Bond energies increase in going from C-N (lowest)to C-O to C-F (highest).Explain this trend based upon the atomic sizes of these atoms as deduced from their positions in the periodic table.
A)In going from nitrogen to oxygen to fluorine the atoms get larger.This means a greater nuclear charge,which translates into stronger chemical bonds.
B)In going from nitrogen to oxygen to fluorine the atoms get smaller.This means a greater nuclear charge,which translates into stronger chemical bonds.
C)In going from nitrogen to oxygen to fluorine the atoms get larger.This means that the bonding atoms are farther apart,which translates into a greater bond energy.
D)In going from nitrogen to oxygen to fluorine the atoms get smaller.This means that the bonding atoms are closer together,which translates into a greater bond energy.

Question

Quizplus · Accepted Answer

As we move from nitrogen to oxygen to fluorine, the atoms get smaller due to the increasing nuclear charge (more protons in the nucleus). This means that the bonding atoms are closer together (the atomic radius decreases) and therefore require more energy to break the bond, resulting in a greater bond energy.

Bond Energies Increase in Going from C-N (Lowest)to C-O to C-F