Question

"in an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the force needed to pull ions apart); the lattice energy, in turn, affects the enthalpy of solution. Based on ion sizes, arrange these compounds by their expected heats of solution." csbr, csi, csf, cscl

Answer 1

As we all know the different atoms and paste in different crystal forms.

Step-by-step explanation:

And when the atoms are brought from infinity to that position position shall be released the energy that can be released on this occasion of bringing the iron from Infinity 2 in that reformist would give lattice energy now you also know that right only for different crystal formations are different.

Hence have different sizes of Ions to now arranging these compounds in terms of energy they have Starting from most endothermic to the most exothermic compounds are CsF < CsCl < CsBr < CsI also it can be added even for greater values.

Answer 2

Step-by-step explanation:

As lattice energy is the amount of force or energy required to pull the ions apart. Therefore, smaller is the size of combining atoms more will the presence of force of attraction in its ions.

Hence, high energy will be needed to break the bond and therefore, an increase in lattice energy will occur.

Since, in the given options the cation is same and only the anion is different. And, electron charge density of fluoride is the highest whereas iodine has the least electron charge density.

Hence, CsF will have the highest lattice enthalpy. Hence, trend of lattice energy for the given compounds will be as follows.

CsF > CsCl > CsBr > CsI

As CsF requires high energy to split into ions so, it will be endothermic in nature.

Thus, we can conclude that the given compounds are arranged by their expected heats of solution (most endothermic to most exothermic) in increasing order as follows.

CsF < CsCl < CsBr < CsI