Electron Configuration and Quantum Number Problems

1)  What are the four quantum numbers and what do they indicate?  

      n is the principal quantum number and is the energy level
      n describes the relative electron cloud size

     l is the sublevel; it describes the shape of the electron cloud

    m, is the orbital; it describes the orientation in space of each orbital

    s is the direction of the spin of the electron 

2)  If an element possesses n = 3, what are the possible l values? 
     What are the possible m values?

     if n = 3, then there are 3 sublevels
     the sublevels would be s=1, p=2, and d=3
     m would be the orbitals 
          s has one orbital; 0
          p has 3 orbitals; -1, 0 1
          d has 5 orbitals;  -2, -1, 0, 1, 2   these would be the possible m values

3a)  Write out the electron configuration for Na, S, Mo, Ne, and Ce. (The whole thing!!!)
3b)  Draw the Lewis dot diagram.
3c)  How many valence electrons does each of those elements have?
3d)  What is the oxidation number for each of those elements?
3e)  What are the quantum numbers for each of those elements?

         Na  1s² 2s² 2p⁶ 3s¹      Na ^.      1 valence electron    +1 oxidation number
                                     3s¹        n=3    L = 1   m = 0  s = +1/2

                                           _..
         S   1s² 2s² 2p⁶ 3s² 3p^{4   ..}  S^{. .}     6 valence electrons   -2 oxidation number
                                     3p⁴        n=3    L = 2   m = -1  s = -1/2

        Mo 1s² 2s² 2p⁶ 3s² 3p⁶4s² 3d¹⁰ 4p⁶ 5s² 4d⁴     Mo^{. .}      
                                    2 valence electrons    +2  oxidation number, transition metal
                                     others possible:
                                     4d⁴        n=4    L = 3   m = 1  s = +1/2

                                       _..
        Ne  1s² 2s² 2p^{6          ..} Ne ^..      8 valence electron    no oxidation number  8 is great!
                                       ^..

                                     2p ⁶       n=2    L = 2   m = 1  s = -1/2

       Ce 1s² 2s² 2p⁶ 3s² 3p⁶4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f²    
       Ce^{. .}     2 valence electrons   +2 oxidation number  
                 lanthanoid metal, others possible
                                     4f²        n=4    L = 4   m = -2  s = +1/2

4)  What is the charge of noble gases? Why? Where do I find noble gases on the periodic table?

      have no charge, not usually ions,  have 8 valence electrons and are considered stable
      group 18 (VIII) far right column on periodic table
      He, Ne, Ar, Kr, Xe, and Rn

5)  What is the charge of halogens? Why? Where do I find them on the periodic table?

      when halogens form ions, they want to gain one electron, so their charge is -1  
      the are on the right hand side of the periodic table next to the noble gases group VII
      F, Cl, Br, I, At

6)  What is the charge of alkaline earth metals? Why? 
     Where do I find them on the periodic table?

      alkaline earth metals have 2 valence electrons so their oxidation number is +2  
      they are the second column from the left, group II
      Be, Mg, Ca, Sr, Ba, Ra

7)  Why are transition metals in transition? Why do you want a list of their charges for the test?

      They have a d sublevel which has less energy than the s level, consequently all transition
      metals have 2 valence electrons.
      The d sublevel electrons may prevent the atom from spinning smoothly, the atom may lose
       more than 2 electrons if it will help balance the atom.  

8) Where are the metalloids?

     metalloids are found to either side of the zigzag line or the staircase line  
     they include B, Al, Si, Ge, As, Sb, Te, Pl, and At