CHEMISTRY COMMUNITY

On the outline it says we should know the following:
• Explain how covalent bond dissociation energy is related to covalent bond multiplicity, atomic radius, and the presence of unpaired electrons.

I understand that covalent bond dissociation is the energy required to break the bond. From my understanding, the greater the multiplicity, the higher the dissociation energy and the greater the number of unpaired electrons, the lower the dissociation energy. Is this correct? How does the atomic radius affect the bond dissociation energy?

That is correct. The larger the atomic radius, the less dissociation energy is needed to break the bond. This is because a longer bond length between two atoms, resulting from the increased distance between two nuclei, requires less energy to be broken.

Are we required to know the bond dissociation energies of diatomic molecules? The table 3.3 on page 93 of the 6th edition gives a list but I dont know if we're required to memorize these.

I don't think we have to know the exact values of the dissociation energies. I would just focus on the relative trends of dissociation energy due to changes in atomic radius (greater radius means lower dissociation energy), multiplicity (greater multiplicity means higher dissociation energy), and number of unpaired electrons (more unpaired electrons means lower dissociation energy).

Does this apply to electronegativity values as well? Do we need to know exact values for the test or just trends?