Let's analyze the given wavelengths and determine which color each wavelength corresponds to according to the provided wavelength ranges:
1. Wavelength: 656 nm
- Checking the given wavelength ranges:
- Red: 700-635 nm
- Orange: 635-590 nm
- Yellow: 590-560 nm
- Green: 560-490 nm
- Blue: 490-450 nm
- Purple: 450-400 nm
- 656 nm falls in the range of Red (700-635 nm).
2. Wavelength: 486 nm
- Checking the given wavelength ranges:
- Red: 700-635 nm
- Orange: 635-590 nm
- Yellow: 590-560 nm
- Green: 560-490 nm
- Blue: 490-450 nm
- Purple: 450-400 nm
- 486 nm falls in the range of Blue (490-450 nm).
3. Wavelength: 434 nm
- Checking the given wavelength ranges:
- Red: 700-635 nm
- Orange: 635-590 nm
- Yellow: 590-560 nm
- Green: 560-490 nm
- Blue: 490-450 nm
- Purple: 450-400 nm
- 434 nm falls in the range of Purple (450-400 nm).
Now categorizing the given wavelengths:
- Red: 656 nm
- Blue: 486 nm
- Purple: 434 nm
Therefore, the student is most likely viewing an emission spectrum with the following strong lines:
- Red line at 656 nm
- Blue line at 486 nm
- Purple line at 434 nm
This matches the following absorption spectrum:
[tex]\[ \boxed{\text{{Red: 656 nm, Blue: 486 nm, Purple: 434 nm}}} \][/tex]
Hence, the conclusion is that the emission spectrum aligns with wavelengths in the red, blue, and purple regions.
