Step-by-step explanation:
Energy levels to be n = 8 and n = 3. Rydberg's equation will allow you calculate the wavelength of the photon emitted by the electron during this transition
1λ = R ⋅ (1/nf^2 − 1/ni^2)
where,
λ - the wavelength of the emitted photon
R - Rydberg's constant = 1.0974 x 10^7m
nf - the final energy = 8
ni - the initial energy level = 3
1/λ = 1.0974 x 10^7 * (1/8^2 − 1/3^2)
= -1.05x 10^6 m.
Using Heinsberg's equation,
E = (h * c)/λ
Calculating the energy of this transition you'll have to multiply Rydberg's equation by h * c
where,
h - Planck's constant = 6.626 x 10^−34 Js
c - the speed of light = 3.0 x 10^8 m/s
So, the transition energy, E = (6.626 x 10^−34 * 3 x 10^8) * -1.05x 10^6
= -2.08 x 10^-19 J.
B.
When an electron transitions from a less excited state to a excited state (higher energy orbit), the difference in energy is absorbed as a photon.
The energy is negative which means energy is lost or dissipated to the surroundings. Therefore, an absorption of photons.