Question

Consider the following portion of the energy-level diagram for hydrogen: n = 4 -0.1361 x 10^-18 J n = 3 -0.2420 x 10^-18 J n = 2 -0.5445 x 10^-18 J n = 1 -2.178 x 10^-18 J In the hydrogen spectrum, what is the wavelength of light associated with the n = 4 to n = 2 electron transition? (c = 2.9979 x 10^8 m/s, h = 6.626 x 10^-34 J·s). 1.03 x 10^-7 m 4.86 x 10^-7 m 1.94 x 10^-18 m 8.21 x 10^2 nm

          Consider the following portion of the energy-level diagram for hydrogen:
n = 4    -0.1361 x 10^-18 J
n = 3    -0.2420 x 10^-18 J
n = 2    -0.5445 x 10^-18 J
n = 1    -2.178 x 10^-18 J
In the hydrogen spectrum, what is the wavelength of light associated with the n = 4 to n = 2 electron transition? (c = 2.9979 x 10^8 m/s, h = 6.626 x 10^-34 J·s).
1.03 x 10^-7 m
4.86 x 10^-7 m
1.94 x 10^-18 m
8.21 x 10^2 nm

Consider the following portion of the energy-level diagram for hydrogen:
n = 4 -0.1361 x 10^-18 J
n = 3 -0.2420 x 10^-18 J
n = 2 -0.5445 x 10^-18 J
n = 1 -2.178 x 10^-18 J
In the hydrogen spectrum, what is the wavelength of light associated with the n = 4 to n = 2 electron transition? (c = 2.9979 x 10^8 m/s, h = 6.626 x 10^-34 J·s).
1.03 x 10^-7 m
4.86 x 10^-7 m
1.94 x 10^-18 m
8.21 x 10^2 nm

Added by Anna S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

05/29/2022

Step 1

The energy of a level is given by the negative of the value provided, so the energy difference (ΔE) is: ΔE = E_4 - E_2 = (-0.1361 x 10^-18) - (-0.5445 x 10^-18) = 0.4084 x 10^-18 J Show more…

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Consider the following portion of the energy-level diagram for hydrogen: n = 4 -0.1361 x 10^-18 J n = 3 -0.2420 x 10^-18 J n = 2 -0.5445 x 10^-18 J n = 1 -2.178 x 10^-18 J In the hydrogen spectrum, what is the wavelength of light associated with the n = 4 to n = 2 electron transition? (c = 2.9979 x 10^8 m/s, h = 6.626 x 10^-34 J·s). 1.03 x 10^-7 m 4.86 x 10^-7 m 1.94 x 10^-18 m 8.21 x 10^2 nm