# Finding the Wavelength of a Photon Emitted by an Electron Transition

• 1.

The electron in a hydrogen atom jumps from the energy level {eq}n=2{/eq} to {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}121.5 \;\rm nm{/eq}

• {eq}111.6 \;\rm nm{/eq}

• {eq}153.6 \;\rm nm{/eq}

• {eq}120.5 \;\rm nm{/eq}

• 2.

The electron in a hydrogen atom jumps from the energy level {eq}n=3{/eq} to {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}121.6 \;\rm nm{/eq}

• {eq}202.6 \;\rm nm{/eq}

• {eq}151.6 \;\rm nm{/eq}

• {eq}102.6 \;\rm nm{/eq}

• 3.

The electron in a hydrogen atom jumps from the energy level {eq}n=4{/eq} to {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}87.3\; \rm nm{/eq}

• {eq}79.3\; \rm nm{/eq}

• {eq}97.3\; \rm nm{/eq}

• {eq}67.3\;\rm nm{/eq}

• 4.

The electron in a hydrogen atom jumps from the energy level {eq}n=3{/eq} to {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}456\; \rm nm{/eq}

• {eq}646\; \rm nm{/eq}

• {eq}656\: \rm nm{/eq}

• {eq}556\; \rm nm{/eq}

• 5.

The electron in a hydrogen atom jumps from the energy level {eq}n=5{/eq} to {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}430\; \rm nm{/eq}

• {eq}332\; \rm nm{/eq}

• {eq}434\; \rm nm{/eq}

• {eq}234\; \rm nm{/eq}

• 6.

The electron in a hydrogen atom jumps from the energy level {eq}n=6{/eq} to {eq}n=3{/eq} and a photon is emitted. What is the wavelength of the emitted photon?

• {eq}109.4 \; \rm nm{/eq}

• {eq}190.4 \; \mu m{/eq}

• {eq}190.4 \; \rm nm{/eq}

• {eq}1.094 \; \mu m{/eq}

• 7.

When an electron in a hydrogen atom jumps from the energy level {eq}n=4{/eq} to {eq}n=3{/eq}, a photon is emitted. What is the wavelength of this photon?

• {eq}1.876 \; \rm nm{/eq}

• {eq}1.875\; \mu m{/eq}

• {eq}1.866\; \mu m{/eq}

• {eq}1.879\; \rm nm{/eq}

• 8.

The electron in a hydrogen atom emits a photon when it jumps from the energy level {eq}n=7{/eq} to {eq}n=3{/eq}. What is the wavelength of this emitted photon?

• {eq}1.05\; \rm nm{/eq}

• {eq}1.2 \; \mu m{/eq}

• {eq}1005\; \rm nm{/eq}

• {eq}1500\; \rm nm{/eq}

• 9.

When an electron jumps from a higher energy level to a lower energy level, it emits photons. In an experiment, the electron in a hydrogen atom jumps from the energy level {eq}n=6{/eq} to the ground state {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}90.9 \; \rm nm{/eq}

• {eq}91.8 \; \mu m{/eq}

• {eq}92.1 \; \rm nm{/eq}

• {eq}93.7 \; \mu m{/eq}

• 10.

If the electron in a hydrogen atom jumps from the energy level {eq}n=5{/eq} to {eq}n=4{/eq}, what should be the wavelength of the emitted photon?

• {eq}4090 \; \rm nm{/eq}

• {eq}3052 \; \rm nm{/eq}

• {eq}4052 \; \rm nm{/eq}

• {eq}4021 \; \rm nm{/eq}

• 11.

What is the wavelength of the emitted photon when the electron in a hydrogen atom jumps from the energy level {eq}n=4{/eq} to {eq}n=2{/eq} ?

• {eq}585.1 \; \rm nm{/eq}

• {eq}486.1 \; \rm nm{/eq}

• {eq}485.1 \; \rm nm{/eq}

• {eq}586.1 \; \rm nm{/eq}

• 12.

The electron in a hydrogen atom emits a photon when it jumps from the higher energy level {eq}n=7{/eq} to the lower energy level {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}395.0 \; \rm nm{/eq}

• {eq}397.0 \; \rm nm{/eq}

• {eq}391.0 \; \rm nm{/eq}

• {eq}394.0 \; \rm nm{/eq}

• 13.

The electron in a hydrogen atom emits a photon when it jumps from the higher energy level {eq}n=7{/eq} to the lowest energy level {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}83.02 \; \rm nm{/eq}

• {eq}63.02 \; \rm nm{/eq}

• {eq}93.02 \; \rm nm{/eq}

• {eq}85.02 \; \rm nm{/eq}

• 14.

The electron in a hydrogen atom emits a photon when it jumps from the higher energy level {eq}n=7{/eq} to the lowest energy level {eq}n=4{/eq}. What is the wavelength of the emitted photon?

• {eq}3277 \; \rm nm{/eq}

• {eq}4177 \; \rm nm{/eq}

• {eq}2166 \; \rm nm{/eq}

• {eq}3165 \; \rm nm{/eq}

• 15.

The electron in a hydrogen atom emits a photon when it jumps from the higher energy level {eq}n=7{/eq} to the lowest energy level {eq}n=5{/eq}. What is the wavelength of the emitted photon?

• {eq}5651 \; \rm nm{/eq}

• {eq}3654 \; \rm nm{/eq}

• {eq}4653 \; \rm nm{/eq}

• {eq}4354 \; \rm nm{/eq}

• 16.

The electron in a hydrogen atom emits a photon when it jumps from the higher energy level {eq}n=7{/eq} to the lowest energy level {eq}n=6{/eq}. What is the wavelength of the emitted photon?

• {eq}12.7 \; \rm \mu m{/eq}

• {eq}12.6 \; \rm \mu m{/eq}

• {eq}12.4 \; \rm \mu m{/eq}

• {eq}12.1 \; \rm \mu m{/eq}

• 17.

The electron in a {eq}\rm Li^{2+}{/eq} ion jumps from the energy level {eq}n=3{/eq} to {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}13.4\; \rm nm{/eq}

• {eq}11.4\; \rm nm{/eq}

• {eq}10.4\; \rm nm{/eq}

• {eq}12.4\; \rm nm{/eq}

• 18.

The electron in a {eq}\rm Li^{2+}{/eq} ion jumps from the energy level {eq}n=3{/eq} to {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}72.9\; \rm nm{/eq}

• {eq}70.9\; \rm nm{/eq}

• {eq}71.9\; \rm nm{/eq}

• {eq}69.9\; \rm nm{/eq}

• 19.

The electron in a {eq}\rm Li^{2+}{/eq} ion jumps from the energy level {eq}n=5{/eq} to the ground state energy level {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}11.6\; \rm nm{/eq}

• {eq}10.6\; \rm nm{/eq}

• {eq}20.6\; \rm nm{/eq}

• {eq}12.6\; \rm nm{/eq}

• 20.

The electron in a hydrogen like {eq}\rm Li^{2+}{/eq} ion jumps from a higher energy level {eq}n=5{/eq} to a lower energy level {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}48.2\; \rm nm{/eq}

• {eq}38.2\; \rm nm{/eq}

• {eq}68.2\; \rm nm{/eq}

• {eq}58.2\; \rm nm{/eq}

• 21.

The electron in a hydrogen like {eq}\rm Li^{2+}{/eq} ion jumps from a higher energy level {eq}n=5{/eq} to a lower energy level {eq}n=3{/eq}. What is the wavelength of the emitted photon?

• {eq}142.4\; \rm nm{/eq}

• {eq}142.5\; \rm nm{/eq}

• {eq}142.8\; \rm nm{/eq}

• {eq}142.1\; \rm nm{/eq}

• 22.

The electron in a hydrogen like {eq}\rm Be^{3+}{/eq} ion jumps from a higher energy level {eq}n=5{/eq} to a lower energy level {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}27.1\; \rm m{/eq}

• {eq}29.1\; \rm nm{/eq}

• {eq}24.1\; \rm nm{/eq}

• {eq}37.1\; \rm nm{/eq}

• 23.

The electron in a hydrogen like {eq}\rm Be^{3+}{/eq} ion jumps from a higher energy level {eq}n=3{/eq} to a lower energy level {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}6.41\; \rm nm{/eq}

• {eq}3.41\; \rm nm{/eq}

• {eq}2.41\; \rm nm{/eq}

• {eq}5.41\; \rm nm{/eq}

• 24.

The electron in a hydrogen like {eq}\rm Be^{3+}{/eq} ion jumps from a higher energy level {eq}n=7{/eq} to a lower energy level {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}4.82\; \rm nm{/eq}

• {eq}5.82\; \rm nm{/eq}

• {eq}3.82\; \rm nm{/eq}

• {eq}9.82\; \rm nm{/eq}

• 25.

The electron in a hydrogen like {eq}\rm Be^{3+}{/eq} ion jumps from a higher energy level {eq}n=5{/eq} to a lower energy level {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}1.8\; \rm nm{/eq}

• {eq}5.9\; \rm nm{/eq}

• {eq}5.6\; \rm nm{/eq}

• {eq}6.8\; \rm \mu m{/eq}

• 26.

The electron in a hydrogen like {eq}\rm B^{4+}{/eq} ion jumps from a higher energy level {eq}n=5{/eq} to a lower energy level {eq}n=2{/eq}. What is the wavelength of the emitted photon?

• {eq}70.4\; \rm nm{/eq}

• {eq}37.4\; \rm nm{/eq}

• {eq}47.4\; \rm nm{/eq}

• {eq}17.4\; \rm nm{/eq}

• 27.

The electron in a hydrogen like {eq}\rm B^{4+}{/eq} ion jumps from a higher energy level {eq}n=3{/eq} to a lower energy level {eq}n=1{/eq}. What is the wavelength of the emitted photon?

• {eq}2.10\; \rm nm{/eq}

• {eq}4.10\; \rm nm{/eq}

• {eq}8.10\; \rm nm{/eq}

• {eq}3.10\; \rm nm{/eq}

• 28.

The electron in a hydrogen like {eq}\rm He^{1+}{/eq} ion jumps from a higher energy level {eq}n=5{/eq} to a lower energy level {eq}n=1{/eq}. The wavelength of the emitted photon is?

• {eq}23.78\; \rm nm{/eq}

• {eq}23.76\; \rm nm{/eq}

• {eq}23.71\; \rm nm{/eq}

• {eq}23.74\; \rm nm{/eq}

• 29.

The electron in a hydrogen like {eq}\rm He^{1+}{/eq} ion jumps from a higher energy level {eq}n=3{/eq} to a lower energy level {eq}n=2{/eq}. The wavelength of the emitted photon is?

• {eq}144.1\; \rm nm{/eq}

• {eq}154.1\; \rm nm{/eq}

• {eq}174.1\; \rm nm{/eq}

• {eq}164.1\; \rm nm{/eq}

• 30.

The electron in a hydrogen like {eq}\rm He^{1+}{/eq} ion makes a transition from a higher energy level {eq}n=6{/eq} to a lower energy level {eq}n=3{/eq}. The wavelength of the emitted photon is?