The \(\text{I}_3^-\) ion adopts a linear geometry, explained by the Valence Shell Electron Pair Repulsion (VSEPR) theory.
The central iodine atom in \(\text{I}_3^-\) possesses three lone pairs and bonds with two outer iodine atoms.
These lone pairs are symmetrically arranged to minimize electron repulsion, yielding a \(180^\circ\) bond angle.
This linear arrangement is typical for triatomic species with symmetrical electron distribution.
Consider the following compounds:
(i) CH₃CH₂Br
(ii) CH₃CH₂CH₂Br
(iii) CH₃CH₂CH₂CH₂Br
Arrange the compounds in the increasing order of their boiling points.
Assertion (A): The boiling points of alkyl halides decrease in the order: RI>RBr>RCl>RF.
Reason (R): The boiling points of alkyl chlorides, bromides and iodides are considerably higher than that of the hydrocarbon of comparable molecular mass.
Arrange the following compounds in increasing order of their boiling point: \[ \text{(CH}_3\text{)}_2\text{NH, CH}_3\text{CH}_2\text{NH}_2, \text{CH}_3\text{CH}_2\text{OH} \]