The decreasing order of ionic nature of the following compound is:a)LiI > NaBr > KCl > CsFb)LiI > KCl > NaBr > CsFc)CsF > NaBr > KCl > LiId)CsF > KCl > NaBr > LiICorrect answer is option 'D'. Can you explain this answer?

Question

The decreasing order of ionic nature of the following compound is:a)LiI &#62; NaBr &#62; KCl &#62; CsFb)LiI &#62; KCl &#62; NaBr &#62; CsFc)CsF &#62; NaBr &#62; KCl &#62; LiId)CsF &#62; KCl &#62; NaBr &#62; LiICorrect answer is option 'D'. Can you explain this answer?

Answer

The decreasing order of ionic nature of the given compounds is:

a) LiI > NaBr > KCl > CsF
b) LiI > KCl > NaBr > CsF
c) CsF > NaBr > KCl > LiI
d) CsF > KCl > NaBr > LiI

Explanation:

Ionic nature is the measure of the degree of electrostatic attraction between oppositely charged ions in a compound. The greater the difference in electronegativity between the two atoms, the more ionic the bond will be.

In the given compounds, the cationic and anionic components are:

LiI: Li+ and I-
NaBr: Na+ and Br-
KCl: K+ and Cl-
CsF: Cs+ and F-

The electronegativity values of these atoms are:

Li: 0.98
Na: 0.93
K: 0.82
Cs: 0.79
I: 2.66
Br: 2.96
Cl: 3.16
F: 3.98

Therefore, the greater the difference in electronegativity between the cation and anion, the more ionic the bond will be.

Now, let's analyze the given options:

a) LiI > NaBr > KCl > CsF
LiI has the highest ionic character because of the large difference in electronegativity between Li and I. CsF has the lowest ionic character because of the smaller difference in electronegativity between Cs and F. Therefore, the decreasing order of ionic character is LiI > NaBr > KCl > CsF.

b) LiI > KCl > NaBr > CsF
The trend is similar to option a), but KCl has a slightly lower ionic character than NaBr. Therefore, the decreasing order of ionic character is LiI > KCl > NaBr > CsF.

c) CsF > NaBr > KCl > LiI
This option is incorrect as it has the opposite trend of increasing ionic character.

d) CsF > KCl > NaBr > LiI
This option is correct as it has the decreasing trend of ionic character, with CsF having the highest and LiI having the lowest ionic character.

Therefore, the correct answer is option d) CsF > KCl > NaBr > LiI.

Answer

Simply use fazan's rule.fazan's rule can predict the covalency in a bond.and it(covalency in a bond) is directly proportional to charge of the CATION and inversly propprtional to size of the CATION.so, therefore in a period from top to bottom size decreases. therefore LiI Will have highest covalency or you may say lowest ionic character in the bond due to small size of Li. .so buss..do it in this way and option d Will be correct.

Here I told about fazan's rule w.r.t cation.but it may also be expressed w.r.t to anions.that will complicate our comprehension.so better we follow this.

Answer

Can be understood properly by knowing some facts about alkali metals and halogens.
such that as we go down the group reactivity of alkali metals increase and reactivity of halogens decrease.
so two most reactive ones are forming bond so will have maximum ionic character.

Answer

Ionic nature of any compound can be explain on the basis of electronegativity difference between the atoms involved in it.
as in case here caesium is less electronegative than fluorine the electronegativity difference between them is around 3.19, while coming towards Potassium Chloride electronegativity difference between potassium and chlorine is 2.34

in sodium Bromide sodium is less electronegative than bromine and its it's electronegativity difference is around 2.03 while Lithium and Iodine has electronegativity difference of 1.68 i. e.

3.19>2.34>2.03>1.68

as it is very clear that there is a decrease in electronegativity difference between the element of the compounds which explains the ionic nature of the compound
hence caesium chloride is most ionic due to high electronegativity difference caesium and fluorine

the decreasing series of ionic character is caesium fluoride greater than potassium chloride greater than sodium Bromide greater than Lithium iodide
hope this will help thank you

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