Chemistry CH 4 Reading Assignment Section 1 Pg 100 1. Define ground and excited states of an atom: 2. What happens to the atom when it goes from the excited state by to ground state? Pg 102-103 3. Describe the Bohr’s Model (Planetary Model) of the atom : 4. What were the limitations of the Bohr Model? Section 2 Pg 104-110 5. According to De Broglie electrons travel around the nucleus in ___ as opposed to Bohr which had them traveling around in direct paths called orbits. 6. What is the Heisenberg Uncertainty Principle: 7. What is Quantum theory? 8. What is an orbital as opposed to an orbit? 9. What are Quantum Numbers (n,l, m,s) used for? 10. Quantum number n is known as the ___ and represents what about the electron in the atom? 11. As n increases, what happens to the energy levels of the electrons? 12. In theory n can be infinite, but in reality what is the highest value for n with our atoms? 13. Quantum number l represents what within the atom? 14. How many sublevels can a level have? 15. Quantum number l is known as the ___ and indicates the ___ of the electron cloud? 16. What are the sublevels called and what shape of the electron cloud do they describe? 17. Fill in the chart: n l #’s assigned 1 s 0 2 3 4 5 18. Quantum number m is known as the ___ and represents the ___ of the electron cloud? 19. Quantum number m also represents the atoms orbitals which are __? 20. Complete the chart n L (equal to n) 1 s 2 s,p 3 4 s,p,d,f 21. 22. 23. 24. 25. 26. m (n2) 1 # assigned to l 0 0,1 1,3=4 total 0,1,2,3 1,3,5,7=16 total # assigned to m 0 0, -1,0,1 0, -1,0,1 -2,-1,0,1,2 -3,-2,-1,0,1,2,3 5 How many directions in space do the following orbitals have s= ___ , p= ___ , d=___, f=____. How many electrons can occupy a single orbital___? How many total electrons can occupy the following orbitals s= ___ , p= ___ , d=___, f=____. The last quantum number s is known as the ____ and represents the ___of the electrons and is given the numerical values of ____. When two electrons occupy the same orbital, they must do what? If I give you the following quantum numbers, you should be able to explain where the electron is within the atom, (3, 2, -2, +1/2 ) Section 3 pg 111- 122 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. What is an electron configuration? What is Aufbau’s principle? What is the Pauli’s exclusion principle? What is Hund’s rule? Draw the diagonal rule: The electron configuration for N with its 7 electrons in 1s22s22p3, what is the electron configuration for Br? Draw is the orbital filling diagram for Br? What is the noble gas (short hand) configuration for Br? Draw the Lewis dot structure for Br? What would be the charge of Br’s ion? Do the same (32-36) for the element Ca….