Download Periodic Trends Review Sheet

Name
Period
Periodic Trends
ATOMIC RADIUS
1. What trend in atomic radius do you see as you go down a group/family on the periodic table?
2. What causes this trend?
3. What trend in atomic radius do you see as you go across a period/row on the periodic table?
4. What causes this trend?
5. Explain how shielding contributes to the atomic radius trend within a group.
6. Circle the atom in each pair that has the largest atomic radius.
a) Al
B
b) S
O
c) Br
d) Na Al
e) O
F
f) Mg
Cl
Ca
7. Put the following elements in order from smallest to largest atomic radius and explain why:
C, O, Sn, Sr.
IONIZATION ENERGY
8. Define ionization energy.
9. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? Why?
10. Na+ and Mg2+ ions each have ten electrons surrounding their nuclei. Which ion would you expect to have the larger radius? Explain your answer.
11. a. Explain why it is harder to remove an inner shell electron than a valence electron from an atom.
b. Explain why sodium forms a 1+ ion (Na+) but magnesium forms a 2+ ion (Mg2+).
12. What trend in ionization energy do you see as you go down a group/family on the periodic table?
13. Put the following elements in order from lowest to highest first ionization energy and explain why: Al, Ar, Cs, Na.
14. Why do magnesium, phosphorus, and zinc exhibit slightly higher first ionization energies than the general trend within each of their periods?
15. Which element in the third period is best represented by the six successive ionization energies listed below? Explain your reasoning.
1st IE
577
ELECTRONEGATIVITY
16. Define electronegativity
2nd IE
1,815
3rd IE
2,740
4th IE
11,600
5th IE
15,000
6th IE
18,310
17. How does the ionic radius of a nonmetal compare with its atomic radius?
18. What trend in electronegativity do you see as you go down a group/family on the periodic table?
19. What causes this trend?
20. What trend in electronegativity do you see as you go across a period/row on the periodic table?
21. What causes this trend?
22. Circle the atom in each pair that has the greater electronegativity.
a) Ca
Ga
b) Li
O
c) Cl
S
d) Br
As
e) Ba
Sr
f) O
S
General Questions
23. Which of the following elements most likely has the highest melting point: I, Mo, Te? Explain why.
24. Which group tends to form +1 ions? ________________________________________________
25. Which group tends to form +2 ions? ________________________________________________
26. Which group tends to form -1 ions? _________________________________________________
27. Which group tends not to form ions or react? __________________________________________
28. Based on the concept of periodic trends, answer the following questions for these atoms: Li, Be, Mg, Na. Be able to defend your answers.
a.
Which element has the highest first ionization energy? ____________________________
b.
Which element has the lowest electronegativity? _________________________________
c.
Which element has the least metallic character? _________________________________
d.
Which element is the largest atom? ___________________________________________
29. Based on the concept of periodic trends, answer the following questions for these atoms: P, S, Cl, F. Be prepared to defend your answers.
a.
Which element has the highest first ionization energy? ____________________________
b.
Which element has the highest electronegativity? ________________________________
c.
Which element has the least metallic character? _________________________________
d.
Which element has the largest ion? ___________________________________________
30. Based on the concept of periodic trends, answer the following questions for these atoms: Au, Zn, S, Si. Be able to defend your answers.
a.
Which element has the highest first ionization energy? ____________________________
b.
Which element has the highest electronegativity? ________________________________
c.
Which element has the most metallic character? _________________________________
d.
Which element has the largest atom? ________________________________________