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Diff Chemistry Name______________ Answer questions 1-25 from studying the graphs. Atomic Radius vs Atomic Number Atomic Radius 250 200 150 Series1 100 50 0 1 5 9 13 17 21 25 29 33 Atomic Number The above graph is a plot of the relative atomic radius and relative ionization energy as a function of the atomic number. Relative means that adjustments were made so that both plots fit on the same graph and are both clearly visible. 1. How does the relative A.R. and I.E. for Li (within the Li to Ne period) compare with one another? 2. How does the relative A.R. and I.E. for Ne (within the Li to Ne period) compare with one another? 3. What happens to the I.E. for the second half of the transition metals? What might be an explanation for this observation? 4. Label Be, Mg, and Ca. Why do these elements have a higher I.E. than the elements B, Al, and Ga? 5. How does the size of the atom and I.E. change moving down a column? Explain why? 6. How does the size of the atom and I.E. change moving left to right across a period? Explain why? 7. How does the size of that atom and subsequent I.E. affect the chemical properties of atoms? Ionization Energy vs Atomic Number Ionization Energy 2500 2000 1500 Se rie s1 1000 500 0 1 4 7 10 13 16 19 22 25 28 31 34 Atomic Number Label the elements He, Ne, Ar, and Kr. These elements belong to the same group, namely, the noble gases. 8. What is the trend concerning ionization energy (IE) going down a column or group of the periodic table? 9. Label elements Li, Na, and K on the chart. 10. What is the trend moving from Li to Ne, Na to Ar, and K to Kr moving from left to right on the periodic table. 11. Circle the transition elements 20-30. If these elements were cut out would the pattern from K to Ar be more like the pattern from Li to Ne and Na to Ar. Explain why. 12. Label Zn on the graph. The elements in the column headed by zinc are sometimes called the pseudonoble gases. Why do you think this name is an apt description? 13. What might produce a spike in IE for Zn? 14. Generally the atoms of metals are (larger or smaller) in size and have (lower or higher) first ionization energies. What do you think? Metals are more likely to (lose or gain) electrons to form (cations or anions). 15. Where on the periodic table are the largest atoms? 16. Where on the periodic table are the atoms with the lowest ionization energy? 17. Where on the periodic table are the atoms most likely to lose electrons to other atoms? 18. In general what is the relationship between atomic radius (size of the atom) and first ionization energy? Comparison Chart of I.E. and A.R. Relative I.E. and A.R. 1.6000 1.4000 1.2000 1.0000 Series1 0.8000 Series2 0.6000 0.4000 0.2000 0.0000 1 5 9 13 17 21 25 29 33 Atomic Number The above graph is a plot of the relative atomic radius and relative ionization energy as a function of the atomic number. Relative means that adjustments were made so that both plots fit on the same graph and are both clearly visible. 19. How does the relative atomic radius and ionization energy for Li (within the Li to Ne period) compare with one another? 20. How does the relative atomic radius and ionization energy for Ne (within the Li to Ne period) compare with one another? 21. What happens to the I.E. for the second half of the transition metals compared to the first half? What might be an explanation for this observation? 22. Label Be, Mg, and Ca. Why do these elements have a higher I.E. than the elements B, Al, and Ga? 23. How does the size of the atom and I.E. change moving down a column? Explain why? 24. How does the size of the atom and I.E. change moving left to right across a period? Explain why? 25. How does the size of that atom and subsequent I.E. affect the chemical properties of atoms?