes of chlorine. Which numerical setup can be used to calculate the atomic mass of the element chlorine? A) (34.97 u)(75.76) + (36.97 u)(24.24) B) (34.97 u)(0.2424) + (36.97 u)(0.7576) C) (34.97 u)(0.7576) + (36.97 u)(0.2424) D) (34.97 u)(24.24) + (36.97 u)(75.76) 41. An orbital is defined as a region of the most probable location of A) an electron B) a neutron C) a nucleus D) a proton 42. Which atom in the ground state has an outermost electron with the most energy? A) Cs B) K C) Li D) Na 43. What is the total number of valence electrons in an atom of germanium in the ground state? A) 8 B) 2 C) 14 D) 4 44. Which statement describes the relative energy of the electrons in the shells of a calcium atom? A) An electron in the first shell has more energy than an electron in the second shell. B) An electron in the first shell has the same amount of energy as an electron in the second shell. C) An electron in the third shell has more energy than an electron in the second shell. D) An electron in the third shell has less energy than an electron in the second shell. 45. Compared to an electron in the first electron shell of an atom, an electron in the third shell of the same atom has A) less mass B) less energy C) more mass D) more energy 46. What is the electron configuration of a sulfur atom in the ground state? A) 2 4 B) 2 6 C) 2 8 4 D) 2 8 6 47. Which atom in the ground state has five electrons in its outer level and ten electrons in its kernel? A) C B) Cl C) Si D) P 48. What is the highest principal energy level for an electron in an atom of sulfur in the ground state? A) 1 B) 2 C) 3 D) 4 49. Which electron configuration represents an excited state for an atom of calcium? A) 2-8-7-1 B) 2-8-7-2 C) 2-8-7-3 D) 2-8-8-2 50. Which electron configuration represents the electrons of an atom of neon in an excited state? A) 2-7 B) 2-8 C) 2-7-1 D) 2-8-1 51. Which electron configuration represents the electrons of an atom in an excited state? A) 2-1 B) 2-7-4 C) 2-8-7 D) 2-4
52. The bright-line spectra produced by four elements are represented in the diagram below. Given the bright-line spectrum of a mixture formed from two of these elements: Which elements are present in this mixture? A) A and D B) A and X C) Z and D D) Z and X
53. The diagram below represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of three of these elements. Which element is not present in the mixture? A) A B) D C) X D) Z 54. The bright-line spectrum of an element in the gaseous phase is produced as A) protons move from lower energy states to higher energy states B) protons move from higher energy states to lower energy states C) electrons move from lower energy states to higher energy states D) electrons move from higher energy states to lower energy states 55. The bright-line spectrum of sodium is produced when energy is A) absorbed as electrons move from higher to lower electron shells B) absorbed as electrons move from lower to higher electron shells C) released as electrons move from higher to lower electron shells D) released as electrons move from lower to higher electron shells
56. The diagram below represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of two of these elements. Which two elements are in this mixture? A) barium and hydrogen B) barium and lithium C) helium and hydrogen D) helium and lithium 57. Which term is defined as the region in an atom where an electron is most likely to be located? A) nucleus B) orbital C) quanta D) spectra 58. According to the wave-mechanical model, an orbital is defined as the A) circular path for electrons B) circular path for neutrons C) most probable location of electrons D) most probable location of neutrons 59. Which group of atomic models is listed in historical order from the earliest to the most recent? A) hard-sphere model, wave-mechanical model, electron-shell model B) hard-sphere model, electron-shell model, wave-mechanical model C) electron-shell model, wave-mechanical model, hard-sphere model D) electron-shell model, hard-sphere model, wave-mechanical model 60. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 61. Which of the following sublevels has the highest energy? A) 2p B) 2s C) 3p D) 3s 62. The greatest absorption of energy occurs as an electron moves from A) 1s to 3s B) 3p to 3s C) 4d to 4s D) 4s to 3p 63. Which electron configuration represents an atom of lithium in an excited state? A) 1s 1 2s 1 B) 1s 1 2s 2 C) 1s 2 2s 1 D) 1s 2 2s 2 64. Which electron configuration represents an atom in the excited state? A) 1s 2 2s 2 2p 5 3s 1 B) 1s 2 2s 2 2p 6 3s 1 C) 1s 2 2s 2 2p 6 3s 2 D) 1s 2 2s 2 2p 6 3s 2 3p 1 65. Which electron configuration represents an atom in an excited state? A) 1s 2 2s 2 B) 1s 2 3p 1 C) 1s 2 2s 2 2p 5 D) 1s 2 2s 2 2p 6 66. What is the total number of valence electrons in an atom with the electron configuration 1s 2 2s 2 2p 5? A) 1 B) 5 C) 7 D) 9
67. Base your answer to the following question on The orbital notation of an atom in the ground state is Which atom is represented by this notation? A) C B) N C) B D) Be 68. Which orbital notation correctly represents a noble gas in the ground state? A) B) C) D) 69. Which orbital notation represents a boron atom in the ground state? A) B) C) D) 70. Which electron notation represents the valence electrons of a phosphorus atom in the ground state? A) B) C) D)