Answer:
a. To determine the energy of the photon needed to excite an electron from the b level to the e level in the Mercury atom, you would need to know the specific energy values for each level. Typically, energy levels are represented in electron volts (eV) or joules (J) in atomic spectroscopy.
b. Once you have determined the energy difference between the b and e levels, you can convert it to joules using the conversion factor 1 eV = 1.602 x 10^(-19) J.
c. The frequency of a photon can be calculated using the equation E = hf, where E is the energy of the photon, h is Planck's constant (6.626 x 10^(-34) J·s), and f is the frequency. Rearranging the equation, you can solve for f: f = E / h.
d. The color of the emitted photon is determined by its wavelength or frequency. The relationship between wavelength (λ) and frequency (f) is given by the equation c = λf, where c is the speed of light (~3 x 10^8 m/s). Different wavelengths correspond to different colors in the electromagnetic spectrum. You can use this relationship to determine the color of the photon once you have its frequency or wavelength.
To obtain specific values for the energy levels, you may need to refer to a reliable reference source or consult a physics or atomic spectroscopy textbook.