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1st EditionButhelezi, Dingrando, Hainen, WistromMatta, Staley, Waterman, Wilbraham1st EditionChristina Clancy4th EditionJohn A. Suchocki, Paul G. Hewitt Youre Reading a Free Preview Page 2 is not shown in this preview. 05_Chem_GRSW_Ch05.SETE 61104 3:30 PM Page 43Name ____________________________________ Date __________ Class ___________________5 ELECTRONS IN ATOMSSECTION 5.1 MODELS OF THE ATOM (pages 127–132)This section summarizes the development of atomic theory. It also explainsthe significance of quantized energies of electrons as they relate to the quan–tum mechanical model of the atom. The Development of Atomic Models (pages 127–128) 1. Complete the table about atomic models and the scientists who developed them.Scientist Model of AtomDalton The atom is a solid indivible mass.ThomsonRutherford The atom is a ball of positive charge with electrons stuck into the ball.Bohr Most of an atoms mass is concentrated in the small, positively charged nucleus.The electrons surround the nucleus and the rest of the atom is empty space. Electrons are arranged in concentric circular paths around the nucleus.2. Is the following sentence true or false? The electrons in an atom can exist between energy levels. _____________fa__ls_e______The Bohr Model (pages 128–129)3. What is a small, discrete unit of energy called? It is called a quantum.4. Circle the letter of the term that completes the sentence correctly. A quantum of energy is the amount of energy required to a. move an electron from its present energy level to the next lower one b. maintain an electron in its present energy level c. move an electron from its present energy level to the next higher one5. In general, the higher the electron is on the energy ladder, the ________f_a_r_th_e_r_________ it is from the nucleus. Chapter 5 Electrons in Atoms 4305_Chem_GRSW_Ch05.SETE 61104 3:30 PM Page Class __________________44 Date ___________________ Name ___________________________CHAPTER 5, Electrons in Atoms (continued) The Quantum Mechanical Model (page 130) 6. What is the difference between the previous models of the atom and the modern quantum mechanical model? ______P__re_v_i_o_u_s__m__o_d_e_ls__d_e_s_c__ri_b_e_d__th_e__m__o_t_io_n__o_f_e_l_e_c_t_ro_ns the same way as the motion of large objects.The quantum mechanical model is not based on the exact path an electron follows around the nucleus.7. Is the following sentence true or false? The quantum mechanical model of the atom estimates the probability of finding an electron in a certain position. ___________t_ru__e________Atomic Orbitals (pages 131–132)8. Circle the letter of the term that correctly answers this question. Which name describes the major energy levels of electrons?a. atomic orbitals b. quantum mechanical numbersc. quantas d. principal quantum numbers (n) 9. Principal energy levels are assigned values in order of ________g_e_n_e_r_a_ll_y_i_n_c_r_e_a_sing energy: n 1, 2, 3, 4, and so forth.10. In the quantum mechanical model the regions where electrons are likely to be found are called ________a_to_m__i_c_o_r_b_it_a_ls___ and are denoted by __________le_t_te__rs________ .11. Match each diagram below with the name of its p orbital, the px, py, or pz.px py pz orbitals12. Use the diagram above. Describe how the px, py, and pz orbitals are similar. The p orbitals are similar because they are all dumbbell shaped.13. Describe how the px, py, and pz orbitals are different. ________T_h_e_p__o_r_b_it_a_ls__h_a_v_e__d_if_fe__rent orientations in space.They are all perpendicular to each other.14. Circle the letter of the formula for the maximum number of electrons that can occupy a principal energy level. Use n for the principal quantum number. a. 2n2 b. n2 c. 2n d. n44 Guided Reading and Study Workbook05_Chem_GRSW_Ch05.SETE 61104 3:30 PM Page 45 Date ___________________ Class __________________ Name ___________________________SECTION 5.2 ELECTRON ARRANGEMENT IN ATOMS (pages 133–136)This section shows you how to apply the aufbau principle, the Pauli exclusionprinciple, and Hunds rule to help you write the electron configurations ofelements. It also explains why the electron configurations for some elementsdiffer from those assigned using the aufbau principle.Electron Configurations (pages 133–135)1. The ways in which electrons are arranged around the nuclei of atoms are called _____________e__le_c_t_r_o_n__c_o_n_f_ig__u_r_a_ti_o_n_s_________ .Match the name of the rule used to find the electron configurations of atoms withthe rule itself.____b___ 2. aufbau principle a. When electrons occupy orbitals of equal energy, one electron enters each____c___ 3. Pauli exclusion orbital until all the orbitals contain principle one electron with parallel spins.____a___ 4. Hunds rule b. Electrons enter orbitals of lowest energy first. c. An atomic orbital may describe at most two electrons.5. Look at the aufbau diagram, Figure 5.7 on page 133. Which atomic orbital is of higher energy, a 4f or a 5p orbital? _______4f6. Fill in the electron configurations for the elements given in the table. Use the orbital filling diagrams to complete the table.Electron Configurations for Some Selected ElementsElement 1 Orbital filling Electron 22 2 2 3 configurationH 11He 1s 2Li 1 221C 1s22s22p 2N 1 22 223O 1s22s22p 4 F 1 22 225Ne 1s22s22p 6Na 1 22 22 631 Chapter 5 Electrons in Atoms 45
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