Which of the following flouride has the highest lattice energy a)NaF b)KF c)CsF d)LiF

The correct option is;

d) LiF

Explanation:

The Lattice energy of ionic compounds can be calculated using the modified Coulomb's law as follows;

Where;

Q₁ and Q₂ =  The ionic charges

k' = A constant depending on the ionic and valence configuration

r₀ = The distance between the two nucleus

Given the four compounds each of the metallic ions are of the same group (group one) have the same (only one) valence electron, and are combined to the same ion (fluoride ion) such that Q₂, is the same for all compounds, the factor that will influence the lattice energy more will be the r₀

The sizes of the atoms Li, Na, K and Cs increases as arranged as such Li has the least r₀, and therefore LiF the least  lattice energy

From chemistry test online, we have;

The lattice energy of LiF = -1045 kJ/mole

The lattice energy of NaF = -924 kJ/mole

The lattice energy of KF = -822 kJ/mole

The lattice energy of CsF = -737 kJ/mole.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.