3 posts • Page 1 of 1
I'm having trouble with a problem from chapter 3 number 87. We're supposed to determine which molecule would have the strongest bond, CF4, CCL4, or CBr4. The book says CF4 would have the strongest bond because it has the shortest bond, but this is an exception to the electronegativity argument. C and F are closer together than the other two elements are to C, why would the CF4 bond be the strongest?
You can approach this problem by thinking about the atomic radius of each halogen. As the distance between the nuclei of the bonded atoms decrease, then the strength of that bond increases. Out of these three halogens, fluorine has the smallest atomic radius, so the nucleus of Carbon and Fluorine are closer compared to that of Carbon and Chlorine or Carbon and Bromine. Since the nucleus of Carbon and Fluorine are the closest, CF4 has the strongest bond out of the three molecules.
Who is online
Users browsing this forum: No registered users and 1 guest