Answer to Question #102678 in General Chemistry for sakshi

Question

(a)Arrive at the Lewis structures of SnCl- and IF4- .
(b)The bond enthalpies of N–N, N=N and N≡N bonds are not in the ratio 1:2:3. Explain the reason.

Answer 1

a)IF₄

SnCl₂

SnCL₃

SnCl₄

b)In a nitrogen molecule, two bonds are a sigma bond and a pi bond; a pi bond is stronger between nitrogen atoms than a sigma bond. The difference in the strength of sigma and pi bonds is due to the large charge of the nucleus of the nitrogen atom. When only one sigma bond is formed, the nuclei of the nitrogen atoms repel each other more strongly and the N – N bond is less strong. When sigma and pi bonds are formed simultaneously, the electron clouds shield the charges of the nuclei and the nuclei begin to be attracted to zones of increased electron density, and nitrogen nuclei with a large charge are attracted more strongly. A stronger bond N = N is formed.The large difference in the strengths of the single and triple nitrogen-nitrogen bonds is the reason that this element does not have a tendency to form chains.