Answer:
For an electron to move from a lower energy level to a higher energy , that electron needs to absorb energy sufficient enough to excite it to make the transition. Hence it is an absorption process. The required energy of transition E = 2.665 x 10⁻²⁰J
Explanation:
Using the Rydberg's equation we can calculate the wavelength of the photon of energy transition as follows:
1/λ = R . (1/nf² - 1/ni²)
where
λ is the required wavelength of the photon needed to be absorbed to excite the electron to transit from level 5 to 6.
(Note that for the electron to transit to from energy level 5 to 6, the photon would have to fall from level 6 to 5 in order to emit the required energy to excite the electron)
R is the Rydberg's constant 1.097 x 10⁷ m⁻¹
nf is the final level of the photon
ni is the initial level of the photon
1/λ = 1.097 x 10⁷ m⁻¹ (1/5² - 1/6²)
1/λ = 1.3407 x 10⁵ m⁻¹
λ = 7.458 x 10⁻⁶ m
This implies that that is the wavelength of the photon required to excite the electron to transit from energy level 5 to 6. Using the equation below, we can calculate the energy of transition as
E = h.c/λ
where
E is the required energy of transition
h is the Planck's constant (6.626 x 10⁻³⁴ Js)
c is the speed of light (3 x 10⁸ms⁻¹)
λ is the wavelength calculated above
E = 6.626 x 10⁻³⁴ Js x 3 x 10⁸ms⁻¹/ 7.458 x 10⁻⁶ m
E = 2.665 x 10⁻²⁰J
