Hybridisation of Benzene

Benzene molecular geometry is such that each carbon atom forms two distinct bonds with two carbon atoms during hybridisation. Thus, Benzene has a Trigonal Planar geometry.

Benzene Molecular Geometry

To understand the benzene molecular geometry meaning, we must understand the benzene molecule’s structure. The benzene molecule comprises six carbon atoms arranged in a ring, each containing one hydrogen atom. We classify Benzene as a hydrocarbon because it contains carbon and hydrogen atoms. The sp2 hybridisation of Benzene is present.

Furthermore, each carbon atom forms two distinct bonds with two additional comparable carbon atoms during the hybridisation process instead of only one bond. Thus, with a bond angle of 120°, Benzene has a Trigonal Planar geometry. Also, Benzene has a planar hexagonal structure with all C-atoms sp2 hybridised because of its hexagonal form.

When we look at its structure, we can see that all Carbon-Carbon bonds are the same length. The remaining cyclic array of six p-orbitals (one on each C) overlaps to produce six molecular orbitals, three bonding, and three anti-bonding. For a benzene molecular geometry example, the Lewis structure of Benzene is made up of six carbon atoms arranged in a planar ring with alternate single and double bonds, with each carbon atom connected to a hydrogen atom by a single bond.

The Valence Shell Electron Pair Repulsion Theory (VSEPR) calculates a molecule’s molecular geometry. According to this hypothesis, a molecule’s geometry and structure are determined by minimising repulsion between valence shell electron pairs. Thus, Each carbon atom makes three bonds, two with surrounding carbon atoms and one with the hydrogen atom, as we explained in the Lewis structure. As a result, carbon contains three bonding electron pairs, resulting in trigonal planar geometry.

Hybridisation of Benzene

Pauling and Slater proposed the concept of hybridisation. They claim that blending distinct atomic orbitals with similar energies produces a new set known as “Hybrid orbitals.”

The number of hybrid orbitals created should be the same as that of mixed atomic orbitals. Valence bond theory will help you understand the concept of hybridisation (VBT). According to this idea, when incompletely filled atomic orbitals meet, a chemical bond is established between two atoms.

Thus, the hybridisation of Benzene can be showcased in the following benzene molecular geometry example. We know that the chemical compound benzene comprises multiple carbon and hydrogen atoms. However, the carbon atoms will need one hydrogen and two carbons to form bonds to produce Benzene. Furthermore, the carbon atom does not have enough unpaired electrons to make the bonds.

Thus, the electronic configuration of carbon is 1s2 2s2 2p2, whereas the hydrogen atom has 1s1 in the ground state. However, once excited, the electronic configuration of the carbon atom changes to 1s2 2s1 2px1 2py1 2pz1. It now has four unpaired electrons in its valence shell. These unpaired electrons will be involved in the creation of bonds. However, not all four carbon orbitals are utilised to create bonds in Benzene.

Because each carbon atom has three sigma bonds with two other surrounding carbon atoms and a hydrogen atom and one bond with one of the nearby carbon atoms, each carbon atom is sp2 hybridised and lies in a single plane at an angle of 120°.

The unhybridized 2pz-orbital will lay perpendicular to the hybridised orbital plane. Two lobes, one above and one below the plane, make up this 2pz orbital. This orbital will form by overlapping sideways with the 2pz orbitals of nearby carbon atoms, resulting in the formation of a π-bond. Thus the reason for the stability of the benzene molecule is the delocalization of π-electrons.

Stability of Benzene

In Benzene, the six-membered ring is a perfect hexagon (all carbon-carbon bonds have the same length of 1.40 Å). The cyclohexatriene contributions should have varying bond lengths, with the double bonds (1.34 Å) being shorter than the single bonds (1.54 Å). The pi-electron delocalization in Benzene is highlighted in this alternative form (circle within a hexagon), which has the advantage of being a single diagram. In situations like this, the electron delocalization indicated by resonance improves the stability of the molecules, and compounds made up of these molecules frequently have outstanding stability and associated features.

Measurements of the heat generated when double bonds in a six-carbon ring are hydrogenated (hydrogen is added catalytically) to give cyclohexane as a common product provided evidence for Benzene’s improved thermodynamic stability. Adding hydrogen to cyclohexene yields cyclohexane, which emits 28.6 kcal per mole of heat. On complete hydrogenation, a cyclohexadiene should release 57.2 kcal per mole, and 1,3,5-cyclohexatriene should release 85.8 kcal per mole if this figure represents the energy cost of inserting one double bond into a six-carbon ring. These hydrogenation heats would reflect the relative thermodynamic stability of the compounds.

1,3-cyclohexadiene is slightly more stable than expected, with a 2 kcal difference, owing to double bond conjugation. On the other hand, Benzene is 36 kcal/mole, more stable than predicted. This type of stability improvement is currently considered a property of all aromatic compounds.

Conclusion

Benzene is an organic molecule classified as an aromatic hydrocarbon since its structure is made up entirely of carbon and hydrogen. Benzene is a highly stable compound and is frequently used in the chemical industry as a solvent or an intermediary in synthesising numerous compounds. The benzene molecule comprises six carbon atoms arranged in a ring, each containing one hydrogen atom.

Thus, through these notes, we have studied benzene molecular geometry meaning and benzene molecular geometry examples to understand the hybridisation of Benzene.

Hybridisation of Benzene

Benzene Molecular Geometry