12.1 Ionization Energy Pair Activity

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12.1 Ionization Energy Pair Activity Powered By Docstoc
					Ionization Energy Teamwork - Work in Pairs
Group Members: (Type your names here)
(Save in Ms. Smith’s Inbox in the designated class period. Save as Chpt 2_IETW_Last, Names.doc)
I would save a copy for yourself as well.

1. Define Molar Ionization Energy.
2. Think about the way a mass spectrometer operates. Describe the basic steps involved and then
   discuss how you might you might modify that apparatus to measure the ionization energy of an
3. Wiki has a table of molar ionization energies for the elements. The 1st through 10th columns refer to
   the 1st electron removed, the 2nd electron removed… You task is to use Excel to construct a scatter
   plot with Z=1-20 on the X axis and FIRST molar ionization energy on the Y. DO NOT do a line of best
   fit. Have Excel connect the dots instead and today we are going to look at the inconsistencies in the
   larger trends. Paste your graph below this question.
4. The theory is that it should be easier to remove an electron from a higher energy level because it is
   further from the positive charge of the nucleus and the lower energy levels provide some shielding.
   This explains the first big drop that you see in your graph from Z=2 to Z=3 (He to Li). Why is He (Z=2)
   higher than H (Z=1)?
5. Your answer from question 4 also explains the increase that we see in the second energy level from
   Z=3 (Li) to Z=10 (Ne). What does this graph tell you about the electron capacity of the first energy
   level (Z=1 to Z=2) compared to the second level (Z=3 to Z=8)?
6. Now think about electron configurations and come up with an explanation for why it takes more
   energy to ionize Be (Z=4) than it does B (Z=5).
7. Take a look at the 2p sublevel (Z=5 to Z=10). Think about the component x, y, and z orbitals. What
   does this graph tell you about how the electrons fill in the orbitals of a p sublevel? Does the data for
   the 3p confirm that theory?

8. Compare the terms first ionization energy and successive ionization energies.
9. Use the same wiki data table to create another graph. The X axis should be the successive ionization
    energies for all 19 of potassium’s electrons and the Y should be the log of the molar ionization
    energy). We use the log function because as more electrons are removed, the pull of the protons
    holds the remaining electrons more tightly. So much so that we must use a logarithmic scale to
    make sense (graphically) of the data. Paste your graph below this question.
10. Give the energy level and sublevel of the first 3 electrons being removed from potassium.
11. Use the graph to explain how it gives evidence for the number of electrons in each energy level.
12. Does your graph give evidence for sub-levels?
13. You can tell how many valence electrons an element has by looking for the first big jump in
    successive ionization energies. Describe two ways the graph for aluminum would differ from the
    one you made for potassium.

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