Answer:
c. greater absolute charges
d. smaller ions
Explanation:
An<em> </em><em>ionic bond</em><em> is an electrostatic force that holds ions together in an ionic compound</em>. The overall stability of a solid ionic compound depends on the interactions of all the ions and not merely on the interaction of a single cation with a single anion. A quantitative measure of the stability of any ionic solid is its <em>lattice energy</em><em>, defined as the energy required to completely separate one mole of a solid ionic compound into gaseous ions.</em>
Lattice energy cannot be measured directly. However, if we know the structure and composition of an ionic compound, we can calculate the compound’s lattice energy by using <em>Coulomb’s law</em><em>, which states that the potential energy (</em><em>E</em><em>) between two ions is directly proportional to the product of their charges and inversely proportional to the distance of separation between them</em>. For a single Li⁺ ion and a single F⁻ ion separated by distance r, the potential energy of the system is given by:
where QLi⁺and QF⁻ are the charges on the Li⁺ and F⁻ ions and k is the proportionality constant. From this equation we can see that the greater the absolute charges and the smaller the ions (smaller r) the greater the potential energy E, which means that the ionic bond will be stronger.
Answer:
See attached picture.
Explanation:
Hello,
In this case, for the given name, you can verify the structure on the attached picture, wherein you can see verify the presence of both the ethyl and methyl radicals at the third carbon as well as the triple bond at the first carbon.
Best regards.
