Energy graphs and the Bohr model

This page gives a more in-depth explanation of how to use energy graphs to comprehend the Bohr model. It explains how to illustrate excited states and photon emissions or absorptions.

by Caitlin Taylor

The Main Idea

Energy graphs and the Bohr model.

This page gives a more in-depth explanation of how to use energy graphs to comprehend the Bohr model. It specifically explains how to illustrate the various aspects such as excited states and photon emissions or absorptions on the energy graphs as well as what each component corresponds to.

A Mathematical Model

The Bohr Model, as explained in more detail on the Bohr Model wiki, page depicts the atom as a small, positively charged nucleus surrounded by electrons which can only be at certain different distances from the proton to which it is bound. Energy is quantized which means that only orbits with certain radii are allowed.[1] These levels are labeled with integer N, known as quantum number, where the lowest energy state is the ground state. Beyond an energy called the ionization potential the single electron of the hydrogen atom is no longer bound to the atom. The Bohr model works well for very simple atoms such as hydrogen.

Electronic Energy levels of a Hydrogen Atom

E = K + Uelectric

1) [math]\displaystyle{ E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}} }[/math]

2) [math]\displaystyle{ E = {\frac{13.6 eV}{N^2}} }[/math] where N = 1,2,3

A Computational Model

Visualize this topic given this glow script written by matter and interactions Bohr Model Glowscript [3]

Examples

Simple

This Bohr model picture helps you visualize the orbit radii of the different excited states of the hydrogen atom described in the Bohr model. It displays how the distances in orbit radii get increasingly larger. This also means that due to the fact that the distance from the center is much larger, the ionization energy is much less. [2]

This visualization of the orbitals in a more graphical way shows that as the distance from the center becomes larger, the ionization energy is much less. [2]

Middling

This graph explains in more detail how each level corresponds to less energy. If the energy reached zero, the electron would be free from the hydrogen nucleus because no energy is holding it on. The levels get exponentially closer as they approach the ionization energy