For the Benzene (C6H6) Molecule: 1. What is the Electron Geometry? 2. How many Electron Groups? 3. How many bonding groups? 4. What is the number of lone pairs 5. What is the hybridization? 6. Is it polar or non-polar?
The Correct Answer and Explanation is:
Correct Answers for Benzene (C6H6):
- Electron Geometry: Trigonal planar
- Number of Electron Groups: 3 per carbon atom
- Number of Bonding Groups: 3 per carbon atom
- Number of Lone Pairs: 0 on carbon atoms
- Hybridization: sp2
- Polarity: Non-polar
Explanation (300 words):
Benzene (C6H6) is an aromatic hydrocarbon composed of six carbon atoms arranged in a planar ring, with each carbon atom bonded to one hydrogen atom. The bonding in benzene is special due to resonance: the double bonds are not fixed between specific carbon atoms, but instead, the electrons are delocalized around the ring. This delocalization creates a stable, symmetrical structure.
Each carbon atom in benzene forms three sigma bonds — two with neighboring carbon atoms and one with a hydrogen atom. These three bonding regions around each carbon result in an electron geometry of trigonal planar, which is associated with sp2 hybridization. In sp2 hybridization, one s orbital mixes with two p orbitals to form three sp2 hybrid orbitals, which lie in a plane at 120-degree angles. The remaining unhybridized p orbital on each carbon overlaps sideways with neighboring p orbitals to form a delocalized pi system above and below the ring.
Each carbon has three electron groups (the sigma bonds), all of which are bonding groups, and zero lone pairs on the carbon atoms. The hydrogens also contribute no lone pairs to the molecule.
Because of its perfect symmetry and equal distribution of electrons, benzene is non-polar. Even though it contains polar bonds (C–H), their effects cancel out due to the molecule’s planar hexagonal shape, resulting in no net dipole moment.
In conclusion, benzene is a planar, symmetrical molecule with sp2 hybridization, three bonding groups and zero lone pairs per carbon, trigonal planar geometry, and non-polar character due to its even electron distribution.
