The task involves calculating the energy of photons for each representative wavelength provided in the table, plotting the data on the given graph, and shading/labeling the x-axis with the corresponding colors.

Step-by-Step Instructions:

1. Energy of Photons Formula: The energy $E$ of a photon can be calculated using the equation: $E = \frac{h \cdot c}{\lambda}$ Where:

   • $h = 6.626 \times 10^{-34} \, \text{J·s}$ (Planck's constant),
   • $c = 3.00 \times 10^8 \, \text{m/s}$ (speed of light),
   • $\lambda$ is the wavelength in meters.

2. Convert Wavelength: Convert the representative wavelengths from nanometers ($\text{nm}$) to meters ($\text{m}$) using: $1 \, \text{nm} = 1 \times 10^{-9} \, \text{m}$

3. Calculate Energy: Substitute the converted wavelength ($\lambda$) into the formula to find $E$ for each color.

4. Plot and Label:

   • Plot the calculated energy values (y-axis) against the given wavelengths (x-axis).
   • Shade and label the x-axis for the corresponding colors using the wavelength regions provided in the table.

Would you like me to calculate the energies for you or clarify anything further? Let me know! Here’s a set of guiding questions to help:

Guiding Questions:

1. What do the energy values tell us about the relationship between wavelength and energy in visible light?
2. How can shading the x-axis with colors help interpret the graph?
3. What units are typically used to express the energy of photons, and why?
4. Why is Planck's constant important in understanding photon energy?
5. How does the color of light correlate with its energy and wavelength?

Tip:

Remember, shorter wavelengths (toward the violet end) correspond to higher energy photons, while longer wavelengths (toward the red end) correspond to lower energy photons!