chemistry hw need help **Transcription for Educational Website:**---**Problem Statement**- **Electron Transition in Hydrogen:** - Initial Energy Level \( n = 8 \) - Final Energy Level \( n = 4 \)- **Constants:** - \( R_H = 2.18 \times 10^{-18} \, \text{J} \) (Rydberg constant for hydrogen) - Speed of light \( = 3.0 \times 10^8 \, \text{m/s} \)**Task:**Calculate the wavelength of the light emitted during this transition.---**Explanation for Calculation:**To find the wavelength of light emitted when an electron transitions between two energy levels in a hydrogen atom, use the following formula derived from the Rydberg formula for hydrogen:\[\frac{1}{\lambda} = R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)\]Where:- \( \lambda \) is the wavelength of light emitted,- \( R_H \) is the Rydberg constant,- \( n_1 \) and \( n_2 \) are the principal quantum numbers of the initial and final energy levels respectively.**Application:**Substitute the given values of \( n_1 = 4 \) and \( n_2 = 8 \) and solve for \( \lambda \).Following this, use the relationship between frequency (\( f \)), speed of light (\( c \)), and wavelength (\( \lambda \)):\[\lambda = \frac{c}{f}\]Where:- \( c = 3.0 \times 10^8 \, \text{m/s} \)This calculation will provide the wavelength of the emitted light in meters.

Name: chemistry hw need help **Transcription for Educational Website:**---**
Uploaded: 2022-10-12T14:10:27.000Z
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Description: chemistry hw need help **Transcription for Educational Website:**---**Problem Statement**- **Electron Transition in Hydrogen:** - Initial Energy Level \( n = 8 \) - Final Energy Level \( n = 4 \)- **Constants:** - \( R_H = 2.18 \times 10^{-18} \,