Given below are two statements : Statement I: SbCI, is more covalent than SbCI3 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 :
Statement I is correct but Statement II is incorrect
Statement I is incorrect but Statement II is correct
Show Solution
The Correct Option isA
Solution and Explanation
To determine the correctness of the statements provided, we need to analyze each one individually in the context of chemical bonding and stability.
Statement I: SbCl5 is more covalent than SbCl3
To understand this statement, we need to look at the concept of covalency and the oxidation states:
SbCl5 involves antimony (Sb) in the +5 oxidation state, while SbCl3 involves Sb in the +3 oxidation state.
According to the Fajan's Rules, the covalency increases with a higher positive charge on the cation because it causes greater polarization of the anion's electron cloud.
Thus, SbCl5, having Sb with a +5 charge and greater polarizing power, is more covalent compared to SbCl3 with the +3 charge.
Statement II: The higher oxides of halogens also tend to be more stable than the lower ones.
This statement involves analyzing the stability of oxides of halogens:
Higher oxides generally mean that the central atom is in a higher oxidation state.
Halogens can form various oxides, and the ones with higher oxidation states tend to be more stable due to the more effective distribution of electron density. This can stabilize the molecule through stronger structure formation.
For example, Cl2O (chlorine monoxide) is less stable compared to ClO2 (chlorine dioxide), and subsequently Cl2O7 is the most stable among chlorine oxides.
Both Statement I and Statement II provide a correct interpretation of chemical principles. Therefore, the correct answer is:
