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Honors Chemistry Name_________________________________ Atomic Structure Period__________ Date_______________ ________________________________________________________________________________________________ Study Guide 9.1 Atomic Orbitals Lesson Objectives Find the wavelength, frequency, speed, and energy of a given EM radiation. Explain through emission spectra that electronic energy levels are quantized. Calculate the difference of energy between two levels given the wavelength or frequency of light emitted. Recognize the basic shapes of s, p and d orbitals. Describe atomic orbitals in a multielectron atom in terms of their relative energies and degeneracy. Reading Guide Read Sections 3-3 (p. 90-99). Handout (p. 277-282, 290-291, 327-331, and 339-340) 1.Define wavelength, frequency, amplitude, and node. (H.O. p. 278-282) 2. What is the relationship between wavelength, frequency, and speed of a wave? (Write a mathematical equation.) What is the speed of light (H.O. p. 282) 3. Arrange the following in increasing energy: gamma rays, infrared radiation, microwaves, radio waves, ultraviolet radiation, visible light, x-rays (p. 92)(H.O. p. 283) 4. What is the relationship between energy, wavelength, and frequency of light? (Write a mathematical equation.) (H.O. p. 281, 339340) 5. Why is it that the light emitted from hydrogen shows discrete lines rather a continuous spectrum?(p. 94) 6. What dos the principal quantum number tells us? What are the possible values for the principle quantum number n? What is an electron shell? (p. 95) (H.O. p. 290-291) 7. What is a subshell/sublevel? How many orbitals in an s-subshell? p-subshell? dsubshell? (H.O. p. 297-298, 330-331) 8. What is the shape of an s-orbital? p-orbital? (p. 96) Additional Practice Handout Study Questions: p. 337 #13 & #14, p. 340 #17, and p. 347 #40 9.2 Concentration Lesson Objectives Write the electron configuration of a neutral atom in long form and short form. Write the electron configuration of an ion in long and short form. Relate the position of an atom on the periodic table and its predicted electron configuration. Identify the number of valence electrons in a given atom or ion. Explain the similarities in chemical in chemical properties, and common monatomic ions formed using their electron configurations. Reading Guide Read Sections 3-3, 4-1, 4-3, and 5-1 (p. 90-99, 119, 133-134, and 160-161) Handout p. 295-297, 330-331, and 358362. 1. State the exclusion principle and explain what it means. (p. 96) (H.O. p. 295) 2. Define ionization energy? (p. 133-134) 3. List the order in which electrons are filled. (p. 97-98) (H.O. p. 297-298) 1s, 2s, 2p, 3s... 4. In an electron configuration, explain what is meant when it is written: 1s2.(p. 97-98) (H.O. p. 331) 5.Identify the s-block, p-block, d=block, and f-block on the periodic table. (p. 119 figure 3) (H.O. p. 358 figure 13.4) 6. Define core electrons and valence electrons. (p. 119, 160-161) Additional Practice Handout Study questions: p. 302 #3 and #5 from the problem section, p. 303 #7, and p. 332 #8 & #9. 9.3 Periodic Trends Lesson Objectives Describe and explain the trend of effective nuclear charge between elements across a period and of shielding by core electrons down a family. Describe and explain the trends of atomic radius, ionization energy and electro negativity across a period and down a family in the periodic table. Compare atomic radius, ionization energy, and electro negativity between two atoms across a period and down a family in the periodic table. Explain the increasing successive ionization energies of an atom. Determine the number of valence electrons in an unknown element given the successive ionization energies. Reading Guide Read Sections 4-3 (p. 133-139) Handout (p. 360-363) 1. How is the atomic radius – the covalent radius- measured? (p. 135-136 figure 20) (H.O. p. 360 figure 13.5) 2. In general, what patterns are observed in the atomic radii going down a family and across a period in the Periodic Table? (p. 135-136 figure 20) (H.O. p. 360 figure 13.5) 3. What is ionization energy? (p. 133) 4. In general, what patterns are observed in ionization energy going down a family and across a period in the Periodic Table? (p. 133-134 figure 18) (H.O. p. 363) 5. How does the size of a cation compare to that of its neutral atom? Size of anion to that of its neutral atom? (p. 139) (H.O. p. 13.5)