A) an electron B) a neutronC) an alpha particle D) a beta particle

1. The mass of a proton is approximately equal to themass of

A) 37 B) 20 C) 3 D) 17

2. What is the number of electrons in an atom that has20 protons and 17 neutrons?

A) a negatively charged nucleus, surrounded bynegatively charged electrons

B) a negatively charged nucleus, surrounded bypositively charged electrons

C) a positively charged nucleus, surrounded bynegatively charged electrons

D) a positively charged nucleus, surrounded bypositively charged electrons

3. Which phrase describes an Al atom?

A) a proton B) an electronC) a helium atom D) a hydrogen atom

4. Which particle has the least mass?

A) C D A B B) C D B AC) D B A C D) D B C A

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) X, proton and Z, electronB) X, proton and Z, neutronC) X, neutron and Z, protonD) X, electron and Z, proton

6. The table below gives the masses of two differentsubatomic particles found in an atom.

Which of the subatomic particles are each paired withtheir corresponding name?

A) 18 B) 19 C) 20 D) 39

7. What is the number of electrons in a potassium atom?

A) a charge of +1 and no massB) a charge of +1 and an approximate mass of 1 uC) no charge and no massD) no charge and an approximate mass of 1 u

8. Which phrase describes the charge and mass of aneutron?

A) a greater magnitude and the same signB) a greater magnitude and the opposite signC) the same magnitude and the same signD) the same magnitude and the opposite sign

9. Compared to the charge of a proton, the charge of anelectron has

A) 1 u B) 0.0005 uC) 1 g D) 0.0005 g

10. What is the approximate mass of a proton?

A) 2– B) 2+ C) 4– D) 4+

11. What is the overall charge of an ion that has 12protons, 10 electrons, and 14 neutrons?

A) A neutral nucleus is surrounded by one or morenegatively charged electrons.

B) A neutral nucleus is surrounded by one or morepositively charged electrons.

C) A positively charged nucleus is surrounded byone or more negatively charged electrons.

D) A positively charged nucleus is surrounded byone or more positively charged electrons.

12. Which statement describes the distribution of chargein an atom?

A) contains protons, neutrons, and electronsB) contains a small, dense nucleusC) has positrons and orbitalsD) is a hard, indivisible sphere

13. As a result of the gold foil experiment, it wasconcluded that an atom

A) passed through the foilB) remained trapped in the foilC) were deflected by the nuclei in gold atomsD) were deflected by the electrons in gold atoms

14. The gold foil experiment led to the conclusion thateach atom in the foil was composed mostly of emptyspace because most alpha particles directed at thefoil

A) An atom is mostly empty space with a dense,positively charged nucleus.

B) An atom is composed of at least three types ofsubatomic particles.

C) An electron has a positive charge and is locatedinside the nucleus.

D) An electron has properties of both waves andparticles.

15. Which conclusion was a direct result of the gold foilexperiment?

A) atomic massB) atomic numberC) selected oxidation statesD) number of valence electrons

16. On the Periodic Table, the number of protons in anatom of an element is indicated by its

A) atomic numberB) mass numberC) number of neutrons plus the number of

electronsD) number of neutrons plus the number of protons

17. All phosphorus atoms have the same

A) 2-8-17-3 B) 2-8-17-4C) 2-8-18-3 D) 2-8-18-4

18. Which electron configuration represents theelectrons in an atom of Ga in an excited state?

A) 7 electronsB) 17 neutronsC) a mass number of 35D) an atomic number of 17

19. Every chlorine atom has

A) 0 B) –2 C) +8 D) +16

20. What is the charge of the nucleus of an oxygenatom?

A) mass number, onlyB) atomic number, onlyC) both mass number and atomic numberD) neither mass number nor atomic number

21. The notation for the nuclide gives informationabout

A) the total number of neutrons in the atom, onlyB) the total number of protons in the atom, onlyC) the total number of protons and the total

number of neutrons in the atomD) the total number of protons and the total

number of electrons in the atom

22. What can be determined if only the atomic numberof an atom is known?

A) 69 B) 79 C) 118 D) 197

23. What is the total number of protons in an atom withthe electron configuration 2-8-18-32-18-1?

A) +5 B) +2 C) +7 D) +1

24. What is the total charge of the nucleus of a nitrogenatom?

A) number of electronsB) number of protonsC) atomic numberD) mass number

25. Compared to an atom of C-12, an atom of C-14 has agreater

A) the least abundant isotopes of the elementB) the naturally occurring isotopes of the elementC) the artificially produced isotopes of the elementD) the natural and artificial isotopes of the element

26. The atomic mass of an element is the weightedaverage of the atomic masses of

A) all of the artificially produced isotopes of MgB) all of the naturally occurring isotopes of MgC) the two most abundant artificially produced

isotopes of MgD) the two most abundant naturally occurring

isotopes of Mg

27. The atomic mass of magnesium is the weightedaverage of the atomic masses of

A) an alpha particle B) an electronC) a neutron D) a positron

28. The mass of a proton is approximately equal to themass of

A) Cl, K, Ar B) Fe, Co, NiC) Te, I, Xe D) Ne, F, Na

29. In which list are the elements arranged in order ofincreasing atomic mass?

A) 9 B) 10 C) 19 D) 28

30. What is the mass number of 199F?

A)B)C)D)

31. An atomic mass unit is defined as exactly

A) A and D B) A and GC) E and D D) E and G

32. The numbers of protons and neutrons in each of fourdifferent atoms are shown in the table below.

Which two atoms represent isotopes of the sameelement?

A) 27 protons and 31 neutronsB) 27 protons and 32 neutronsC) 59 protons and 60 neutronsD) 60 protons and 60 neutrons

33. The nucleus of an atom of cobalt-58 contains

A) the same mass number and the same atomicnumber

B) the same mass number but different atomicnumbers

C) different mass numbers but the same atomicnumber

D) different mass numbers and different atomicnumbers

34. All the isotopes of a given atom have

A) B)C) D)

35. Which notations represent different isotopes of theelement sodium?

A) D and E, only B) D, E, and QC) Q and R, only D) Q, R, and E

36. Each diagram below represents the nucleus of adifferent atom.

Which diagrams represent nuclei of the sameelement?

A) and B) and C) and D) and

37. Which two notations represent different isotopes of the same element?

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)

38. The table below gives the atomic mass and theabundance of the two naturally occurring isotopes ofbromine.

Which numerical setup can be used to calculate theatomic mass of the element bromine?

A) (0.6011)(68.926 u) + (0.3989)(70.925 u)B) (60.11)(68.926 u) + (39.89)(70.925 u)aC) (0.6011)(70.925 u) + (0.3989)(68.926 u)D) (60.11)(70.925 u) + (39.89)(68.926 u)

39. Some information about the two naturally occurringisotopes of gallium is given in the table below.

Which numerical setup can be used to calculate theatomic mass of gallium?

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)

40. The table below gives the atomic mass and the abundance of the two naturally occurring isotopes ofchlorine.

Which numerical setup can be used to calculate the atomic mass of the element chlorine?

A) an electron B) a neutronC) a nucleus D) a proton

41. An orbital is defined as a region of the mostprobable location of

A) Cs B) K C) Li D) Na

42. Which atom in the ground state has an outermostelectron with the most energy?

A) 8 B) 2 C) 14 D) 4

43. What is the total number of valence electrons in anatom of germanium in the ground state?

A) An electron in the first shell has more energythan an electron in the second shell.

B) An electron in the first shell has the sameamount of energy as an electron in the secondshell.

C) An electron in the third shell has more energythan an electron in the second shell.

D) An electron in the third shell has less energythan an electron in the second shell.

44. Which statement describes the relative energy of theelectrons in the shells of a calcium atom?

A) less mass B) less energyC) more mass D) more energy

45. Compared to an electron in the first electron shell ofan atom, an electron in the third shell of the sameatom has

A) 2–4 B) 2–6C) 2–8–4 D) 2–8–6

46. What is the electron configuration of a sulfur atom inthe ground state?

A) C B) Cl C) Si D) P

47. Which atom in the ground state has five electrons inits outer level and ten electrons in its kernel?

A) 1 B) 2 C) 3 D) 4

48. What is the highest principal energy level for anelectron in an atom of sulfur in the ground state?

A) 2-8-7-1 B) 2-8-7-2C) 2-8-7-3 D) 2-8-8-2

49. Which electron configuration represents an excitedstate for an atom of calcium?

A) 2-7 B) 2-8 C) 2-7-1 D) 2-8-1

50. Which electron configuration represents theelectrons of an atom of neon in an excited state?

A) 2-1 B) 2-7-4 C) 2-8-7 D) 2-4

51. Which electron configuration represents theelectrons of an atom in an excited state?

A) A and D B) A and X C) Z and D D) Z and X

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 B) D C) X D) Z

53. The diagram below represents the bright-line spectra of four elements and a bright-line spectrumproduced by a mixture of three of these elements.

Which element is not present in the mixture?

A) protons move from lower energy states tohigher energy states

B) protons move from higher energy states tolower energy states

C) electrons move from lower energy states tohigher energy states

D) electrons move from higher energy states tolower energy states

54. The bright-line spectrum of an element in thegaseous phase is produced as

A) absorbed as electrons move from higher tolower electron shells

B) absorbed as electrons move from lower tohigher electron shells

C) released as electrons move from higher to lowerelectron shells

D) released as electrons move from lower to higherelectron shells

55. The bright-line spectrum of sodium is producedwhen energy is

A) barium and hydrogen B) barium and lithiumC) helium and hydrogen D) helium and lithium

56. The diagram below represents the bright-line spectra of four elements and a bright-line spectrumproduced by a mixture of two of these elements.

Which two elements are in this mixture?

A) nucleus B) orbitalC) quanta D) spectra

57. Which term is defined as the region in an atomwhere an electron is most likely to be located?

A) circular path for electronsB) circular path for neutronsC) most probable location of electronsD) most probable location of neutrons

58. According to the wave-mechanical model, an orbitalis defined as the

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

59. Which group of atomic models is listed in historicalorder from the earliest to the most recent?

A) 5s B) 5p C) 3s D) 6p

60. An electron will emit energy in quanta when itsenergy state changes from 4p to

A) 2p B) 2s C) 3p D) 3s

61. Which of the following sublevels has the highestenergy?

A) 1s to 3s B) 3p to 3sC) 4d to 4s D) 4s to 3p

62. The greatest absorption of energy occurs as anelectron moves from

A) 1s12s1 B) 1s12s2

C) 1s22s1 D) 1s22s2

63. Which electron configuration represents an atom oflithium in an excited state?

A) 1s22s22p53s1 B) 1s22s22p63s1

C) 1s22s22p63s2 D) 1s22s22p63s23p1

64. Which electron configuration represents an atom inthe excited state?

A) 1s22s2 B) 1s23p1

C) 1s22s22p5 D) 1s22s22p6

65. Which electron configuration represents an atom inan excited state?

A) 1 B) 5 C) 7 D) 9

66. What is the total number of valence electrons in anatom with the electron configuration 1s22s22p5?

67. Base your answer to the following question on Theorbital notation of an atom in the ground state is

A) C B) N C) B D) Be

Which atom is represented by this notation?

A)

B)

C)

D)

68. Which orbital notation correctly represents a noblegas in the ground state?

A)

B)

C)

D)

69. Which orbital notation represents a boron atom inthe ground state?

A)

B)

C)

D)

70. Which electron notation represents the valenceelectrons of a phosphorus atom in the ground state?