Bohr’s model of the atom was valuable in demonstrating how electrons were capable of absorbing and releasing energy and how atomic emission spectra were created. However, the model did not really explain why electrons should exist only in fixed circular orbits rather than being able to exist in a limitless number of orbits all with different energies. In order to explain why atomic energy states are quantized, scientists needed to rethink the way in which they viewed the nature of the electron and its movement.

### de Broglie Wave Equation

Planck’s investigation of the emission spectra of hot objects and the subsequent studies into the photoelectric effect had proven that light was capable of behaving both as a wave and as a particle. It seemed reasonable to wonder if electrons could also have a dual wave-particle nature. In 1924, French scientist Louis de Broglie (1892-1987) derived an equation that described the wave nature of any particle. Particularly, the wavelength \begin{align*}(\lambda)\end{align*} of any moving object is given by:

\begin{align*}\lambda=\frac{h}{mv}\end{align*}

In this equation, \begin{align*}h\end{align*} is Planck’s constant, \begin{align*}m\end{align*} is the mass of the particle in kg, and \begin{align*}v\end{align*} is the velocity of the particle in m/s. The problem below shows how to calculate the wavelength of the electron.

#### Sample Problem: de Broglie Wave Equation

An electron of mass 9.11 × 10^{-31} kg moves at nearly the speed of light. Using a velocity of 3.00 × 10^{8} m/s, calculate the wavelength of the electron.

*Step 1: List the known quantities and plan the problem.*

Known

- mass \begin{align*}(m)\end{align*} = 9.11 × 10
^{-31}kg - Planck's constant \begin{align*}(h)\end{align*} = 6.6262 10
^{-34}× J • s - velocity \begin{align*}(v)\end{align*} = 3.00 × 10
^{8}m/s

Unknown

- wavelength
*\begin{align*}(\lambda)\end{align*}*

Apply the **de Broglie wave equation** \begin{align*}\lambda=\frac{h}{mv}\end{align*} to solve for the wavelength of the moving electron.

*Step 2: Calculate*

\begin{align*}\lambda=\frac{h}{mv}=\frac{6.626 \times 10^{-34}\ \text{J} \cdot \text{s}}{(9.11 \times 10^{-31} \ \text{kg}) \times (3.00 \times 10^8 \ \text{m/s})}=2.42 \times 10^{-12} \ \text{m}\end{align*}

*Step 3: Think about your result.*

This very small wavelength is about 1/20th of the diameter of a hydrogen atom. Looking at the equation, as the speed of the electron decreases, its wavelength increases. The wavelengths of everyday large objects with much greater masses should be very small.

If we were to calculate the wavelength of a 0.145 kg baseball thrown at a speed of 40 m/s, we would come up with an extremely short wavelength on the order of 10^{-34} m. This wavelength is impossible to detect even with advanced scientific equipment. Indeed, while all objects move with wavelike motion, we never notice it because the wavelengths are far too short. On the other hand, particles with measurable wavelengths are all very small. However, the wave nature of the electron proved to be a key development in a new understanding of the nature of the electron. An electron that is confined to a particular space around the nucleus of an atom can only move around that atom in such a way that its electron wave “fits” the size of the atom correctly. This means that the frequencies of electron waves are **quantized**. Based on the \begin{align*}E=hv\end{align*} equation, the quantized frequencies means that electrons can only exist in an atom at specific energies, as Bohr had previously theorized.

#### Summary

- The deBroglie wave equations allows calculation of the wavelength of any moving object.
- As the speed of the electron decreases, its wavelength increases.

#### Practice

Use the link below to practice calculations using the deBroglie wave equation:

http://science.widener.edu/svb/tutorial/debrogliecsn7.html

#### Review

*Questions*

- What did the Bohr model not explain?
- State the deBroglie wave equation.
- What happens as the speed of the electron decreases?