Electron Configuration and Periodic Table Comprehensive Review Sheet

AMHS Honors Chemistry Electron Configuration and Periodic Table Comprehensive Review Sheet 1. In the hydrogen atom, what information do we get from t...
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AMHS Honors Chemistry

Electron Configuration and Periodic Table Comprehensive Review Sheet 1. In the hydrogen atom, what information do we get from the values n, l, m l and ms? What are the names of the quantum numbers represented with those symbols?

2. How do the 2p and 3p orbitals differ from each other?

3. Which of the following orbital designations are incorrect? For each that is incorrect, explain why it is incorrect. 1p, 2d, 9s, 4f, 7d, 3f

4. Which of the following sets of quantum numbers are not allowed? State what is wrong with any set that is incorrect. a. n=2, l=1, ml=-1 b. n=1, l=1, ml=0 c. n=8, l=7, ml=-8 5. How many maximum electrons can be described by the following quantum numbers? Example: n=2, l=1, ml=-1 Answer: Three quantum numbers defines one orbital so you can only place a maximum of 2 electrons inside so the answer is 2! a. n=3

b. n=3, l=2

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c. n=5, ms = +1/2 (this one is tricky!) d. 2,1,0 e. 4,3 c. 6,3,+1/2 d. 3,3,-2,-1/2 e. n=5

6. Identify the following elements given the information: a. 3,1,1,-1/2 b. 4,2,1,+1/2 c. 4,3,-3,-1/2 7. Write the electron configurations for the following ions. Li+1, Ba+2+, Ag+1, Al+3, P-3, Sn+2, Sn+4 For each ion, give a brief explanation for the reason for the oxidation numbers of these ions.

AMHS Honors Chemistry

8. How many electrons does the 3rd main energy level hold?

9. If n=3, how many possible orbital shapes can there be?

10. What is the total number of orbitals that can exist at the 6 th energy level?

11. How many electrons can a single orbital of in the 3d level hold?

12. If the 6th energy level contains 28 electrons, how many more can it hold?

13. Give examples of 2 elements that have electron configuration exceptions and explain the reason for the exception.

14. Describe the relationship between frequency, wavelength, energy, and speed using the appropriate equations and discuss the type of proportional relationship that exists between frequency and wavelength and frequency and energy.

15. Discuss the process that occurs when electricity is passed through a tube of hydrogen gas and the electromagnetic spectrum is produced. What would be different about the light produced by another type of gas in a discharge tube and why?

AMHS Honors Chemistry

16. Arrange the following elements in order of smallest to largest radius: a. Na, Cs, Rb, Li b. Si, Mg, Cl, Na Be sure you understand why the elements are arranged this way and aren’t just memorizing the general trend! [Good chance this explanation will be on the test!] 17. Arrange the following elements in order of largest to smallest electronegativity. a. Li, C, N, Be, O b. Te, S, Po, O Be sure you understand why the elements are arranged this way and aren’t just memorizing the general trend! 18. Circle the element in the following pairs that has the largest ionization energy. a. Na or Mg b. Na or Cs c. Li or O d. Cl or Br 19. For the following elements, draw orbital filling diagrams and list the possible oxidation states for the elements based on the orbital filling diagrams. a. Mo

b. Fe

c. Sc

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20. For the following ions, state the Noble Gas they are isoelectronic with. Then, arrange the ions in order of smallest radius to largest radius. N-3, O-2, F-1, Na+1, Mg+2, Al+3

21. Which of the following elements have the largest second ionization energy? Mg, Al, P, or Na

Explain the reasoning behind your answer!

22. Consider the following orderings . (A) Al< Si < P < S (B) Be < Mg < Ca < Sr (C) I < Br < Cl < F (D) Na+ < Mg +2 < Al+3 < Si+4

[This is a good example of a typical multiple-choice test question!]

Which of these orderings gives the correct trend in ionization energy? a. (C) b. (A) and (B) c. (A) and (D) d. (A) and (C) and (D) e. None of these.

22. Write the names of the following groups (families) or “blocks” on the periodic table. Group I: _____________________________________ Group II: ____________________________________ Group 17: ___________________________________ Group 18: ___________________________________ 4f Block: ____________________________________ 5f Block: ____________________________________ 23. How would you identify the radioactive elements on the periodic table?

AMHS Honors Chemistry

24. Describe the reactivity of elements in Group I and Group 17 and explain how you came up with your answer for each group.

25. Consider an element whose outermost electron configuration is 4s2 3d10 4px. a. To which period does this element belong? ______________ b. Suppose it is a halogen, what is the value of “x”? ________________ c. Suppose it is a halogen, what would the oxidation number be? ____________ 26. Thoroughly explain how the Z-effect and shielding is responsible for most periodic trends we have discussed.

27. Copper’s electron configuration may be predicted to be 4s 23d9 but is actually 4s13d10. Which configuration is more stable and why? Predict the possible oxidation state(s) of copper.

28. Pick two elements from group 14 which will have very different properties (both chemical and physical) and explain why these two elements are from the same group but are markedly different. Make sure you list some of their expected physical and chemical characteristics!