Question

What is false about \(\mathrm{H}_{2} \mathrm{O}_{2} ?\) (a) Pale blue liquid (b) Can be oxidized by \(\mathrm{O}_{3}\) (c) Act as both oxidizing and reducing agent (d) Two \(-\mathrm{OH}\) bonds lie in the same plane

Short answer

Option (d) is false; the \(-\mathrm{OH}\) bonds in \(\mathrm{H}_{2}\mathrm{O}_{2}\) do not lie in the same plane.

Step-by-step solution

Understanding the Question

We need to identify which statement among the given options about hydrogen peroxide, \( \mathrm{H}_2\mathrm{O}_2 \), is false. The options relate to its physical appearance and chemical properties.

Analyzing Option (a)

Hydrogen peroxide is known to be a pale blue liquid that appears colorless in a diluted form. Thus, option (a) is true.

Analyzing Option (b)

Hydrogen peroxide can indeed be oxidized by stronger oxidizing agents such as ozone, \( \mathrm{O}_3 \). Therefore, option (b) is true.

Analyzing Option (c)

\( \mathrm{H}_2\mathrm{O}_2 \) is known to act as both an oxidizing and a reducing agent in different reactions. Thus, option (c) is also a true statement.

Analyzing Option (d)

The molecular structure of \( \mathrm{H}_2\mathrm{O}_2 \) is non-planar due to the repulsion between lone pairs that causes it to have a skewed shape (also known as a 'V' shape). Therefore, the hydroxyl \(-\mathrm{OH}\) groups do not lie in the same plane, making option (d) the false statement.

Key concepts

Oxidizing Agent

Hydrogen peroxide (_2]O_2) is a unique chemical because it can function as an oxidizing agent. This means it has the ability to accept electrons from other substances. As an oxidizing agent, _2]O_2 can facilitate the oxidation of other compounds, often converting them to oxides, thus increasing their oxidation state.

Key characteristics include:

• In oxidation reactions, _2]O_2 shows its readiness to break down and release oxygen. This is due to the compound being relatively unstable.
• The released oxygen can then interact with other substances, driving chemical reactions where other elements or compounds lose electrons.
• Common applications include bleaching, disinfection, and treating wastewater, leveraging its oxidizing properties.

This duality in reaction allows hydrogen peroxide to be frequently used in processes that require effective oxidation.

Reducing Agent

In addition to being an oxidizing agent, hydrogen peroxide (_2]O_2) can also act as a reducing agent. A reducing agent donates electrons to another substance, thereby reducing its oxidation state.

Some nuanced features of _2]O_2 as a reducing agent include:

• In some chemical reactions, _2]O_2 donates electrons, leading to the reduction of other elements. This process often involves hydrogen peroxide itself decomposing into water, thereby losing oxygen.
• The dual ability to both donate and accept electrons is what makes _2]O_2 a versatile reagent in chemistry, especially in redox reactions.

The capability to act both ways is largely due to the unique electronic structure and molecular properties of hydrogen peroxide.

Molecular Structure

The molecular structure of hydrogen peroxide (_2]O_2) plays a significant role in its chemical behavior. It consists of two hydrogen (H) atoms and two oxygen (O) atoms, forming a characteristic non-planar shape.

Here are some notable features:

• The _2]O_2 molecule has a dihedral angle due to the repulsion between the lone pairs on the oxygen atoms, resulting in a skewed, non-linear formation.
• This configuration is responsible for its specific chemical properties, including its reactivity and interaction with other substances.
• The bond between the two oxygen atoms is somewhat weak, which contributes to the molecule's instability and readiness to participate in various chemical reactions.

Understanding the molecular structure is key to grasping how _2]O_2 behaves in both oxidizing and reducing scenarios.

Chemical Properties

Hydrogen peroxide is a well-studied compound with several interesting chemical properties that make it useful in various applications.

Important chemical properties encompass:

• Instability: It decomposes readily into water and oxygen, especially in the presence of light, heat, or certain chemical catalysts.
• Concentration-dependent effects: At low concentrations, it's often used as a mild antiseptic or disinfectant, whereas higher concentrations are employed in industrial processes.
• Reactive capabilities: Its dual role as oxidizing and reducing agent allows it to participate in a wide range of chemical reactions.

These properties not only explain _2]O_2's behavior in chemical processes but also highlight its broad applicability in industries ranging from healthcare to manufacturing.