Question

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.

Answer 1

Answer:

From the highest to the lowest

Third excited state (n=4) $\rightarrow$ Second excited state (n=3) $\rightarrow$ First excited state (n=2) $\rightarrow$ 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 electron is able to revolve in certain stable orbits around the nucleus without radiating any energy
• Electrons can only gain and lose energy by jumping from one allowed orbit to another, absorbing or emitting electromagnetic radiation with a frequency ν determined by the energy difference of the levels according to the Planck relation:${\displaystyle \Delta E=E_{2}-E_{1}$ = hv, where h = planck's constant.

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)