Final answer:
The hybridization of the central carbon atoms in 2-butene is sp2. The approximate energy required to break the C-C bond in 2-butene is 372 kJ/mol or 2.46 x 10^-19 J/molecule. The exact wavelength of light required for the cis-trans isomerization of one molecule of 2-butene cannot be calculated without specific values for Planck's constant and the speed of light.
Step-by-step explanation:
The hybridization of the two central carbon atoms in 2-butene is sp2. The central carbon atoms in the double bond are each bonded to three other atoms, resulting in trigonal planar geometry and sp2 hybridization.
To determine the energy required to break the C-C bond in 2-butene, we can use the table of bond energies. The approximate energy required to break the C-C bond in 2-butene is around 372 kJ/mol or 2.46 x 10^-19 J/molecule.
The wavelength of light required for the cis-trans isomerization of one molecule of 2-butene can be determined using the equation E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. However, we were not provided with specific values for Planck's constant or the speed of light, so it is not possible to calculate the exact wavelength of light required.