Question

Simplified. The absorption spectra of ions have been used to identify the presence of the elements in the atmospheres of the sun and other stars. What is the energy of a photon (in J) that is absorbed by He ions, when an electron is excited from the Bohr orbit with n

Answer 1

The answer is "
`3.83 * 10^9 \ m`"

Step-by-step explanation:

Z=2, so the equation is
`E= (-4B)/(n^2)`

Calculate the value for E when:

n=2 and n=9

The energy is the difference in transformation, name the energy delta E Deduct these two energies

In this transition, the wavelength of the photon emitted is:

`\Delta E=2.18 * 10^(-18) ( (1)/(4)- (1)/(81))`

`\lambda = (h c)/(\Delta E)`

`h ( Planck's\ constant) = 6.62 * 10^((-34)) \ Js \\\\ speed \ of \ light = 3 * 10^(8) \ (m)/(s)\\\\= \frac{6.62 * 10^((-34)) * 3 * 10^ {8}}{2.18 * 10^(-18)} ((1)/(4)- (1)/(81)) \\\\=3.83 * 10^9 \ m\\\\`