91Ó°ÊÓ

What are the predominant interactions when oppositely charged ions are a. far apart? b. at internuclear distances close to \(r_{0} ?\) c. very close together (at a distance that is less than the sum of the ionic radii)?

Bond energies are typically reported as average values for a range of bonds in a molecule rather than as specific values for a single bond? Why?

If the bonds in the products are weaker than those in the reactants, is a reaction exothermic or endothermic? Explain your answer.

Several factors contribute to the stability of ionic compounds. Describe one type of interaction that destabilizes ionic compounds. Describe the interactions that stabilizeionic compounds.

Calculate the percent ionic character of HF (dipole moment \(=1.826 \mathrm{D}\) ) if the \(\mathrm{H}-\mathrm{F}\) bond distance is \(92 \mathrm{pm}\).

Although formal charges do not represent actual charges on atoms in molecules or ions, they are still useful. Why?

How would the lattice energy of an ionic compound consisting of a monovalent cation and a divalent anion compare with the lattice energy of an ionic compound containing a monovalent cation and a monovalent anion, if the internuclear distance was the same in both compounds? Explain your answer.

Calculate the percent ionic character of CO (dipole moment \(=0.110 \mathrm{D}\) ) if the \(\mathrm{C}\) - \(\mathrm{O}\) distance is \(113 \mathrm{pm} .\)

Why are resonance structures important?

What is the relationship between the electrostatic attractive energy between charged particles and the distance between the particles?