What is carbon monoxide? The structure of the molecule

Carbon monoxide, also known as carbon monoxide, has a very strong molecular composition, is inert in its chemical properties and poorly soluble in water. This compound is also incredibly toxic, when it enters the respiratory system, it combines with the hemoglobin of the blood, and it stops transferring oxygen to tissues and organs.

Chemical names and formula

Carbon monoxide is also known under other names, including carbon monoxide II. In everyday life it is usually called carbon monoxide. This carbon monoxide is a toxic, colorless and tasteless gas that is odorless. Its chemical formula is CO, and the mass of one molecule is 28.01 g / mol.

Effects on the body

Carbon monoxide combines with hemoglobin to form carboxyhemoglobin, which has no oxygen capacity. Inhalation of its vapors causes damage to the central nervous system (CNS) and suffocation. The resulting lack of oxygen causes headache, dizziness, decreased pulse and respiratory rate, leading to fainting and subsequent death of the body.

Toxic gas

Carbon monoxide is produced by the partial combustion of substances containing carbon, for example, in internal combustion engines. The compound contains 1 carbon atom, covalently bound to 1 oxygen atom. Carbon monoxide is very toxic, and this is one of the most common causes of fatal poisonings around the world. Exposure can lead to damage to the heart and other organs.

What is the use of carbon monoxide?

Despite its serious toxicity, carbon monoxide is extremely useful - thanks to modern technology, a number of vital products are created from it. Carbon monoxide, although today considered a pollutant, has always been present in nature, but not in such quantities as, for example, carbon dioxide.

Errors are those who believe that there is no carbon monoxide compound in nature. CO dissolves in molten volcanic rock at high pressures in the earth's mantle. The content of carbon oxides in volcanic gases varies from less than 0.01% to 2%, depending on the volcano. Since the natural of this compound is not a constant value, it is not possible to accurately measure natural gas emissions.

Chemical properties

Carbon monoxide (CO formula) refers to non-salt-forming or indifferent oxides. However, at a temperature of +200 ^o C it reacts with sodium hydroxide. During this chemical process , sodium formate is formed:

NaOH + CO = HCOONa (salt of formic acid).

The properties of carbon monoxide are based on its reducing ability. Carbon monoxide:

• Can react with oxygen: 2CO + O ₂ = 2CO _2;
• Is able to react with halogens: CO + Cl ₂ = COCl ₂ (phosgene);
• Has a unique property to recover pure metals from their oxides: Fe ₂ O ₃ + 3CO = 2Fe + 3CO _2;
• Forms carbonyls of metals: Fe + 5CO = Fe (CO) _5;
• Perfectly soluble in chloroform, acetic acid, ethanol, ammonium hydroxide and benzene.

Molecule structure

Two atoms, of which, in fact, the carbon monoxide (CO) molecule consists, are connected by a triple bond. Two of them are formed by the fusion of p-electrons of carbon atoms with oxygen, and the third is due to a special mechanism due to the free 2p-orbitals of carbon and 2p-electron oxygen pairs. This structure provides the molecule with high strength.

A bit of history

Even Aristotle from ancient Greece described the toxic fumes produced by burning coals. The mechanism of death itself was not known. However, one of the ancient methods of execution was the locking of the transgressing law in the steam room, where the embers were located. Greek physician Galen suggested that some changes occur in the air that cause harm when inhaled.

During the Second World War, a gas mixture with carbon monoxide admixtures was used as fuel for motor vehicles in parts of the world where there was a limited amount of gasoline and diesel fuel. Externally (with some exceptions) generators of charcoal or wood gas were installed, and a mixture of atmospheric nitrogen, carbon monoxide and a small amount of other gases was supplied to the gas mixer. This was the so-called wood gas.

Oxidation of carbon monoxide

Carbon monoxide is formed by partial oxidation of carbon-containing compounds. CO is formed when oxygen is not sufficient to produce carbon dioxide (CO ₂ ), for example, when a kiln or an internal combustion engine is operating in an enclosed space. If oxygen is present, as well as some other atmospheric concentrations, carbon monoxide burns, emitting blue light, forming carbon dioxide, known as carbon dioxide.

Coal gas, widely used prior to the 1960s of the last century for indoor lighting, cooking and heating, had CO in its composition as an advantageous fuel component. Some processes in modern technologies, such as iron smelting, still produce carbon monoxide as a by-product. The very CO compound is oxidized to CO ₂ at room temperature.

Is there a CO in nature?

Is there carbon monoxide in nature? One of its naturally occurring sources is photochemical reactions occurring in the troposphere. These processes are supposed to generate about 5 × 10 ¹² kg of substance e. Other sources, as mentioned above, are volcanoes, forest fires and other types of burning.

Molecular properties

Carbon monoxide has a molar mass of 28.0, which makes it slightly less dense than air. The length of the bond between the two atoms is 112.8 micrometers. It is close enough that it provides one of the most powerful chemical bonds. Both elements in the CO compound together have about 10 electrons in one valence shell.

As a rule, a double bond arises in organic carbonyl compounds. A characteristic feature of the CO molecule is that between the atoms there is a strong triple bond with 6 common electrons in 3 bound molecular orbitals. Since 4 of the common electrons originate from an oxygen atom and only 2 from carbon, one bound orbital is occupied by two electrons from O ₂ , forming a dative or dipole bond. This causes the polarization C ← O of a molecule with a small charge of "-" on carbon and a small charge of "+" on oxygen.

The remaining two connected orbitals occupy one charged particle from carbon and one from oxygen. The molecule is asymmetric: oxygen has a larger electron density than carbon, and is also slightly positively charged compared to negative carbon.

Receiving

In the industry, the production of carbon monoxide CO is carried out by heating without access of air to carbon dioxide or water vapor with coal:

СО ₂ + С = 2СО;

H ₂ O + C = CO + H _2.

The last mixture obtained is also called water or synthesis gas. In laboratory conditions, carbon monoxide II by exposing organic acids to concentrated sulfuric acid, which acts as a water-removal agent:

HCOOH = CO + H ₂ O;

H ₂ C ₂ O ₄ = CO ₂ + H ₂ O.

The main symptoms and help in poisoning CO

Is carbon monoxide poisoning? Yes, and very strong. Carbon monoxide poisoning is the most frequent phenomenon in the world. The most common symptoms are:

• Feeling of weakness;
• nausea;
• dizziness;
• fatigue;
• irritability;
• Poor appetite;
• headache;
• disorientation;
• Impaired vision;
• Vomiting;
• fainting;
• Convulsions.

The exposure to this toxic gas can lead to significant damage, which can often lead to prolonged chronic pathological conditions. Carbon monoxide can cause serious damage to the fetus of a pregnant woman. Victims, for example, after a fire, should be given immediate assistance. Urgently need to call an ambulance, give access to fresh air, remove the shortness of clothing, calm, warm. Severe poisoning, as a rule, is treated only under the supervision of doctors, in the hospital.

Application

Carbon monoxide, as already said, is toxic and dangerous, but it is one of the basic compounds that are used in modern industry for organic synthesis. CO is used to produce pure metals, carbonyls, phosgene, carbon sulphoxide, methyl alcohol, formamide, aromatic aldehydes, formic acid. This substance is also used as fuel. Despite its toxicity and toxicity, it is often used as a raw material for obtaining various substances in the chemical industry.

Carbon monoxide and carbon dioxide: what's the difference?

Monoxide and carbon dioxide (CO and CO ₂ ) are often mistaken for each other. Both gases are odorless and colorless, and both have a negative effect on the cardiovascular system. Both gases can enter the body through inhalation, skin and eyes. These compounds, when exposed to a living organism, have a number of common symptoms - headaches, dizziness, convulsions and hallucinations. Most people have difficulty in determining the difference and do not understand that car exhausts emit both CO and CO ₂ . Indoors, an increase in the concentration of these gases can be dangerous to the health and safety of a person exposed to them. What is the difference?

At high concentrations, both can be fatal. The difference is that CO ₂ is the common natural gas necessary for all plant and animal life. CO is not a common occurrence. This is a by-product of anoxic fuel combustion. The critical chemical difference is that CO ₂ contains one carbon atom and two oxygen atoms, whereas CO only has one. Carbon dioxide is non-flammable, while monoxide has a high probability of ignition.

Carbon dioxide naturally occurs in the atmosphere: people and animals breathe oxygen and exhale carbon dioxide, that is, living beings are able to withstand it in small amounts. This gas is also necessary for the realization of photosynthesis by plants. However, carbon monoxide does not naturally arise in the atmosphere and can cause health problems even at low concentrations. The density of both gases is also different. Carbon dioxide is heavier and denser than air, while carbon monoxide is slightly lighter. This feature should be taken into account when installing the appropriate sensors in the homes.