Lithium is known to have the smallest size among all alkali metals. This is the primary reason why the Li+ ion has the ability to polarize water molecules more easily when compared to other alkali metals.

Reaction of calcium metal with water – When calcium metal reacts with water, it reacts less violently. It produces a hydroxide known as calcium hydroxide (a cloudy white precipitate), and the bubbles of hydrogen gas produced are stuck to the surface of calcium. Due to which it floats over the water surface.

At room temperature, calcium reacts with oxygen, forming a thin layer of CaO, that protects the metal from further oxidation. Calcium can be ignited and will when burning react with both oxygen and nitrogen forming calcium oxide, CaO, and calcium nitride, Ca3N2.

CaO2

Alkali metals like sodium and potassium are kept in kerosene as they react with moisture and air.

Alkali metals react with water by losing electrons to form a hydroxide. Lithium has the least quantum shells so its outer shell electrons are close to the nucleus. As a result of this attraction, it is hard for lithium to lose electrons. Thus lithium is the least reactive among all Group I metals.

Why does Lithium have High Hydration Enthalpy? The lithium-ion has by far the highest hydration enthalpy in Group 1 and the small fluoride ion has by far the highest hydration enthalpy in Group 7. Lithium exerts the greatest polarizing effect out of all the alkali metals on the negative ion.

The crystalline structure of salt is loose enough to bind to water molecules and become hydrated easily. Sodium chloride or salt tends to absorb the water vapor in the air or contact liquid water.

Hydrates are inorganic salts “containing water molecules combined in a definite ratio as an integral part of the crystal” that are either bound to a metal center or that have crystallized with the metal complex. Such hydrates are also said to contain water of crystallization or water of hydration.

Examples of hydrates are gypsum (commonly used in the manufacturing of wallboard, cement and plaster of Paris), Borax (used in many cosmetic, cleaning and laundry products) and epsom salt (used as a natural remedy and exfoliant). Hydrates are often used in skin care products to infuse moisture into the body.

A hydrated salt is a crystalline salt molecule that is loosely attached to a certain number of water molecules. Salt is created when an acid’s anion and a base’s cation are combined to produce an acid-base molecule. In a hydrated salt, the water molecules are incorporated into the crystalline structure of the salt.

Answer. when water of crystallisation is removed from salt by heating, it becomes anhydrous and its colour changes.

A salt which has a number of water molecules associated with the ions within its crystalline structure is called Hydrated salt. Examples of hydrated salts are: Washing Soda-Na2CO3. 10H2O.

The difference between hydration and hydrolysis is that hydrolysis is the process of breaking of compounds using water, whereas hydration is defined as the electrophilic addition reaction, and there is no cleavage of the original molecule. In hydration, the water molecules are added to the substance.

: a chemical process of decomposition involving the splitting of a bond and the addition of the hydrogen cation and the hydroxide anion of water.

Hydrolysis is an organic chemical reaction that involves adding water to break apart molecules. This reaction is used for both biological and chemical applications. A way to remember the term hydrolysis is to think of ‘reaction with water.

Thus, a hydrolysis reaction is the cleavage of chemical bonds by the addition of water or a base that supplies the hydroxyl ion ( OH−). A chemical bond is cleaved, and two new bonds are formed, each one having either the hydrogen component (H) or the hydroxyl component (OH) of the water molecule.

In both cases, Si is the central atom and have same oxidation state and have same electron density, so, in both cases hydrolysis takes place at same rate.

Dissolving a salt of a weak acid or base in water is an example of a hydrolysis reaction. Strong acids may also be hydrolyzed. For example, dissolving sulfuric acid in water yields hydronium and bisulfate.