Question

What is the approximate $ H - C - H $ bond angle in $ C{H_3}^ + $ ?

Answer 1

Hint :The angle between two bonds or the angle between two orbitals that hold a pair of bonding electrons around the central atom in a complex molecule or an ion, is known as the bond angle. This angle is generally determined using the spectroscopic process and the result is computed in degrees. This angle helps to determine the shape of the molecules by providing a precise picture of the distribution of the bonded electron pairs around the atoms. It also determines the form of the molecules.

Complete Step By Step Answer:
The geometry of the carbon atom is dependent on the hybridization of the carbon atom. Hybridization is the process of combining two atomic orbitals with the same energy levels to produce a degenerated new class of orbitals. Quantum mechanics is used to explain this intermixing. The ion $ C{H_3}^ + $ contains a carbon atom that is $ s{p^2} $ hybridized. As a result of the hybridized carbon, the geometry of this atom is trigonal planar. The $ H - C - H $ bond angle is $ {120^ \circ } $ in this situation. However, the carbon atom in $ C{H_4} $ is a $ s{p^3} $ hybridized carbon, the structure around it is tetrahedral. The $ H - C - H $ bond angle is $ {100.5^ \circ } $ in this situation.
Thus, the $ H - C - H $ bond angle is $ {120^ \circ } $ in the $ C{H_3}^ + $ ion.

Note :
The ion $ C{H_3}^ + $ is known as Methylium or the methyl cation and has a molecular weight of $ 15.035 $ gram per mole. It is a vacation. The methyl cation is trigonal planar shaped as its carbon atom is $ s{p^2} $ hybridized and no lone pair is present .