Electron Configurations                                      Name _____________________

 

1.         Use the formula 2n2 to predict the number of electrons that each of the following

energy levels could potentially hold.

 

            2: ________           5: _______             6:  72           7: _________

 

2.         How many electrons can each of the following sublevels hold?

 

            S: ________          P: _________          D: 10          F: _________

 

3.         Circle the error in each of the following electron configurations and in the space beside it explain what is wrong. 

 

            1s2  2s1 2p6 3s2 3p6 4s2                the 2s orbital should be filled before an electrons go into the 2p orbital

 

            1s2  2s2 2p7 3s2 3p6 4s2                ___________________________________________

 

            1s2  2s2 2p6 3s2 3p6 3d10 4s2          ___________________________________________

 

1s2  2s2 2p6 3s2 3p6  4s2 3d10 4p8   ___________________________________________

 

1s2  1p6 2s2 2p6 3s2 3p6  4s2 3d10 4p3           _______________________________________

 

 

4.         In each of the following pairs, determine which sublevel has the lowest energy

            a)  3d, 4s  _______     b) 2p, 3s  _______     c) 3d, 4p 3d      d) 5f, 7s ______

 

5.         The electron configuration for Li is 1s2  2s1  write the predicted configuration for

each of the following elements. 

Consolidate electrons by using a noble gas.  

example:   31Ga:   [Ar]  4S2  4P1

 

9F:        [   ]

 

23V:      [   ]

 

60Nd:    [  Xe ]   6s2 4f4

 

82Pb:     [   ]

 

97Bk:     [   ]

 

11Na:    [   ]

 

6.         How many orbitals are there in each of the following sublevels?

 

            S: ________          P: _________          D: 5          F: _________

 

More fun with those wacky electrons on back

 

7.         Fill in the orbital diagrams for each of the following elements.  Label the each

orbital as to energy level and sublevel and show how  many electrons each holds.

(note that some of the orbitals shown may not be needed). 

Consolidate as many electrons as you can by using noble gases

(ex   Sodium could be written [Ne]   ­    )

                                                                                                                                               

  Ex:  16S [Ne]   ­¯        ­¯        ­         ­        

                        3s         3p         3p         3p

 

Note:  show the predicted electron arrangement

 

 

6C  [     ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___    

 

 

 

 

15P  [     ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___    

 

 

 

 

27Co  [ Ar   ] ­¯_   ­¯_     ­­¯_    ­__   ­__   _­__    ___     ___     ___    ___    ___      ___     ___    

                     4s                 

 


                                                 3d     

keep the electrons unpaired until all orbitals in the sublevel have an electron, then begin pairing

 

 

72Hf  [     ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___    

 

 

 

 

22Ti  [     ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___    

 

 

 

 

34Se  [     ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___    

 

 

 

 

62Sm  [    ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___    

 

 

 

 

95Am  [     ] ___     ­___    ___    ___    ___    ___     ___     ___    ___    ___      ___    ___    ___