Which of the following statement(s) is/are correct ? (1) Chlorine dioxide \(\left(\mathrm{ClO}_{2}\right)\) is powerful oxidising agent but bleaching action is lower than \(\mathrm{Cl}_{2}\) (2) \(\mathrm{ClO}_{2}\) in alkaline solution undergoes disproportionation. (3) \(\mathrm{SF}_{4}\) has a square planar shape with \(\mathrm{S}\) having two lone pair of electrons. (4) Sulphur tetrafluoride hydrolysed by water to give \(\mathrm{SO}_{2}\) and \(\mathrm{HF}\)

Oxidizing agents are substances that gain electrons and, in the process, get reduced. These agents facilitate the oxidation of other substances. Chlorine dioxide \((\mathrm{ClO_{2}})\) is a powerful oxidizing agent due to its high affinity for electrons.
Oxidizing agents are vital in various chemical reactions, including bleaching and disinfection. The bleaching action of \((\mathrm{ClO_{2}})\) is actually stronger than chlorine \((\mathrm{Cl_{2}})\), contrary to some misconceptions.
Tips to identify oxidizing agents include recognizing substances that have high electronegativity or many oxygen atoms. Elements like oxygen, chlorine, and fluorine are often parts of strong oxidizing agents.

Disproportionation reactions are unique chemical processes where a single substance acts as both the oxidizing agent and the reducing agent, leading to the formation of two different products.
A classic example is the reaction of chlorine dioxide \((\mathrm{ClO_{2}})\) in alkaline solutions. In this scenario, \( \mathrm{ClO_{2}} \) is both reduced and oxidized, creating \( \mathrm{ClO_{3}^{-}} \) and \( \mathrm{ClO_{2}^{-}} \).
These reactions are essential in different industrial processes, including the treatment of water and in bleaching.

Molecular geometry dictates how atoms in a molecule are spatially arranged, which significantly influences the molecule's properties and reactivity. According to the VSEPR theory, the shape adapts to minimize electron pair repulsion.
For example, sulfur tetrafluoride \((\mathrm{SF_{4}})\) does not have a square planar shape; instead, it has a seesaw geometry due to the lone pair of electrons on the sulfur atom.
Understanding the molecular geometry helps predict reaction mechanisms and the behavior of a molecule in different chemical environments.

Hydrolysis reactions involve the breaking of a chemical bond through the addition of water. This reaction is common in the decomposition of compounds.
A notable example is the hydrolysis of sulfur tetrafluoride \((\mathrm{SF_{4}})\), which produces sulfur dioxide \((\mathrm{SO_{2}})\) and hydrogen fluoride \((\mathrm{HF}}\). This follows the equation: \[ \mathrm{SF_{4} + 2H_{2}O \rightarrow SO_{2} + 4HF} \].
Hydrolysis reactions are crucial in various biological and industrial processes, including digestion and the manufacturing of chemicals.