5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.

Transcription

1 1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added one at a time to the lowest energy orbitals available according to a. the Pauli exclusion principle. c. the Aufbau principle. b. Hund s rule. d. Planck s constant. 3. Once the electron in a hydrogen atom absorbs a quantum of energy, it: a. is now in its ground state. c. has released a photon. b. is now in its excited state. d. none of these a. c. b. d. 4. Which of the above graphs a, b, c, or d most likely represents the distribution (in 2-D) of a 1s-electron cloud around a hydrogen atom nucleus, if the average distance from the nucleus were plotted on the x-axis and the number of electrons per unit of area were plotted on the y-axis? 5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d. 4s 2 3d 10 4p 7 6. The statement that all elements want to be noble gases is a way of expressing the a. octet rule. c. triad rule. b. rule of octaves d. orbital principle. 7. An atom may be radioactive if the nucleus contains a. too many neutrons. c. more than 83 protons. b. too few protons. d. any of the above. 8. If the electron configuration of an element is 1s 2 2s 2 2p 6 3s 2 3p 5, the element is: a. iron. b. chlorine. c. bromine. d. phosphorus.

2 2 c E = h 9. The chemical symbol for the ion with 34 protons and 36 electrons is which of the following? a. 2 Yb b. Se 2+ c. Yb 2- d. Se 2- e. 2 Se 10. Which of the following accounts for the fact that electrons surround the nucleus of an atom? a. gravity b. strong nuclear force c. weak nuclear force d. electromagnetism 11. How many protons are in the isotope bismuth-214? a. 208 b. 83 c. 131 d. 214 e The chemical symbol for the ion with 23 protons and 18 electrons is which of the following? a. Na 5+ b. V 5+ c. V 5- d. Na 5- e. 5 Na The graph to the left plots the number protons of various elements from the periodic table against the number of neutrons. Which of the labeled points on the graph a., b., c., d., or e. is best described by each of the following statements? (Use each only once.) 13. Indicates a one-to-one ratio of protons to neutrons. 14. Indicates the beginning of a series of elements whose most abundant isotopes are radioactive. 15. Indicates an increasing number of protons. 16. Indicates an increasing number of neutrons. 17. Indicates a belt of stability, in which are found elements whose nuclei do not spontaneously decay. a. b. c. d. 18. Which of the above orbital-shape schematics *, a., b., c., or d., represents a single s orbital? * Think of these representations as two-dimensional cross-sections of the three-dimensional orbitals, as discussed in class. The dot at the origin of the coordinate system is the indicated axis, perpendicular to the plane of the page, projecting out of the page (and, for that matter, into the page).

3 3 c E = h a. b. c. d. 19. Which of the above orbital-shape schematics, a., b., c., or d., represents a single d yz orbital? a. b. c. d. 20. Which of the above orbital-shape schematics, a., b., c., or d., represents a single p z orbital? 21. Are cations (a) bigger or (b) smaller than their neutral counterparts? 22. How many unpaired electrons are in nitrogen? a. one b. two c. three d. four e. five 23. How many valence electrons are in nitrogen? a. one b. two c. three d. four e. five 24. On Independence Day, when you are watching fireworks with your family and your little brother or sister (or a talking dog) asks you what causes the yellow, bright red, and bluishgreen colors in the explosions, you should correctly reply: a. Sodium, potassium, and ethyl alcohol ions, respectively. b. Sodium, strontium, and copper ions, respectively. c. Copper, strontium, and potassium ions, respectively. d. Barium, lithium, and calcium ions, respectively. 25. Which have shorter wavelengths, (a) microwaves or (b) gamma rays? 26. The quantum mechanical model of the atom: a. is concerned with the probability of finding an electron in a certain position. b. was proposed by Neils Bohr. c. defines the exact path of an electron around the nucleus. d. has many analogies in the visible world.

4 4 c E = h 27. Which of the following was responsible for determining that electrons were part of the substructure of atoms? a. Millikan s oil-drop experiment. c. Rutherford s gold-foil experiment. b. Thomson s cathode-ray experiment. d. Dalton s ball-bearing experiment. 28. A cathode ray a. is deflected by a negatively charged plate. b. consists of photons with no mass. c. is deflected by a positively charged plate. d. is unaffected by a magnet. 29. Which of the following is the number of neutrons in molybdenum-96? a. 42 b. 96 c. 54 d. 138 e The product(s) for the beta decay of francium-223 is(are) which of the following? a. b. 223 Rn c. Ra 1 88 d. e Ra Ra The products for the alpha decay of a. samarium-146 and 4 He Gd Rn are which of the following? c. gold-146 and an alpha particle b. Nd-60 and a helium nucleus d. Dy-154 and an alpha particle 32. How many protons, neutrons, and electrons are present in the following ion? a. 13 protons, 6 neutrons, and 4 electrons b. 6 protons, 13 neutrons, and 10 electrons c. 6 protons, 7 neutrons, and 4 electrons d. 6 protons, 7 neutrons, and 10 electrons e. 6 protons, 7 neutrons, and 4 electrons 33. How many protons, neutrons, and electrons are present in uranium-238? a. 92 protons, 92 electrons, and 146 neutrons b. 92 protons, 146 electrons, and 92 neutrons c. 92 protons, 92 neutrons, and 146 electrons d. 238 protons, 238 neutrons, and 238 electrons e. 146 protons, 238 neutrons, and 92 electrons 34. How many protons, neutrons, and electrons are present in following ion? a. 58 protons, 82 electrons, and 61 neutrons b. 82 protons, 58 electrons, and 140 neutrons c. 58 protons, 82 neutrons, and 61 electrons d. 140 protons, 58 neutrons, and 3 electrons e. 58 protons, 82 neutrons, and 55 electrons

5 5 c E = h 35. The frequency and energy of electromagnetic radiation are: a. directly related. b. unrelated. c. inversely related. d. equal. 36. In order to occupy the same orbital, two electrons must have: a. parallel spin. c. opposite charge. b. different energies. d. opposite spin. 37. What is the total number of orbitals in the third principal energy level? a. 1 b. 9 c. 4 d What is the total number of sublevels in the fourth principal energy level? a. 1 b. 9 c. 4 d What is the maximum number of electrons allowed in the third energy level? a. 2 b. 18 c. 8 d What is the maximum number of electrons that can occupy one orbital? a. 1 b. 8 c. 2 d The electron configuration for nitrogen is: a. 1s 2 2s 2 2p 3. b. 1s 2 2s 2 2p 6. c. 1s 2 2s 2 2p 5. d. 1s 2 2s 2 2p 6 3s The atom whose electron configuration is 1s 2 2s 2 2p 6 3s 2 3p 1 is: a. B. b. Na. c. Al. d. Ga. 43. The valence electron configuration for Ca is: a. 3s 2. b. 2s 1. c. 4s 2. d. 4s Among the following groups of atoms, which have the same number of valence electrons? a. H, He c. Mg, Al, Ca, Ga b. Li, Be, N, Ne d. N, P, As, Bi 45. How many unpaired electrons are there in a phosphorus atom? a. one b. two c. three d. four e. five 46. How many unpaired electrons are there in a chlorine atom? a. one b. two c. three d. four e. five 47. The electrical charges in an atom are located a. only in the nucleus. c. on protons and electrons. b. on protons and neutrons. d. on protons, neutrons, and electrons. 48. An electron orbital is a region of space around the nucleus of an atom where there is a probability of finding an electron with a particular energy. a. 99% b. 66% c. 60% d. 90% e. 100% 49. Which of the following is not a metalloid (or semimetal)?

6 6 c E = h a. aluminium b. germanium c. arsenic d. antimony e. tellurium Refer to the above graph for the following three questions. 50. What family of elements collectively has the highest first ionization energies? a. the alkali metals c. the halogens b. the alkaline-earth metals d. the noble gases 51. What family of elements collectively has the lowest first ionization energies? a. the alkali metals c. the halogens b. the alkaline-earth metals d. the noble gases 52. The general trend for first ionization energy on the periodic table is a. increasing from left to right across a period and down a group. b. increasing from right to left across a period and down a group. c. decreasing from left to right across a period and down a group. d. decreasing from right to left across a period and down a group. 53. For which of following period-five elements would you expect the largest jump between the first and second ionization energies? a. rubidium b. strontium c. antimony d. tellurium e. iodine 54. Which of the following accounts for the general periodic trend of decreasing atomic radii across a period, despite the fact that the number of subatomic particles is increasing? a. Shielding is constant. d. both a and b b. Nuclear charge is increasing. e. both b and c c. Electronegativity is decreasing.

7 7 c E = h Refer to the table and graph below to answer the six questions that follow: H Li Na K Rb Cs Be Mg Ca Sr Ba B Al Ga In Tl C Si Ge Sn Pb N P As Sb Bi O S Se Te Po F Cl Br I At Key: H = symbol; 37 = atomic radius (pm); 1312 = 1 st ionization energy (kj/mol); 2.1 = electronegativity Which graph (line) represents the general periodic trend seen in atomic radii? a. 1 b. 2 c What element is represented by the peak labelled 3? a. lithium b. fluorine c. neon d. cesium e. astatine 57. What element is represented by the peak labelled 2? a. iodine b. tellurium c. bromine d. cesium e. xenon

8 8 c E = h 58. Which element has the highest electronegativity? a. lithium b. cesium c. helium d. fluorine e. astatine 59. Which of the following are parallel, or similar, trends? a. electronegativity and atomic radius d. atomic radius and 1 st ionization energy b. 1 st ionization energy and electronegativity e. All three trends are parallel. c. None of these trends are similar. 60. Which of the following are opposite trends? a. electronegativity and atomic radius d. both a and c b. 1 st ionization energy and electronegativity e. both a and d c. atomic radius and 1 st ionization energy 61. Which of the following mini activity series correctly lists the metals in order of most reactive to least reactive (as should have been done in the lab exercise)? a. Sn, Mg, Zn, Cu, Ag d. Ag, Cu, Sn, Zn, Mg b. Mg, Zn, Cu, Sn, Ag e. Mg, Zn, Sn, Cu, Ag c. Zn, Mg, Sn, Cu, Ag 62. Which of the following series of elements correctly lists the metals in order of least dense to most dense? a. C, Si, Ge, Sn, Pb d. C, Sn, Ge, Si, Pb b. C, Si, Sn, Ge, Pb e. Si, C, Ge, Sn, Pb c. Pb, Sn, Ge, Si, C 63. Which of the following figures is the most accurate visual representation of the quantum mechanical model of a lithium atom? e. a. b. c d. 64. Which of the above figures a., b., c., d., or e. is perhaps the view that enlightened people living in Dalton s time (19 th Century) had of the atom, based on his theory? 65. Which of the following groups would in general be the most reactive of the four? a. alkali metals c. alkaline-earth metals b. transition metals d. nobel gases 66. Which of the following would form the most reactive ions (should they form)? a. alkali metals c. alkaline-earth metals b. transition metals d. nobel gases 67. Would you expect (a) arsenic or (b) sulfur to have the higher first ionization energy of the two?

9 9 c E = h For the following statements, indicate whether (a) Dalton, (b) Thomson, (c) Millikan, (d) Rutherford, or (e) Bohr was responsible. 68. Atoms have a positively charged core called a nucleus. 69. A given compound always has the same relative numbers and kinds of atoms. 70. Negative charges are distributed evenly throughout the atom s positively charged interior, much the same way that fruits (and who knows what else) are distributed throughout the English desert known as plum pudding (a view of the atom now known to be incorrect). 71. The mass of an electron is 9.11 x gram. 72. Atoms of one element are never changed into atoms of another element as a result of any [chemical] reaction. 73. Atoms are mostly empty space. 74. Electrons occupy specific energy levels around the nucleus of an atom. For the following, indicate whether the statement is (a) always true, (b) sometimes true, or (c) never true. 75. All elements on the periodic table are represented in their neutral state. 76. A proton and an electron are of equal mass, whereas the mass of a neutron is negligible hence the symbol, n o : n to the zero power. 77. Atoms of the same element are identical yet differ from those of every other element. 78. The atomic number of an element determines that element s identity. 79. Atoms are the smallest particles of an element that retain the identity of the element in question. 80. Shielding is constant across a period on the periodic table. 81. Hydrogen is an alkali metal. 82. Increasing density within a family of elements on the periodic table is a periodic chemical property. 83. The strong nuclear force dominates the electrostatic repulsion of protons thereby allowing protons to concentrate in the nucleus of an atom. 84. The most reactive ions are those formed from elements found in groups on the far left and far right of the periodic table barring the noble gases. 85. Many nonmetals are gases at room temperature. 86. Transition metals have two valence electrons, those of the s sublevel preceding them on the periodic table.

10 10 c E = h Match each numbered item with a letter to the left that best corresponds. Letters may be used more than once. 87. calcium 88. lead 89. antimony 90. beryllium 91. arsenic a. alkaline-earth metal b. halogen c. transition metal d. metalloid (semimetal) e. carbon family 92. bromine 93. boron 94. barium Match each numbered item with a letter to the left that best corresponds. Letters may be used more than once. 95. orbitals begin to fill in the third principal energy level 96. cesium 97. aluminum 98. orbitals begin filling in the second principal energy level 99. mercury a. s-block b. p-block c. d-block d. f-block 100. orbitals begin filling in the fourth principal energy level