4. Does a higher principal energy level (n) mean that the electron is closer to or farther away from the nucleus?
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1 Name: Period: Unit 4 Homework Chemistry 1 The Wave Mechanical Model of the Atom 1. Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom). 2. Explain why we cannot exactly specify the location of an electron in an atom but can discuss only where an electron is most likely to be at any given time. The Hydrogen Orbitals 3. Why are the orbitals of the hydrogen atom described as "probability maps"? Why are the edges of the hydrogen orbitals sometimes drawn to appear "fuzzy? 4. Does a higher principal energy level (n) mean that the electron is closer to or farther away from the nucleus? 5. If an electron moves from the 1s orbital to the 2s orbital, its energy increases or decreases. Explain which. The Wave Mechanical Model: Further Development 1
2 6. What is the Pauli exclusion principle? How many electrons can occupy an orbital, according to this principle? Why? 7. Which of the following orbital designations is (are) not correct? a. 2p c. 3f b. 1d d. 4s Electron Arrangements Orbitals per energy level Shell n Orbitals 1 n = 1 1s 2 n = 2 2s 2p x, 2p y, 2p z 3 n = 3 3s 3p x, 3p y, 3p z 3d, 3d, 3d, 3d, 3d 4 n = 4 4s 4p x, 4p y, 4p z 4d, 4d, 4d, 4d, 4d 4f, 4f, 4f, 4f, 4f, 4f, 4f Orbitals Being Filled for Elements in the Periodic Table 2
3 8. Which orbital is the first to be filled in any atom? Why? 9. Write the full electron configuration (1s 2 2s 2, etc.) for each of the following elements. a. helium, Z = 2 b. potassium, Z = 19 c. fluorine, Z = Write the full electron configuration (1s 2 2s 2, etc.) for each of the following elements. a. calcium, Z = 20 b. zinc, Z = 30 c. strontium, Z = Using the symbol of the previous noble gas to indicate the core electrons, write the valence-electron configuration for each of the following elements. a. francium, Z = 87 b. yttrium, Z = 39 c. cerium, Z = Which electrons of an atom are the valence electrons? Why are these electrons especially important? 13. Circle the valence electrons in the electron configurations written for the elements in question 11. 3
4 14. How are the electron arrangements in a given group (vertical column) of the periodic table related? 15. How many 4d electrons are found in each of the following elements? a. yttrium, Z = 39 b. zirconium, Z = 40 c. strontium, Z = 38 d. cadmium, Z = Write the complete orbital diagram for each of the following elements, using boxes or lines to represent orbitals and arrows to represent electrons. You may use the noble gas notation. a. aluminum, Z = 13 b. phosphorus, Z = 15 c. bromine, Z = 35 d. argon, Z = How many valence electrons does each of the following atoms possess? a. sodium, Z = 11 b. calcium, Z = 20 c. iodine, Z = 53 d. nitrogen, Z = Why do we believe that the valence electrons of calcium and potassium reside in the 4s orbital rather than in the 3d orbital? 4
5 19. Write the electron configurations for the following elements and analyze the number of paired and unpaired electrons in each atom. You may use the Noble Gas notation. a. Potassium: Number of paired electrons number of unpaired electrons b. Sulfur: Number of paired electrons number of unpaired electrons c. Vanadium: Number of paired electons number of unpaired electrons d. Iridium: Number of paired electons number of unpaired electrons e. Mercury: Number of paired electrons number of unpaired electrons 5
6 6
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