Given the equation: this equation represents the formation of a (1) fluoride ion, which is smaller in radius than a fluorine atom (2) fluoride ion, which is larger in radius than a fluorine atom (3) fluorine atom, which is smaller in radius than a fluoride ion (4) fluorine atom, which is larger is radius than a fluoride ion

Question

Nancy Martinez

Chemistry

17 March, 22:19

Given the equation: this equation represents the formation of a (1) fluoride ion, which is smaller in radius than a fluorine atom (2) fluoride ion, which is larger in radius than a fluorine atom (3) fluorine atom, which is smaller in radius than a fluoride ion (4) fluorine atom, which is larger is radius than a fluoride ion

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Answers (1)

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Butler · Answer 1

Correct Answer: Option 2 and 3 i. e. (2) fluoride ion, which is larger in radius than a fluorine atom (3) fluorine atom, which is smaller in radius than a fluoride ion

Reason:

Atomic radius of an atom/ion depends upon effective nuclear charge. Atomic radius and effective nuclear charge has inverse relation. When an electron added in a atom, as in the case of F + e - → F-, the effective nuclear charge decreases. This is because, in F atom there are 9 protons and 9 electrons, while in F - ion there are 9 protons and 10 electrons. Since, effective nuclear charge has decreased, the atomic size of F - is more as compared to F atom.