Oxides of Carbon

INTRODUCTION

Sulfur Oxides 

The oxides of sulphur are inorganic compounds that are entirely composed of atoms of sulphur and oxygen, with no other elements. Sulphur dioxide (SO2) and sulphur trioxide (SO3) are the two most common sulphur oxides found in the Earth’s lower atmosphere, respectively (SO3). 

Sulfur Oxides of Significant Importance

While there are many different types of sulphur oxides, the two most important are as follows:

Sulfur dioxide ,SO2

Sulphur dioxide is one of the most common sulphur oxides that can be found on the earth and even in space, and it is found in large quantities. It is a colourless gas that can be poisonous at times. It is also soluble in water. High concentrations of this gas can be harmful to living things when they are exposed to them. It has the potential to cause negative health effects in humans.

The Physical Characteristics of Sulfur Dioxide

• Sulphur dioxide is a colourless, acidic gas with a pungent and suffocating odour that can be inhaled.
• It can be liquefied with relative ease.
• This substance is highly soluble in water, and its aqueous solution (H2SO3) has a naturally acidic pH.
• It is a powerful reducing agent, and as a result, it reduces halogens to halogen acids, turns acidified K2Cr2O7 solution green, and 

K2Cr2O7+3SO2+H2SO4 → K2SO4+Cr2(SO4)3+H2O

Sulfur Dioxide has a variety of applications.

• Sulfur dioxide is used in the production of H2SO4 (hydrogen peroxide).
• It is employed in the sugar industry for the purpose of refining cane juice.

• For use in fumigation, as a germicide, and as a fruit preservation agent.
• Liquid SO2 is used as a non-aqueous solvent as well as a refrigerant in various applications.

Sulfur trioxide,SO3

When sulphur dioxide is oxidised, the compound sulphur trioxide is frequently formed. This chemical compound can occur in a variety of forms in a white crystalline solid, but it is most common in a white crystalline solid. When it is in liquid form, it has no discernible colour. It is a highly reactive substance that reacts violently with water when exposed to it. The vapour form of sulphur trioxide is considered to be a major pollutant and is one of the components of acid rain when it is present in high concentrations. 

Properties

• It is an acidic oxide that dissolves in water to form the compound H2SO4. The result is that it reacts with CaO to form CaSO4 and decomposes carbonates to release CO2
• Chlorosulphonic (HOSO2CI) acid is formed when it reacts with HCl .
• Because of its strong oxidising properties, it is used in many industries.

Carbon oxides 

When combined with oxygen, carbon produces two important gases: carbon monoxide (CO) and carbon dioxide (CO2). Carbon oxides are important constituents of the atmosphere, and they are also components of the carbon cycle.

Carbon dioxide is naturally produced by the body’s metabolism and respiration, and it is consumed by plants during their photosynthesis process. Since the beginning of the industrial revolution, increased industrial activity has resulted in an increase in carbon dioxide emissions that has lasted for more than a hundred years.

Atomic orbitals  involved in their molecular orbitals

Chemical bonding is more of an interpretation of the molecules in terms of their properties than it is a physical bond. We can begin by reviewing the electronic configurations of carbon and oxygen based on the results of the quantum mechanical approach:

C: 1s2 2s2 2p2

O:  1s2 2s2 2p4

As a result, carbon has four valence electrons, whereas oxygen has six valence electrons Chemical bonding can take place in the s and p atomic orbitals, respectively.

Applications of carbon oxides 

• Carbon oxides are valuable commodities that can be used for a variety of purposes. It is called synthetic gas because it is capable of being converted into methanol when exposed to a catalyst. Synthetic gas is composed of carbon monoxide and hydrogen. Many metal carbonyls have been synthesised over the course of the last few decades. 
• Carbon dioxide can also be used as an industrial gas for a variety of purposes. A large amount of it is used in the food and beverage industry. Here are a few examples of how it can be used.
• Producing carbonated beverages manufacturing urea, CO(NH2)2, as fertiliser promoting plant growth in greenhouse manufacturing dry ice fire extinguishers providing an inert atmosphere for fruit and vegetable preservation using supercritical fluid for solvent extraction manufacturing urea, CO(NH2)2, as fertiliser

Nitrogen Oxides 

It is possible to produce a number of nitrogen oxides when nitrogen reacts with oxygen. Its oxides have a range of oxidation states ranging from +1 to +5, with the majority being +1.  

Dinitrogen oxide, N2O 

Nitrogen oxide is a gaseous compound with neutral properties that is colourless and non-flammable in nature. It is more commonly referred to as “laughing gas.” A high-temperature decomposition of ammonium nitrate yields dinitrogen oxide, which is used to make fertiliser.

NH4NO3 →N2O + H2O

Nitrogen monoxide, NO

Carbon monoxide is a colourless gaseous compound that is formed when oxygen is consumed. Its bonding structure contains an unpaired electron, and it belongs to the class of heteronuclear diatomic molecules, which are diatomic molecules with a single electron. The reduction of dilute nitric acid with copper results in the formation of nitrogen monoxide.

Dinitrogen trioxide ,N2O3

Dinitrogen trioxide (N2O3) is a deep blue solid with an acidic nature that is formed when nitrogen is combined with oxygen. This compound can only be isolated at low temperatures, which means in both the liquid and solid phases. As the temperature rises, the equilibrium favours the formation of constituent gases, which is beneficial to the environment. Dinitrogen trioxide is made by mixing equal parts of nitric oxide and nitrogen dioxide and then cooling the mixture to temperatures below 21 degrees Celsius (6 degrees Fahrenheit).

NO + NO2 → N2O3

Nitrogen dioxide, NO2

Nitrogen dioxide is a toxic gas that is reddish-brown in colour and has a characteristic sharp, biting odour. It is a major air pollutant because of its presence in the atmosphere. It is acidic in nature due to the +4 oxidation state of nitrogen in its composition. Nitrogen dioxide is produced by the thermal decomposition of metal nitrates, such as lead nitrate, in the presence of heat:

2Pb(NO3)2→ 2PbO + 4NO2

Dinitrogen, N2O4

A colourless solid, dinitrogen tetroxide (N2O4) exists in equilibrium with nitrogen dioxide and is a byproduct of the decomposition of nitrogen dioxide. In addition to being a powerful oxidizer, it is also used in the synthesis of many chemical compounds as a reagent.

Dinitrogen Pentoxide, N2O5

N2O5 (dinitrogen pentoxide) is a colourless solid that sublimes at temperatures slightly higher than room temperature. It is an unstable and potentially hazardous oxidizer that was used as a reagent in the process of nitration when dissolved in chloroform. Dinitrogen pentoxide is produced by dehydrating nitric acid (HNO3) in the presence of phosphorus (V) oxide 

CONCLUSION

The oxides of sulphur are inorganic compounds that are entirely composed of atoms of sulphur and oxygen, with no other elements. Sulphur dioxide (SO2) and sulphur trioxide (SO3) are the two most common sulphur oxides found in the Earth’s lower atmosphere, respectively (SO3).When combined with oxygen, carbon produces two important gases: carbon monoxide (CO) and carbon dioxide (CO2). Carbon oxides are important constituents of the atmosphere, and they are also components of the carbon cycle.It is possible to produce a number of nitrogen oxides when nitrogen reacts with oxygen. Its oxides have a range of oxidation states ranging from +1 to +5, with the majority being +1. Nitrogen oxides with nitrogen in the higher oxidation state are more acidic than nitrogen oxides with nitrogen in the lower oxidation state.