Tetravalency of Carbon - Explanation, Properties, FAQs

What is meant by the Tetravalency of Carbon?

Ground state of the carbon kingdom is 1s², 2s², 2p². It has 4 electrons of valence, so the chances of forming four bonds are higher. Bonds formed by s orbital electrons will not be the same as those of orbital electrons. So in building one CH₄ molecule, there will be a combination of 1 C atom with 4 H. atoms.

The following types of bonds can be formed: C (s) -H (s), C (s) -H (s), C (p) -H (s) and C (p) -H (s). Of the four bonds, we have two ‘directing’ methods C (p) -H (s) and two non-directing bonds C (s) -H (s). (Note: Since we know that orbitals are round and have no direction and p orbitals have three sides x, y, and z-axis.) Bond strength will also vary as C (p) - H (s) bond ) will be slightly stronger than the C (s) -H (s) bond as the spacing is strong.

But almost all CH₄ bonds are the same. This creates a problem. To solve this problem, hybridization theory is proposed. It makes sense especially when atomic orbitals are mixed with new hybrid orbitals that are well suited to electron bonding to form chemical bonds. three p and one s-orbital combined to give four sp³ combined orbitals.

Similarly, we can also get sp and sp² hybridization. The only change will be that sp² will have only two p orbit. Now from the VSEPR concept, we know that sp and sp² compound molecules are organized. While the combined sp³ molecules take up the tetrahedral structure to become more stable (this structure leads to a lower energy state).

The angle present between each carbon atom and hydrogen atom is 109.5 in tetrahedral geometry, 120 in sp2 and 180 in sp hybridization. Methane will therefore have sp³ hybridization with a tetrahedral shape. While the examples of sp and sp² hybridization are acetylene and ethene in a planar sequence. We can now clearly understand that ethane will have two unmixed p orbital from each sp² carbon that will interact with each other to form a pi bond. So with this, we can see that double bonding is just a combination of two unmarried bonds.

Due to certain features of the material, Carbon has established its value among other things.

The factors that make carbon very important are:

Catenation

Tetravalency

Carbon atom size

Although there is no specific definition, compounds that are solid, liquid or air containing carbon atoms attached to their molecules are known as organic compounds. Let’s see how the soft carbon environment affects carbon.

Also read -

• NCERT Solutions for Class 11 Chemistry
• NCERT Solutions for Class 12 Chemistry
• NCERT Solutions for All Subjects

Tetravalency Definition:

Tetravalency meaning: "The element that is capable of bonding with other atoms of elements or with the atoms of other monovalent element is known as Tetravalency" or a tetravalence is state of an atom with four electrons available for covalent chemical bonding in its valence.

• mention about 4 bonds in definition

For Example: carbon has valency four so it is capable of bonding to other four atoms of carbon

Tetravalency Meaning:

The situation of having a valency of four (4) is known as Tetravalency.

Valency of carbon in Carbon dioxide

CO₂ is a carbon dioxide that contains carbon and oxygen in a ratio 1: 2. In the electron dot structure of matter carbon shares two of its electrons with oxygen. Carbon needs only four electrons to stabilize, and oxygen needs 2 electrons. Therefore, the valency of carbon in CO₂ is 4. Carbon cannot have a valency of 2 and the valency of carbon is four. Because the carbon and oxygen between the two pi bond bonds is the carbon atom in hand 2 electrons and the other 2 electrons share oxygen atoms. Any time the carbon in the valency of cells is four. At any other time the carbon atom that makes the extra free electron attached to the carbon atom valency has four but it works for a good charge.

Carbon synthesis

Hybridization is the idea of assembling atomic orbitals to make new hybrid orbital suitable to represent their binding sites. Combined orbital aids help to explain the formation of cellular orbitals without being a major part of the valence bond concept. The word hybrid applies to atomic orbitals that contribute to merging. For example, in methane its chemical formula CH₄, a group of sp³ orbitals grows by combining one s-orbital with three p-orbitals in a carbon atom. These orbitals are directly related to the four hydrogen atoms placed on top of a standard tetrahedron. Ethene (C₂H₄) contains a double bond between carbon atoms. Here, carbon combines in sp².

In sp² hybridization, 2s orbital have two of the three 2p orbital available which forms a complete 3sp² orbital with a p-orbital left. In ethane, two carbon atoms form a sigma bond by attaching two sp² orbital bonds, whereas every carbon atom forms two bonds that combine with hydrogen by dividing all s-sp² at 120o angles.

The pi bond between carbon atoms grows by a combination of 2p-2p. Hydrogen-carbon bonds of equal length and strength satisfy the experimental evidence. Many bonds exist between different atoms. When two oxygen atoms are brought towards the opposite sides of a carbon atom in CO₂, one atom between the p orbitals in the oxygen forms a binding bond with any atom present between the p-orbitals of carbon. Here, sp hybridization forms two double bonds.

What is catenation?

It can be defined as the atomic bonding of the atoms of an object to form chains and bracelets. This definition can be expanded to include layouts such as two-dimensional catenation and space lattices similar to a three-dimensional catenation.

The most common examples of organic catenation are:

Carbon

Silicon

Sulfur

Boron

Childbirth occurs easily in carbon, forming bonds that form long chains and structures with other carbon atoms. That is why a large number of organic compounds are found in nature. Carbon is best known for its food, for its analysis of carbon-soluble chemical structures. Carbon is not the only material capable of forming such catenae, however, and many other key elements of the group are capable of forming a wide variety of catenae, including silicon, sulfur and boron.

Also Read:

• NCERT solutions for Class 11 Chemistry Chapter 13 Hydrocarbons
• NCERT Exemplar Class 11 Chemistry Solutions Chapter 13 Hydrocarbons
• NCERT notes Class 11 Chemistry Chapter 13 Hydrocarbons

Property of catenation in Group 4

All items of the carbon family or of the fourth family group show photography material. The first member from the family has a very high tendency to soften.

The following are interesting trends:

C> Si> Ge> Sn> Pb

The tendency to give birth reduces the group. This is because the size of the atom increases down in the group and the strength of the covalent bond decreases. Therefore, the catenation property reduces the group.

What is the tendency to get caught in C, Si, and Ge?

The tendency for catenation detection in C, Si, and Ge is as follows: Ge <Si <C

Ge bond strength is very low so the tendency to catch food is very low. Also, an increase in the size and length of the bond will lead to a reduction in the tendency to get caught.

Also check-

• NCERT Exemplar Class 11th Chemistry Solutions
• NCERT Exemplar Class 12th Chemistry Solutions
• NCERT Exemplar Solutions for All Subjects

NCERT Chemistry Notes:

• NCERT Notes Class 11th Chemistry
• NCERT Notes Class 12th Chemistry
• NCERT Notes For All Subjects