When we shine light on an atom, it can absorbs this radiation, stimulating its electrons to jump to a more energetic energy level. This lasts too little time, and when the electrons come back to their original (fundamental) energy level, they emit the same energy they had absorbed before. This energy levels, though, are quantized. And by what I've understood, the atoms can only ABSORB and emit some discrete frequencies. So, I'm confused about the following: Consider the hydrogen atom. To pass from the n=1 to the n=2 energy level, we need a radiation of 13,6 (1/1² - 1/2²) = 10,2 eV. What would happen if we shine a monochromatic light of energy hf = 10,3 eV? Would the atom absorb that radiation?