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Neils Bohr’s model of the hydrogen atom explained the unique set of spectral emission or absorbtion...

Neils Bohr’s model of the hydrogen atom explained the unique set of spectral emission or absorbtion lines seen for hydrogen or other atoms. Pick the statment that best summarizes the model. 1. The electrons all formed one single continuous ring around the nucleus. When light was shone at the atom, this ring expanded. Becuase the electrons were further apart and higher in energy, light was absorbed as this happened. The color of light absorbed was related to the number of electrons in the ring. 2. The electrons were trapped inside the nucleus and specific amounts of energy (specific colors of light) were needed to release them. This varied from one element to an- other. 3. The electrons occupied discrete circular orbits; closer orbits were lower in energy. Emission lines were caused by electrons in excited atoms jumping from outer orbits to closer orbits. Each jump corresponded to a specific amount of energy released. 4. As the hydrogen atom only had one elec- tron, it only emitted certain colors of light as it orbited around the nucleus. Larger atoms had more electrons so more colors were seen.

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Ans:3. The electrons occupied discrete circular orbits; closer orbits were lower in energy. Emission lines were caused by electrons in excited atoms jumping from outer orbits to closer orbits. Each jump corresponded to a specific amount of energy released.

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Image source:http://abyss.uoregon.edu/~js/glossary/bohr_atom.html

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