Question

Which of the following oxides of chlorine is obtained by passing dry chlorine over silver chlorate at \(90^{\circ} \mathrm{C}\) ? (a) \(\mathrm{ClO}_{4}\) (b) \(\mathrm{ClO}_{3}\) (c) \(\mathrm{Cl}_{2} \mathrm{O}\) (d) \(\mathrm{ClO}_{2}^{3}\)

Short answer

The correct answer is (b) \(\text{ClO}_3\).

Step-by-step solution

Understand the Reaction Conditions

The problem states that dry chlorine is passed over silver chlorate at \(90^{\circ} \mathrm{C}\). This indicates a chemical reaction where silver chlorate \(\text{AgClO}_3\) will react with chlorine gas \(\text{Cl}_2\). Identifying the reaction conditions helps in predicting the product formed.

Identify Potential Reaction Mechanisms

Consider the chemical reaction that occurs. When dry chlorine is passed over silver chlorate, the common reaction known is the decomposition or a displacement reaction. Generally, in such reactions, the oxidizing nature of \( \text{AgClO}_3 \) can form certain chlorine oxides.

Determine Possible Chlorine Oxides

Based on known chemical behavior, when silver chlorate decomposes or is acted upon by chlorine, one potential oxide of chlorine that could form is chlorine dioxide \(\text{ClO}_2\). Other potential oxides to consider adopting this chemical pathway include \(\text{Cl}_2\text{O}_7\) or \(\text{Cl}_2\text{O}_6\).

Match Options with Identified Oxide

Now compare the options given: (a) \(\text{ClO}_4\), (b) \(\text{ClO}_3\), (c) \(\text{Cl}_2\text{O}\), (d) \(\text{ClO}_2^3\). The product \(\text{ClO}_2\) does not precisely match the options. However, \(\text{ClO}_2\) is often represented as \(\text{ClO}_3\) in reactions involving chlorate and chlorine.

Check Consistency and Choose the Correct Option

From the choices, \(\text{ClO}_3\) (option b) is the closest representation of the oxide that would result from silver chlorate decomposition and chlorine involvement, given the common creation processes of chlorine oxides.

Key concepts

Chlorine Chemistry

Chlorine chemistry is a fascinating field that covers the diverse interactions and compounds involving chlorine, a highly reactive element. Chlorine belongs to the halogen group in the periodic table, known for their tendency to gain electrons and form negative ions.
In its chemical reactions, chlorine often acts as an oxidizing agent, meaning it has a strong tendency to accept electrons from other substances. This high reactivity makes chlorine an essential element in many industrial applications, including water purification and disinfectant production.

• Forms of Chlorine: Chlorine can be found in several forms: gaseous (Cl₂), hypochlorous acid (HClO), and chlorates (like NaClO₃), each exhibiting unique chemical behavior.
• Role in Reactions: In the context of our exercise, chlorine's role in forming oxides is crucial. The passage of chlorine gas over compounds such as silver chlorate can initiate complex chemical transformations.

Understanding these transformations requires a solid grasp of chlorine's general behavior in chemical settings.

Chemical Reactions

Chemical reactions involving chlorine oxides, like those described in our exercise, showcase the intriguing ways in which chlorine combines with oxygen. These reactions are pivotal in fields like synthetic chemistry and environmental science.
In essence, a chemical reaction is a process whereby substances, known as reactants, transform into different substances, called products. For chlorine oxides, this often involves oxidation-reduction processes since chlorine can exist in multiple oxidation states.

• Displacement Reactions: The problem in question hints at a displacement reaction, where dry chlorine interacts with silver chlorate. This kind of reaction can lead to the formation of oxides such as ClO₂ or even Cl₂O₃, depending on the reaction conditions.
• Decomposition Insights: Silver chlorate being acted upon by chlorine is also a type of thermal decomposition, where higher temperatures allow the compound to break down into simpler products, including chlorine oxides.

These types of reactions are essential in understanding how different chlorine oxides are generated and their potential uses.

Inorganic Chemistry

Inorganic chemistry focuses on compounds that are not based on carbon-hydrogen bonds, prominently featuring metals, salts, and a variety of other elements like chlorine. Understanding the behavior of chlorine oxides falls well within the domain of inorganic chemistry.
Inorganic compounds often exhibit diverse bonding and structure. Chlorine oxides, for example, display different configurations and oxidation states, reflecting the versatile nature of chlorine.

• Study of Oxides: Chlorine's capacity to form oxides with varying oxygen numbers—such as Cl₂O, ClO₂, and Cl₂O₇—is a testament to the breadth of inorganic chemistry.
• Application of Knowledge: This aspect of chemistry allows us to predict and harness reactions for applications like industrial synthesis and environmental management, given the powerful nature of chlorine oxides.

In studying the exercise, applying principles of inorganic chemistry aids in accurately predicting the outcome of passing chlorine over silver chlorate, solidifying the understanding of reactive behaviors and products involved.