Chemistry – Unit 10 Atomic Data Study
Part 1: Ionization Energy Analysis
Complete the following in your lab notebook. Use complete thoughts and
explanations!!!
Right Side Items:
Chemistry – Unit 10 Atomic Data Study
Part 2: Periodic Trends Analysis
Complete the following in your lab notebook. Use complete thoughts and
explanations!!!
Right Side Items:
Trends in 1st Ionization Energy:
1. Discuss and define Ionization Energy:
1. What is meant by “1st ionization energy”?
2. Using the IE and radii Excel file, plot graphs of successive ionization
energies for boron (B), silicon (Si), and calcium (Ca).
2. Using the data in the table of ionization energies, plot the first ionization
energy (IE1) vs. the atomic number (Z) for the first 20 elements.
Compare the graphs – what are the common features? What are the
differences?
Explain; draw sketches if necessary.
3. Group the electrons for each element based on ionization energies. How
many electrons are in each group? Discuss and justify your groupings!
(Hint: to better differentiate between groups, you can change the
scale of the vertical axis by double clicking the axis and selecting
the “scale” tab.)
Left Side Items:
Examine the graph of 1st ionization energy vs atomic number. Can a
periodic trend be observed? If so, describe the trend.
3. Which group (or chemical family) has the highest ionization energies?
Which group has the lowest?
Trends in atomic radius:
4. What is meant by “atomic radius”?
5. Using the data in the table on the 2nd sheet in the workbook, plot the
atomic radius (in nm) vs. the atomic number.
Examine the graph of atomic radius vs atomic number. Can a periodic
trend be observed? If so, describe the trend.
4. Is there a maximum number of electrons that can fit in each group? If
so, what is it? Explain/justify your response.
6. For a given period (a row in the Periodic Table), which group (a column
in the table) appears to have the largest atomic radii? Which group has
the smallest?
5. Plot graphs of successive ionization energies for a few more atoms.
Does the evidence support your answer to #4? Explain.
Left Side Item:
Concluding thought:
6. Write a paragraph summarizing the patterns you found in the table of
successive ionization energies.
7. What appears to be the relationship between trends in IE and atomic
radii? Discuss and Explain!!!
Chemistry – Unit 10 Atomic Data Study
Part 3: Atomic Model Extension
Right Side: Complete a Bohr Model representation of the indicated atoms:
Boron (B):
Nitrogen (N):
Fluorine (F):
Sodium (Na):
Left Side Item: Now lets discuss how we can model atoms without
committing to the invented idea of an orbit.
1. Draw energy well diagrams for B, N, F and Na.
2. Use these diagrams to explain the trend in 1st ionization energy as you
move across a period. Explain why IE1 for sodium is so much lower
than it is for fluorine.
3. Now, use these diagrams to explain the trend in atomic radii as you
move across a period. Explain why fluorine is smaller than oxygen, yet
sodium is not smaller yet than fluorine.