5. How did Bohr use the hydrogen emission spectrum to extend classical physics i

Question

5. How did Bohr use the hydrogen emission spectrum to extend classical physics into quantunm physics enabling him to explain that electrons are allowed to exist in defined shells and that transitions between shells can only occur in defined intervals? 6. Answer the following questions regarding quantum numbers. a. Which pair of quantum numbers determines the energy of an electron in an orbital? Why? b. What are the shapes of the s, p, and d orbitals? c. Write a set of quantum numbers for an electron in a 4f orbital

Explanation / Answer

The hydrogen spectrum contained only a few lines. This was the main observation of Bohr which made him draw conclusions about the electron orbits. he believed that the lines were the result of light being released or absorbed as an electron moved from one orbit to another in the atom. As the electron moved further away from the nucleus it would become excited as it absorbed light causing the electron to become more charged. As the electron relaxed it would release energy. As the electrons moved in between these lines energy continued to transfer.

He suggested that electrons could only have classical motions.

electrons in atom orbit the nucleus.

electrons can orbit stably in an orbit without radiating any energy. These are called the energy levels.

Electrons can gain energy or lose energy when they move from one orbit to another or say one energy level to another energy level.

These ideas very much appear to be of quantum physics. This is the reason that we say that Bohr theory is first order approximation of hydrogen atom.

Bohr model is still commonly taught to introduce students to quantum mechanics or energy level diagrams before moving on to the more accurate, but more complex, valence shell atom.

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