Inorganic Chemistry (B.A./B.Sc) 1st Sem Previous Year Solved Question Paper 2022

Isoelectronic species are atoms, ions, or molecules that have the same number of electrons. Despite having different atomic numbers or chemical species, these isoelectronic entities share a common electron configuration, making them similar in terms of electron distribution.

Two examples of isoelectronic species include:

1. O2- (Oxygen Anion) and F- (Fluorine Anion):

 - Oxygen in its neutral state has 8 electrons, while fluorine in its neutral state has 9 electrons. When these atoms gain an extra electron to become anions, they both have 10 electrons. This results in the formation of O2- and F-, which are isoelectronic with 10 electrons each.

2. Neon (Ne) and Fluoride Ion (F-):
 - Neon is an inert gas with 10 electrons in its neutral state. When fluorine gains an electron to form the fluoride ion (F-), it also has 10 electrons. Therefore, Ne and F- are isoelectronic with 10 electrons each.

Isoelectronic species often exhibit similar chemical behavior due to their shared electron configuration, even though they may have different atomic numbers or chemical properties in other respects. This concept is valuable in understanding and predicting the chemical properties of various elements and ions.