Periodic Trends Problems Review
PSI Chemistry
Name_________________________________
Atomic Size
Classwork
1. Put the following elements in order of increasing atomic size:
P, Cs, Sn, F, Sr, Tl
2. Put the following elements in order of increasing atomic size:
Ca, Rb, K, O, Al, As
3. Put the following elements in order of decreasing atomic size:
Ga, Fr, Br, Si, Na, N
4. Put the following elements in order of decreasing atomic size:
Po, Sn, Fr, Rb, Cl, Li
Homework
5. Put the following elements in order of increasing atomic size:
Ra, F, Al, Ne, H, He,
6. Put the following elements in order of increasing atomic size:
Ar, Ca, Mg, O, N, At
7. Put the following elements in order of decreasing atomic size:
B, P, I, Sb, Be, Pb
8. Put the following elements in order of decreasing atomic size:
N, As, Kr, Fr, S, O
Ions and Ionic Size
Classwork
9. Predict which ions the following elements will produce:
a. Nitrogen
b. Oxygen
c. Flourine
d. Lithium
e. Potassium
f.
Barium
g. Chlorine
h. Argon
i.
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Carbon
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10. Put the following ions in order of increasing ionic size:
Si, Si+2, Si+4, Si-4
11. Put the following ions in order of increasing ionic size:
Mn, Mn+2, Mn+3, Mn+4, Mn+7
12. Put the following ions in order of increasing ionic size:
N-3, N, P-3, C-4, O-2
13. , Put the following ions in order of increasing ionic size:
Po+2, Sn+2, Fr+, Rb+, Cl-, Li+
Homework
14. Predict which ions the following elements will produce:
a. Beryllium
b. Boron
c. Sulfur
d. Iodine
e. Astatine
f.
Sodium
g. Hydrogen
h. Helium
i.
Aluminium
15. Put the following ions in order of increasing ionic size:
Sb, Sb+5, Sb+3, Sb-3
16. Put the following ions in order of increasing ionic size:
V, V+2, V+3, V+4, V+5
17. Put the following ions in order of increasing ionic size:
B+3, P-3, I-, Sb-3, Be+2, Pb+4
18. , Put the following ions in order of increasing ionic size:
N-3, As-3, Kr, Fr+, S-2, O-2
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Electronegativity
Classwork
19. Put the following elements in order of increasing electronegativity:
P, Cs, Sn, F, Sr, Tl
20. Put the following elements in order of increasing electronegativity:
Ca, Rb, K, O, Al, As
21. Put the following elements in order of decreasing electronegativity:
Ga, Fr, Br, Si, Na, N
22. Put the following elements in order of decreasing electronegativity:
Po, Sn, Fr, Rb, Cl, Li
Homework
23. Put the following elements in order of increasing electronegativity:
Ra, F, Al, Ne, H, He
24. Put the following elements in order of increasing electronegativity:
Ar, Ca, Mg, O, N, At
25. Put the following elements in order of decreasing electronegativity:
B, P, I, Sb, Be, Pb
26. Put the following elements in order of decreasing electronegativity:
N, As, Kr, Fr, S, O
Ionization Energy
Classwork
27. Put the following elements in order of increasing first ionization energy:
P, Cs, Sn, F, Sr, Tl
28. Put the following elements in order of increasing first ionization energy:
Ca, Rb, K, O, Al, As
29. Put the following elements in order of increasing first ionization energy:
Ga, Fr, Br, Si, Na, N
30. Put the following elements in order of increasing first ionization energy:
Po, Sn, Fr, Rb, Cl, Li
Homework
31. Put the following elements in order of increasing first ionization energy:
Ra, F, Al, Ne, H, He
32. Put the following elements in order of increasing first ionization energy:
Ar, Ca, Mg, O, N, At
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33. Put the following elements in order of increasing first ionization energy:
B, P, I, Sb, Be, Pb
34. Put the following elements in order of increasing first ionization energy:
N, As, Kr, Fr, S, O
Metallic Character (ӿ)
Classwork
35. Put the following elements in order of increasing metallic character:
P, Cs, Sn, F, Sr, Tl
36. Put the following elements in order of increasing metallic character:
Ca, Rb, K, O, Al, As
37. Put the following elements in order of decreasing metallic character:
Ga, Fr, Br, Si, Na, N
38. Put the following elements in order of decreasing metallic character:
Po, Sn, Fr, Rb, Cl, Li
Homework
39. Put the following elements in order of increasing metallic character:
Ra, F, Al, Ne, H, He
40. Put the following elements in order of increasing metallic character:
Ar, Ca, Mg, O, N, At
41. Put the following elements in order of decreasing metallic character:
B, P, I, Sb, Be, Pb
42. Put the following elements in order of decreasing metallic character:
N, As, Kr, Fr, S, O
43. Consider the element Cesium.
a. What is the most common ion that Cesium forms?
b. Which is larger neutral Cesium or the ion named in part 1? Why?
44. Consider the element Barium.
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a. Describe Barium’s atomic radius. Justify your response using one or more of these
terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle
quantum number and/or energy level.
b. Describe Barium’s’s first ionization energy. Justify your response using one or more
of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size,
principle quantum number and/or energy level.
c. Describe Barium’s’s electronegativity.
d. Describe Barium’s’s metallic character. []
45. Consider the element Rubidium.
a. Describe Rubidium’s atomic radius. Justify your response using one or more of these
terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle
quantum number and/or energy level.
b. Describe Rubidium’s first ionization energy. Justify your response using one or more
of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size,
principle quantum number and/or energy level.
c. Describe Rubidium’s electronegativity.
d. Describe cesium’s metallic character. []
46. Compare Cesium and Barium
a. Which element has the larger atomic radius?
b. Cesium and Barium both commonly form Cations. Which Cation will be smaller?
c. Samples of Cesium and Barium are both put in beakers of water and left to react.
Based on electronegativity, which will react more readily? Explain your answer.
d. How does Cesium’s first ionization energy compare to Bariums? How might this
difference affect your answer in part c?
47. Compare Rubidium and Barium
a. Which element has the larger atomic radius?
b. Rubidium and Barium both commonly form Cations. Which Cation will be smaller?
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c. Samples of Rubidium and Barium are both put in beakers of water and left to react.
Based on electronegativity, which will react more readily? Explain your answer.
d. How does Rubidium’s first ionization energy compare to Bariums? How might this
difference affect your answer in part c?
48. Compare Cesium and Rubidium
a. Which element has the larger atomic radius?
b. Cesium and Rubidium both commonly form Cations. Which Cation will be smaller?
c. Samples of Cesium and Rubidium are both put in beakers of water and left to react.
Based on electronegativity, which will react more readily? Explain your answer.
d. How does Cesium’s first ionization energy compare to Rubidium? How might this
difference affect your answer in part c?
49. Consider Nitrogen
a. What is the most common ion that Nitrogen forms?
b. Which is larger, neutral Nitrogen or the ion named in part 1? Why?
50. Consider Phosphorus.
a. Describe Phosphorus’s atomic radius. Justify your response using one or more of
these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size,
principle quantum number and/or energy level.
b. * Describe Phosphorus’s first ionization energy. Justify your response using one or
more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic
size, principle quantum number and/or energy level.
c. Describe Phosphorus’s electronegativity.
d. Describe Phosphorus’s metallic character. []
51. Consider Carbon.
a. Describe Carbon’s atomic radius. Justify your response using one or more of these
terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle
quantum number and/or energy level.
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b. Describe Carbon’s first ionization energy. Justify your response using one or more of
these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size,
principle quantum number and/or energy level.
c. Describe Carbon’s electronegativity.
d. Describe Carbon’s metallic character. []
52. Compare Nitrogen and Phosphorus
a. Which element has the larger atomic radius?
b. Nitrogen and Phosphorus both commonly form Anions. Which Anion will be smaller?
c. Samples of Nitrogen and Phosphorus are both put in beakers of water and left to
react. Based on electronegativity, which will react more readily? Explain your
answer.
d. How does Nitrogen’s first ionization energy compare to Phosphorus’? How might this
difference affect your answer in part c?
53. Compare Nitrogen and Carbon
a. Which element has the larger atomic radius?
b. Nitrogen and Carbon both commonly form Anions. Which Anion will be smaller?
c. Samples of Nitrogen and Carbon are both put in beakers of water and left to react.
Based on electronegativity, which will react more readily? Explain your answer.
d. How does Nitrogen’s first ionization energy compare to Carbon’s? How might this
difference affect your answer in part c?
54. Compare Phosphorus and Carbon
a. Which element has the larger atomic radius?
b. Phosphorus and Carbon both commonly form Anions. Which Anion will be smaller?
c. Samples of Phosphorus and Carbon are both put in beakers of water and left to
react. Based on electronegativity, which will react more readily? Explain your
answer.
d. How does Phosphorus’s first ionization energy compare to Carbon’s? How might this
difference affect your answer in part c?
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ANSWERS:
Atomic Size
Classwork
1.
2.
3.
4.
F, P, Sn, Tl, Sr, Cs
O, Al, As, Ca, K, Rb
Fr, Na, Ga, Si, Br, N
Fr, Rb, Po, Sn, Li, Cl
Homework
5.
6.
7.
8.
He, H, Ne, F, Al, Ra
O, N, Ar, Mg, Ca, At
Pb, Sb, I, Be, P, B
Fr, As, Kr, S, N, O
Ions and Ionic Size
Classwork
9.
a. N-3
b. O-2
c. Fd. Li+
e. K+
f. Ba+2
g. Clh. Ar (no ion formed)
i. C-4
10. Si+4, Si+2, Si, Si-2
11. Mn+7, Mn+4, Mn+3, Mn+2, Mn
12. O-2, N, N-3, C-4, P-3
13. Li+, Cl-, Rb+, Sn+2, Po+2 ,Fr+
Homework
14.
a. Be+2
b. B+3
c. S-2
d. Ie. Atf. Na+
g. H+ or Hh. He (no ion formed)
i. Al+3
+5
15. Sb , Sb+3, Sb, Sb-3
16. V+5, V+4, V+3, V+2, V
17. B+3, Be+2, P-3, I-, Sb-3, Pb+4
18. O-2, N-3, S-2, Kr, As-3, Fr+
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Periodic Trends
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Electronegativity
Classwork
19. Cs, Sr, Tl, Sn, P, F
20. Rb, K, Ca, Al, As, O
21. N, Br, Si, Ga, Na, Fr
22. Cl, Po, Sn, Li, Rb, Fr
Homework
23. Ra, Ne, He, Al, H, F
24. Ca, Mg, Ar, At, N, O
25. I, P, B, Sb, Pb, Be
26. O, N, S, As, Kr, Fr
Ionization Energy
Classwork
27. Cs, Tl, Sr, Sn, P, F
28. Rb, K, Ca, As, Al, O
29. Fr, Na, Ga, Si, N, Br
30. Fr, Rb, Li, Po, Sn, Cl
Homework
31. Ra, Al, H, F, Ne, He
32. Ca, Mg, At, O, N, Ar
33. Pb, Be, Sb, B, P, I
34. Fr, As, S, O, N, Kr
Metallic Character (ӿ)
Classwork
35. F, P, Sn, Tl, Sr, Cs
36. O, As, Al, Ca, K, Rb
37. Fr, Na, Ga, Si, Br, N
38. Fr, Rb, Li, Po, Sn, Cl
Homework
39. He, Ne, F, H, Al, Ra
40. Ar, O, N, At, Mg, Ca
41. Br, Pb, Sb, B, P, I
42. Fr, As, S, N, O, Kr
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43. Consider the element Cesium.
a. Cs+
b. Neutral Cesium
44. Consider the element Barium.
a. Because Barium is towards the bottom left of the periodic it has a radius bigger
than most other atoms.
b. Compared to most other elements Barium’s first ionization energy is high since
once Barium gives up an electron it achieves a half full s orbital instead of a full s
orbital making it less stable.
c. Barium is not very electronegative compared to most other atoms. It will usually
form a cation.
d. Barium is very metallic.
45. Consider the element Rubidium.
a. Because Rubidium is towards the bottom left of the periodic it has a radius bigger
than most other atoms.
b. Compared to most other elements Rubidium’s first ionization energy is low since
once Rubidium gives up an electron it achieves a full energy level giving it a
noble gas configuration.
c. Rubidium is not very electronegative compared to most other atoms. It will
usually form a cation.
d. Rubidium is very metallic.
46. Compare Cesium and Barium
a. Cesium has the larger radius
b. Cesium’s cation will be larger since it only loses 1 electron whereas Barium loses
two electrons. This means Barium has a higher effective nuclear charge then
Cesium thereby drawing Barium’s electrons closer to the nucleus and decreasing
the ions size compared to Cesium.
c. Since Cesium is less electronegative then Barium and both Cesium and Barium
are much less electronegative then hydrogen and oxygen (the elements in water)
Cesium will be more reactive.
d. Cesium’s first ionization energy should be lower than Barium’s which further adds
to it being more likely to react.
47. Compare Rubidium and Barium
a. Barium
b. Barium’s cation will be larger since it has more “shells” of electrons.
c. Rubidium since in losing an electron it gains more stability whereas Barium
(which already has a full s orbital) is more stable then rubidium.
d. Since rubidium’s first ionization energy is lower than barium, it is still more likely
to react.
48. Compare Cesium and Rubidium
a. Cesium
b. Cesium’s cation will be larger since it has more “shells” of electrons
c. Cesium since it is less electronegative.
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d. Both Cesium and Rubidium are Alkali metals so their ionization energies are
equivalent (although Cesium’s is probably slightly lower). Therefore, the effect of
ionization energy is negligible
49. Consider Nitrogen
a. N3b. Nitrogen’s anion
50. Consider Phosphorus.
a. Phosphorus is smaller than most other atoms since it is near the top right corner
of the periodic table.
b. Since phosphorus has a half filled p orbital, its first ionization energy will be
higher than other elements around it.
c. Phosphorus is more electronegative then most other elements.
d. Phosphorus is not very metallic.
51. Consider Carbon.
a. Carbon is smaller than most other atoms since it is near the top right corner of
the periodic table.
b. Carbon’s first ionization energy does not differ much from other elements in its
same period.
c. Carbon is more electronegative then most other elements.
d. Carbon is not very metallic.
52. Compare Nitrogen and Phosphorus
a. Phosphorus
b. Nitrogen since phosphorus has another “shell” of electrons compared to nitrogen.
c. Since nitrogen is so much more electronegative then phosphorus it is more likely
to react then phosphorus.
d. Since nitrogen and phosphorus are both in the same family on the periodic table,
difference in their reactivities because of ionization energy are negligible.
53. Compare Nitrogen and Carbon
a. Carbon
b. Nitrogen, since it is only gaining 3 electrons where as carbon is gaining 4.
c. Nitrogen since it is more electronegative.
d. Nitrogen’s first ionization energy should be higher than carbon which would lower
its likelihood to react. However because of how much more electronegative
nitrogen is it probably will still react.
54. Compare Phosphorus and Carbon
a. Phosphorus
b. Carbon since phosphorus has an extra “shell” even after it has become an anion.
c. Carbon since it is slightly more electronegative
d. Because Phosphorus’s first ionization energy is so much higher than carbon’s,
this makes phosphorus even less likely to react when added to water.
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