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9. Bohr’s model said that electrons move in circular orbits around the nucleus. Each circular orbit represents an excited state farther from the nucleus. 10. The fact that light could act both as a wave and as a particle led de Brogue and Schrodinger to suggest that an electron might also exhibit characteristics of both waves and particles. When Schrodinger used these ideas to analyze the problem mathematically, the wave mechanical model of the atom was the result.
11. a. The probability of finding an electron within an orbital is 90%, but some locations within the orbital shape are more likely to contain an electron at any given time than are others. So this statement is false.
b. The electron does tend to spend most of its time around the nucleus. This statement is true. c. Bohr thought that electrons traveled in circular orbits around the nucleus, but the current model says that electrons are found in orbitals. We do not know their exact paths. This statement is false.
12.
a. The orbital shape represents a probability cloud. It is true that an electron will be found within the orbital 90% of the time. b. The orbital marks the area of 90% probability. It does not mark the surface on which the electron travels. This statement is false. c. Ten percent of the time, an electron will be found outside the orbital. This statement is false.
13. a. The third principal energy level, n=3, contains three sublevels. b. There are five orbitals in the 3d sublevel.
c. i and ii represents orbitals; iii is ap orbital. 14. Each principal energy level has n sublevels, so the fifth principal energy level, n=5, would have five sublevels. 15. 4 is the principal energy level,p is the sublevel type, x is the specific orbital within thep sublevel, and the superscript 1 says that there is one electron in the orbital. 16. Each orbital can hold two electrons. 17. The period or row number indicates which s andp orbitals are being filled for elements in that row. For example, antimony, which is in row five, has filled its 5s orbitals and 4d orbitals and is filling 5p orbitals. 18. a. ls2s 22p 3s3p
Is 2s 35 3p
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b. Aluminum has three valence electrons and ten core electrons.
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c. Calcium would have a lower ionization energy than bromine. d. Rubidium would have a lower ionization energy than lithium. e. Radon would have a lower ionization energy than neon. f. Strontium would have a lower ionization energy than bromine. 26.
a. Neon would have a smaller atomic size than xenon. b. Iodine would have a smaller atomic size than indium. c. Sodium would have a smaller atomic size than cesium. d. Fluorine would have a smaller atomic size than strontium. e. Bismuth would have a smaller atomic size than barium.
f. Chlorine would have a smaller atomic size than aluminum.
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