Join WhatsApp Icon JEE WhatsApp Group
Question 34

Given below are two statements:
Statement I: SbCl$$_5$$ is more covalent than SbCl$$_3$$
Statement II: The higher oxides of halogens also tend to be more stable than the lower ones.
In the light of the above statements, choose the most appropriate answer from the options given below.

Solution

Share


Analysis of Statement I

"Statement I: SbCl5 is more covalent than SbCl3"

According to Fajans' Rules, covalent character increases with an increase in the charge of the cation. In SbCl5, Antimony is in a +5 oxidation state, whereas in SbCl3, it is in a +3 oxidation state.

The higher positive charge (+5) creates a higher charge density, leading to greater polarizing power to distort the electron cloud of the chloride anions. Therefore, SbCl5 is significantly more covalent than SbCl3.

Status: Correct

Analysis of Statement II

"Statement II: The higher oxides of halogens also tend to be more stable than the lower ones."

According to standard periodic trends (specifically outlined in NCERT p-block chemistry), the higher oxides of halogens (where the halogen is in a higher oxidation state) are generally more stable than those in lower oxidation states.

For example, in the case of chlorine, higher oxides like Cl2O7 (where Cl is +7) are much more stable and less prone to violent decomposition compared to lower oxides like Cl2O or ClO2, due to kinetic factors and multiple bond stabilization characters.

Status: Correct

Correct Option: C (Both Statement I and Statement II are correct)

Get AI Help

Create a FREE account and get:

  • Free JEE Mains Previous Papers PDF
  • Take JEE Mains paper tests
Ask AI