Question:
: Noble gases have positive electron affinity.
: Noble gases have stable closed shell electronic configuration.
: Noble gases have positive electron affinity.
: Noble gases have stable closed shell electronic configuration.
Updated On: Jul 28, 2022
- If both Assertion: and Reason: are true and the Reason: is the correct explanation of the Assertion:
- If both Assertion: and Reason: are true but the Reason: is not the correct explanation of the Assertion:
- If Assertion: is true but Reason: is false
- If both Assertion: and Reason: are false
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The Correct Option is A
Solution and Explanation
Noble gases have stable closed shell electronic configuration. Thus, in order to add an electron to an isolated noble gas atom, energy have to given. Hence, noble gases have positive electron affinity. Hence, Reason: is correct for Assertion:.
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Concepts Used:
Group 18 Elements
The Group 18 elements, also known as noble gases except for Helium, are inert in nature because they have completely filled ns2 np6 electronic configuration in their valence shells. These gases also have high ionization enthalpy and more positive electron gain enthalpy. All these elements are chemically unreactive i.e. they don’t form many compounds.
Group 18 Elements consist of six elements. They are as mentioned below:
- Helium (He)
- Neon (Ne)
- Argon (Ar)
- Krypton (Kr)
- Xenon (Xe)
- Radon (Rn)
Electronic Configuration:
The electronic configuration of Group 18 Elements along with their symbol and atomic number is given in the tabulated form below:
Trends in the Atomic Properties:
- Atomic Radius: The nuclear radii increment on moving down the group with increasing nuclear number. This is a result of the expansion of another shell at each progressive element on moving down the group.
- Electron Gain Enthalpy: Group 18 elements exhibit very stable electronic configurations. They do not have any tendency to accept an electron.
- Ionisation Potential: They have high ionisation potentials, thanks to their closed electronic configurations. This value decreases on moving down the group due to an expansion in the nuclear size.