Question

Consider the following energy level diagram for hydrogen. n=7 E7 = -4.445 x 10^-20 J n=6 E6 = -6.050 x 10^-20 J n=5 E5 = -8.712 x 10^-20 J n=4 E4 = -1.361 x 10^-19 J n=3 E3 = -2.420 x 10^-19 J What is the wavelength (in nm) of a photon emitted during the transition of an electron from n=7 to n=3?

          Consider the following energy level diagram for hydrogen.

n=7 E7 = -4.445 x 10^-20 J
n=6 E6 = -6.050 x 10^-20 J

n=5 E5 = -8.712 x 10^-20 J

n=4 E4 = -1.361 x 10^-19 J

n=3 E3 = -2.420 x 10^-19 J

What is the wavelength (in nm) of a photon emitted during the transition of an electron from n=7 to n=3?

Consider the following energy level diagram for hydrogen.

n=7 E7 = -4.445 x 10^-20 J
n=6 E6 = -6.050 x 10^-20 J

n=5 E5 = -8.712 x 10^-20 J

n=4 E4 = -1.361 x 10^-19 J

n=3 E3 = -2.420 x 10^-19 J

What is the wavelength (in nm) of a photon emitted during the transition of an electron from n=7 to n=3?

Added by Jennifer S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

07/18/2022

Step 1

Given: Energy at n = 3 (E3) = -2.420 x 10^(-19) J Energy at n = 7 (E7) = -4.445 x 10^(-20) J Change in energy (ΔE) = E3 - E7 ΔE = (-2.420 x 10^(-19) J) - (-4.445 x 10^(-20) J) ΔE = -2.420 x 10^(-19) J + 4.445 x 10^(-20) J ΔE = -1.976 x 10^(-19) J Show more…

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Consider the following energy level diagram for hydrogen: n = 7 E7 = -4.445 x 10^-20 J n = 6 E6 = -6.050 x 10^-20 J n = 5 E5 = -8.712 x 10^-20 J n = 4 E4 = -1.361 x 10^-19 J n = 3 E3 = -2.420 x 10^-19 J What is the wavelength (in nm) of a photon emitted during the transition of an electron from n = 7 to n = 3?