Use the valence bond theory to describe the bonding in the C 2 H 2 Cl 2 molecule

Question

Use the valence bond theory to describe the bonding in the C2H2Cl2 molecule.

A. There are two central atoms, C and C. Both C atoms are attached to one H, one C, and one Cl atom each, and each C atom also has a lone pair of electrons. There are therefore 4 electron groups around each C atom, so the electron-group geometry around each C atom is tetrahedral. To facilitate this geometry, each C atom's orbitals are hybridized as sp3 orbitals. There are therefore 5 sigma bonds and 0 pi bonds in this molecule. B. There are two central atoms, C and C. Both C atoms are attached to one H, one C, and one Cl atom each. There are therefore 3 electron groups around each C atom, so the electron-group geometry around each C atom is trigonal planar. To facilitate this geometry, each C atom's orbitals are hybridized as sp2 orbitals, with one of the sp2 orbitals overlapping with an unhybridized p orbital of a Cl atom, and another sp2 orbital overlapping with the unhybridized s orbital of a H atom, and the third sp2 orbital overlapping with the sp2 orbital of the other C atom. Also, each C atom has its fourth valence electron residing in an unhybridized p orbital, and these unhybridized p orbitals in each C atom overlap with each other to form a pi bond. There are therefore 5 sigma bonds and 1 pi bond in this molecule. C. There are two central atoms, C and C. Both C atoms are attached to one H, one C, and one Cl atom each. There are therefore 3 electron groups around each C atom, so the electron-group geometry around each C atom is trigonal planar. To facilitate this geometry, each C atom's orbitals are hybridized as sp3 orbitals, with one of the sp3 orbitals overlapping with an unhybridized p orbital of a Cl atom, and another sp3 orbital overlapping with the unhybridized s orbital of a H atom, and the third and fourth sp2 orbitals overlapping with the unhybridized p orbitals of the Cl atoms to form pi bonds. There are therefore 5 sigma bonds and 2 pi bonds in this molecule.

Explanation / Answer

B. There are two central atoms, C and C. Both C atoms are attached to one H, one C, and one Cl atom each. There are therefore 3 electron groups around each C atom, so the electron-group geometry around each C atom is trigonal planar. To facilitate this geometry, each C atom's orbitals are hybridized as sp2 orbitals, with one of the sp2 orbitals overlapping with an unhybridized p orbital of a Cl atom, and another sp2 orbital overlapping with the unhybridized s orbital of a H atom, and the third sp2 orbital overlapping with the sp2 orbital of the other C atom. Also, each C atom has its fourth valence electron residing in an unhybridized p orbital, and these unhybridized p orbitals in each C atom overlap with each other to form a pi bond. There are therefore 5 sigma bonds and 1 pi bond in this molecule.

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