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Transcript
Chemistry
Unit 5 – Electronic Structure and Periodicity
Mini-Lab
Name: _____________________________
Date: _________________
Period: ________________
Periodicity
Objective: Find out how ionization energy changes down a group and across a period on the periodic
table.
Materials: textbook pp. 855-857, Appendix A (Properties of Elements), graphing paper, pencil, ruler
Procedure:
1. Using data from Appendix A of your textbook, create a line graph of atomic number vs. ionization
energy. Plot the ionization energy (y-axis) of the first 54 elements against their atomic number (x-axis).
2. Label each point on the graph with the symbol of the element.
Analysis and Conclusion
1. Describe the general shape of the graph.
2. Name all elements that correspond to the highest points on the graph. Where are these elements located
on the periodic table?
3. Which elements correspond to the lowest points on the graph? Where are these elements located on the
periodic table?
4. Look at the points corresponding to Li, Be, B, C, N, O and Ne. These elements belong to the same
period. How does ionization energy change from left to right of a period?
5. Look at the points corresponding to Li, Na, K and Rb These elements belong to the same group. How
does ionization energy change from top to bottom of a group?
6 Draw an outline of the periodic table and using arrows show how ionization energy changes from left to
right and from top to bottom of the periodic table.
Atomic Size and Ionization Energy
7. Alkali metals are among the biggest atoms within their respective periods. They also have lowest
ionization energies. Explain why, in general, big atoms have low ionization energies.