Producing hydrogen atoms from H2 molecules requires 436 kJ/mol to break H-?H bonds. For the longest-?wavelength photon capable of breaking a single H-?H bond, calculate ?. Next, express the energy required to break a single H-?H bond as a percentage of the ground state energy of the hydrogen atom (with electron in the 1s-?orbital). [Hint: the numerical value of the constant RE = R·h·c is 2.18 x 10-?18 J/atom.] Use the Bohr energy En to calculate which n corresponds to the strength of the H-?H bond. [Hint: the n you calculate won't be an integer.] Finally, round up n to the nearest integer. If an electron in energy level n (rounded) of the Hydrogen atom absorbs a photon with wavelength ? (calculated above), how much kinetic energy will it have after it escapes the atom?