Questions: Rank the following colors of light from lowest energy to highest energy: blue (λ=453 nm), red (λ=670 nm), green (λ=525 nm), yellow (λ=572 nm). Select one: a. red, yellow, green, blue b. blue, yellow, green, red c. red, green, yellow, blue d. blue, green, yellow, red

Rank the following colors of light from lowest energy to highest energy: blue (λ=453 nm), red (λ=670 nm), green (λ=525 nm), yellow (λ=572 nm).

Select one:
a. red, yellow, green, blue
b. blue, yellow, green, red
c. red, green, yellow, blue
d. blue, green, yellow, red

Transcript text: Rank the following colors of light from lowest energy to highest energy: blue $(\lambda=453 \mathrm{~nm})$, red ( $\lambda=$ $670 \mathrm{~nm})$, green $(\lambda=525 \mathrm{~nm})$, yellow $(\lambda=572 \mathrm{~nm})$. Select one: a. red, yellow, green, blue b. blue, yellow, green, red c. red, green, yellow, blue d. blue, green, yellow, red

Solution

Solution Steps

Step 1: Understand the Relationship Between Wavelength and Energy

The energy of a photon is inversely proportional to its wavelength. This relationship is given by the equation: \[ E = \frac{hc}{\lambda} \] where $ E $ is the energy, $ h $ is Planck's constant, $ c $ is the speed of light, and $ \lambda $ is the wavelength. Therefore, shorter wavelengths correspond to higher energy.

Step 2: List the Wavelengths of the Given Colors