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5. What equation did Schrodinger solve? _____________________________
What did his solutions show about the electron (hint 3D space)? _____________________
6. Define Hund's Rule ______________________________________________________________
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7. How many electrons will fill the 2nd energy level? _____________________
8. How many orbitals are in the fourth energy level? ______________________
9. How many electrons do you need to fill the 4th row of Periodic Table? ________________
10. Can you have a 3f subenergy level and why? ________________________________
11. Define isotope and give the symbolic representation of an isotope.
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12. #n = ____ - _____
13. Circle the one that is located on the Periodic Table: Atomic Number or Mass Number.
14. Define Valence electron: _____________________________ and
how can you find from the Periodic Table: _______________________
15. Define atomic mass.
:
Write the electron configurations for the following elements. Make sure to separate the last subenergy level into its orbitals. Where appropriate, give the # of valence electron.
1. As
2. Ag
3. Bi
4.Give the #p,#n and #e for the following isotopes:
a. Ca-42
b. C-13
c. U-238
After printing out the tables in [Two Calculating Atomic Mass Table], use the information from your table of isotopes to calculate the atomic mass of sulfur and oxygen.