Electron Configuration - DOC

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                                     Chemistry 1
Electron Configuration (pages 127-141)

   1. Define what is meant by electron configuration.



   2. What is the difference between an orbit and an electron orbital?


   3. In your own words describe the shapes of the s, p, and d orbitals.
          a. S-orbital                    b. p-orbital                        c. d-orbital



   4. What is the meaning of the term principal quantum number?


   5. How does the Aufbau Principle work? That is, what does it mean to say that orbitals are filled
      from the bottom up?



   6. What is Hund’s Rule? That is, how do you go about filling up electron orbitals according to this
      rule?


   7. Explain what is meant by the Pauli Exclusion Principle?

   8. Using the rules/principles above and the example below, diagram the electron orbitals for the following:
      a. H                                           b. Li

       c. Al                                            d. N

       e. K                                             f. Zn

       Example:
       Here is an example of the
       orbitals having been filled
       in by the rules. The
       element Sulfur has 16
       electrons and starting
       from the bottom up you
       place two (1 Up and 1
       Down) in the 1s orbital.
       Next, 2 electrons are
       placed in 2s and then one
       in each of the 2p orbitals
    until there is one in each orbital. Then the rest of the electrons are filled into the 2p orbitals.
    After that the 3s orbital is filled and then the 3p. Electrons are placed in the boxes of the 3p
    orbitals one at a time until there is one in each orbital. After that the remaining electron is placed
    as part of a pair in the first 3p box.
    The shorthand notation for the electron configuration of Sulfur is 1s2 2s2 2p6 3s2 3p4. In that
    notation 1s2 means principal quantum number 1, s-type orbital, 2 e-; 2s2 means principal
    quantum number 2, s-type orbital, 2 e-; 2p6 means principal quantum number 2, p-type orbital, 6
    e-; 3s2 means principal quantum number 3, s-type orbital, 2 e-; and, finally, 3p4 means principal
    quantum number 3, p-type orbital, 4 e-.

9. Using the rule/principles above, write the full ground state electron configurations for the following
   elements.
   a. H                                              b. Li

    c. Al                                            d. N

    e. K                                             f. Zn

10. In the following shorthand notation for the configuration of electrons, tell what each part means:
    1s2 2s2 2p6 3s2 3p6 4s2 3d5. (For example: 1s2 means that in the shell with principal quantum
    number 1 there are two electrons in an s orbital.)
        a. 2s2 ____________________________________________________________________

        b. 2p6 ____________________________________________________________________

        c. 3s2 ____________________________________________________________________

        d. 3p6 ____________________________________________________________________

        e. 4s2 ____________________________________________________________________

        f. 3d5 ____________________________________________________________________

11. Why does the 4s orbital get filled with electrons before any electrons can be placed into a 3d
    orbital?

12. Use the noble-gas notation for the following elements’ electron configuration:
    a. Cl                                           b. I

    c. Pb                                            d. Ag

    e. Ca                                            f. Au

13. What is the difference between electron-dot diagrams, and the orbital diagrams?



14. What are valence electrons?
15. Make an electron-dot diagram to show valance electrons for the following elements.

   a.     He               b.     Be              c.    C                 d.   O

16. What do we mean when we say an element belongs to the p block of the periodic table?



17. What groups (columns) in the periodic table are included in the
      a. s block?
        b. p block?
        c. d block?
        d. Where is the f-block?
18. Noble gases have very stable electron configurations. At which orbital type (s, p, d or f) does
    their electron configuration end?

19. Oxygen and sodium do not have electron configurations that are the same as the Noble gases.
   What may these atoms do that will give them a configuration like a Noble gas?

20. Fill up Worksheet attached.
21. Get ready for a quiz.
Answer Key
Electron Configuration (pages 127-141)

   22. Define what is meant by electron configuration.



   23. What is the difference between an orbit and an electron orbital?


   24. In your own words describe the shapes of the s, p, and d orbitals.
           a. S-orbital                    b. p-orbital                        c. d-orbital



   25. What is the meaning of the term principal quantum number?


   26. How does the Aufbau Principle work? That is, what does it mean to say that orbitals are filled
       from the bottom up?



   27. What is Hund’s Rule? That is, how do you go about filling up electron orbitals according to this
       rule?


   28. Explain what is meant by the Pauli Exclusion Principle?

   29. Using the rules/principles above and the example below, diagram the electron orbitals for the following:
       a. H                                           b. Li

       c. Al                                             d. N

       e. K                                              f. Zn

       Example:
       Here is an example of the
       orbitals having been filled
       in by the rules. The
       element Sulfur has 16
       electrons and starting
       from the bottom up you
       place two (1 Up and 1
       Down) in the 1s orbital.
       Next, 2 electrons are
       placed in 2s and then one
       in each of the 2p orbitals
    until there is one in each orbital. Then the rest of the electrons are filled into the 2p orbitals.
    After that the 3s orbital is filled and then the 3p. Electrons are placed in the boxes of the 3p
    orbitals one at a time until there is one in each orbital. After that the remaining electron is placed
    as part of a pair in the first 3p box.
    The shorthand notation for the electron configuration of Sulfur is 1s2 2s2 2p6 3s2 3p4. In that
    notation 1s2 means principal quantum number 1, s-type orbital, 2 e-; 2s2 means principal
    quantum number 2, s-type orbital, 2 e-; 2p6 means principal quantum number 2, p-type orbital, 6
    e-; 3s2 means principal quantum number 3, s-type orbital, 2 e-; and, finally, 3p4 means principal
    quantum number 3, p-type orbital, 4 e-.

30. Using the rule/principles above, write the full ground state electron configurations for the following
    elements.
    a. H                                              b. Li

    c. Al                                            d. N

    e. K                                             f. Zn

31. In the following shorthand notation for the configuration of electrons, tell what each part means:
    1s2 2s2 2p6 3s2 3p6 4s2 3d5. (For example: 1s2 means that in the shell with principal quantum
    number 1 there are two electrons in an s orbital.)
        a. 2s2 ____________________________________________________________________

        b. 2p6 ____________________________________________________________________

        c. 3s2 ____________________________________________________________________

        d. 3p6 ____________________________________________________________________

        e. 4s2 ____________________________________________________________________

        f. 3d5 ____________________________________________________________________

32. Why does the 4s orbital get filled with electrons before any electrons can be placed into a 3d
    orbital?

33. Use the noble-gas notation for the following elements’ electron configuration:
    b. Cl                                           b. I

    c. Pb                                            d. Ag

    e. Ca                                            f. Au

34. What is the difference between electron-dot diagrams, and the orbital diagrams?



35. What are valence electrons?
36. Make an electron-dot diagram to show valance electrons for the following elements.

   b.     He               b.     Be              c.    C                 d.   O

37. What do we mean when we say an element belongs to the p block of the periodic table?



38. What groups (columns) in the periodic table are included in the
      a. s block?
        b. p block?
        c. d block?
        d. Where is the f-block?
39. Noble gases have very stable electron configurations. At which orbital type (s, p, d or f) does
    their electron configuration end?

40. Oxygen and sodium do not have electron configurations that are the same as the Noble gases.
   What may these atoms do that will give them a configuration like a Noble gas?

41. Fill up Worksheet attached.
42. Get ready for a quiz.

				
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