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How to determine if a compound is electron rich, electron precise?


Asked by Dominik Herman on Dec 02, 2021 Electron



BH3, BF3, AlCl3 are examples. Anions are all electron rich and cations are electron deficit. You should always see the no. of electrons before saying if the given compound, if neutral, is electron rich, precise or deficient. In first case, the molecule will have a net negative charge. In second case, the molecule will have no charge.
In fact,
An example is SO2. Sulphur has a total of 10 electrons bounded to it. 4 bond pairs and a lone pair. These act as good Lewis bases. If the central atom has precisely 8 electrons, it’s said to be electron precise, H2O, NH3 all are examples.
Furthermore, For example- NH3 (i) Electron Deficient Hybrides – Group 13 hydrides (Compounds with hydrogen), mainly Hydrides of Al and B are calledelectron deficient hydrides. (ii) Electron Precise Hydride –The type of hydride in which the number of electrons present is equal to the number of electron required (octet or duplet).
Keeping this in consideration,
Electron rich: The type of hydrides which have more number of electrons than required for bonding are called electron-rich hydrides. The excess number of electrons are mainly the lone pair of electrons on the central atom. These types of compounds are usually formed by groups 15, 16 and 17 elements.
Just so,
Electron precise: The type of hydrides that have the exact number of electrons to form a covalent bond are called electron precise. These types of compounds are usually formed by group 14 elements. The compounds usually have a tetrahedral shape. Example CH 4, SiH 4, etc.