Chemistry

Problem

A photon with energy

4.0\times10^{-19}\,\text{J}

is absorbed by a molecule. Which of the following transitions is the absorption most likely to cause? (Use

h=6.63\times10^{-34}\,\text{J\,s}

and

c=3.00\times10^{8}\,\text{m\,s}^{-1}

if needed.) a) A vibrational transition of a polar bond b) Ionization of the molecule by removing a valence electron c) An electronic transition producing an excited electronic state d) A rotational transition that changes the

J

quantum number by 1

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