Name: ______________________________________ Date: ___________________ Electron Configuration Conceptual Review
1. Which model of the atom do we currently accept? Quantum Mechanical (QM) Model 2. What is the lowest possible energy level? n = 1 (1st energy level) 3. How many electrons can fit in the 2nd energy level? 2n2 = 2(2)2 = 8 electrons 4. Typically, do electrons have a greater amount of energy if they are closer to the nucleus? No – typically energy increases as electrons move farther from the nucleus 5. Can an electron be found in between two energy levels? No 6. If n = 3 is already full, what energy level does the next electron occupy? n = 4 7. How can you know precisely where an electron is? You can’t (Heisenberg Uncertainty Principle) 8. Can an electron be found in the location n = 2.8? No 9. Which energy level is farther from the nucleus, n = 2 or n = 5? 10. What is the maximum number of electrons that can fit in n = 3? 2n2 = 2(3)2 = 18 electrons 11. Name the four sublevels that exist in atoms. s, p, d, and f 12. Which gives a more specific location: an orbital or an energy level? (assuming you know n already) 13. How many electrons can fit into an s sublevel? 2 electrons (only 1 orbital in an s sublevel) 14. What is the shape of a p subshell? Dumbbell 15. In which energy level does the f orbital start to appear? n = 4 16. What is the maximum number of electrons that can fit in an atomic orbital? 2 electrons per orbital 17. List the sublevels that can exist in the 1st energy level. Only s (1s) 18. Which is bigger: an atom whose highest n is n = 2 or an atom whose highest n is n = 4? B/c n = 4 is farther from the nucleus 19. How many orbitals are in the sublevel shaped like a sphere? s sublevel only has 1 orbital 20. How many orbitals are in the 4p sublevel? 3 orbitals 21. How many orbitals are in the 3d sublevel? 5 orbitals 22. List the allowed sublevel values for n = 1. Only s 23. Circle any sublevels that do not exist in atoms: a. 3s c. 3f e. 1s g. 2d b. 1p d. 2p f. 4d h. 3p 24. How many electrons can fill the 1s sublevel? 2 electrons in any s sublevel 25. How many electrons can fill the 3p sublevel? 6 electrons in any p sublevel 26. How many electrons can fill the 2d sublevel? 0 electrons (the 2d sublevel does not exist) 27. How many electrons can fill the 4f sublevel? 14 electrons in any f sublevel 28. If you have 6 electrons in the 3rd energy level how many more must you add so that it’s full? Maximum number of electrons per energy level is 2n2 = 2(3)2 = 18 electrons, so if you only have 6 to start with you can add 12 more electrons to fill the 3rd energy level. 29. Name the lowest value for n in which a d sublevel may be found. n = 3 30. The number of orbitals in a given energy level is determined by the sublevels (shapes). 31. What denotes the shape of the electron density: the energy level or the sublevel? (s is sphere, p is dumbbell, etc.) 32. How many orbitals can fill the n = 4 shell? You can have 4s, 4p, 4d, and 4f. 4s has 1 orbital; 4p has 3; 4d has 5; and 4f has 7. So 1 + 3 + 5 + 7 = 16 total orbitals. OR since you know 2n2 = 2(4)2 = 32 total electrons, which is 32 ÷ 2 = 16 total orbitals. 33. What subshells can exist in the 3rd principal energy level? When n = 3 you can have s, p, or d subshells.