ionic radius of cs

Ionic Radius - It is defined as the distance from the centre of the nucleus upto the last shell containing the electro..

It is defined as the distance from the centre of the nucleus upto the last shell containing the electron..

Being the first elements of each period, alkali metals have the largest atomic and ionic radii in their respective periods. As we move within a period, the atomic radius and ionic radius tend to decrease due to increase in the effective nuclear charge. On mo..

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 distance ..

The atomic and ionic radii of alkaline Earth metals are smaller than the corresponding members of the alkali metals. This is due to the fact of Group 2 elements having a higher nuclear charge allow electrons to be attracted more towards the nucleus. This reduces the size of atomic and ..

Ionic hydrides are white or light grey crystalline solids. They behave like salts. They have high melting and boiling points. They conduct electricity in fused state liberating hydrogen at the anode. The negative charge of the hydrogen on them is proved by electrolysis of molten l..

Crystal structure Examples Co-ordination number Number of formula units per unit cell Rock Salt (NaCl) Type Halides of Li, Na, K, Rb, AgF, AgBr Na + = 6 Cl - = 6 4 Caesium Chloride type CsCl, CsBr, CsI, TiCl, TiBr, Til ..

Radius Ratio Rules - For the stability of an ionic compound, each cation should be surrounded by maximum number of anions and vice versa. The number of oppositely charged ions surrounding each ion is called its co-ordination number. The larger is the size of the cation the great..

This type of defect is shown by highly ionic compounds which have High coordination number Cations and anions of similar sizes Examples: KCl, NaCl, KBr and Cs..

The alkali metal ions are highly hydrated. The smaller the size of the ion, the greater is the degree of hydration. Thus, Li + ion gets much more hydrated than Na + ion which in turn is more hydrated than K + ion and so on. The extent of hydration decreases down the group. As a result of larger..