5 posts • Page 1 of 1
After the test last week, I realized I'm still not understanding energies and bond lengths. I get that as the more bonds are added the greater the strength and the shorter the length, but what if we are comparing two single bonds but one is a C-C and the other is a C-P. How would this differ? And what needs to be taken into consideration.
Formal charge should be taken into consideration. When it comes to single bonds, you just need to take the formal charge for each of the elements in the molecule and use their electronegativities to determine which bond is stronger.
bond length most greatly affects its strength, double and triple bonds are shorter and therefore stronger than a single bond but when comparing two single bonds it is important to look at electronegativity a greater difference in electro negativity between atoms suggests a stronger bond.
Who is online
Users browsing this forum: No registered users and 1 guest