Chemistry Chapter 9 Review. 2. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x s -1.

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1 Chemistry Chapter 9 Review 1. What is the frequency of radiation that has a wavelength of 4.7 x 10-5 cm? 2. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x s The further the electron is from the nucleus, the energy the electron has. 4. A(n) is often thought of as a region of space in which there is a high probability of finding an electron. 5. What is the term used to label the energy levels of electrons? 6. How are s orbitals different from p orbitals? 7. How many electrons can each of the following orbitals hold? a. 2s = d. 6d = b. 3p = e. 4p = c. 5f = f. 3d = 8. How many p orbitals can there be in any energy level? 9. What is the maximum number of electrons in the 3 rd principle energy level? 10. How many orbitals are in each of the following sublevels?? a. 4p sublevel c. 4f sublevel b. 3d sublevel d. 2s sublevel

2 11. Using arrows, show how the following orbitals will fill with electrons. Electron Configuration Mg 1s 2 2s 2 2p 6 3s 2 Cl 1s 2 2s 2 2p 6 3s 2 3p 5 Si 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2s 2p 3s 3p 4s 3d Ti 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d Write the complete electron configuration for each atom on the blank line. a. Lithium b. Fluorine c. Carbon d. Argon e. Sulfur f. Nickel g. Rubidium h. Xeon

3 13. What elements are represented by each of the following electron configurations? a. 1s 2 2s 2 2p 5 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 4 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p a. What are valence electrons? b. Explain how an atom s valence electron configuration determines its place on the periodic table. c. List the number of valence electrons for the following atoms: potassium = magnesium = carbon = nitrogen = 15. Place the following orbitals in order of increasing energy: 1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p 16. What two elements are exceptions to the way we normally write electron configurations? Write the expected and the actual configuration of each. What rules are followed? What rules are violated? 17. Identify each element as a metal, metalloid, or nonmetal. a. fluorine d. phosphorus b. germanium e. lithium c. zinc f. oxygen

4 18. Circle the transition metals below. magnesium titanium chromium mercury aluminum Which block (s, p, d, or f) are the transition metals found? 19. Give two examples of elements for each category. a. Noble gases b. Halogens c. Alkali metals d. Alkaline earth metals 20. Explain why the s-block of the periodic table is two groups wide, the p-block is six groups wide, and the d- block is ten groups wide. 21. Why do the elements potassium and sodium have similar chemical and physical properties? 22. Identify the element that: a. Contains a full 3 rd energy level c. Outer energy level is 4s 2 b. Contains 3 electrons in the 2p level d. Contains 5 electrons in the 4d level 23. Write the electron configuration for the element fitting each of the following descriptions. a. The metal in Group 15 b. The halogen in period 3 c. The alkali metal in period 2 d. The transition metal that is liquid at room temperature

5 23. Write the complete electronic configuration (1s 2 2s 2...) and the orbital box diagram for the Cl atom. 25. Write the electronic configuration, using the abbreviated noble gas form, for the following atoms. a. Si b. Ni c. Ag d. La 26. How many unpaired electrons are there in an atom of sulfur? 27. Arrange the following elements in order of increasing size: Al, B, C, K, and Na 28. Periodic trends. Explain each answer briefly. a. Rank the following in order of increasing atomic radius: O, S, F. b. Which has the largest first ionization energy: Si, S, or Se? c. Place the following in order of increasing first ionization energy: Cs, Sr, Ba. 29. Answer the following questions about the elements with the electron configurations shown here: A = [Ar]4s 2 B = [Ar]3d 10 4s 2 4p 5 a. Is element A a metal, metalloid, or nonmetal? b. Is element B a metal, metalloid, or nonmetal? c. Which element is expected to have the larger ionization energy? d. Which element is expected to have the smaller atomic radius? 30. The configuration of an element is [Ar]3d 3 4s 2 a. What is the identity of the element? b. In what group and period in the Periodic Table is the element found? c. Is the element a nonmetal, a main group element, a transition element, a lanthanide element, or an actinide element?