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| Understanding the concepts
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Check your answers |
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| 1.a.
| One of the ways in which energy travels through space is by electromagnetic radiation. List some various types of electromagnetic radiation. Check your answer by referencing Figure 10.4 in the text.
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| b.
| Three ways to characterize electromagnetic radiation are wavelength, frequency, and velocity. What are wavelength and frequency? View the Electromagnetic Wave Visualization on the CD. Are wavelength and frequency related?
View the Refraction of White Light Visualization on the CD to see the visible region of electromagnetic radiation. Does red light have a longer or shorter wavelength than violet light? Which color of light travels at the faster velocity? Review Figure 10.4 in the text to help answer these questions.
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| c.
| Another quantity associated with any wavelength of electromagnetic radiation is energy. How does electromagnetic radiation apparently transfer energy?
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| 2.a.
| View the H2 Line Spectrum Visualization on the CD. It is important to understand why only specific colors of light are emitted in the H2 line spectrum. Read the concept and narration in the animation; if you need more help understanding this concept, review Section 10.4 of the text. |
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| b.
| Each element has its own unique allowed energy levels for the electrons, thus each substance emits visible light of different wavelengths. Open and view the Flame Test and Pickle Light Visualizations on the CD to reinforce this idea.
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| 3.a.
| From our current model of the atom, the allowed energy levels for the electrons are designated with the letters s, p, d, and f. Each letter designation has a certain shape associated with it. The shape of an orbital represents with 90% probability where the electron can be located. Why can't one be 100% sure where the electron is? Describe the shapes and orientations of the s and p orbitals. Check yourself by viewing the CD Visualizations on the various s and p orbitals. |
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| b.
| How many different 3d orbitals are there? How many electrons can occupy the 3d orbitals? To review the shapes and orientations of the d orbitals, see Figure 10.28 in the text. How many different 4f orbitals are there? How many electrons can occupy the 4f orbitals? What is the difference between a 3s and a 4s orbital or between a 2px and a 3px orbital? |
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| 4.a.
| What are electron configurations? The best way to determine electron configurations for the various elements is to use the periodic table. A key to this process is breaking down the periodic table into four blocks of elements where each block represents a different sublevel being filled. What are the four blocks of elements and which sublevel does each block represent? Check yourself by reviewing Figure 10.31 in the text. |
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| b.
| The only way to excel at writing electron configuration is to practice. For some practice with electron configurations, do Problems 10.56, 10.60, 10.62, and 10.64 in the text. |
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| 5.a.
| Many properties of atoms can be predicted from the periodic table. What are valence electrons? What is the relationship between valence electrons and a group in the periodic table? How are valence electron configurations related to the chemical properties of a group? |
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| b.
| Define ionization energy. What is the periodic trend in ionization energy? |
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| c.
| What is the general periodic trend with atomic size? The trend is the exact opposite of the ionization energy trend. Does this make sense? Explain. |
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| 6.
| Open Key Words on the CD and test your ability to define the important terms presented in Chapter 10. |
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| 7.
| Test your understanding of Chapter 10 by taking the ACE quizzes on the Web site |
