Question

1. which of the following wavelengths would have the highest energy? clear all 677 m 5400 m 200 m 35 m

Explanation:

Step1: Recall energy - wavelength relation

The energy of a photon is given by $E = \frac{hc}{\lambda}$, where $h$ is Planck's constant, $c$ is the speed of light, and $\lambda$ is the wavelength. Energy is inversely - proportional to wavelength.

Step2: Compare given wavelengths

We have wavelengths $\lambda_1=677\ nm$, $\lambda_2 = 5400\ nm$, $\lambda_3=200\ nm$, $\lambda_4 = 35\ nm$. Since $E\propto\frac{1}{\lambda}$, the smaller the wavelength, the higher the energy.

Step3: Identify the smallest wavelength

Among $677\ nm$, $5400\ nm$, $200\ nm$, and $35\ nm$, the smallest wavelength is $35\ nm$.

Answer:

$35\ nm$