Question

1. a bohr model representation of the h atom is shown below with several electron transitions depicted by arrows: a. which transitions are absorptions and which are emissions? (use letters a,b,c,d,e, & f) i. absorptions: ii. emissions: b. rank the emissions in terms of increasing energy. (least energy to most energy) c. rank the absorptions in terms of increasing wavelength of light absorbed. (shortest wavelength to longest wavelength)

Explanation:

Step1: Recall absorption and emission rules

Absorption occurs when an electron moves from a lower - energy level to a higher - energy level. Emission occurs when an electron moves from a higher - energy level to a lower - energy level.

Step2: Identify absorptions

Absorptions are when electrons move up levels. So, Absorptions: A, B, C

Step3: Identify emissions

Emissions are when electrons move down levels. So, Emissions: D, E, F

Step4: Recall energy formula for emissions

The energy of an emission is given by $E = h
u=\frac{hc}{\lambda}$, where $h$ is Planck's constant, $
u$ is frequency and $\lambda$ is wavelength. The energy of an emission is proportional to the difference in energy levels. The smaller the difference in energy levels, the lower the energy of the emission. For emissions D, E, F, the order of increasing energy is D < E < F.

Step5: Recall wavelength - energy relation for absorptions

For absorptions, the energy of the absorbed photon is $E=\frac{hc}{\lambda}$. Higher energy corresponds to shorter wavelength. The order of increasing wavelength (decreasing energy) for absorptions A, B, C is C < B < A.

Answer:

a. i. Absorptions: A, B, C
ii. Emissions: D, E, F
b. D < E < F
c. C < B < A