Question

question 29 of 30 the emission spectrum of hydrogen is shown below. what do the lines in the spectrum show?
h spectrum image with 410, 434, 486, 656 nm labels
a. light with wavelengths of 410 nm, 434 nm, 486 nm, and 656 nm corresponds with the four energy levels in hydrogen.
b. light with wavelengths of 410 nm, 434 nm, 486 nm, and 656 nm is given off when electrons fall to lower energy levels.
c. light with wavelengths between 410 nm to 434 nm, 434 to 486 nm, and 486 to 656 nm corresponds with the three energy levels in hydrogen.
d. only light with wavelengths of 410 nm, 434 nm, 486 nm, and 656 nm is not taken in during energy transitions.

Explanation:

To solve this, we analyze each option:

• Option A: Hydrogen has more than four energy levels, and the lines correspond to electron transitions, not directly to energy levels. Eliminate A.
• Option B: In the hydrogen emission spectrum, lines are formed when electrons fall from higher to lower energy levels, emitting light of specific wavelengths (410 nm, 434 nm, 486 nm, 656 nm here). This matches the concept of emission spectrum.
• Option C: The lines are discrete wavelengths, not ranges, and hydrogen has more energy levels. Eliminate C.
• Option D: The lines represent emitted light (not absorbed), and the description of "not taken in" is incorrect. Eliminate D.

Answer:

B. Light with wavelengths of 410 nm, 434 nm, 486 nm, and 656 nm is given off when electrons fall to lower energy levels.