Chemical Reactivity of Calcium Carbonate with Halogen

One of the most important calcium compounds is calcium carbonate, often known as CaCO3, which is a major constituent of many minerals and plants, including limestone, marble, chalk, oyster shells, and coral. Calcium carbonate acquired from natural sources is used as a filler in a number of goods, including ceramics, glass, plastics, and paint, as well as a raw material in the manufacturing of calcium oxide. It is also used as a beginning material in the creation of calcium oxide. Synthetic calcium carbonate, sometimes known as “precipitated” calcium carbonate, is used in applications where high purity is required, such as in medicine (antacids and dietary calcium supplements), food (baking powder), and laboratory research and development.

Reaction of Halogen and Calcium Carbonate

Halogens

Group 17 includes halogen elements including fluorine, chlorine, bromine, iodine, and astatine. FLUORINE (Yellow) CHlorine (Green) Bromine (Red) and Iodine (Purple) are all gasses at ambient temperature. As a radioactive element, astatine can only be found in very minute levels in nature. As diatomic molecules, all of the halogens are known. They have large ionization energies and are the most electronegative elements. ns2np5 electron arrangement allows them to react easily with Group 1 and 2 metal; each halogen is likely to pick up one electron and each Group 1 or Group 2 element is likely to lose one or two electrons. As a result, metals in Groups 1 and 2 of all the main group elements have the strongest reactions with halogens.

Alkaline Earth metals

When alkaline earth metals react, hydrated halides are produced. These halides, with the exception of those containing beryllium, are ionic (the least metallic of the group). Due to the fact that alkaline earth metals prefer to lose electrons and halogen atoms tend to gain electrons, the following chemical reaction occurs between these two groups:

M + X2 → MX2

Where, M denotes any Group 2 metal and

X denotes fluorine, chlorine, bromine, or iodine.

Calcium chloride anhydrous has a strong affinity for water, absorbing sufficient to dissolve its own crystal lattice. It can be synthesised either directly from limestone or as a by-product of the Solvay Process.

Calcium rapidly interacts with halogens to generate their dihalides. Exothermic reactions occur with fluorine and chlorine, whereas endothermic reactions occur with bromine and iodine.

Ca(s) + F2(g)  →  CaF2(s)

Ca(s) + Cl2(g)  →  CaCl2(s)

Ca(s) + Br2(g)  →  CaBr2(s)

Ca(s) + I2(g)  →  CaI2(s)

Commercial Production of Calcium carbonate 

Calcium carbonate is commercially available in two grades. Industrially, both grades compete on the basis of particle size and the features imparted to a product.

Ground Calcium Carbonate – Calcium carbonate that has been extracted and processed from naturally occurring deposits. GCC crystals are rhombohedral in form and have a larger size distribution.

Calcium Carbonate Precipitated — Calcium carbonate precipitated chemically via a carbocation process or as a by-product of certain bulk chemical operations. PCC crystal structure varies according to the product, but the particles are more uniform and regular in size distribution.

PCC has finer particles, a greater purity, is less abrasive, and typically has a brighter appearance than GCC.

Physical properties of Calcium carbonate

• Calcium Carbonate is a powdery substance.
• When heated to 1200K, it decomposes to generate carbon dioxide.
• When it combines with dilute acid, it produces carbon dioxide as a by-product.
• Calcium carbonate decomposes at a temperature of 1200K to generate calcium oxide and carbon dioxide.
• Calcium carbonate creates carbon dioxide when it reacts with dilute acids.
• The molecular weight of CaCO3 is 100.0869 g/mol.

Reaction of calcium carbonate with fluorine

CaCO3 is quickly turned into CaF2 when a KF solution is used at room temperature to make it. The reaction of microcrystalline calcium carbonate powder with potassium fluoride solution is being looked into. This happens at room temperature and makes a white powder that flows. The reaction of microcrystalline calcium carbonate powder with potassium fluoride solution is being looked into. This happens at room temperature and makes a white powder that flows.

CaCO3 + KF (soln.) →  CaF2

Reaction of calcium carbonate with chlorine

Hypochlorous acid and calcium chloride are generated when chlorine is added to water containing calcium carbonate in suspension, with carbon dioxide being released, and the hypochlorous acid and calcium chloride can be separated by distillation.

CaCO3 + 2Cl2 + H2O → CaCl2 + 2HClO + CO2

Reaction of calcium carbonate with bromine

CaCO3 + Br2 →  CaBr + CO3

Reaction of calcium carbonate with iodine

When calcium carbonate interacts with potassium iodide, potassium carbonate (potash) and calcium iodide are formed. This is an example of a Displacement reaction.

CaCO3 + 2KI → CaI2 + K2CO3

CONCLUSION

In this article we learned about the various properties and reactions that occur between calcium carbonate and halogens along with some physical properties of CaCO3 and some commercial production methods of it. 

Calcium carbonate is a very common chemical that is initially encountered in school classrooms due to the widespread use of chalk (a type of CaCO3). Additionally, it is found in a variety of forms, including marble and limestone. Although they come in a variety of shapes, they are chemically the same and only physically differ. Additionally, they are referred to as calcite.

It is also one of the most widely used compounds, initially encountered in school classrooms, where chalk (a type of CaCO3) is used. It is found in the earth’s crust. It is available in a variety of forms, including limestone and marble. Although they come in a variety of shapes, they are chemically the same and only physically differ.