Consider the following information for sodium and chlorine: Atomic radius: Na (186 pm) and Cl (100pm)...
Consider the following information for sodium and
chlorine:
Atomic radius: Na (186 pm) and Cl (100pm)
Ionic radius: Na+(102pm) and Cl-(181pm)
Why does the atomic radius decrease while ionic radius
increase?
The outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do.
Monatomic ions are bigger than the atoms from which they are formed.
The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do.
The inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion.
The inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do.
Homework Answers
The outermost electrons in chloride experience a smaller effective nuclear charge than those sodium cation do that's why in chloride there is less attraction between outermost electron and nucleus so greater radius
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Consider the following information for sodium and
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Help with explanation if possible.
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