In the classical view of the atom, Bohr pictured electrons orbiting the positively charged nucleus similar to how the planets orbit the Sun. While this picture was not entirely correct, it provides a good framework in which to make calculations about the energies of electrons. Different from the predictions of Newtonian mechanics, which allows any energy to be possible, Bohr described the electron orbits (now called orbitals) as having specific energies. Rank the following electron energy states according to their electron energies.

From the highest to the lowest

Third excited state (n=4) Second excited state (n=3) First excited state (n=2) Ground state (n=1)

Explanation:

The Bohr Model, by Niels Bohr, is a planetary model in which the negatively charged electrons orbit a small, positively charged nucleus similar to the planets orbiting the sun. Niels Bohr in his model states that:

The lowest value of n is 1, which is the ground state

n = principal quantum number

Therefore, from the highest to the lowest, the energy levels are ranked as:

Third excited state (n=4)

Second excited state (n=3)

First excited state (n=2)

Ground state (n=1)

what experimental evidence led scientists to change from the previous model to this one?

a few of the positive particles aimed at a gold foil seemed to bounce back.

the colors of light emitted from heated atoms had very specific energies.

experiments with water vapor showed that elements combine in specific proportions.

cathode rays were bent in the same way whenever a magnet was brought near them.