I was researching about electronegativity when I looked up what a graph of electronegativity within the periodic table is. And, this appeared. I scanned it, matching up everything I knew about the elements up to that table. Yep, Group 1 is all light colored; yea, the nonmetals are all really dark blue culminating in fluorine; and yes, the noble gases are mostly zero (with the exception of the traitors xenon and krypton, which coincidentally are also the only electronegative noble gases!)
But while I was scanning the page from Wikipedia on noble gas compounds, I suddenly realized that there was a compound called xenon hexafluoroplatinate, meaning that xenon could bond with...platinum? Checking the table, I was astonished to find that the entire noble metal group was actually more electronegative then the metals surrounding them! Why?! Aren't they extremely non-reactive? How then can they crave electrons even more then regular metals?
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