Explain the following: Neon is not known to form compounds.
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The reasoning of chemistry of anything follows the observation. The art of explaining the observations is chemistry.
We know that Xe forms some fluoride/chloride compounds (unstable as they may be) but He, Ne, etc do not. Why?
F and Cl are extremely electronegative elements and tend to form F- and Cl- ions easily. In other words, they will form compounds only when they can polarize the electron cloud towards them, ie, cause ionization.
Ionization enthalpy of He is too large. It cannot be suplied by the negative electron gain enthalpy of F/Cl. This is because both electrons in He are in s orbitals, being too close to the powerful nucleus and cannot be easily extracted.
Reasons for Ne are similar.
As you move down the group, the nuclear size increases and so does the distance of the outermost electrons from the nucleus. Corrospondingly, it becomes easier to extract the electron, especially by a powerful electronegative species like F. And bang! there goes your XeF2, XeF4, etc.
Just a matter of energy consideration.
All reactions are a tradeoff between competing forces. In He/Ne, the powerful electrostatic attraction between the electrons and nucleus wins, while in Xe, the powerful electronegativity of F wins.
We know that Xe forms some fluoride/chloride compounds (unstable as they may be) but He, Ne, etc do not. Why?
F and Cl are extremely electronegative elements and tend to form F- and Cl- ions easily. In other words, they will form compounds only when they can polarize the electron cloud towards them, ie, cause ionization.
Ionization enthalpy of He is too large. It cannot be suplied by the negative electron gain enthalpy of F/Cl. This is because both electrons in He are in s orbitals, being too close to the powerful nucleus and cannot be easily extracted.
Reasons for Ne are similar.
As you move down the group, the nuclear size increases and so does the distance of the outermost electrons from the nucleus. Corrospondingly, it becomes easier to extract the electron, especially by a powerful electronegative species like F. And bang! there goes your XeF2, XeF4, etc.
Just a matter of energy consideration.
All reactions are a tradeoff between competing forces. In He/Ne, the powerful electrostatic attraction between the electrons and nucleus wins, while in Xe, the powerful electronegativity of F wins.
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Answered by
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Yes. This statement that Neon is not known to form compounds is true. This is because it is a noble gas and noble gases are not known to form compounds. This is because noble gases have completed their octave, ie they have eight electrons in their outermost shell (duplet, ie two electrons in the outermost shell for helium). So, since, they are stable, they don't need to gain, loose or share electrons with other elements (and even with other atoms of thier own element to form molecules) and thus, don't form compounds or molecules.
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