A) What is the approximate wavelength emitted from helium represented by the bright yellow emission line below? What is it's frequency in HZ and energy in eV? (1 eV= 1.6 x 10-19 joules). B) If the excited helium electron that emits a yellow photon in this line starts with a potential energy of 8 eV, what is the potential energy of the electron afterwards? Assume that the emission of a yellow photon is allowed by the laws of quantum mechanics. Also don't worry about the other electron.
A) What is the approximate wavelength emitted from helium represented by the bright yellow emission line below? What is it's frequency in HZ and energy in eV? (1 eV= 1.6 x 10-19 joules). B) If the excited helium electron that emits a yellow photon in this line starts with a potential energy of 8 eV, what is the potential energy of the electron afterwards? Assume that the emission of a yellow photon is allowed by the laws of quantum mechanics. Also don't worry about the other electron.
A) What is the approximate wavelength emitted from helium represented by the bright yellow emission line below? What is it's frequency in HZ and energy in eV? (1 eV= 1.6 x 10-19 joules). B) If the excited helium electron that emits a yellow photon in this line starts with a potential energy of 8 eV, what is the potential energy of the electron afterwards? Assume that the emission of a yellow photon is allowed by the laws of quantum mechanics. Also don't worry about the other electron.
A) What is the approximate wavelength emitted from helium represented by the bright yellow emission line below? What is it's frequency in HZ and energy in eV? (1 eV= 1.6 x 10-19 joules).
B) If the excited helium electron that emits a yellow photon in this line starts with a potential energy of 8 eV, what is the potential energy of the electron afterwards? Assume that the emission of a yellow photon is allowed by the laws of quantum mechanics. Also don't worry about the other electron.
Transcribed Image Text:**Visible Light Spectrum**
The image above represents the visible light spectrum, illustrating the range of electromagnetic wavelengths that the human eye can perceive. This spectrum is displayed from approximately 400 nm to 700 nm.
**Color Range Explanation:**
- **400-450 nm (Violet to Blue):** The spectrum begins with violet tones, transitioning into shades of blue as wavelengths increase. The intensity of the color bands can indicate absorption or emission lines within this range.
- **450-500 nm (Blue to Cyan):** As we move further, the colors shift towards cyan, with several noticeable lines where energy levels correspond to specific frequencies.
- **500-550 nm (Cyan to Green):** In this range, colors transition from cyan to green, representing mid-range wavelengths often associated with natural phenomena like plant foliage.
- **550-600 nm (Green to Yellow):** The spectrum progresses to yellow hues, marking the transition between higher energy greens and lower energy yellows.
- **600-650 nm (Yellow to Orange):** Here the colors glide from yellow to orange, indicating longer wavelengths and lower frequencies.
- **650-700 nm (Orange to Red):** Finally, the spectrum culminates in the red zone, the visible light with the longest wavelength and lowest frequency perceivable by the human eye.
**Educational Significance:**
Understanding the visible light spectrum is crucial in fields like physics, astronomy, and chemistry. It aids in interpreting phenomena like the Doppler effect, spectral analysis, and photosynthesis processes. Each distinct absorption or emission line can provide insights into the composition and behavior of materials and celestial bodies.
Branch of physics that deals with the behavior of particles at a subatomic level.
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