) Consider the below statements about N3-, O2- and F- ions. i. They have the same electronic configuration. ii. The order of nuclear charge is N3-<O2-<F- iii. The order of radii is N3-<O2-<F- Select the correct answer about the true statements. A) Only i is true. B) Only iii is true. C) Both i and ii are true. D) Both i and iii are true. E) All i, ii and iii are true.
Question
) Consider the below statements about N3-, O2- and F- ions.
i. They have the same electronic configuration. ii. The order of nuclear charge is N3-<O2-<F- iii. The order of radii is N3-<O2-<F-
Select the correct answer about the true statements. A) Only i is true. B) Only iii is true. C) Both i and ii are true. D) Both i and iii are true. E) All i, ii and iii are true.
Solution
Let's analyze each statement:
i. They have the same electronic configuration.
N3-, O2-, and F- all have the same electron configuration as the noble gas Neon (Ne), which is 1s2 2s2 2p6. So, this statement is true.
ii. The order of nuclear charge is N3-<O2-<F-
The nuclear charge is the charge of the nucleus, which is equal to the number of protons. Nitrogen (N) has 7 protons, Oxygen (O) has 8, and Fluorine (F) has 9. Therefore, the order of nuclear charge is indeed N3-<O2-<F-. This statement is also true.
iii. The order of radii is N3-<O2-<F-
The size of an ion is determined by the number of electron shells and the effective nuclear charge. In this case, all three ions have the same number of electron shells, so the size is determined by the effective nuclear charge. The greater the nuclear charge, the smaller the ion, because the electrons are pulled closer to the nucleus. Therefore, the order of radii is actually N3->O2->F-, not N3-<O2-<F-. This statement is false.
So, the correct answer is:
C) Both i and ii are true.
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