Question

Match the hydrogen emission line wavelength with the corresponding energy level transition.

Wavelengths:
410 nm
434 nm
486 nm
656 nm

Transitions:
a) (n = 1 rightarrow n = 2)
b) (n = 2 rightarrow n = 3)
c) (n = 3 rightarrow n = 4)
d) (n = 4 rightarrow n = 5)

Answer 1

The correct hydrogen emission line wavelengths and corresponding energy level transitions are 410 nm (n = 6 to n = 2), 434 nm (n = 5 to n = 2), 486 nm (n = 4 to n = 2), and 656 nm (n = 3 to n = 2), all part of the Balmer series.

Step-by-step explanation:

When matching the hydrogen emission line wavelengths with the corresponding energy level transitions, it's important to use the information given about the Balmer series of lines. Each given wavelength corresponds to a transition from a higher energy level to the second energy level (n=2) for hydrogen atoms. Here are the correct pairs:

• 410 nm corresponds to the transition from (n = 6 to n = 2)
• 434 nm corresponds to the transition from (n = 5 to n = 2)
• 486 nm corresponds to the transition from (n = 4 to n = 2)
• 656 nm corresponds to the transition from (n = 3 to n = 2)

Note that the transitions provided in the question options (a), (b), (c), and (d) do not match the correct transitions for the Balmer series wavelengths given. Transitions such as (n = 1 to n = 2) and (n = 2 to n = 3) represent different series of emission lines, such as the Lyman and Paschen series, respectively.