[sam12103]

57. 

Two elements have the following first through fourth ionization energies. Deduce the group in the 
periodic table to which they probably belong. Explain briefly 

Ionization Energy   Element 1      Element 2
(kJ/mol)      

1st IE         1086.2      577.4
2ndIE         2352         1816.6
3rdIE         4620         2744.6
4thIE       6222         11575

Answer in the back of textbook
Using the date provided, deduce the group in the periodic table to which Element 1 and Element 2 belong:

               Element 1      Element 2      
∆from 2nd IP to 1st IP      1266         1239
∆from 3nd IP to 2st IP      2268         928
∆from 4nd IP to 3st IP      1602         8830

The large difference between the 3rd IP and 2nd IP for Element 1 indicates that the 3rd electron is probably from an s subshell while the first 2 electrons are from a p subshell, so Element 1 is probably from Group IVA
A quick look at element 2’s data shows a very large increase between the 3rd and 4th IP. This might be typical of an element in Group III, in which the 1st electron would be removed from a “p” sublevel while the 2nd and 3rd electron would reside in an “s” sublevel


Can you please explain to me how on earth is someone suppose to approach this problem. I found it very difficult.