Which of the following ions is smallest,why? N^3-,O^2,F
Answers
-ve sign means more of electrons and +ve sign means lack of electrons.
Here N3- with atomic no. 7 has 7+3= 10 electrons
O2- witha tomic no. 8 has 8+2 = 10 electrons
F- with atomic no. 9 has 9+1= 10 electrons
Na+ with atomcatomic no. 11 has 9-1= 10 electrons
Mg2+with atomcatomic no. 12 has 12-2= 10 electrons
Al3+with atomcatomic no. 13 has 13-3= 10 electrons
Since all these ions have 10 electrons in their shell therefore these are isoelectronic speicies
The more + the charge, the smaller the ionic radius. Remember that - means adding electrons. These electrons go in the outermost shells. Also, when an atom loses electrons, it clings ever more tightly to the ones it has left, further reducing the ionic radius. therefore the order of ionic radii will be →
AL3+ Mg2+ Na+ F- O2- N3- (increasing order)
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Answer: The ion with the smallest size is O^2-.
The size of an ion is determined by the electron configuration and the effective nuclear charge. In the case of O^2-, it has 10 electrons, which are distributed in two shells. The effective nuclear charge of O^2- is 8, due to the loss of two electrons. The smaller size of O^2- makes it more stable and less reactive compared to N^3- and F-.
In contrast, N^3- has 11 electrons and a more positive effective nuclear charge of 7, which makes it larger and more reactive. F- has 9 electrons and a more positive effective nuclear charge of 9, which also makes it larger and more reactive.
Therefore, O^2- is the smallest ion among N^3-, O^2-, and F-.
Learn more about electron configuration here
https://brainly.com/question/26084288
Learn more about effective nuclear charge here
https://brainly.in/question/23048070
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