Question

‘The strength of ionic bond in $MgC{l}_2$ is greater than in $NaCl$.’ Arrange the following key points that are essential to explain the above said statement in a correct sequence.

(1) Comparison of sizes of respective ions of Na and Mg
(2) Factors affecting strength of ionic bond
(3) Effect of size and electronegativity difference on the strength
(4) Comparison of electronegativity difference of the respective constituents in both the compounds

• A. 4, 3, 2, 1
• B. 2, 3, 1, 4
• C. 2, 1, 4, 3
• D. 4, 1, 3, 2

Answer 1

The correct option is B

2, 3, 1, 4

Explanation for Correct option:

The correct sequence for explaining the strength of ionic bond in $MgC{l}_2$ is greater than in $NaCl$

2.Factors affecting strength of ionic bond - we need to consider the factors that effect the ionic bond strength to compare the ionic bond between $MgC{l}_2$ and $NaCl$

3.Effect of size and electronegativity difference on the strength - Cation size is inversely proportional to Ionic bond strength and directly proportional to the electronegativity difference between the bonded atoms.

1.Comparison of sizes of respective ions of Na and Mg - Size of cation decides the lattice energy and hence the ionic strength.

$Cationsize\alpha \frac{1}{latticeenergy}$

4.Comparison of electronegativity difference of the respective constituents in both the compounds.

$E.Ndifference\alpha latticeenergy$

Hence, the correct option is (B).