factors influencing the stability of ionic compounds

Low ionisation energy Ionisation energy is the amount of energy, which is required to remove the most loosely bound electron(s) from an isolated gaseous atom to form a positive ion. In forming an ionic bond, one atom must form a cation by losing one or more electrons. In gene..

The inter-ionic attraction - It is the intersection between the ions of the solute at low concentrations. It is not much at low concentrations the inter-ionic cone is very less, but at high concentrations it is appreciable. fig 5.1 The negative ion is pulled to the negative pole..

Influence on the Reactions of other Functional Groups - The presence of nitro group facilitates nucleophilic substitution of otherwise unreactive aromatic halides by stabilizing the intermediate carbanio..

Factors Influencing the Formation of an Ionic Bond - The conditions which favour the formation of an ionic bond a..

Ionic Radii - These are radii of ions in ionic crystals. Ionic radius may be defined as the effective distance from the center of nucleus of an ion up to which it has an influence on its electron cloud. In ionic compounds the inter nuclear..

High ionisation energy Elements that have higher ionisation energies cannot form ionic bonds, as they cannot lose electrons easily. Instead, they acquire stability by mutual sharing of electrons, and therefore form covalent bond..

such as linear, triangular, square planar, pyramidal, octahedral etc. The shape of a molecule affects its chemical and physical properties. For instance, some of the unique properties of water are due to the angular shape of its molecule (H 2 O). The stability and the self-replicating pro..

. This is due to the inert pair effect. The elements in their lower oxidation state of + 2 are expected to form ionic bonds whereas in the higher oxidation state of + 4 these can form only covalent bonds in their compounds. This indirectly means that as we move down the group, t..

As in the case of S, the important oxidation states observed for Se and Te are also 2, +2, +4 and +6. The chalcogenide dianions (E 2 - ) exist only in their compounds with the most electropositive elements. By and large, chalcogens with the exception of polonium, display non-metallic cova..

Some important group trends are: (a) On account of high ionization enthalpies, simple M 4 + ions of the group are not known. (b) Unlike carbon the other elements of the group form compounds having coordination numbers higher than 4 like (SiF 5 ) - , (SiF 6 ) 2 - and (PbCl 6 ) 2 - . (c) In..