Interactive Activity—Bohr Model Bohr assumed that the orbits in which electrons

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Interactive Activity—Bohr Model

Bohr assumed that the orbits in which electrons move are at specific and fixed distances from the nucleus of an atom. The energies of these orbits are also fixed, and when an electron moves from one orbit to another, energy is either absorbed or released. These electronic transitions result in the line spectrum of an atom.

Click on the image to explore the interactive activity, which shows the Bohr model of a hydrogen atom and demonstrates the relationship between the line spectrum and electronic transitions.

In the interactive activity, you will see the Bohr model of a hydrogen atom. To the right side, you will see the energy-level diagram for the hydrogen atom; this diagram also shows the energy of each state (E1 through E6) and the energy changes (E) associated with electronic transitions. You can set the initial and the final energy states for an electronic transition, and then click on the "Animate Transition" button. The bottom part of the interactive activity displays the line spectrum for hydrogen, and the line that blinks in the spectrum will correspond to the particular transition you have selected.

Part A

In the interactive activity, select the initial and the final states for an electronic transition, and then select "Animate Transition" to observe the electronic transition. Below the energy-level diagram for the hydrogen atom, the displayed label indicate whether light is absorbed or emitted for the particular transition. The line that blinks in the line spectrum will correspond to the particular transition you have selected.

Classify the following electronic transitions depending upon whether they represent the absorption or emission of light.

Drag the appropriate items to their respective bins.

i did this and it was incorrect

light absorbed

(initital state n=1 to final state n=5, inititial state n=1 to final state n=3,initial state n=2 to final state n=5)

light emittted

(initial state n=6 to final state n=5,initial state n=4 to final state n=2,initial state n=5 to final state n=3,initial state n=3 to final state n=4,initial state n=3 to final state n=1)

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Part C

An electron undergoes a transition from an initial (ni) to a final (nf ) energy state. The energies of the ni and nf  energy states are 2.179×1018 J and 8.720×1020 J, respectively.

Calculate the wavelength () of the light in nanometers (nm) corresponding to the energy change (E) value of this transition. You can use the following values for your calculations:

Plancks constant (h)speed of light (c)1 m===6.626×1034 Js2.998×108 m/s109 nm

Express your answer in nanometers to four significant figures.

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Explanation / Answer

To be honest, I don't have very much aknowledge in the theory for part A, but I can help you with part C. You need to use the following equation:

E = hc/L

E = 2.179x10-18 - 8.72x10-20 = 2.0918x10-18 J

6.63x10-34 Js * 2.998x108 m/s / L = 2.0918x10-18 J

L = 95.0222 nm

Post part A in a new question, so you can get a faster answer.

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