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Statement-1 : Argon is used in the labor...

Statement-1 : Argon is used in the laboratory for handling substances that are air-sensitive.
Statement-2 : Argon is inert towards chemical reactivity due to the completely filled valence shell electronic configuration, high ionization enthalpy and more positive electron gain enthalpy.

A

Statement-1 is True, Statement-2 is True,Statement-2 is a correct explanation for Statement-1.

B

Statement-1 is True, Statement-2 is True,Statement-2 is NOT a correct explanation for Statement-1.

C

Statement-1 is True, Statement-2 is False

D

Statement-1 is False, Statement-2 is True

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the statements regarding Argon, let's break down the reasoning step by step: ### Step 1: Understanding Statement 1 **Statement 1**: Argon is used in the laboratory for handling substances that are air-sensitive. - **Explanation**: Air-sensitive substances are those that react with components of air, such as oxygen and moisture. Argon, being a noble gas, does not react with these components, making it an ideal atmosphere for handling such substances. ### Step 2: Understanding Statement 2 **Statement 2**: Argon is inert towards chemical reactivity due to the completely filled valence shell electronic configuration, high ionization enthalpy, and more positive electron gain enthalpy. - **Explanation**: Argon has a complete octet in its valence shell (8 electrons), which makes it stable and unreactive. The high ionization enthalpy means that it requires a lot of energy to remove an electron from Argon, and the positive electron gain enthalpy indicates that it does not readily accept additional electrons. This combination of factors contributes to its inertness. ### Step 3: Evaluating the Truth of Statements - Both statements are true: - **Statement 1** is true because Argon is used to create an inert atmosphere for air-sensitive reactions. - **Statement 2** is true because Argon's electronic configuration and energy properties explain its lack of reactivity. ### Step 4: Establishing the Relationship Between the Statements - **Explanation**: Statement 2 provides the reason for the truth of Statement 1. Since Argon is inert due to its electronic configuration and energy properties, it is suitable for handling air-sensitive substances. ### Conclusion Both statements are true, and Statement 2 correctly explains Statement 1. Therefore, the correct option is that both statements are true, and Statement 2 is the correct explanation for Statement 1. ---
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The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words, the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group, the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour, and also with metallic and non-metallic character respectively, of the elements. Which of the following statements is correct?

The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words, the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group, the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour, and also with metallic and non-metallic character respectively, of the elements. The correct order of the metallic character is:

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