Some Important Compounds

Elements that are classified as s-block elements in the Periodic Table are those whose final electron enters the outermost s-orbital. Considering that the s-orbital can only accommodate two electrons, the s-block of the Periodic Table is composed of two groups (1 & 2) that are related to each other. Among the elements that make up Group 1 of the Periodic Table are the following: lithium, sodium, potassium, rubidium, caesium, and francium. The alkali metals are a group of elements that are related to alkali metals. Among the elements that belong to Group 2 are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). With the exception of beryllium, all of these elements are collectively referred to as alkaline earth metals (AEM).

Some of the most important compounds from Group 1 

Sodium Carbonate(Washing Soda)

The Solvay Process is the most common method of producing sodium carbonate. In this process, the low solubility of sodium hydrogencarbonate is exploited, as a result of which it precipitates during the reaction of sodium chloride with ammonium hydrogen carbonate. The latter is made by passing CO2 through a concentrated solution of sodium chloride saturated with ammonia, where it reacts with the ammonium chloride to form ammonium carbonate and then ammonium hydrogen carbonate.

Its physical properties are as follows: sodium carbonate (Na2CO3.10H2O), is a white crystalline solid that exists as a decahydrate. This is referred to as washing soda. It is very easily dissolved in water. When the temperature reaches 373 degrees Celsius, the monohydrate becomes completely anhydrous and transforms into a white powder known as soda ash.

It has a variety of applications, including water softening, laundry, and cleaning. It is used in the production of glass, soap, borax, and caustic soda, among other things. In the paper, paint, and textile industries, it is used as a binder. It is an important laboratory reagent that is used in both qualitative and quantitative applications.

Sodium Chloride,NaCl.

A major source of sodium chloride is seawater, which contains 2.7 to 2.9 percent sodium chloride by mass. Sea water evaporation is the primary method of producing common salt in tropical countries such as India. In order to obtain pure sodium chloride, the crude salt is dissolved in a small amount of water and filtered to remove any insoluble impurities before being concentrated further. Following that, the solution is saturated with hydrogen chloride gas. Crystals of pure sodium chloride are formed during the separation process. As a result of being more soluble than sodium chloride, calcium and magnesium chloride remain in solution.

The melting point of sodium chloride is 1081 degrees K. At 273 degrees K, it has a solubility of 36.0 g per 100 g of water. The solubility does not increase significantly as a function of increasing temperature.

It is used as a common salt or table salt in the home for a variety of purposes. 

Sodium Hydroxide, Caustic Soda, NaOH.

It is generally accepted that sodium hydroxide is produced commercially through the electrolysis of sodium chloride in the Castner-Kellner cell. A brine solution is electrolyzed with a mercury cathode and a carbon anode in order to remove the salt from it. In the presence of mercury, sodium metal discharged at the cathode reacts with it to form sodium amalgam. The anode is responsible for the production of chlorine gas.

Sodium hydroxide is a white, translucent solid that has a corrosive taste. It melts at 591 K. This compound is easily soluble in water and forms a strong alkaline solution when combined with other ingredients. Sodium hydroxide crystals have a deliquescent consistency. 

It is used in the production of soap, paper, artificial silk, and a variety of chemicals, as well as in petroleum refining, bauxite purification, the textile industry (for mercerising cotton fabrics), the preparation of pure fats and oils, and as a laboratory reagent. It is also used in the production of synthetic silk.

Sodium hydrogen carbonate, Baking Soda, NaHCO3.

It is possible to produce sodium hydrogencarbonate by saturating a solution of sodium carbonate in carbon dioxide. Because sodium hydrogencarbonate is less soluble than water, the white crystalline powder is separated from the water.

Sodium hydrogencarbonate is a mild antiseptic that can be used to treat skin infections like acne. It is used in the manufacture of fire extinguishers.

Some of the most important compounds from Group 2 

Calcium Oxide (also known as quicklime, CaO)

It is an important raw material in the production of cement and is the most affordable form of alkali available. It is used in the manufacture of sodium carbonate from caustic soda, which is a byproduct of the process. In addition, it is used in the purification of sugar and the production of dyeing agents and chemicals.

Calcium Hydroxide (Slaked Lime), Ca(OH)2

It is a chemical compound composed of calcium and oxygen. Calcium hydroxide is made by diluting quick lime (CaO) with water and allowing it to dissolve. It is a white amorphous powder with a crystalline structure. It is only a marginally soluble compound in water. Lime water is the aqueous solution of slaked lime, and milk of lime is a suspension of slaked lime in water that is used to make lime water. As a result of the formation of calcium carbonate when carbon dioxide is passed through lime water, the water becomes milky in appearance.

Calcium Carbonate, CaCO3

Calcium carbonate can be found in nature in a variety of forms such as limestone, chalk, marble, and so on. It can be made by passing carbon dioxide through slaked lime or by mixing sodium carbonate and calcium chloride together in a suitable container. An excessive amount of carbon dioxide should be avoided because it can result in the formation of water-soluble calcium hydrogencarbonate.. Calcium carbonate is a powder that is white and fluffy. When it comes to water, it’s almost insoluble. 

Used as a building material in the form of marble as well as in the production of quick lime are among its applications. Specially precipitated calcium carbonate (CaCO3) is widely used in the production of high-quality paper. Besides being an antacid, it’s also used in toothpaste as a mild abrasive, as a component of chewing gum, and as a filler in cosmetics.

Conclusion

A similarity exists between the chemistry of alkaline earth metals and the chemistry and composition of alkali metals. In the case of alkaline earth metals, however, some differences occur as a result of reduced atomic and ionic sizes, as well as increased cationic charges. Their oxides and hydroxides are less basic than the oxides and hydroxides of alkali metals, which is a good thing. Limestone, calcium oxide (lime), calcium hydroxide (slaked lime), calcium sulphate (Plaster of Paris), calcium carbonate (limestone), and cement are some of the most important industrially important calcium compounds.