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Chapter 11: Problem 98

Select the incorrect statement about the following: [J.E.E. (W.B.) 2008] (a) \(\mathrm{O}_{3}\) is used as germicide for purification of air (b) In \(\mathrm{O}_{3}, \mathrm{O}-\mathrm{O}\) bond length is identical with that of molecular oxygen . (c) \(\mathrm{O}_{3}\) molecule is angular in shape C (d) \(\mathrm{O}_{3}\) is an oxidising agent \(\Gamma\)

Short Answer

Expert verified
Option (b) is incorrect.

Step by step solution

01

Understand the Question

Identify which statement among the given options is incorrect regarding the chemical properties of ozone, \( \mathrm{O}_{3} \). Each option presents a fact about ozone, and you must evaluate them.
02

Analyze Option (a)

Option (a) states that \( \mathrm{O}_{3} \) is used as a germicide for purification of air. This is correct because ozone is known for its ability to kill bacteria and remove airborne contaminants, making it effective for air purification.
03

Analyze Option (b)

Option (b) suggests that the \( \mathrm{O}-\mathrm{O} \) bond length in ozone is identical to that of molecular oxygen \( \mathrm{O}_{2} \). This is incorrect because in \( \mathrm{O}_{3} \), the \( \mathrm{O}-\mathrm{O} \) bond length differs from that in \( \mathrm{O}_{2} \), due to the resonance structures in ozone.
04

Analyze Option (c)

Option (c) indicates that the \( \mathrm{O}_{3} \) molecule is angular in shape. This is correct; ozone has a bent shape due to the lone pairs on the central oxygen atom causing a V-shape with an bond angle of approximately 117 degrees.
05

Analyze Option (d)

Option (d) asserts that \( \mathrm{O}_{3} \) is an oxidizing agent. This statement is correct as ozone is a strong oxidizing agent and can readily accept electrons, making it capable of oxidizing other substances.
06

Conclusion: Identify Incorrect Statement

After analyzing all options, the incorrect statement is option (b) since it incorrectly states that the \( \mathrm{O}-\mathrm{O} \) bond length in \( \mathrm{O}_{3} \) is identical to that in \( \mathrm{O}_{2} \), which it is not due to resonance effects in ozone's structure.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Ozone as an oxidizing agent
Ozone, with the chemical formula \( \mathrm{O}_3 \), acts as a powerful oxidizing agent. Its ability to oxidize stems from its high reactivity and willingness to accept electrons from other substances. This property allows ozone to react with a variety of substances, effectively breaking down pollutants and harmful organisms.
  • Ozone's strength as an oxidizing agent makes it useful in water treatment processes. It helps in disinfecting and sterilizing water by killing bacteria and viruses.
  • In the atmosphere, ozone can react with industrial pollutants, such as nitrogen oxides, playing a critical role in reducing harmful emissions.
  • Ozone is also used in various industrial processes where its oxidizing properties are harnessed for bleaching, deodorizing, and decolorizing products.
As a result, ozone is invaluable in both environmental cleaning and industrial applications, making it much more than just a component of the Earth's stratosphere.
Ozone bond length
The bond length in ozone (\(\mathrm{O}_3\)) is unique and differs significantly from the dioxygen (\(\mathrm{O}_2\)) molecule. Unlike molecular oxygen, which has a standard double bond with a length of approximately \(121 ext{ pm}\), ozone consists of two equivalent \(\mathrm{O}-\mathrm{O}\) bonds in a resonating structure. This results in a bond length averaging around \(128 ext{ pm}\).
  • The concept of resonance in ozone contributes to its \(\mathrm{O}-\mathrm{O}\) bond having a character between a single and a double bond.
  • This causes the bond length to be longer than a double bond in \(\mathrm{O}_2\), yet shorter than a typical single bond found in other molecules.
  • Understanding this bond length is crucial when studying ozone's chemical reactivity and stability, as well as its role in atmospheric chemistry.
The intermediate bond length is a direct consequence of the molecular structure of ozone involving resonance forms, which equally distribute the double bond character across both oxygen-oxygen connections.
Ozone molecular shape
The shape of the ozone molecule (\(\mathrm{O}_3\)) is angular or bent, which can be attributed to its molecular geometry. The central oxygen atom shares single bonds with the two other oxygen atoms, forming a bond angle that is neither linear nor a perfect 90-degree bend.
  • The bond angle in an ozone molecule is approximately \(117\degree\), resulting in its distinguished bent shape.
  • This structure occurs due to the lone pairs of electrons on the central oxygen atom which repel the bonded pairs, causing a V-shaped molecular geometry.
  • The angular shape of ozone not only defines its spatial arrangement but also impacts its polar nature and reactivity.
The bent molecular geometry plays a significant role in the physical and chemical properties of ozone, influencing how it interacts with light and other chemical substances in the atmosphere.

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Most popular questions from this chapter

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