1. Calculate the energies predicted in the following transitions for the hydrogen atom. Showall of your work for at least one example.Theoretical ABalmer SeriesnmcolorAE=Er – Eininf410.1Violet6434.0Violet43486.1Green-Red656.222. Explain why an element only emits certain colors (wavelengths) of light instead of a fullrainbow.

Given: Planck's constant, h=6.626×10-34J·sSpeed of light, c=3×108m/sWavelength of violet, λ1=410.1nm=410.1×10-9mWavelength of violet, λ2=434nm=434×10-9mWavelength of green, λ3=486.1nm=486.1×10-9mWavelength of red, λ4=656.2nm=656.2×10-9m 1) The expression of the change in energy is: ∆E=hcλ .... (1)For violet 1, substitute the value in equation (1). ∆E=6.626×10-34×3×108410.1×10-9∆E=19.878×10-26410.1×10-9∆E=0.0484×10-17J For violet 2, substitute the value in equation (1). ∆E=6.626×10-34×3×108434×10-9∆E=19.878×10-26434×10-9∆E=0.0458×10-17J For green, substitute the value in equation (1). ∆E=6.626×10-34×3×108486.1×10-9∆E=19.878×10-26486.1×10-9∆E=0.0408×10-17J For red, substitute the value in equation (1). ∆E=6.626×10-34×3×108656.2×10-9∆E=19.878×10-26656.2×10-9∆E=0.0302×10-17J 2) An atom's electrons can only inhabit a limited number of energy levels. When an electron goes to a lower energy level, only certain transitions are conceivable, and hence only certain wavelengths are emitted. Since elements only release light at specific wavelengths and frequencies, not all wavelengths and frequencies of light are emitted. When an electron jumps from a higher energy level to a lower energy level, photons are released, which are responsible for color. The color of the light emitted is likewise determined by the energy differential. As each element's orbitals have distinct energies, the color varies from one element to the next.

Answered: Calculate the energies predicted in the…