Animated Solution for Chemistry - s and p-Block Elements: From the following statements regarding $H_2{O}_2$, choose the incorrect statement.

Hydrogen peroxide ($H_2{O}_2$) is one of those fascinating molecules in chemistry that refuses to be boxed into a single category. It is a chemical chameleon, capable of adapting its behavior based on the environment it finds itself in. But why does it behave this way? The secret lies in the oxidation state of its oxygen atoms.

In a molecule of $H_2{O}_2$, the oxygen atoms are bonded to each other in a peroxide linkage ($-O-O-$). Because of this unique structure, the oxidation state of oxygen is $-1$. Now, oxygen typically prefers an oxidation state of $-2$ (as in water, $H_{2}O$) or $0$ (as in oxygen gas, $O_2$). The $-1$ state is an intermediate, unstable middle ground.

Because it is sitting right in the middle, $H_2{O}_2$ has two choices. It can either lose electrons to increase its oxidation state to $0$, thereby acting as a reducing agent. Or, it can gain electrons to decrease its oxidation state to $-2$, acting as an oxidising agent. This dual capability completely invalidates the claim that it can only act as an oxidising agent.

Hydrogen peroxide is notoriously unstable. The $O-O$ single bond is relatively weak, and the molecule is eager to decompose into more stable products: water and oxygen gas.

This decomposition is not just spontaneous; it is highly sensitive to external catalysts. Exposure to light (photons) provides enough energy to break the bonds, accelerating the breakdown. Similarly, rough surfaces like ordinary glass, or trace metals found in dust particles, act as catalysts for this decomposition.

To prevent this, chemists have devised specific storage protocols. $H_2{O}_2$ is stored in dark-colored bottles to block out light. Furthermore, these bottles are often lined with wax or made of plastic to provide a perfectly smooth, non-reactive surface, and they are kept strictly away from dust.

When we evaluate the given statements, it becomes clear that statements (b), (c), and (d) accurately describe the physical realities of handling hydrogen peroxide. It decomposes in light, requires wax-lined dark bottles, and must be kept away from dust. The only incorrect statement is (a), which falsely limits $H_2{O}_2$ to being solely an oxidising agent. Understanding the fundamental oxidation states makes this conclusion both logical and inevitable.