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Advanced Chemistry I
Periodic Trends Practice Problems
Effective Nuclear Charge
1. Explain why effective nuclear charge becomes greater as you move left to right across the table.
2. Explain why effective nuclear charge becomes smaller as you move top to bottom on the table.
Atomic Radius
3. Why does atomic radius decrease in going from left to right across a period in the periodic table?
4. Which of the following has the largest atomic radius?
a. Na
b. Cl
c. Ne
d. S
e. Li
5. Which of the following has the largest atomic radius?
a. C
b. Si
c. Sn
d. Pb
6. Which atom should have the largest atomic radius?
a. Br
b. Cl
c. Se
d. Ge
e. C
Electron Affinity
7. Name a group with a very low electron affinity.
8. Which atom should have the smallest electron affinity?
a. Cl
b. O
c. I
d. Br
9. Which atom should have the largest electron affinity?
a. C
b. N
c. O
d. F
10. What 3 groups of elements have negative electron affinities?
Ionization Energy
11. Define ionization energy. What 2 groups of elements have the lowest ionization energies?
12. What group of elements in the periodic table has the highest ionization energies?
13. Based on periodic trends, which one of the following elements has the lowest ionization energy?
a. K
b. S
c. Se
d. Li
e. Br
14. Based on periodic trends, which one of the following elements has the largest ionization energy?
a. K
b. S
c. Cl
d. Se
e. Br
15. Which atom should have the greatest ionization energy?
a. Se
b. Te
c. Na
d. Si
e. S
16. Why does sodium have a higher ionization energy than cesium?
17. Why does sodium have a lower ionization energy than magnesium?
Bonus: Which of the following has a very low ionization energy and a very positive electron affinity?
a. K
b. Ne
c. I
d. Fe
e. N
Bonus: Which of the following atoms has both a high ionization energy and a very small electron affinity?
a. K
b. Ne
c. Br
d. Fe
e. N