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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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All the noble gases are colourless and tasteless monoatomic gases. In general, noble gases are least reactive and their inertness to chemical reactivity is attributed to the following reasons. Reactive and their inertness to chemical reactivity is attributed to the following reasons. (i)Except helium, all have completely filled ns^(2)np^(6) electronic configuration in their valence shells. (ii)All have high ionisation enthalpy and more positive electron gain enthalpy. However, a number of xenon compounds mainly with most electronegative elements like fluorine and oxygen have been synthesized under different conditions and fluorides of xenon have been used as an oxidising agent and a fluorinating agent in many of the chemical reactions Select the correct statement.

All the noble gases are colourless and tasteless monoatomic gases. In general, noble gases are least reactive and their inertness to chemical reactivity is attributed to the following reasons. Reactive and their inertness to chemical reactivity is attributed to the following reasons. (i)Except helium, all have completely filled ns^(2)np^(6) electronic configuration in their valence shells. (ii)All have high ionisation enthalpy and more positive electron gain enthalpy. However, a number of xenon compounds mainly with most electronegative elements like fluorine and oxygen have been synthesized under different conditions and fluorides of xenon have been used as an oxidising agent and a fluorinating agent in many of the chemical reactions The correct order of the abundance of various noble gases in air is :

Statement-1: Second electron gain enthalpy of halogens is always positive. Statement-2: Fluorine has most negative electron gain enthalpy.

Statement-1 :Helium and beryllium both are chemically inert. Statement-2 : Helium and beryllium have similar outer electronic configuration of the type ns^(2)

Statement-1 : Electron gain enthalpy of Cl is largest in periodic table. Statement-2 : Halogen's have largest electron gain enthalpy in a period.

Statement-1: Third ionisation energy of phosphorous is larger than sulphur. Statement-2: There is a larger amount of stability associated with filled s-and p-sub-shells (a noble gas electron configuration) which corresponds to having eight electrons in the valence shell of an atom or ion.

Statement-1 : Ionization energy of s-electrons are more than the p-electrons for the same shell. Statement-2 : s electrons are closer to the nucleus than p-electrons, hence, more tightly attached.

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:

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. Considering the elements B, C, N, F and Si , the correct order of their non-metallic character is:

RESONANCE ENGLISH-P BLOCK ELEMENTS-SINGLE CHOICE TYPE
  1. What are the products formed in the reaction of xenon hexafluoride wit...

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  2. Which of the following pair will give chlorine gas most quickly, upon ...

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  3. Iodine is liberated from KI solution when treated with :

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  4. HI can be prepared by all the following methods except

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  5. Select correct statement(s)

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  6. What products are expected from the disproportionation reaction of hyp...

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  7. Select the correct order(s).

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  8. A solution of KI(3) in water contains :

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  9. Which of the following statement(s) is/are incorrect for noble gases ?

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  10. Statement-1 :Hypochlorous acid (HCIO) acts as a powerful oxidising and...

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  11. Statement-1 : All interhalogens are paramagnetic Statement-2 : AB t...

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  12. Assertion: HClO(4) is a stronger acid than HClO(3). Reason: Oxidati...

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  13. Statement-1 : Fluorine is obtained by the interaction of K2MnF6 with l...

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  14. Statement-1 : Fluorine with sodium hydroxide solution does not undergo...

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  15. Statement-1 : Xenon hexafluoride is kept in silica-lined vessel. Sta...

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  16. Statement-1 : Argon is used in the laboratory for handling substances ...

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  17. Noble gases have very low melting and boiling points because.

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  18. All the noble gases are colourless and tasteless monoatomic gases. In ...

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  19. All the noble gases are colourless and tasteless monoatomic gases. In ...

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  20. Identify the incorrect statement with respect to XeF(2)

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