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3.03 Chemistry Assignment By Matthew H.

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Matthew Hunnefield

on 18 October 2012

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Transcript of 3.03 Chemistry Assignment By Matthew H.

Part I: Atomic Radius Trend Going Across the Periodic Table 3.03 Chemistry Assignment
By Matthew H. Part II: Atomic Radius Trend Going
Down a Group Part III: Analysis and Conclusion
(10 points total)
After completing both graphs, answer the questions below in complete sentences. Both the question and your answer should be included in the document (along with the two graphs) that you submit to your instructor.
1. Refer to the graph that you created in Part I of this assignment. Describe the general trend or patterns that you observed in the atomic radius as you go across the periodic table. (2 points)
It looks like the atomic radius is bigger if the atomic number is small. This may be because of the decrease of the pull that the protons give the electrons the smaller the atomic number.

2. In Part II of this assignment, you graphed the atomic radius of some elements from group 14 on the periodic table. What is the general trend for atomic radius going down that group? (2 points)
It looks like the atomic radius is bigger when the atomic number in the same collumn is bigger. This is probably because of the electrons in the inner shells. They give more shielding for the outer electrons so that they could spread out more.

3. What element in Period 5 of the periodic table is a member of Group 14? (1 point)
It appears that tin is both in period five and group 14.

4. The word interpolate means to use a given line graph to find unknown points between the plotted points of the graph. Use your line graph from Part II to interpolate, or estimate, atomic radius of Tin (Sn). (1 point)
After looking at the graph, I think tin may have a radius of about 150. 5. Tin’s actual atomic radius is 140 pm. Use the math equation below to determine the percent error of your estimated value. (2 points)
After doing the math, it appears that I was a little over 7% in error.

6. The atomic radius you estimated from your graph is most likely not exactly the same as the true atomic radius of tin. There is a small percent error. What do you think caused this error? (2 points)
I think what caused the error was the difference in the big line that I drew from 4 to 6 and the different properties of the atom. Due to the different electron shells in an atom, the electron cloud always varies. Sometimes it varies greatly, and sometimes it barely changes.
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